Redox Reactions Questions

We provide redox reactions practice exercises, instructions, and a learning material that allows learners to study outside of the classroom. We focus on redox reactions skills mastery so, below you will get all questions that are also asking in the competition exam beside that classroom.

Redox Reactions Questions

List of redox reactions Questions

Question NoQuestionsClass
1The oxidation number of Fe in
( boldsymbol{K}_{4} boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6} ) is?
( A cdot+6 )
B. +4
( c cdot+3 )
D. +2
11
2Out of ( F e O_{4}^{2-}, F e C l_{3}, F e C l_{2} ) and ( F e )
This question has multiple correct options
A. best reducing agent is ( F e )
B. best oxidising agent is ( F e O_{4}^{2} )
c. best oxidising agent is ( F e C l_{3} )
D. best reducing agent is ( F e O_{4}^{2} )
11
3In three test tubes ( P, Q ) and ( R ) iron nails
water, oil and anhydrous calcium
chloride is taken. Among these test tubes, in which test tubes corrosion of
nails will not take place?
( A cdot P, Q ) and ( R )
B. P and R
c. P and ( Q )
D. Q and
11
4. 31 Assertion (A) The decomposition of hydrogen peroxide to form water
and oxygen is an example of disproportionation reaction.
Reason (R) The oxygen of peroxide is in -1 oxidation state and it is
converted to zero oxidation state in 0, and -2 oxidation state in H20.
(a) Both A and Rare true and R is the correct explanation of A
(b) Both A and Rare true but R is not the correct explanation of A
(c) A is true but R is false
(d) Both A and Rare false
11
5Which of the following has been arranged in order of increasing oxidation number of nitrogen?
A. ( N H_{3}<N_{2} O_{5}<N O<N_{2} )
B . ( N O_{2}^{+}<N O_{3}^{-}<N O_{2}^{-}<N_{3}^{-} )
C . ( N H_{4}^{+}<N_{2} H_{4}<N H_{2} O H<N_{2} O )
D. ( N O_{2}<N a N_{3}<N H_{4}^{+}<N_{2} O )
11
6Balance the following equation by oxidation number method
¡) ( K_{2} C r_{2} O_{7}+K I+H_{2} S O_{4} rightarrow )
( boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
ii) ( K M n O_{4}+N a_{2} S O_{3} rightarrow M n O_{2}+ )
( N a_{2} S O_{4}+K O H )
iii) ( boldsymbol{C u}+boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{C u}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+ )
( N O_{2}+H_{2} O )
iv) ( K M n O_{4}+H_{2} C_{2} O_{4}+H_{2} S O_{4} rightarrow )
( boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{C} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
11
7The oxidation number of iodine in ( I F_{5} ) is11
8When Carbon monoxide is passed over heated copper oxide it gives:
A. ( C O_{2} )
в. ( C O )
( c cdot O_{2} )
D. all of these
11
9Examples of few compounds in a particular oxidation state are given Mark the example which is not correct.
A. Phosphorus in + 1 oxidation state – ( H_{3} P O_{2} )
B. Chlorine in +7 oxidation state – ( H C l O )
c. Chromium in +6 oxidation state ( -C r O_{2} C l_{2} )
D. Carbon in 0 oxidation state ( -C_{12} H_{22} O_{1} )
11
10Which equation is correctly labeled
oxidation or reduction?
( mathbf{A} cdot H_{2} S=S+2 e^{-}+2 H^{+} )
oxidation
B ( cdot S O_{2}+4 e^{-}+2 H_{2} O=S+4 O H^{-} )
oxidation
( mathbf{C} cdot N H_{3}+H C l=N H_{4}++C l_{2}^{-} )
oxidation
D. ( N a C l+A g N O_{3}=A g C l+N a N O_{3} )
reduction
( mathrm{E} cdot M n^{2+}=M n O_{4} )
reduction
11
11State the characteristic of chemical
reaction which takes place when
1) Lead reacts with KI
2) Zinc reacts with HCl
3) Reaction of candle wax
11
12After balancing and reducing the coefficients to lowest whole number
terms, What is the coefficient of ( boldsymbol{H}_{2} boldsymbol{O} ) ?
( boldsymbol{H} boldsymbol{C l}+boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} rightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{K} boldsymbol{C l}+ )
( M n C l_{2}+C l_{2} )
( A cdot 1 )
B. 2
( c .5 )
D. 8
E . 16
11
13Balance the following redox reactions by the ion-electron method in basis
medium
( M n O_{4}^{-}(a q)+I^{-}(a q) rightarrow M n O_{2}(s)+ )
( boldsymbol{I}_{2}(boldsymbol{s}) )
11
14( boldsymbol{H} boldsymbol{C l}(boldsymbol{a q})+boldsymbol{Z n}(boldsymbol{s}) rightarrow boldsymbol{Z n l}_{2}(boldsymbol{a q})+ )
( boldsymbol{H}_{2}(boldsymbol{g}) )
In the above reaction ( boldsymbol{H} boldsymbol{C l} ) (aq) play a
role as:
A. bronsted acid
B. oxidizing agent
c. reducing agemt
D. precipitate
E. cathode
11
1520. Which is the poorest reducing agent?
(a) Atomic hydrogen (b) Nascent hydrogen
(c) Dihydrogen (d) All have same reducing
strength
11
16The total number of ( boldsymbol{H}_{2} boldsymbol{O} ) molecules
present in the balanced chemical
reaction is :
( M n O_{4}^{ominus}+F e^{2+} longrightarrow M n^{2+}+F e^{3+}( ) in
alkaline medium)
11
17Hydrogen sulphide ( left(boldsymbol{H}_{2} boldsymbol{S}right) ) is a strong reducing agent. Which of the following reactions shows its reducing action?
A ( cdot C dleft(N O_{3}right)_{2}+H_{2} S rightarrow C d S+2 H N O_{3} )
B. ( C u S O_{4}+H_{2} S rightarrow C u S+H_{2} S O_{4} )
c. ( 2 mathrm{FeCl}_{3}+mathrm{H}_{2} mathrm{S} rightarrow 2 mathrm{Fe} mathrm{Cl}_{2}+2 mathrm{HCI}+mathrm{S} )
D. ( P bleft(N O_{3}right)_{2}+H_{2} S rightarrow P b S+2 C H_{3} C O O H )
11
18A redox reaction is shown in the
diagrams. Identify the reaction.
( left.mathbf{A} cdot Z n(s)+C u_{(a q)}^{2+} rightarrow Z n_{(a q)}^{2+}+C u_{(} sright) )
B. ( left.C u(s)+2 A g_{a q}^{+} rightarrow C u_{(a q)}^{2+}+2 A g_{(} sright) )
C ( cdot 2 A g(s)+C u_{(a q)}^{2+} rightarrow 2 A g_{(a q)}^{+}+C u(s) )
( left.mathbf{D} cdot C u_{(} sright)+Z n_{(a q)}^{2+} rightarrow C u_{(a q)}^{2+}+Z n(s) )
11
19Assertion
Combining equal volumes of ( 0.2 M )
( A g N O_{3}, ) and ( 0.2 M H C l ) does not
produce a precipitate of ( boldsymbol{A} boldsymbol{g} boldsymbol{C l} )
Reason
The silver ion is rapidly reduced to silver metal, producing chlorine gas.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
20The oxidation number of ( C ) atom in
( C H_{2} C l_{2} ) and ( C C l_{4} ) are respectively
( A cdot-2 ) and -4
B. 0 and -4
( c .0 ) and 4
D. 2 and 4
11
21( H_{3} P O_{4} ) is a tri basic acid and one of its
salt is ( N a H_{2} P O_{4} . ) What volume in ml of
1M NaOH solution should be added to
( 12 g ) of ( N a H_{2} P O_{4} ) to convert it into
( N a_{3} P O_{4} ? )
11
22Complete and balance the following
compound ( boldsymbol{A l} boldsymbol{B} boldsymbol{r}_{3}+boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}+ )
[
boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{4} rightarrow boldsymbol{K}_{3} boldsymbol{P} boldsymbol{O}_{4}+boldsymbol{A} boldsymbol{l} boldsymbol{P} boldsymbol{O}_{4}+
]
11
23Assign oxidation number to the
underlined element in ( boldsymbol{H}_{2} underline{S}_{2} boldsymbol{O}_{7} )
11
24What is redox reaction? In the reaction
( Z n O+C rightarrow Z n+C O ) which
substance gets oxidised and which gets reduced?
11
25The oxidation number of ‘N’ in NOCIO:
( A cdot+3 )
B. +1
( c cdot+2 )
( D cdot+7 )
11
26What is the number of moles of
( K M n O_{4} ) that will be needed to react
completely with one mole of ferrous oxalate in an acidic medium?
11
27Calculate the oxidation number of ( M n )
in the product formed on strongly
heating ( M n_{2} O_{7} )
(write absolute value of an answer)
11
28The oxidation states of ( P ) atom in
( boldsymbol{P O C l}_{3}, boldsymbol{H}_{2} boldsymbol{P O}_{3} ) and ( boldsymbol{H}_{4} boldsymbol{P}_{2} boldsymbol{O}_{6} )
respectively are:
( mathbf{A} cdot+5,+4,+4 )
B. +5,+5,+4
( mathbf{c} cdot+4,+4,+5 )
( mathbf{D} cdot+3,+4,+5 )
11
29Balance the following reaction.
( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{P b C l}_{2}(boldsymbol{a q}) longrightarrow boldsymbol{P b}(boldsymbol{s})+ )
( Z n C l_{2}(a q) )
( mathbf{A} cdot Z n(s)+P b C l_{2}(a q) longrightarrow P b(s)+Z n C l_{2}(a q) )
B ( cdot 2 Z n(s)+P b C l_{2}(a q) longrightarrow P b(s)+2 Z n C l_{2}(a q) )
( mathbf{c} cdot Z n(s)+2 P b C l_{2}(a q) longrightarrow P b(s)+Z n C l_{2}(a q) )
D ( cdot Z n(s)+2 P b C l_{2}(a q) longrightarrow P b(s)+2 Z n C l_{2}(a q) )
11
30In which of the following reactions,
( H_{2} O_{2} ) acts as a reducing reagent?
A ( cdot P b O_{2(s)}+H_{2} O_{2(a g)} rightarrow P b O_{(s)}+H_{2} O_{(i)}+O_{2(g)} )
B. ( N a_{2} S O_{3(a g)}+H_{2} O_{2(a g)} rightarrow N a_{2} S O_{4(a g)}+H_{2} O_{(i)} )
C ( cdot 2 K I_{(a)}+H_{2} O_{2(a)} rightarrow 2 K O H_{(a q)}+I_{2(s)} )
D. All the above
11
31Number of moles of ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) reduced
by one mole of iodide ions is :
A . 3
B. ( frac{1}{3} )
( c .6 )
D.
11
32The sum of the oxidation numbers of all
the carbons in ( C_{6} H_{5} C H O ) is :
( A cdot O )
( B cdot+2 )
( c cdot+4 )
D. – –
11
33Which equation represents charge
balanced equation for a solution of ( boldsymbol{H}_{2} boldsymbol{S} )
in water?
( mathbf{A} cdotleft[H^{+}right]=2left[S^{2-}right]+left[H S^{-}right]+left[O H^{-}right] )
B ( cdotleft[H^{+}right]=left[O H^{-}right] )
C ( cdotleft[H^{+}right]=left[S^{2-}right]+left[H S^{-}right]+left[H^{+}right] )
D. ( left[H^{+}right]=left[S^{2-}right]+left[H S^{-}right]+left[O H^{-}right] )
11
34Which of the following reactions
involves oxidation and reduction?
( mathbf{A} cdot N a B r+H C l rightarrow N a C l+H B r )
B. ( H B r+A g N O_{3} rightarrow A g B r+H N O_{3} )
( mathbf{c} cdot H_{2}+B r_{2} rightarrow 2 H B r )
D. ( N a_{2} O+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+H_{2} O )
11
35Hydrolysis of ( X e F_{6} ) in strongly alkaline solution is an auto-redox process.
If true enter 1 , else enter 0
( A )
11
36What will be the octane number of best
fuel?
A. 80
B. 81
( c cdot 82 )
D. 83
11
37Balance the following equation.
( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}_{2} boldsymbol{O}_{3}+ )
( boldsymbol{S}_{8}+boldsymbol{H}_{2} boldsymbol{O} )
( mathbf{A} cdot 24 H_{2} S+8 C r_{2} O_{7}^{2-}+16 H^{+} rightarrow 8 C r_{2} O_{3}+3 S_{8}+32 H_{2} O )
B ( cdot 24 H_{2} S+3 C r_{2} O_{7}^{2-}+6 H^{+} rightarrow 7 C r_{2} O_{3}+3 S_{8}+32 H_{2} O )
( mathbf{c} cdot 24 H_{2} S+8 C r_{2} O_{7}^{2-}+5 H^{+} rightarrow 6 C r_{2} O_{3}+4 S_{8}+32 H_{2} O )
D. None of these
11
38A student places a strip of solid magnesium metal into a beaker full of
( 100 . m L ) of ( 3.0 mathrm{M} ) hydrochloric acid
solution. The student observes bubbling and the disappearance of the magnesium metal.
Which species is being oxidized and which species is being reduced in this
reaction?
A. Magnesium being oxidized and the chloride ion is being reduced.
B. Magnesium being oxidized and the hydrogen ion is being reduced.
c. Magnesium being reduced and the chloride ion is being oxidized.
D. Magnesium being reduced and the hydrogen ion is being oxidized.
11
39Which statement(s) is/are not correct
about the reaction?
( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow )
( boldsymbol{I}_{2}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(l) boldsymbol{I}_{2}(boldsymbol{a} boldsymbol{q})+ )
( mathbf{2} N a_{2} S_{2} O_{3} rightarrow N a_{2} S_{4} O_{6}+2 N a I ? )
This question has multiple correct options
A. The ( I_{2} ) formed is consumed completely in the second state is confirmed by addition of starch just before its complete consumption
B. The reaction process is called clock reaction because the appearance of blue colour on addition of starch is like an alarm given by clock
c. Sulphur is oxidised whereas iodine is oxidised and reduced during whole process
D. ( H_{2} O_{2} ) acts as reducing agent
11
40It is a chemical reaction where two
reactants, each containing the same element but with a different oxidation
number, will form a product in which the elements involved reach the same
oxidation number. This reaction is
called:
A. Comproportionation reaction
B. Disproportionation reaction
c. Reduction
D. Double displacement reaction
11
41Write the type of reaction. Ethene is burnt in the presence of oxygen to form carbon dioxide, water
and releases heat and light.
A. Endothermic reaction
B. Combustion reaction
c. Redox reaction
D. Esterificaton reaction
11
42Assertion
Fluorine always exhibits an oxidation
state of -1 in its compounds.
Reason
Fluorine has maximum
electronegativity and it contain seven electrons in its valence shell.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
43Balance the following redox reactions in basc medium:
[
M n O_{4}^{-}+I^{-} longrightarrow M n O_{2}+I O_{3}^{-}
]
A ( cdot 2 M n O_{4}^{-}+I^{-}+H_{2} O longrightarrow 2 M n O_{2}+I O_{3}^{-}+2 O H^{-} )
B. ( 3 M n O_{4}^{-}+I^{-}+H_{2} O longrightarrow 4 M n O_{2}+I O_{3}^{-}+2 O H^{-} )
( mathrm{c} cdot 3 mathrm{Mn} mathrm{O}_{4}^{-}+I^{-}+mathrm{H}_{2} mathrm{O} longrightarrow 5 mathrm{MnO}_{2}+mathrm{IO}_{3}^{-}+2 mathrm{OH}^{-} )
D. None of these
11
44Although ( C u^{+} ) disproportionates in
aqueous solution as ( 2 C u^{+}(a q) rightarrow )
( boldsymbol{C u}(boldsymbol{s})+boldsymbol{C u}^{2+}(boldsymbol{a q}) . ) Write down a
reaction in which disproportionation is reversed.
A ( cdot C u(s)+C u^{2+}(a q)+2 C l^{-} rightarrow C u C l(s) )
в. ( C u(l)+C u^{2+}(a q)+2 C l^{-} rightarrow C u C l(l) )
c. ( C u(s)+C u^{+}(a q)+C l^{-} rightarrow C u C l(s) )
D. None of these
11
45Which of the following species will not exhibit disproportionation reaction?
A ( cdot C l O^{-} )
B. ( C l O_{2}^{-} )
( mathrm{c} cdot mathrm{ClO}_{3}^{-} )
D. ( C l O_{4}^{-} )
11
46Which of the following statement is
correct?
A. Oxidation involves gain of electron
B. Substance which is reduced is reducing agent
C. Exothermic process involves absorption of heat
D. Oxidation involves loss of electrons
11
47Q7. Write the cell reactions:
Zn Zn2+(1M) / Cd2+(1M) Cd
E° Zn + Zn = -0.76 V, E° Cd2+/Cd = 0.40 V
72+ Coolt
11
48( Delta_{r} H ) of which of the following reaction
is zero?
( mathbf{A} cdot H_{2(g)} rightarrow 2 H_{(g)}^{+}+2 e^{-} )
B. ( 2 H_{(g)}+a q rightarrow 2 H_{(a q)}^{+}+2 e^{-} )
( mathbf{c} cdot 2 H_{(g)} rightarrow 2 H_{(g)}^{+}+2 e^{-} )
D. ( H_{2(g)}+a q rightarrow 2 H_{(a q)}^{+}+2 e^{-} )
11
49Q4. Find out the oxidation state of sodium in Na,O
in Mo
11
50The ( M n^{3+} ) ion is unstable in solution
and undergoes disproportionation to ( operatorname{give} M n^{2+}, M n O_{2} ) and ( H^{+} ) ion. Write a
balanced ionic equation for the reaction.
11
51The complete balanced equation is:
( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{K}_{2} boldsymbol{C r} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow )
A ( cdot 3 mathrm{H}_{2} S+2 mathrm{K}_{2} mathrm{CrO}_{4}+5 mathrm{H}_{2} mathrm{SO}_{4} rightarrow mathrm{Cr}_{2}left(mathrm{SO}_{4}right)_{3}+ )
( 2 K_{2} S O_{4}+8 H_{2} O+3 S )
B. ( 3 H_{2} S+K_{2} C r O_{4}+5 H_{2} S O_{4} rightarrow C r_{2}left(S O_{4}right)_{3}+ )
( K_{2} S O_{4}+8 H_{2} O+3 S )
c. ( H_{2} S+2 K_{2} C r O_{4}+3 H_{2} S O_{4} rightarrow C r_{2}left(S O_{4}right)_{3}+ )
( 2 K_{2} S O_{4}+8 H_{2} O+3 S )
D. none of these
11
52Which is not redox change?
( mathbf{A} cdot C a C O_{3} rightarrow C a O+C O_{2} )
( mathbf{B} cdot 2 H_{2}+O_{2} rightarrow 2 H_{2} O )
( mathrm{c} cdot_{N a}+H_{2} O rightarrow N a O H+frac{1}{2} H_{2} )
D. ( M n C I_{3} rightarrow M n C I_{2}+frac{1}{2} C I_{2} )
11
53The balanced molecular equation is :
A. ( C l_{2}+H_{2} O+N a_{2} S_{2} O_{3} rightarrow N a_{2} S O_{4}+S+2 H C l )
в. ( C l_{2}+N a_{2} S_{2} O_{3} rightarrow 2 N a C l+N a_{2} S O_{4} )
c. ( quad C l_{2}+S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S+C l )
D. none of these
11
54Amongst the following, identify the species with an atom in +6 oxidation
state.
( mathbf{A} cdotleft[M n O_{4}right]^{-} )
B . ( left[operatorname{Cr}(C N)_{6}right]^{3-} )
( mathrm{c} cdot mathrm{Cr}_{2} mathrm{O}_{3} )
D. ( operatorname{Cr} mathrm{O}_{2} mathrm{Cl}_{2} )
11
55An amount of 0.2 mole of ( A O_{3}^{-} ) gains 1.2
mole of electron in a process. Assuming that there is no change in oxidation state of oxygen, determine the oxidation state of ‘A’ in product:
( A cdot+1 )
B. –
( c cdot 0 )
( D cdot+6 )
11
56Mixture of ( boldsymbol{N a I}(boldsymbol{s})+boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}(boldsymbol{s})+ )
conc. ( H_{2} S O_{4} ) when heated in a test
tube dark vapours evolve
A. ( I_{2} )
в. ( N a_{2} )
( mathrm{c} cdot H_{2} )
D. All the above
11
57( boldsymbol{A}^{+} boldsymbol{B}^{-}+boldsymbol{C}^{+} boldsymbol{D}^{-} longrightarrow boldsymbol{A}^{+} boldsymbol{D}^{-}+boldsymbol{C}^{+} boldsymbol{B}^{-} )
Identify the above generalized type of
reaction:
A. Chemical replacement reaction
B. Chemical double decomposition reaction
c. Chemical displacement reaction
D. Chemical combination reaction
11
58Reduction of the metal centre in
aqueous permanganate ion involves:
This question has multiple correct options
A. 3 electrons in neutral medium
B. 5 electrons in neutral medium
c. 1 electron in alkaline medium
D. 5 electrons in acidic medium
11
59Which of the following statements is not correct about the given reaction? ( boldsymbol{K}_{4}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6} frac{text {Oxidation}}{boldsymbol{leftrightarrow}} boldsymbol{F} boldsymbol{e}^{3+}+boldsymbol{C O}_{2}+right. )
( mathbf{N} boldsymbol{O}_{mathbf{3}}^{-} )
A. Fe is oxidised from ( F e^{2+} ) to ( F e^{3 text { – }} )
B. Carbon is oxidised from ( C^{2+} ) to ( C^{4+} ).
c. ( mathrm{N} ) is oxidised from ( N^{3} ) – to ( N^{5+} )
D. Carbon is not oxidised
11
60A redox reaction is one in which:
A. both the substances are reduced
B. both the substances are oxidized
c. an acid is neutralized by the base
D. one substance is oxidized, while the other is reduced
11
61The reaction, ( A B rightarrow A+B ) is a:
This question has multiple correct options
A. Decombination reaction
B. Combination reaction
c. chemical composition
D. Decomposition reaction
11
62Which of the following is true about the reaction ( boldsymbol{F} boldsymbol{e}+boldsymbol{S} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{S} ? )
This question has multiple correct options
A ( cdot F e+2 e^{-} rightarrow F e^{2+} )
B. ( F e rightarrow F e^{2+}+2 e^{-} )
C ( cdot F e^{2+} rightarrow F e+2 e^{-} )
D. ( S rightarrow S^{2-}+2 e^{-} )
E ( . S+2 e^{-} rightarrow S )
11
630.16 Which of the following electrodes will act as anodes, which connected to
Standard Hydrogen Electrode ?
(a) AI/AP+ E = -1.66
(6) Fe/Fe2+
= -0.44
(c) Cu/Cu2+
E = +0.34
(d) F2 (g)/2F- (aq) E=0287
11
64Assertion
( H_{3} P O_{2} ) can act as strong reducing agent and gives disproportionation reaction on heating.
Reason
Due to presence of one ( -O H ) group and
( boldsymbol{P}-boldsymbol{H} ) group, ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{2} ) is a monobasic
bronsted acid.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
65Calculate the oxidation number of ( F e ) in
( boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right] )
11
66Which of the following substances undergo(s) disproportionation reactions under basic medium?
This question has multiple correct options
A. ( F_{2} )
в. ( P_{4} )
( mathrm{c} cdot S_{8} )
D. ( B r_{2} )
11
67The number of moles of ( K M n O_{4} ) that will be needed to react completely with
one mole of ferrour oxalate ( F eleft(C_{2} O_{4}right) ) in acidic solution is :
( mathbf{A} cdot mathbf{1} )
B. ( frac{2}{5} )
( c cdot frac{3}{5} )
D.
11
68Balance the following equation:
( boldsymbol{C u}(boldsymbol{s})+boldsymbol{A} boldsymbol{u}^{oplus} longrightarrow boldsymbol{A u}(boldsymbol{s})+boldsymbol{C u}^{2+} )
( mathbf{A} cdot C u(s)+2 A u^{oplus} longrightarrow A u(s)+C u^{2+} )
B ( cdot C u(s)+2 A u^{oplus} longrightarrow 2 A u(s)+C u^{2+} )
( mathbf{c} cdot 2 C u(s)+A u^{oplus} longrightarrow 2 A u(s)+2 C u^{2+} )
D ( cdot 2 C u(s)+A u^{oplus} longrightarrow 2 A u(s)+C u^{2+} )
11
69Match the Column-I with Column-II.11
70Balance the following redox reaction ( left(boldsymbol{C r}_{2} boldsymbol{O}_{7}right)_{(a q)}^{2-}+boldsymbol{F} boldsymbol{e}_{(a q)}^{2+} rightarrow boldsymbol{C r}_{(a q)}^{3+}+boldsymbol{F} boldsymbol{e}_{(a q)}^{3+} )
(acidic medium)
11
71In double decomposition reaction are exchanged11
72Assertion
In the titration of ( N a_{2} C O_{3} ) with ( H C l )
using methyl orange indicator, the volume required at the equivalence
point is twice that of the acid required using phenolphthalein indicator.
Reason
Two mole of ( H C l ) are required for the
complete neutralization of one mole of
( N a_{2} C O_{3} )
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is incorrect but Reason is correct
D. Both Assertion and Reason are correct
11
73Balance the following equation and find the values of ( a, b, c, d ) ( boldsymbol{a} boldsymbol{P b O}_{2}+boldsymbol{b C l}^{ominus} longrightarrow boldsymbol{c} boldsymbol{C l O}^{ominus}+ )
( boldsymbol{d}left[boldsymbol{P b}(boldsymbol{O H})_{3}right]^{ominus}(text { in basic solution }) )
В. ( a=1, b=1, c=1, d=1 )
c. ( a=2, b=1, c=1, d=2 )
D. ( a=1, b=1, c=2, d=2 )
11
74Hydrogen atom in the basic medium is balanced by which of the following species?
A ( cdot O H^{-} )
в. ( H^{+} )
c. ( H_{3} O^{+} )
D. ( H_{2} )
11
75Give the oxidation state of underlined.
( boldsymbol{C a O C l}_{2} )
11
76Which one of the following leads to redox reaction?
A. ( A g N O_{3}+H C l )
в. ( K O H+H C l )
c. ( K I+C l_{2} )
D. ( N H_{3}+H C l )
11
77Find the oxidation number of ( mathrm{P} ) in ( boldsymbol{P} boldsymbol{H}_{4}^{+} )11
78When the gases; sulphur dioxide and hydrogen sulphide mix in the presence
of water, the reaction ( S O_{2}+2 H_{2} S rightarrow )
( 2 H_{2} O+3 S ) occurs
Here hydrogen sulphide is acting as:
A. an oxidizing agent
B. a reducing agent
c. a dehydrating agent
D. a catalyst
11
79Above diagram represents an atom ( X )
Atom ‘X’ is a reducing agent.
A . True
B. False
11
80What is the oxidation state of central
( operatorname{atom} operatorname{in} C aleft[P t C l_{4}right] ? )
( mathbf{A} cdot mathbf{1} )
B . 2
( c .3 )
D. 4
11
81The sum of the oxidation numbers of all
the atoms in a neutral molecule is
equal to:
A. zero
B. one
c. three
D. four
11
82The other name of comproportionation
is:
A. disproportionation
B. proportionation
c. symproportionation
D. antiproportionation
11
83The compound(s) which generate(s) ( N_{2} ) gas upon thermal decomposition below
( 300^{circ} mathrm{C} ) is/are:
This question has multiple correct options
A. ( N H_{4} N O_{3} )
B. ( left(N H_{4}right)_{2} C r_{2} O_{7} )
c. ( B aleft(N_{3}right)_{2} )
D. ( M g_{3} N_{2} )
11
848. Consider the following reaction,
(NH2)2Cr2O, –> N2 + Cr,O, +4H,0
(a) it is an example of intramolecular redox reaction
(b) it is an example of intermolecular redox reaction
(C) NH4 ion is a reducing agent and Cr,04 is an
oxidizing agent
(d) it is an example of disproportionation reaction
11
85Balance the following equation:
( boldsymbol{C u O}+boldsymbol{N H}_{3} rightarrow boldsymbol{N}_{2}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u} )
11
86Write balanced chemical equations for
the conversion of ( C r O_{4}^{2-} ) to ( C r_{2} O_{7}^{2-} ) in acidic medium and ( C r_{2} O_{7}^{2-} ) to ( C r O_{4}^{2-} )
in basic medium.
11
87( boldsymbol{C l O}^{-} rightleftarrows boldsymbol{C l O}_{3}^{-}+boldsymbol{C l}^{-} )
When the equation for the reaction represented above is balanced with
coefficients reduced to the lowest
whole-umber terms, correct statements
include which of the following?
I. The coefficient for ( C l^{-} ) is 4
II. The coefficient for ( C l O_{3}^{-} ) is 2
III. The coefficient for ( C l O^{-} ) is 3
A. I only
B. II only
C. III only
D. I and II only
E . I, II and III only
11
88Assertion
Statement ( 1: H g C l_{2} ) and ( S n C l_{2} ) exist
together in an aqueous solution.
Reason

Statement ( 2: S n C l_{2} ) is a strong
reducing agent.
A. Statement 1 is true, Statement 2 is true and Statement 2 is correct explanation for Statement
B. Statement 1 is true, Statement 2 is true and Statement 2 is not the correct explanation for Statement
c. Statement 1 is true, Statement 2 is false
D. Statement 1 is false, Statement 2 is true

11
894 mol of a solution containing ( boldsymbol{A}^{boldsymbol{n}} ) requires 1.6 mol of ( M n O_{4}^{ominus} ) for the oxidation of ( A^{n+} ) to ( A O_{3}^{ominus} ) in acidic
medium. The value of ( n ) is :
A . 1
B . 2
( c .3 )
D.
11
900.1M of ( boldsymbol{H} boldsymbol{A} ) is titrated with ( mathbf{0 . 1} boldsymbol{M} )
( N a O H, ) calculate ( p H ) at end point ( operatorname{Given} K(H A)=5 times 10^{-6} ) and ( alpha ll 1 )
11
91Find the oxidation number of ( N & C l ) in
( N O C l_{4} ) respectively is:
( A cdot+3,+6 )
B. +2,+6
( mathrm{c} cdot+3,+7 )
( mathrm{D} cdot+2,+7 )
11
92When the equation: ( C_{2} H_{6}+O_{2} rightarrow )
( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is completely
balanced using the lowest whole number coefficients, the sum of
the coefficients will be :
A . 4
B. 9.
c. 19
D. 15.5
E. 1
11
93In the reaction: ( 3 C l_{2}+6 N a O H longrightarrow )
( mathbf{5} N a C l+N a C l O_{3}+3 H_{2} O, C l_{2} ) acts
purely as an oxidizing agent.
If true enter 1 , else enter 0 .
A.
11
94Identify ( M ) and ( N ) in the following
reaction.
Copper glance controlledheating in presence
( boldsymbol{M}+boldsymbol{S O}_{2} uparrow )
( boldsymbol{M} stackrel{N}{longrightarrow} boldsymbol{C} boldsymbol{u}+boldsymbol{S} boldsymbol{O}_{2} uparrow )
( boldsymbol{M} stackrel{N}{longrightarrow} boldsymbol{C} boldsymbol{u}+boldsymbol{S} boldsymbol{O}_{2} uparrow )
A . ( M=C u_{2} O ; N= ) self reduction
B. ( M=C u_{2} O+C u_{2} S ; N= ) self reduction
c. ( M=C u_{2} O ; N= ) carbon reduction
D. ( M=C u_{2} O ; N= ) electrolytic reduction
11
95In the reaction ( 2 N a_{2} S_{2} O_{3}+I_{2} rightarrow )
( N a_{2} S_{4} O_{6}+2 N a I, ) the oxidation state
of sulphur is :
A. decreased
B. increased
c. unchanged
D. none of these
11
96( 100 mathrm{mL} ) solution of ( 0.1 mathrm{M} H C l ) was
titrated with 0.2 ( N a O H ) solution. The
titration was discontinued after the
addition of ( 30 mathrm{mL} ) of ( mathrm{NaOH.} ) The
remaining titration was completed with the addition of 0.5 M ( K O H . ) The volume
of ( K O H ) required for completing the titration is:
( A cdot 8 m L )
в. ( 16 m L )
c. ( 32 m L )
D. ( 64 m L )
11
97Which of the following is not a disproportionation reaction?
( mathbf{A} cdot stackrel{ominus}{O} H+B r_{2} longrightarrow B r^{ominus}+B r O_{3}^{mathbf{j}} )
в. ( C u_{2} O+2 H^{oplus} rightarrow C u+C u^{2+}+H_{2} O )
( mathrm{c} cdot(C N)^{ominus} rightarrow C O_{3}^{2-}+N O_{3}^{circ} )
D ( cdot(C N)_{2}+2 hat{O} H rightarrow C N^{ominus}+C N O^{ominus}+H_{2} O )
11
98( boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{4} boldsymbol{C} rightarrow boldsymbol{B} boldsymbol{a} boldsymbol{S}+boldsymbol{4} boldsymbol{C} boldsymbol{O} )
In above reaction, write for each
reactant that undergoes oxidation or reduction and identify the type of
reaction.
11
99The reaction of ( K M n O_{4} ) and ( mathrm{HCl} )
results in
A. Oxidation of ( mathrm{Mn} ) in ( mathrm{KMnO}_{4} ) and production of ( mathrm{Cl}_{2} )
B. Reduction of Mn in ( K M n O_{4} ) and production of ( H_{2} )
C. Oxidation of ( mathrm{Mn} ) in ( mathrm{KMnO}_{4} ) and production of ( mathrm{H}_{2} )
D. Reduction of Mn in ( K M n O_{4} ) and production of ( C l_{2} )
11
100Balance the following equation by
oxidation number method.
( A l+K M n O_{4}+H_{2} S O_{4} rightarrow )
( boldsymbol{A l}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{S} boldsymbol{O}_{4}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
11
101Determine the oxidation state of Cr in
( left[boldsymbol{C r}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4} boldsymbol{C l}_{2}right] boldsymbol{C l} )
( A cdot+3 )
B . – –
( c cdot+2 )
( D cdot+4 )
11
102The oxidation number of ( mathrm{N} ) and ( C l ) in
( N O C l O_{4} ) respectively are :
( A cdot+2 ) and +7
B. +3 and +7
( c cdot-3 ) and +5
D. +2 and -7
11
103Oxidation number of ( ^{prime} boldsymbol{N}^{prime} ) in ( boldsymbol{N}_{3} boldsymbol{H} )
(hydrazoic acid) is:
( ^{A} cdot-frac{1}{3} )
B. +3
c. 0
D. –
11
104( K M n O_{4} ) reacts with oxalic acid
according to the equation ( 2 M n O_{4}^{-}+5 C_{2} O_{4}^{2-}+16 H^{+} rightarrow )
( mathbf{2} M n^{2+}+mathbf{1 0} C O_{2}+mathbf{8} H_{2} O )

Here ( , 20 m L ) of ( 0.1 mathrm{M} K M n O_{4} ) is
equivalent to:

This question has multiple correct options
A ( cdot 120 m L ) of 0.25 M ( H_{2} C_{2} O_{4} )
B. ( 50 m L ) of 0.10 M ( H_{2} C_{2} O_{4} )
c. ( 25 m L ) of 0.20 M ( H_{2} C_{2} O_{4} )
D. ( 50 m L ) of ( 0.20 mathrm{M} mathrm{H}_{2} mathrm{C}_{2} mathrm{O}_{4} )

11
105n ( N i(C O)_{4}, ) the oxidation state of Ni is:
( A cdot 4 )
B.
( c cdot 2 )
D. 8
11
106What would be the stoichiometric
coefficient of hydrochloric acid in the following equation?
( boldsymbol{C l}_{2}+_{–} boldsymbol{H}_{2} boldsymbol{O} rightarrow_{–} boldsymbol{H} boldsymbol{C l}+_{-} )
( boldsymbol{H} boldsymbol{C l O}_{3} )
( A )
B. 3
( c cdot 5 )
D. 10
11
107Balance the following equations by ion electron method.
( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{N} boldsymbol{O}_{2}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
11
108Electrolysis of water to form hydrogen
and oxygen gases is :
A. precipitation
B. oxidation-reduction
c. distillation
D. hydration
E. condensation
11
109The species undergoin disproportionation is:
( mathbf{A} cdot B r O_{4}^{-} )
B. ( B r O_{3}^{-} )
( mathbf{c} cdot H B r O )
( mathbf{D} cdot B r )
11
110Which of the following is an example of a disproportionation reaction?
A. ( C a C O_{3} rightarrow C a O+C O_{2} )
в. ( 2 H C u C l_{2} rightarrow C u+C u^{2+}+4 C l^{-}+2 H^{+} )
c. ( P C l_{5} rightarrow P C l_{3}+C l_{2} )
D. ( 2 H_{2} S+S O_{2} rightarrow 2 H_{2} O+3 S )
11
111Sodium chloride and sodium iodide
react with concentrated sulfuric acid
Which statements are correct?
1. Sodium chloride is not oxidised by concentrated sulfuric acid.
2. No colour change is seen when concentrated sulfuric acid is added to
sodium chloride
3. Sodium iodide is oxidised by concentrated sulfuric acid.
A. 1,2 and 3 are correct
B. 1 and 2 only are correct
c. 2 and 3 only are correct
D. 1 only is correct
11
112For decolourisation of 1 mole of acidified
( K M n O_{4} ) the moles of ( H_{2} O_{2} ) required
are:
A ( cdot 1 / 2 )
B. 3/2
( c cdot 5 / 2 )
D. 7/2
11
1131 mol of ferric oxalate is oxidised
completely by ( x ) mol of ( M n O_{4}^{-} ) in acidic medium. Then, ( x ) is :
A . 1.2
в. 1.6
c. 1.8
D. 1.5
11
114Balance the following ionic equations
(i) ( boldsymbol{C} boldsymbol{r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{H}^{+}+boldsymbol{I}^{-} rightarrow boldsymbol{C} boldsymbol{r}^{boldsymbol{3}+}+ )
( boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
(ii) ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{F} boldsymbol{e}_{2}^{+}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}^{3+}+ )
( boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{H}_{2} boldsymbol{O} )
(iii) ( M n O^{4-}+S O_{3}^{2-}+H^{+} rightarrow )
( M n^{2+}+S O_{4}^{2-}+H_{2} O )
(iv) ( M n O^{4-}+H^{+}+B r^{-} rightarrow M n^{2+}+ )
( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
11
115Which of the following will act as
anodes when connected to standard
hydrogen electrode?
This question has multiple correct options
( mathbf{A} cdot A l / A l^{3+} ; quad E^{-}=-1.66 )
( mathbf{B} cdot F e / F e^{2+} ; quad E^{-}=-0.44 )
( mathbf{c} cdot C u / C u^{2+} ; quad E^{-}=+0.34 )
D ( cdot F_{2}(g) / 2 F^{-}(a q) ; quad E^{-}=+2.87 )
11
116Which of the following is a non-redox
process?
This question has multiple correct options
A ( cdot S O_{4}^{2-} rightarrow S O_{3} )
B. ( C r_{2} O_{7}^{2-} rightarrow C r O_{4}^{2} )
( mathbf{c} cdot P O_{4}^{3-} rightarrow P_{2} O_{7}^{4} )
( mathrm{D} cdot C_{2} O_{4}^{-2} rightarrow C O_{2} )
11
117When benzaldehyde is oxidised to give benzoic acid then the oxidation state of
carbon of aldehydic group is changed from:
( mathbf{A} cdot+2 ) to +3
B. +1 to +3
c. zero to +2
D. No change
11
118The reaction,
( 3 C l O^{-}(a q) rightarrow C l O_{3}^{-}(a q)+2 C l^{-} )
A. Oxidation reaction
B. Reduction reaction
c. Disproportionation reaction
D. neutralisation reaction
11
119The number of moles of ( K M n O_{4} ) that will be needed to react completely with one mole of sulphite ion in acidic
solution is:
A . ( 3 / 5 )
B. 2/5
c. ( 4 / 5 )
( D )
11
120State whether the given statement is true or false.
( X^{2+}+2 e^{-} rightarrow X ) is an example of
oxidation.
A. True
B. False
11
121Assertion
Decomposition of hydrogen peroxide is an example of disproportionation
reaction.
Reason
In a disproportionation reaction, an
element in one oxidation state is
simultaneously oxidised and reduced.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
1222.1 Which of the following is not an example of redox reactions
(a) CuO+ H Cu+ H,O
(b) Fe,, + 3C0 2 Fe + 300,
(c) 2K+F, 2KF
(d) BaCl, HSO Baso, + 2HCI
11
123In the electrochemical series, metals
are arranged in order of their tendency
to
A. release halogens from their salts
B. become reduced
c. react with water
D. lose electrons
11
124Match the reactions in Column I with
nature of the reactions/type of the products in Column II.
11
125Q. 35 Why does fluorine not show disproportionation reaction?11
126Which of the following shows highest oxidation number in combined state?
A. ( O s )
в. ( R u )
c. Both (1) & (2)
D. None
11
127In which of the following reactions does
( O_{2} ) acts as an oxidant?
This question has multiple correct options
( mathbf{A} cdot 3 O_{2} rightarrow 2 O_{3} )
B. ( 2 F_{2}+O_{2} rightarrow 2 F_{2} ) O
c. ( N_{2}+O_{2} rightarrow 2 N O )
D. ( C+O_{2} rightarrow C O_{2} )
11
128Which one of the following compounds involve in disproportionation reaction with water?
A. ( X e F_{2} )
в. ( X e F_{4} )
c. ( X e F_{6} )
D. ( X e O_{2} F_{2} )
11
129The ratio of number of moles of
( K M n O_{4} ) and ( K_{2} C r_{2} O_{7} ) required to
oxidise ( 0.1 mathrm{mol} mathrm{Sn}^{+4} ) in acidic medium:
A .6: 5
B. 5: 6
c. 1: 2
D. 2: 1
11
130Identify from the reaction the reactants that undergo oxidation and reduction ( F e+S rightarrow F e S )11
131Which of the following is a redox reaction?
A ( cdot C a C O_{3} rightarrow C a O+C O_{2} )
в. ( H_{2}+C l_{2} rightarrow 2 H C l )
( mathrm{c} cdot mathrm{CaO}+2 mathrm{HCl} rightarrow mathrm{CaCl}_{2}+mathrm{H}_{2} mathrm{O} )
D. ( N a O H+H C l rightarrow N a C l+H_{2} O )
11
132Assertion
All the stoichiometric calculations are
based on law of conservation of mass.
Reason

In redox reactions, both oxidation and
reduction takes place simultaneously.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect

11
133The redox reaction among the following
is :
( mathbf{A} cdot ) reaction of ( left[mathrm{Co}left(mathrm{H}_{2} mathrm{O}right)_{6}right] mathrm{Cl}_{3} ) with ( mathrm{AgNO}_{3} )
B. formation of ozone from atmospheric oxygen in the presence of sunlight
C. combination of dinitrogen with dioxygen at ( 2000 K )
D. reaction of ( H_{2} S O_{4} ) with ( N a O H )
11
134The coefficient of ( boldsymbol{I}^{-}, boldsymbol{I} boldsymbol{O}_{3}^{-} ) and ( boldsymbol{H}^{+} ) in
the redox reaction, ( boldsymbol{I}^{-}+boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+} rightarrow )
( I_{2}+H_{2} O, ) in the balanced form
respectively are:
( mathbf{A} cdot 5,1,6 )
в. 1,5,6
c. 6,1,5
D. 5,6,1
11
135What is the oxidation number of ( boldsymbol{H} ) and
( C l ) in ( H C l O_{4} ) respectively?
( A cdot+1,+7 )
B. +2,+6
( mathrm{c} cdot+3,+7 )
( mathrm{D} cdot+2,+7 )
11
136Which of the following show non-zero multiple oxidation state?
A . ( S )
B. ( O )
( c cdot Z n )
D. ( H )
11
137Assertion
The oxidation state of Cr in
( A l_{2}left(C r_{2} O_{7}right)_{3} ) is +3
Reason
As a neutral compound, the sum of the oxidation numbers of all the atoms
must equal zero
A. Both assertion and reason are correct and reason is the correct explanation for assertion
B. Both assertion and reason are correct but reason is not the correct explanation for assertion
c. Assertion is correct but reason is incorrect
D. Both assertion and reason are incorrect
11
138Which of the following cell
representations is/are correct?
This question has multiple correct options
( left.mathbf{A} cdot P l, H_{2}(1 b a r)|H C I(a q)| C l_{2}(1 b a r)right) P t )
B . ( H gleft|H g_{2} C l_{2}(S)right| H C l(a q) mid H_{2}(1 b a r), P t )
( mathbf{c} cdot A t|A g C l(s)| K C I(a q)left|H g_{2}(s)right| H g )
D ( cdot P t_{3} H_{2}(1 b a r)|H l| A u l(s) mid A mu )
11
139Balanced chemical equation imply which of the following?
A. Numbers of atoms are conserved in a chemica change
B. Numbers of molecules are conserved in a chemica change
c. volume is conserved in a chemical change
D. ‘A’ and ‘B’
E . ‘B’ and ‘C’
11
140Give the oxidation state of underlined.
( N H 4 N O_{3} )
11
141The values of coefficients to balance the
following reaction are:
( boldsymbol{C r}(boldsymbol{O H})_{3}+boldsymbol{C l O}^{-}+boldsymbol{O H}^{-} rightarrow )
( boldsymbol{C r} boldsymbol{O}_{4}^{2-}+boldsymbol{C l}^{-}+boldsymbol{H}_{2} boldsymbol{O} ? )
A ( cdot operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(3), C r O_{4}^{2-}-(3), C l^{-}-(3) )
B. ( operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(4), C r O_{4}^{2-}-(3), C l^{-}-(2) )
c. ( operatorname{Cr}(O H)_{3}-(2), operatorname{ClO}^{-}-(4), operatorname{Cr} O_{4}^{2-}-(4), C l^{-}-(2) )
D. ( operatorname{Cr}(O H)_{3}-(2), C l O^{-}-(3), C r O_{4}^{2-}-(2), C l^{-}-(3) )
11
142Calculate oxidation number of central
( operatorname{atom} operatorname{in}left[boldsymbol{K}_{4}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right]right. )
11
143When ( S O_{2} ) is passed in acidified potassium dichromate solution, the oxidation number of ( S ) is changed from:
( A cdot+4 ) to zero
B. +4 to +2
( mathbf{c} cdot+4 ) to +6
D. +6 to +4
11
144State True or False.
The following reaction is a
disproportionation reaction. ( N H_{4} N O_{3} stackrel{Delta}{longrightarrow} N_{2} O+2 H_{2} O )
11
145Which of the following is redox
reaction?
( mathbf{A} cdot N a O H+H C I rightarrow N a C l+H_{2} O )
B. ( A g N O_{3}+K l rightarrow A g l+K N O_{3} )
( mathbf{c} cdot B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} )
( mathbf{D} cdot operatorname{Sn} C l_{2}+H g C l_{2} rightarrow S n C l_{4}+H g )
11
146Q. 32 Assertion (A) Redox couple is the combination of oxidised and reduced
form of a substance involved in an oxidation or reduction half cell.
Reason (R) In the representation 3+ 2+ and Eo2+ Fe / Fe and
Cu²+ / Cu are redox couples.
(a) Both A and R are true and R is the correct explanation of
A T
(b) Both A and Rare true but Ris not the correct explanation of A
(c) A is true but R is false
(d) Both A and Rare false anh
MOMA (A) not
11
147Select Redox reaction from the
following:
A ( . Z n+C u S O_{4} rightarrow Z n S O_{4}+C u )
в. ( C a O+2 H C l rightarrow C a C l_{2}+H_{2} O )
c. ( N a O H+2 H C l rightarrow N a C l+H_{2} O )
D. ( C a C O_{3} rightarrow C a O+C O_{2} )
11
148Which of the following reactions is not a
redox reaction?
A ( cdot A g^{+}+C l^{-} rightarrow A g C l )
B. ( Z n(s)+C u^{2+}(a q .) rightarrow Z n^{2+}(a q .)+C u(s) )
( mathrm{c} cdot 2 M g(s)+O_{2}(g) rightarrow 2 M g O )
D. ( F e O+C rightarrow F e+C O )
11
149Which is the best description of the
behaviour of bromine in the reaction
given below?
( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{B} boldsymbol{r}_{2} rightarrow boldsymbol{H} boldsymbol{O} boldsymbol{B} boldsymbol{r}+boldsymbol{H} boldsymbol{B} boldsymbol{r} )
A. Proton acceptor only
B. Both oxidised and reduced
c. oxidised only
D. Reduced only
11
150Which of the following statement is TRUE for the electrochemical Daniel cell
A. Electron flow from Zinc electrode to copper electrode.
B. Current flows from zinc electrode to copper electrode
c. cation moves towards copper electrode.
D. cation moves towards zinc electrode
11
151Q. 23 Calculate the oxidation number of each sulphur atom in the following
compounds.
(a) Na,s,o (b) Na 5.0 (c) Na,SO (d) Na SOA
TER
11
152Complete and balance the following
compound ( boldsymbol{S n}+mathbf{2 K O H}+mathbf{4 H}_{mathbf{2}} boldsymbol{O} rightarrow )
( t )
11
153Q14. Define Oxidation and Reduction in terms of oxidation number.11
154Q. 36 Write redox couples involved in the reactions (a) to (d) given in
question 34.
11
155What is the oxidation state of ( boldsymbol{T} boldsymbol{h} ) in
organometallic compound
( left[T h H O Rleft(C_{5} M e_{5}right)_{2}right] ? )
A ( .+1 )
B. +2
( c cdot+4 )
D. +3
11
156State True or False.
In a galvanic cell, reduction occurs at
cathode.
A. True
B. False
11
157What is the oxidation number for As in
the chemical formula for arsenic acid,
( boldsymbol{H}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4} ? )
( A cdot+1 )
( B .+2 )
( c cdot+3 )
( D cdot+4 )
( E cdot+5 )
11
158Which gas is evolved when ( P b O_{2} ) is
treated with conc ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ? )
A ( . N O_{2} )
в. ( O_{2} )
c. ( N_{2} )
D. ( N_{2} ) O
11
1593.
(d) is
Consi
oxidis
Which one of the following is a combination reaction?
(a) Formation of a mixture of carbon monoxide and
hydrogen. When steam is passed over red hot iron.
(b) Reaction of water with sodium metal to form sodium
hydroxide and hydrogen.
© Ca(OH)2 + Na CO2 — 2NaOH+CaCO3
(d) Preparation of stannic chloride (Tin (iv) chloride) by
passing chlorine gas into molten tin (Sn).
(a) s
(0)
10. Cuo
Abo
(a)
11
160Number of peroxy linkage in
( boldsymbol{K}_{3} boldsymbol{C r}left(boldsymbol{O}_{2}right)_{x} ) having oxidation number of
( C r ) as +5 is :
11
161The oxidation number of iron in ( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4} )
is:
( A cdot+2 )
B. +3
( c cdot frac{8}{3} )
D. ( frac{2}{3} )
11
162Reaction of iron filings with powdered
sulfur is a ( _{–}- ) – process.
A. precipitation
B. oxidation-reduction
C. distillation
D. hydration
E. condensation
11
163f the balanced reaction is as given
below, find the value of ( x, y ) and ( z )
( boldsymbol{C u}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4}^{2+}(boldsymbol{a q})+boldsymbol{S}_{2} boldsymbol{O}_{4}^{2-}(boldsymbol{a q})+ )
( boldsymbol{x} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{y} boldsymbol{S} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{C} boldsymbol{u}(boldsymbol{s}) )
( +z N H_{3}(a q)+2 H_{2} O )
A. ( x=4, y=2, z=4 )
в. ( x=3, y=2, z=3 )
c. ( x=4, y=3, z=4 )
D. None of the above
11
164( boldsymbol{S} boldsymbol{i} boldsymbol{O}_{2}(boldsymbol{s})+boldsymbol{N} boldsymbol{a} boldsymbol{O} boldsymbol{H}(boldsymbol{l}) rightarrow boldsymbol{N} boldsymbol{a}_{2} boldsymbol{S} boldsymbol{i} boldsymbol{O}_{3}(boldsymbol{a} boldsymbol{q}) )
( +? )
A ( cdot H_{2} O(l) )
в. ( H_{2}(g) )
c. ( H_{3} O^{+} )
D. ( O H^{-} )
11
165How many moles of electrons are involved in the conversion of 1 mole
( C r_{2} O_{7}^{2-} ) into ( C r^{3+} ) ion?
11
166Balance the following equation by
oxidation number method.
( M n O_{4}^{2-}+H^{+} rightarrow M n O_{2}+ )
( M n O_{4}^{-}+H_{2} O )
11
167Choose the correct statements –
This question has multiple correct options
( mathbf{A} cdot C_{2} H_{6}+O_{2} rightarrow C O_{2}+H_{2} O ) is an unbalanced
combustion reaction.
B. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} ) is a balanced combustion
reaction.
C ( . A+B C rightarrow A C+B ) represents a single replacement
reactions.
D. ( H N O_{3}+C a(O H)_{2} rightarrow C aleft(N O_{3}right)_{2}+2 H_{2} O ) is an
unbalanced neutralization reaction.
11
168Which of the following arrangements represent increasing oxidation number
of the central atom?
A ( cdot C r O_{2}^{-}, C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4} )
B . ( C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-} )
c. ( C r O_{2}^{-}, C l O_{3}^{-}, M n O_{4}^{-}, C r O_{4}^{2} )
D. ( C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-}, C l O_{3} )
11
169Assertion
( N H_{4} N O_{3} ) undergoes a redox reaction
to give ( N_{2} O ) and ( H_{2} O )
Reason
It is a disproportionation reaction.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
170Which of the following statements is
correct for oxidation reaction?
A. Loss or removal of electron.
B. Removal of hydrogen atom.
C. Removal or loss of electropositive radical or element
D. All the above statements are correct
11
171The oxidant which cannot act as a
reducing agent is :
( A cdot S O_{2} )
в. ( N O_{2} )
( c cdot C O_{2} )
D. ( C l O_{2} )
11
172For the reaction, ( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{O C l}^{-} rightarrow )
( N_{2} H_{4}+C l^{-} ) occurring in basic
medium, the coefficient of ( N_{2} H_{4} ) in the
balanced equation will be :
( mathbf{A} cdot mathbf{1} )
B. 2
( c cdot 3 )
D. 4
11
173( boldsymbol{C u} boldsymbol{O}+boldsymbol{H}_{2} longrightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u}, ) reaction is
an example of :
A. redox reaction
B. synthesis reaction
c. neutralisation
D. analysis reaction
11
174What is the oxidation number of ( C l ) in
the ( C l O_{3}^{-} ) ion?
( A cdot-1 )
B. +5
( c cdot-5 )
( D cdot+7 )
11
175Which of the following is a redox
reaction?
( mathbf{A} cdot 2 C r O_{4}^{2-}+2 H^{+} rightarrow C r_{2} O_{7}^{2-}+H_{2} O )
В ( cdot quad C u S O_{4}+4 N H_{3} rightarrowleft[C uleft(N H_{3}right)_{4}right] S O_{4} )
( mathbf{c} cdot N a_{2} S_{2} O_{3}+I_{2} rightarrow N a_{2} S_{4} O_{6}+N a I )
D. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O )
11
176During the oxidation of ( M n^{2+} ) to
( M n O_{4}^{-} ) by ( P b O_{2} ) in acid medium, the number of moles of acid consumed per
mole of ( M n^{2+} ) ion is
A .4
B. 1/2
( c cdot 2 )
D. 1/4
11
177When ( 6 times 10^{22} ) electrons are used in the
electrolysis of a metalic salt, ( 1.9 mathrm{gm} ) of the metal is deposited at the cathode The atomic weight of that metal Is 57 So oxidation state of the metal in the
salt is:
( A cdot+2 )
( B cdot+3 )
( c cdot+1 )
( D cdot+4 )
11
178In the reaction ( M g+C l_{2} rightarrow M g C l_{2} )
Chlorine may be regarded as:
A. an oxidising agent
B. a reducing agent
c. a catalyst
D. providing an inert medium
11
179Which one of the following reactions is not a redox reaction?
A ( cdot I_{2}+2 F e^{2+} rightarrow 2 I^{-}+2 F e^{3+} )
в. ( H C l+N a O H rightarrow N a C l+H_{2} O )
c. ( 2 M g+O_{2} rightarrow 2 M g O )
D. ( Z n+C u^{2+} rightarrow Z n^{2+}+C u )
11
180A list of reactions are given below.
(a) ( boldsymbol{F e}+mathbf{2 H C l} rightarrow boldsymbol{F e C l}_{2}+boldsymbol{H}_{2} )
(b) ( boldsymbol{F e} boldsymbol{S}+boldsymbol{2} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{2}+boldsymbol{H}_{2} boldsymbol{S} )
(c) ( boldsymbol{F} boldsymbol{e}+boldsymbol{S} stackrel{boldsymbol{Delta}}{longrightarrow} boldsymbol{F} boldsymbol{e} boldsymbol{S} )
(d) ( boldsymbol{N a C l}+boldsymbol{H}_{2} boldsymbol{S O}_{4} stackrel{<200^{circ} boldsymbol{C}}{longrightarrow} )
( N a H S O_{4}+H C l )
( (e) C u S O_{4}+H_{2} S rightarrow C u S+H_{2} S O_{4} )
( (f) S+H_{2} S O_{4} rightarrow 3 S O_{2}+H_{2} O )
Identify redox reactions.
( A cdot a, c ) and ( f )
B. d and f
( c cdot c ) and ( d )
D. c, d and f
11
1815.
Assertion : A redox reaction involves both oxidation and
reduction.
Reason: SO, +2H, S — → 2H 0+3S is an example of
redox reaction.
11
182Q4. What is the source of electrical energy in a galvanic cell?11
183Which of the followings are correct regarding complexometric titration?
A. A titration in which colour is changed due to formation of complex
B. Usually occur when d-block elements are involved
c. Usually happen when chelating ligands are involved
D. All of the above
11
184Oxidation state of ‘S’ in sodium
tetrathionate is :
( mathbf{A} cdot+5,0,0,+5 )
в. +6,+6,0
( mathbf{c} cdot+4,+2,+5 )
D. +2,0,+2,+3
11
185A student prepares for an
experiment involving a voltaic cell. Which of the following is needed the least to perform the experiment?
A. Burette
B. Salt bridge
c. Strip of zinc metal
D. copper wire
E. Solution of zinc sulfate
11
186Q. 24 Balance the following equations by
following equations by the oxidation number method.
(a) Fet + H + Cr,0,2 Cr3+ + Fe** + H20
(b) 12 + NO; NO, +10;
(c) I, +,0 – +50%
(d) MnO2 +0,0% → Mn2+ + CO2
11
187In volcanic eruptions, Sulphur undergoes following reaction:
( mathbf{2} boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{S} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{3} boldsymbol{S}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{O} )
A. Disproportionation
B. Comproportionation
c. Neutralisation
D. Displacement
11
188How many moles of electrons are
needed in the balanced equation for the oxidation of ethanol (1 mol) to acetic
( operatorname{acid} ?left(C_{2} H_{5} O H rightarrow C H_{3} C O O Hright) )
( mathbf{A} cdot mathbf{1} )
B . 2
( c .3 )
D. 4
11
189An example of oxidation-reduction
reaction is:
( mathbf{A} cdot B C l_{3}+C l^{-} rightarrow B C l_{4} )
B. ( H C N+H_{2} O rightarrow H_{3} O^{+}+C N^{-} )
( mathbf{c} cdot H_{2} O_{2}+2 B r^{-}+2 H^{+} rightarrow 2 H_{2} O+B r_{2} )
D. ( 2 N H_{3}(g) rightarrow N_{2}(g)+3 H_{2}(g) )
11
190For the Daniel cell involving the cell reaction ( Z n_{(s)}+C u_{(a q)}^{+2} rightleftharpoons )
( Z n^{+2}_{(a q)}+C u_{(s)} ) the standard free
energies of formation of ( Z n_{(s)}, C u_{(s)} ) ( C u_{(a q)}^{+2} ) and ( Z n_{(a q)}^{+2} ) are 0,0,64.4
KJ/Mole and -154.0 KJ/Mole,
respectively. Calculate the standard
EMF of the cell?
A. 2.13 Volts
B. 1.13 Volts
c. ( 2.26 mathrm{Volts} )
D. 3.42Volts
11
191Oxidation state of ( boldsymbol{C r} ) in ( boldsymbol{K}_{3}left[boldsymbol{C r}left(boldsymbol{C}_{2} boldsymbol{O}_{4}right)_{3}right] )
is :
11
192( boldsymbol{C H}_{2}=boldsymbol{C H}_{2}+boldsymbol{H}_{2} stackrel{N i}{rightarrow} boldsymbol{C H}_{3}-boldsymbol{C H}_{3} ) is
an addition reaction. ( boldsymbol{C H} equiv boldsymbol{C H}+boldsymbol{H}_{2} stackrel{N i}{rightarrow} ? )
Predict and write the products.
11
193. 12 Which of the following statement(s) is/are not true about the following
decomposition reaction?
2KCLO, – 2KCL + 302
(a) Potassium is undergoing oxidation
(b) Chlorine is undergoing oxidation
S 0591910
(c) Oxygen is reduced
(d) None of the species are undergoing oxidation or reduction
11
194Balance the following equation by ion electron method:
( boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+}+boldsymbol{H}_{2} boldsymbol{O} rightarrow )
( boldsymbol{H}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}+boldsymbol{N} boldsymbol{O}+boldsymbol{S} )
11
195Oxygen can show positive oxidation state in its compounds with:
A. Fluorine
B. Nitrogen
c. Hydrogen
D. Sulphur
11
196In the reaction ( boldsymbol{P b O}+boldsymbol{C} rightarrow boldsymbol{P b}+boldsymbol{C O} )
A. ( P b O ) is oxidised
B. c acts as oxidising agentt
( c cdot c ) acts as a reducing agent
D. This reaction does not represent a redox reaction
11
197Write the chemical equations to
represent the following reactions. The disproportionation of ( mathrm{SnO} ) to ( mathrm{Sn} ) and
( operatorname{Sn} O_{2} ) is ( 2 S n O rightarrow S n+S n O_{2} )
If true enter 1 , else enter 0
11
198Assertion
For the reaction, ( N a_{2} C O_{3}+H C l rightarrow )
( N a C l+N a H C O_{3}, ) the suitable
indicator is phenolphthalein.
Reason
Phenolphthalein provides its colour in
acidic medium.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
199The reaction ( boldsymbol{A} boldsymbol{g}^{2+}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{g}(s) rightarrow )
( 2 A g^{+}(a q) ) is an example of
This question has multiple correct options
A. disproportionation
B. proportionation
c. comproportionation
D. symproportionation
11
200Consider the following reaction:
( boldsymbol{C l}_{2}+boldsymbol{S}^{2-} longrightarrow boldsymbol{S}+boldsymbol{C l}^{-} )
The above reaction is a
disproportionation reaction. Is it True or False? Explain why?
11
201Balance the following equation by
oxidation number method.
( Z n+H N O_{3} rightarrow Z nleft(N O_{3}right)_{2}+ )
( N H_{4} N O_{3}+H_{2} O )
11
202Balance the following equation by ion electron method.
( boldsymbol{C o}^{2+}+boldsymbol{N} boldsymbol{O}_{2}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{C} boldsymbol{o}^{3+}+ )
( N O+H_{2} O )
11
203Fill the blank.
( $ $ 2{text { Ca }}_{-}{3}left{text { lleft }left(P{0}_{-}{4} mid text { right }right)right. )
3. ( {2}+6 operatorname{si}{0}_{-}{2}+10 C ) lrightarrow ( {P )
( -{4}+mid ) text ( {-} operatorname{casi}{0}_{-}{3 )
( 3+10 cos $ )
( A cdot 2 )
B. 4
( c .5 )
D. 6
E . 8
11
204The oxidation number of ( sin H_{2} S_{2} O_{8} )
is:
( A cdot+2 )
( B cdot+4 )
( c cdot+6 )
( D cdot+7 )
11
205In balancing the following half-reaction:
( boldsymbol{C N}^{-} longrightarrow boldsymbol{C N O}^{-}(boldsymbol{s k e l e t a l}), ) the
number of electrons that must be added
on the right is :
11
206The oxidation state of the most
electronegative element in the products
of the reaction between ( B a O_{2} ) and
( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) is:
A. 0 and -1
B. – – 1 and – 2
c. – – a and o
D. – 2 and +1
11
207Which of the following is/are autoredox
reactions?
This question has multiple correct options
A ( cdot P_{4}+O H longrightarrow H_{2} P O_{2}^{ominus}+P H_{3} )
B . ( S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S )
( mathrm{c} cdot mathrm{H}_{2} mathrm{O}_{2} longrightarrow mathrm{H}_{2} mathrm{O}+mathrm{O}_{2} )
D. ( _{A g C l}+N H_{3} rightarrowleft[A gleft(N H_{3}right)_{2}right] C l )
11
208Which among the following are
intramolecular redox reactions?
This question has multiple correct options
A. ( P C l_{5} rightarrow P C l_{3}+C l_{2} )
в. ( C H O-C H O+O H^{-} rightarrow C O O^{-}-C H_{2} O H )
c. ( 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} )
D. ( N H_{4} N O_{2} longrightarrow N_{2}+2 H_{2} O )
11
209Balance the following below equation.
( boldsymbol{A u}+boldsymbol{N O}_{3}^{-}+boldsymbol{C l}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{A u} boldsymbol{C l}_{4}^{-}+ )
( N O_{2}+H_{2} O )
A ( cdot A u+3 N O_{3}^{-}+4 C l^{-}+6 H^{+} rightarrow A u C l_{4}^{-}+3 N O_{2}+ )
( 3 H_{2} O )
B . ( A u+2 N O_{3}^{-}+5 C l^{-}+8 H^{+} rightarrow A u C l_{4}^{-}+6 N O_{2}+ )
( 3 H_{2} O )
c. ( A u+4 N O_{3}^{-}+2 C l^{-}+6 H^{+} rightarrow A u C l_{4}^{-}+5 N O_{2}+ )
( 3 H_{2} O )
D. None of these
11
210A certain amount of a reducing agent
reduces x mole of ( K M n O_{4} ) and y mole
of ( K_{2} C r_{2} O_{7} ) in different experiments in acidic medium. If the change in oxidation state in reducing agent is same in both experiments, ( boldsymbol{x}: boldsymbol{y} )
A . 5: 3
B. 3: 5
( c .5: 6 )
D. 6: 5
11
211In which of the following reactions there is a change in the oxidation number of nitrogen atom?
A ( .2 N O_{2} rightarrow N_{2} O_{4} )
B. ( N H_{3}+4 N H_{3} rightarrowleft[C uleft(N H_{3}right)_{4}right] S O_{4} )
c. ( 2 N a_{2} S_{2} O_{3}+I_{2} rightarrow N a_{2} S_{4} O_{6}+2 N a I )
D. None of these
11
212Which of the following involves reduction?
A. conversion of an anion to atom
B. conversion of a cation to atom
c. both these
D. none of these
11
213Balance the following equation by ion electron method.
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{H}^{+}+boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-} rightarrow boldsymbol{C r}^{3+}+ )
( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
11
214In which compound among the following, carbon has a zero oxidation
state?
A ( . C H_{4} )
в. ( C H_{3} C l )
c. ( C H_{2} C l_{2} )
D. ( C C l_{4} )
11
215Find the sum of the coefficients when
given equation is balanced.
( boldsymbol{A l}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{C a}(boldsymbol{O H})_{2} rightarrow boldsymbol{A l}(boldsymbol{O H})_{3}+ )
( boldsymbol{C} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4} )
A . 5
B. 6
( c cdot 7 )
D. 8
E . 9
11
2160.29 Assertion (A) Among halogens fluorine is the best oxidant.
Reason (R) Fluorine is the most electronegative atom.
(a) Both A and Rare true and R is the correct explanation of A
(b) Both A and R are true but R is not the correct explanation of A
(c) A is true but R is false
(d) Both A and Rare false
h
otanden
otru
but recon is not the corrent oynlanation of
11
217When ( K M n O_{4} ) act as an oxidising agent and ultimately form ( M n O_{4}^{2-}, M n O_{2}, M n_{2} O_{3} ) and ( M n^{2+} )
then the numbers of electrons
transferred in each case, respectively,
are :
A .4,3,1,5
B. 1, 5, 3, 7
( c cdot 1,3,4,5 )
D. 3, 5, 7,
11
218The oxidation state of the underlined
element in the given compound is:
( B a_{2} X e O_{2} )
( A cdot+2 )
( B cdot+3 )
( c cdot+4 )
D.
11
219On the basis of the following ( E^{o} ) values, the strongest oxidising agent is:
( left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-} longrightarrowleft[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{boldsymbol{3}+}+ )
( boldsymbol{e}^{-}, boldsymbol{E}^{o}=-mathbf{0 . 3 5} boldsymbol{V} )
( boldsymbol{F} boldsymbol{e}^{2+} rightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-1} )
( boldsymbol{F} boldsymbol{e}^{2+} rightarrow boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}+boldsymbol{e}^{-1} ; boldsymbol{E}^{boldsymbol{o}}=-boldsymbol{0 . 7 7} boldsymbol{V} )
A ( cdot F e^{3} )
в. ( left[F e(C N)_{6}right]^{3-} )
( mathrm{c} cdotleft[mathrm{Fe}(mathrm{CN})_{6}right]^{4} )
D. ( F e^{2} )
11
220Total number of electrons involved per
molecule in the oxidation of ( F e C_{2} O_{4} ) to
( F e^{3+} ) and ( C O_{2} ) is :
( mathbf{A} cdot mathbf{3} )
B. 2
( c cdot 4 )
D. none of these
11
221The following reaction is an example of
( a: )
( mathbf{4} boldsymbol{N} boldsymbol{H}_{3}(boldsymbol{g})+mathbf{5} boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{4} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+ )
( mathbf{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) )
(i) displacement reaction
(ii) combination reaction
(iii) redox reaction
(iv) neutralisation reaction
( A ). (i) and (iv)
B. (ii) and (iii)
c. (i) and (iii)
D. (iii) and (iv)
11
222“In moist air, copper corrodes to
produce a green layer on the surface”. For this, the reaction is :
( boldsymbol{C u}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C O}_{2}+boldsymbol{O}_{2} rightarrow boldsymbol{C u} boldsymbol{C O}_{3} )
( boldsymbol{C u}(boldsymbol{O} boldsymbol{H})_{2} )
If the statement is true enter 1 else
enter 0
11
223Redox reactions are reactions during which electron transfer takes place.
Here magnesium atom transfers two
electrons one each to the two chlorine
atoms
i) What are the products of this
reaction?
ii) Write the balanced equation for the
complete reaction.
iii) Which element is being oxidized?
iv) Which element is being reduced?
v) Write the reduction part of the
reaction?
11
224Write balanced net ionic equation for
the following reaction in acidic solution
( boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{a} boldsymbol{q})+boldsymbol{A} boldsymbol{s}_{4}(boldsymbol{s})+boldsymbol{P} boldsymbol{b}_{3} boldsymbol{O}_{4}(boldsymbol{s}) rightarrow )
( boldsymbol{P b S O}_{4}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{-}(boldsymbol{a} boldsymbol{q}) )
11
225The tendency of two species to disproportionate can be determined by examining the:
A. Phase diagram
B. Volume vs Temperature graph
c. Frost diagram
D. Heat capacity vsTemperature graph
11
226Chlorine is in +1 oxidation state in:
A. нс
B. ( mathrm{HClO}_{4} )
c. ( A & B ) both
D. none of these
11
227Q. 11 Which of the following elements does not show disproportionation
tendency?
(a) CI
(b) Br
(d) I
teagency.
(b) B
(c) F
11
228Balance the following equation:
( N H_{3}+O_{2} rightarrow N O+H_{2} O )
11
229When ( H_{2} S ) is passed into aqueous ( S O_{2} )
( mathbf{A} cdot H_{2} S ) is converted to yellow precipitate of sulphur.
B. ( S O_{2} ) is converted to yellow precipitate of sulphur.
C . a clear solution of ( H_{2} S O_{4} ) is formed.
D. ( S O_{2} ) as well as ( H_{2} S ) are converted into a yellow precipitate of sulphur
11
230Balance the following equation.
( boldsymbol{P}_{2} boldsymbol{H}_{4} rightarrow boldsymbol{P} boldsymbol{H}_{3}+boldsymbol{P}_{4} boldsymbol{H}_{2} )
11
231. 6 The oxidation number of an element in a compound is evaluated on the
basis of certain rules. Which of the following is incorrect in this respect?
(a) The oxidation number of hydrogen is always +1
(b) The algebraic sum of all the oxidation numbers in a compound is zero
(c) An element in the free or the uncombined state bears oxidation number zero
(d) In all its compounds, the oxidation number of fluorine is -1
11
232Which of the following reaction shows
reduction of water?
A ( cdot 2 H_{2} O+2 N a rightarrow 2 N a O H+H_{2} )
B ( cdot 6 C O_{2}+12 H_{2} O rightarrow C_{6} H_{1} 2 O_{6}+6 H_{2} O+6 O_{2} )
( mathbf{c} cdot 2 F_{2}+2 H_{2} O rightarrow 4 H^{+}+4 F^{-}+O_{2} )
D. ( P_{4} O_{1} 0+6 H_{2} O rightarrow 4 H_{3} P O_{4} )
11
233Reaction of iron filings with powered sulfur is known as:
A. precipitation
B. oxidation-reduction
c. distillation
D. hydration
E. condensation
11
234Which of the following species are oxidised and reduced in the following (unbalanced) reaction?
( boldsymbol{C}+boldsymbol{Z} boldsymbol{n} boldsymbol{O} longrightarrow boldsymbol{Z} boldsymbol{n}+boldsymbol{C O} )
A. zno Reduced ; c Oxidizedd
B. c Reduced ; zno Oxidizedd
c. Neither of them reduced or oxidized
D. None of the above
11
235What product is formed when
cyclohexanone is oxidised?
A. НООС( cdotleft(C H_{2}right)_{4} cdot )СООН
в. ( C H_{3} C H_{2} C O O H )
c. ( C H_{3}left(C H_{2}right)_{4} cdot C O O H )
D. None of the above
11
236The reaction ( : Z n^{2+}(a q)+ )
( mathbf{2} e^{-} rightarrow boldsymbol{Z} boldsymbol{n} )
( (s) ) has a electrode
potential of ( 0.76 V ) This means:
11
237In the reaction:
( 2 F e C l_{2}+C l_{2} rightarrow 2 F e C l_{3} )
Chlorine may be regarded as:
A. an oxidising agent
B. a reducing agent
c. a catalyst
D. providing an inert medium
11
238Which of these reactions are redox
reactions?
( 16 N O(g)+4 N H_{3}(g) rightarrow 5 N_{2}(g)+ )
( mathbf{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) )
( 22 S O_{2}(g)+O_{2}(g) rightarrow 2 S O_{3}(g) )
3. ( boldsymbol{S O}_{3}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) rightarrow boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}(boldsymbol{g}) )
A .1,2 and 3 are correct
B. 1 and 2 only are correct
c. 2 and 3 only are correct
D. 1 only is correct
11
239Balance the given below reaction
( boldsymbol{x} boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{y} boldsymbol{N} boldsymbol{a} boldsymbol{O} boldsymbol{H}+boldsymbol{z} boldsymbol{N} boldsymbol{a} boldsymbol{C l} boldsymbol{O}_{3} rightarrow )
( boldsymbol{a} boldsymbol{N} boldsymbol{a}_{3} boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}+boldsymbol{b} boldsymbol{N} boldsymbol{a}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{c} boldsymbol{N} boldsymbol{a} boldsymbol{C l O}+ )
( d H_{2} O ) Calculate the value of ( (x-y+z+a) )
b+c), when the molar coefficient are in simplest whole number ratio.
11
240TEL is a compound used as:
( A ). antibiotic
B. antiswptic
c. antiknocking
D. antioxidant
11
241Which of the following is an example of oxidation?
A ( cdot S n^{+2}-2 e^{-} rightarrow S n^{+} )
B. ( F e^{+3}+e^{-} rightarrow F e^{+} )
c. ( C l_{2}+2 e^{-} rightarrow 2 C l )
D. None of the above
11
242Which of the following statement is correct for a galvanic cell?
A. Reduction occurs at cathode
B. Oxidation occurs at anode
c. Electrons flow anode to cathode
D. All the statements are correct
11
243Balance the following redox reaction ( M n O_{4}^{ominus}(a q)+I^{ominus}(a q) rightarrow M n O_{2}(s)+ )
( boldsymbol{I}_{2}(boldsymbol{s}) )
What is the coefficient of ( boldsymbol{I}^{-} ) ?
11
244Oxidation number of sodium in sodium
amalgam is:
( A cdot+2 )
B. +1
( c cdot-2 )
D. zero
11
245Sodium forms an oxide containing one oxygen atom for every two atoms of sodium. What is the coefficient of
sodium in the balanced equation for the
reaction of sodium with oxygen to form this oxide?
( mathbf{A} cdot mathbf{0} )
B. 1
c. 2
D. 3
( E .4 )
11
246Consider the reaction: ( C l_{2}+2 K I rightarrow )
( boldsymbol{I}_{2}+2 boldsymbol{K} boldsymbol{C l} )
Which species will be reduced at the cathode?
A ( cdot C l_{2} )
В. ( I_{2} )
c. ( I^{-} )
D. ( C l )
11
247Balance the following equations by
oxidation number method.
( boldsymbol{K} boldsymbol{I}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{I}_{2}+boldsymbol{S} boldsymbol{O}_{2}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
11
248( F e^{2+} ) is oxidised by ( M n O_{4}^{-} ) or ( C r_{2} O_{7}^{2-} ) in acidic medium. What is new
oxidation number of Fe?
( A cdot+3 )
B. +1
( c cdot+2 )
D. +4
11
249Which of the following is a redox
reaction?
( mathbf{A} cdot N a C l+K N O_{3} rightarrow N a N O_{3}+K C l )
B ( cdot C a C_{2} O_{4}+2 H C l rightarrow C a C l_{2}+H_{2} C_{2} O_{4} )
( mathbf{c} cdot M g(O H)_{2}+2 N H_{4} C l rightarrow M g C l_{2}+2 N H_{4} O H )
( mathbf{D} cdot Z n+2 A g C N rightarrow 2 A g+Z n(C N)_{2} )
11
250In the redox reaction: ( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}+ )
( boldsymbol{y} boldsymbol{P} boldsymbol{b} boldsymbol{O}_{2}+boldsymbol{z} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{H} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}+ )
( boldsymbol{P b}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{H}_{2} boldsymbol{O} )
A. ( x=2, y=5, z=10 )
в. ( x=2, y=7, z=8 )
c. ( x=2, y=5, z=8 )
D. ( x=2, y=5, z=5 )
11
251What would be the stoichiometric
coefficient of hydrochloric acid in the following equation? ( -C l_{2}+_{-} H_{2} O rightarrow_{-} H C l+_{-} H C l O_{3} )
A . 1
B. 3
c. 5
D. 10
11
2520.37 Find out the oxidation number of chlorine in the following compounds
and arrange them in increasing order of oxidation number of chlorine.
NaClO4, NaClO3, NaClO, KCLO, C120,, CLO3, C120, NaCl, Cl2, CLO2.
Which oxidation state is not present in any of the above compounds?
11
253Consider the following reaction:
( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{y} boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-}+boldsymbol{z} boldsymbol{H}^{+} rightarrow )
( boldsymbol{x} boldsymbol{M} boldsymbol{n}^{2+}+mathbf{2} boldsymbol{y} boldsymbol{C} boldsymbol{O}_{2}+frac{boldsymbol{z}}{2} boldsymbol{H}_{2} boldsymbol{O} . ) The values
of ( x, y ) and ( z ) in the reaction are, respectively:
A .2,5 and 16
B. 5,2 and 8
c. 5,2 and 16
D. 2,5 and 8
11
254In the electrochemical cell:
( Z nleft|Z n S O_{4}(0.01 M)right|left|C u S O_{4}(1.0 M)right| C )
the emf of this Daniel cell is ( E_{1} . ) When
the concentration of ( Z n S O_{4} ) is changed
to ( 1.0 M ) and that of ( C u S O_{4} ) changed to
( mathbf{0 . 0 1} boldsymbol{M}, ) the emf changes to ( boldsymbol{E}_{2} . ) From the followings, which one is the
relationship between ( boldsymbol{E}_{1} ) and ( boldsymbol{E}_{2} ? ) (Given, ( left.frac{boldsymbol{R T}}{boldsymbol{F}}=mathbf{0 . 0 5 9}right) )
A ( . E_{2}=0 neq E_{1} )
B ( . E_{1}=E_{2} )
c. ( E_{1}E_{2} )
11
255Which of the following does not exist?
This question has multiple correct options
( A cdot H S_{6} )
B. ( mathrm{HPO}_{4} )
( mathbf{c} cdot ) Fel ( _{3} )
D. ( mathrm{HClO}_{4} )
11
256The process of reduction involves:
A. removal of hydrogen
B. gain of electrons
C. addition of oxygen
D. loss of electrons
11
257One of the fuel cells uses the reaction of
hydrogen and oxygen to form water. Write down the cell reaction taking place in the anode and cathode of that fuel cell.
11
258Find the oxidation and reduction
process for the following reaction:
( boldsymbol{C H}_{2}=boldsymbol{C H}_{2}+boldsymbol{H}_{2} rightarrow boldsymbol{C H}_{3}-boldsymbol{C H}_{3} )
11
259Change of orange color of chromium(VI) to green color of chromium(III)
indicates presence of a:
A. reducing agent
B. oxidizing agent
c. reagent
D. drying agent
11
260The oxidation number of underlined
element in ( underline{M} boldsymbol{n}_{3} boldsymbol{O}_{4} ) compound is :
( A cdot frac{8}{3} )
B. ( frac{7}{3} )
( c cdot frac{8}{5} )
D. none of these
11
261True statements for the chemical
reaction of the formation of lithium
oxide is:
( 4 L i(s)+O_{2}(g) rightarrow 2 L i_{2} O(s) )
A. lithium metal is the oxidizing agent
B. oxygen gas is the reducing agent
c. lithium is oxidized
D. oxygen is oxidized
E. oxygen loses two electrons to become ( O^{-2} ) ion
11
262In the reaction ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{C l}_{2} rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}+ )
( S, ) the oxidizing agent is :
A ( . H_{2} )
в. ( C l_{2} )
c. ( H C l )
D. ( S )
11
263In the reaction of ( H I ) with ( H_{2} S O_{4} ) the
oxidation state of sulphur is changed to
-2. Identify the correct balanced
equation
A ( cdot H_{2} S O_{4}+2 H I rightarrow S O_{2}+2 H_{2} O+I_{2} )
в. ( H_{2} S O_{4}+6 H I rightarrow S+4 H_{2} O+3 I_{2} )
c. ( H_{2} S O_{4}+8 H I rightarrow H_{2} S+4 H_{2} O+4 I_{2} )
D. All of the above
11
264Give two examples for oxidation reduction reaction11
265Photographic paper is developed with
alkaline hydroquinone
Select correct statement
A. Hydroquinone is the oxidant
B. ( A g^{+} ) is the oxidant
( mathrm{c} cdot B r^{-} ) is the oxidant
D. ( A g^{+} ) is the reductant
11
266Two elements combine to form one
compound in a displacement reaction.
A. True
B. False
11
267If true enter 1 , else enter 0 .
( H C H O ) disproportionates in presence
of ( boldsymbol{O} boldsymbol{H}^{-} )
( A )
11
268In Ostwald’s process for the manufacture of nitric acid, the first step involves the oxidation of ammonia
gas by oxygen gas to give nitric oxide gas and steam. What is the maximum
weight of nitric oxide that can be obtained starting only with 10.00 g. of ammonia and 20.00 g of oxygen?
11
269When ferrous oxalte is titrated against
( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) m eq. of ( boldsymbol{F} boldsymbol{e}^{2+}, boldsymbol{C}_{2} boldsymbol{O}_{4}^{2-} ) and
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-} ) in the redox reaction are ( boldsymbol{X}, boldsymbol{Y} )
and ( Z ) respectively, then:-
A ( . X=Y )
в. ( X+Y=Z )
c. ( X+2 Y=Z )
D. ( 2 X+6 Y+6 Z )
11
27032. Browning of paper in
books is caused by
(1) frequent use
(2) lack of aeration
(3) collection of dust
(4) oxidation of cellulose
11
271(a) Give one example of redox reaction.
(b) Draw the labelled diagram of electrolytic decomposition of water
11
272What occurs most often in nature:
oxidation or reduction?
A. Oxidation.
B. Reduction.
c. Both occur equally
D. Depends on the scenario
11
273Which of the following oxoacid of phosphorous does not disproportionate?
A ( . H_{3} P O_{2} )
в. ( H_{3} P O_{4} )
c. ( H_{3} P O_{3} )
D. All of these
11
274An element, which never as a positive oxidation state in any of its compounds is:
A. boron
B. oxygen
c. chlorine
D. fluorine
11
275If the balanced reaction is as given below, find the value of ( x, y ) and ( z )
( boldsymbol{T} boldsymbol{i}_{2} boldsymbol{O}_{3}(boldsymbol{s})+boldsymbol{x} boldsymbol{N} boldsymbol{H}_{2} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) rightarrow )
( 2 T i O H(s)+y N_{2}(g)+z H_{2} O )
A. ( x=4, y=2, z=5 )
в. ( x=3, y=2, z=5 )
c. ( x=4, y=2, z=4 )
D. None of the above
11
276The oxidation number of phosphorus in ( boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}right)_{2} ) is:
( A cdot+3 )
B. +2
( c cdot+1 )
D. –
11
277Identify the substance oxidised, reduced, oxidising agent and reducing agent for the following reaction.
( boldsymbol{H} boldsymbol{C H O}_{(l)}+mathbf{2}left[boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right]_{(a q)}^{+}+ )
( mathbf{3} boldsymbol{O} boldsymbol{H}_{(boldsymbol{a q})}^{-} rightarrow mathbf{2} boldsymbol{A} boldsymbol{g}_{(s)}+boldsymbol{H} boldsymbol{C O O}_{(boldsymbol{a q})}^{-}+ )
( mathbf{4} boldsymbol{N} boldsymbol{H}_{3(a q)}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O}_{(l)} )
11
278Write half-reactions using electrons.
( boldsymbol{C r}_{2} boldsymbol{O}_{2}^{boldsymbol{7}-}+boldsymbol{6} boldsymbol{F} boldsymbol{e}^{boldsymbol{2}+}+mathbf{1 4} boldsymbol{H}^{+} longrightarrow )
( 2 C r^{3+}+6 F e^{3+}+7 H_{2} O )
A. Oxidation : ( F e^{2+} longrightarrow F e^{3+}+e^{-} ); Reduction:
[
C r_{2} O_{2}^{7-}+14 H^{+}+6 e^{-} longrightarrow 2 C r^{2+}+7 H_{2} O
]
B. Oxidation: ( 3 F e^{2+} longrightarrow 3 F e^{3+}+e^{-} ); Reduction:
( mathrm{Cr}_{2} mathrm{O}_{2}^{7-}+14 mathrm{H}^{+}+6 e^{-} longrightarrow 2 mathrm{Cr}^{2+}+7 mathrm{H}_{2} mathrm{O} )
C. Oxidation : ( 2 F e^{2+} longrightarrow 2 F e^{3+}+e^{-} ); Reduction:
( mathrm{Cr}_{2} mathrm{O}_{2}^{7-}+14 mathrm{H}^{+}+6 e^{-} longrightarrow 2 mathrm{Cr}^{2+}+7 mathrm{H}_{2} mathrm{O} )
D. Oxidation: ( 3 F e^{2+} longrightarrow F e^{3+}+3 e^{-} ; ) Reduction :
( C r_{2} O_{2}^{7-}+14 H^{+}+3 e^{-} longrightarrow 2 C r^{2+}+7 H_{2} O )
11
279Select the oxidant in the given
reactions.
( boldsymbol{K} boldsymbol{I} boldsymbol{O}_{3}+boldsymbol{5} boldsymbol{K} boldsymbol{I}+boldsymbol{6} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{3} boldsymbol{I}_{2}+ )
( 6 K C l+3 H_{2} O )
11
280Which element among the following will not have an oxidation number of ( -1 ? )
A. ( F ) in ( H F )
B. ( C l ) in ( N a C l )
( c cdot O operatorname{in} H_{2} O_{2} )
D. ( F ) in ( N a F )
E ( . H ) in ( N a_{2} H P O_{4} )
11
281Which of the following is a
decomposition reaction?
( mathbf{A} cdot 3 N a(s)+F e B r_{3}(a q) rightarrow 3 N a B r(a q)+F e(s) )
B. ( N a O H(a q)+H N O_{3}(a q) rightarrow N a N O_{3}(a q)+H_{2} O(l) )
( mathbf{c} cdot 2 N a H C O_{3}(s) rightarrow N a_{2} C O_{3}(s)+C O_{2}(g)+H_{2} O(l) )
D. ( 3 H_{2}(g)+N_{2}(g) rightarrow 2 N H_{3}(g) )
11
282When ( mathrm{K}_{2} mathrm{Cr}_{2} mathrm{O}_{7} ) is converted into
( mathrm{K}_{2} mathrm{Cr} mathrm{O}_{4}, ) the change in oxidation number of Cr is
A .
B. 6
( c cdot 4 )
D. 3
11
283State the type of chemical reaction involved in given reaction,
a] Calcium + oxygen ( rightarrow ) Calcium oxide
A. Displacement Reactions
B. Decomposition Reactions
c. combination Reactions
D. Neutralization Reactions
11
2841
9.
Consider the following reaction and tell which one is the
oxidising reagent.
SO2 +2H2S → 2H 0+3S
(a) SOM
(b) HAS
(c) H2O
(d) S
So, *211,5 2,0
11
285The elements undergoing reduction and oxidation during the reaction,
( left(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+ )
( 4 H_{2} O ) are respectively:
( A cdot N ) and ( C r )
B. Crand N
c. ( mathrm{N} ) and 0
D. Crand 0
11
286The reaction, ( 2 H_{2} O(l) rightarrow 4 H^{+}(a q .)+ )
( O_{2}(g)+4 e^{-} ) is?
A. A oxidation reaction
B. A hydrolysis reaction
C. A solvolysis reaction
D. An oscillatory reaction
E. An acid catalyst reaction
11
287The missing term in the following equation is ( 2 F e^{3+}+S n^{2+} rightarrow 2 F e^{2+}+ )
( ldots . ? )
( A cdot S n^{4} )
в. ( S n^{3} )
( c cdot s n^{2} )
D. ( S n^{+} )
11
288Q. 27 Match Column I with Column II for the oxidation states of the central
atoms.
Column 1 Column II
CrO
B. Mno 2 4
C VO
D. Fef-
А.
+3
11
289( A l+M n O_{4}^{-} rightarrow A l(O H)_{4}^{-}+M n O_{2} )
For this reaction the oxidation state of
( A l ) and ( M n ) in the product are respectively:
( mathbf{A} cdot+3 a n d+4 )
B. +4 and +4
c. +3 and +7
D. +2 and +4
11
290Write the name of the cell which is
generally used in transistors. Write the
reactions taking place at the anode and the cathode of this cell.
11
291Oxidation state of oxygen in hydrogen peroxide is?
A . –
B. +1
( c cdot 0 )
( D cdot-2 )
11
292Q21. The Mn+ ion is unstable in solution and undergoes disproportionation to give Mn2+, MnO2
and H ion. Write a balanced ionic equation for the reaction.
1
1
1
11
293A dilute Ferrous sulphate solution was gradually added to the beaker containing acidified permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation?
A. ( K M n O_{4} ) is an oxidizing agent, it oxidizes ( F e S O_{4} )
B. ( F e S O_{4} ) acts as an oxidizing agent and oxidizes ( K M n O_{4} )
c. The colour disappears due to dilution: no reaction is involved
D. ( K M n O_{4} ) is an unstable compound and decompose presence of ( F e S O_{4} ) to a colourless compound
11
294In the ethylene molecule the two carbon atoms have the oxidation numbers.
A . -1,-1
в. -2,-2
c. -1,-2
D. +2,-2
11
295Reducing agents does not include:
A. chlorine
B. carbon
c. potassium iodide
D. carbon monoxide
11
296Which of the following reactions is/are disproportionation reaction(s)?
This question has multiple correct options
A ( cdot C l_{2}+2 stackrel{ominus}{O} H rightarrow C l^{ominus}+C l O^{ominus}+H_{2} O )
в. ( 2 H C u C l_{2} rightarrow C u+C u^{2+}+4 C l^{ominus}+2 H^{oplus} )
c. ( _{H C H O}+stackrel{ominus}{O H} longrightarrow C H_{3} O H+H C O O^{circ} )
D. ( M g C O_{3} rightarrow M g O+C O_{2} )
11
297Complete and balance the following
compound. Acidic solution of ( F e^{2+} ) ion gives a brown ring when it comes in
contact with ( N O^{-} 3 ) ion. Complete the
following reaction of this process.
[
begin{array}{l}
{left[boldsymbol{F e}left(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]^{2+}+boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{H}^{+} rightarrow} \
——+left[boldsymbol{F} eleft(boldsymbol{H}_{2} boldsymbol{O}right)_{6}right]^{3+}+boldsymbol{H}_{2} boldsymbol{O}
end{array}
]
11
298What are the oxidation number of the
underlined elements in ( underline{C} boldsymbol{H}_{3} underline{boldsymbol{C}} boldsymbol{O} boldsymbol{O} boldsymbol{H} )
11
299Which of the following is true of
oxidation-reduction reactions?
A. The reducing agent is reduced at the cathode.
B. The oxidizing agent is oxidized at the anode.
C. The oxidizing agent is reduced at the cathode.
D. The reducing agent is oxidized at the cathode.
11
300Hydrogen gas will reduce:
A. hot cupric oxide
B. hot ferric oxide
c. hot stanic oxide
D. hot aluminium oxide
11
301In the reaction, ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{2} boldsymbol{A} boldsymbol{g}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow )
( boldsymbol{C u}^{2+}+mathbf{2} boldsymbol{A} boldsymbol{g}(boldsymbol{s}) )
A ( cdot ) cu(s) is oxidised to ( C u^{2} )
B. ( operatorname{Cu}(mathrm{s}) ) reduced to ( C u^{2+}(a q) )
c. ( operatorname{Ag} ) (aq) is oxidised to ( mathrm{Ag} ) (s)
D. Both Cu(s) and ( A g^{+} ) (aq) are oxidised
11
302Calculate the oxidation no. of sulphur in
( boldsymbol{H}_{2} underline{boldsymbol{S}}_{4} boldsymbol{O}_{boldsymbol{6}} )
11
303What is the oxidation number of carbon
in carbon suboxide ( left(C_{3} O_{2}right) ? )
11
304Q Type your question
appropriate choice.
Column I 11
( (A) )
[
begin{array}{l}
left.3 M g_{(} sright)+ \
N_{2(g)} stackrel{Delta}{longrightarrow} quad(i) quad text { Displacement }
end{array}
]
( N_{2}(g) longrightarrow )
( M g_{3} N_{2(s)} )
[
begin{array}{l}
left.N a H_{(} sright)+ \
left.H_{2} O_{(} lright) rightarrow
end{array}
]
( (B) )
[
N a O H_{(a q)}+
]
( (i i) )
Decomposition
( H_{2(g)} )
[
3 C l O_{(a q)}^{-} rightarrow
]
( (C) )
( 2 C l_{(a q)}^{-}+ ) ( (i i i) ) Combination
( mathrm{ClO}^{-}_{(a q)} )
[
2 K C l O_{3(s)} rightarrow
]
( (D) )
( left.2 K C l_{(} sright)+ ) ( (i v) ) Disproportiona
( 3 O_{2(g)} )
( mathbf{A} cdot(A) rightarrow(i),(B) rightarrow(i i i),(C) rightarrow(i i), D rightarrow(i v) )
B ( .(A) rightarrow(i v),(B) rightarrow(i i i),(C) rightarrow(i i), D rightarrow(i) )
( mathbf{c} cdot(A) rightarrow(i i),(B) rightarrow(i),(C) rightarrow(i i i), D rightarrow(i v) )
( mathbf{D} cdot(A) rightarrow(i i i),(B) rightarrow(i),(C) rightarrow(i v), D rightarrow(i i) )
11
305State whether the given statement is
true or false:
Combination is the reverse of
decomposition reaction
A. True
B. False
11
306What do you mean by oxidation and
reduction?
11
307( mathrm{Cu}(s)+mathrm{NO}_{3}^{-}(a q)+mathrm{H}^{+}(a q) rightarrow mathrm{Cu}^{2+}(a q) )
( +mathrm{NO}_{2}(g)+mathrm{H}_{2} mathrm{O}(1) )
If the above equation is balanced with lowest whole number coefficients, find
the coefficient for ( mathrm{H}+(mathrm{aq}) )
A
B. 2
( c cdot 3 )
D. 4
E. 5
11
308The yellow coloured solution of chromate salt changes to orange colour on acidification due to the formation of :
A ( cdot C r^{3} )
B. ( C r_{2} O_{7}^{2} )
( mathrm{c} cdot mathrm{Cr} mathrm{O}_{4} )
( mathrm{D} cdot mathrm{Cr}_{2} mathrm{O}_{3} )
11
309Balance the following equation, when it occurs in basic medium.
[
boldsymbol{C l O}_{boldsymbol{3}}^{-} longrightarrow boldsymbol{C l}^{-}
]
A ( cdot C l O_{3}^{-}+3 H_{2} O+6 e rightarrow C l^{-}+6 O H^{-} )
B . ( C l O_{3}^{-}+3 H_{2} O+5 e rightarrow C l^{-}+6 O H^{-} )
c. ( 3 C l O_{3}^{-}+3 H_{2} O+3 e rightarrow C l^{-}+3 O H )
D. None of these
11
310The oxidation number of ( C r ) in ( C r O_{5} )
which has the following structure is:
( A cdot+4 )
B. +5
( c cdot+6 )
( D )
11
311Balance the following redox reactions:
( boldsymbol{S}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{I}_{2}(boldsymbol{s}) longrightarrow boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q})+ )
( boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) )
A ( cdot S^{2-}(a q)+4 I_{2}(s)+4 H_{2} O(l) rightarrow 8 I^{-}(a q)+S O_{4}^{2-}(a q)+ )
( 8 H^{+}(a q) )
B . ( S^{2-}(a q)+6 I_{2}(s)+4 H_{2} O(l) longrightarrow 8 I^{-}(a q)+4 S O_{4}^{2-}(a q)+ )
( 8 H^{+}(a q) )
( mathbf{c} cdot 3 S^{2-}(a q)+4 I_{2}(s)+4 H_{2} O(l) longrightarrow )
( 8 I^{-}(a q)+5 S O_{4}^{2-}(a q)+8 H^{+}(a q) )
D ( cdot 2 S^{2-}(a q)+4 I_{2}(s)+H_{2} O(l) rightarrow 8 I^{-}(a q)+S O_{4}^{2-}(a q)+ )
( 8 H^{+}(a q) )
11
312Which of the following reactions do not
involve oxidation or reduction:
A ( cdot 2 R b+2 H_{2} O rightarrow 2 R b O H+H_{2} )
в. ( 2 C u I_{2} rightarrow 2 C u+I_{2} )
c. ( N H_{4} C l+N a O H rightarrow N a C l+N H_{3}+H_{2} O )
D. None of these.
11
313The balanced chemical reaction with
( boldsymbol{C l}_{2} ) is
A ( cdot C l_{2}+2 N a_{2} S_{2} O_{3} rightarrow 2 N a C l+N a_{2} S_{4} O_{6} )
в. ( C l_{2}+H_{2} O+N a_{2} S_{2} O_{3} rightarrow N a_{2} S O_{4}+2 H C l+S )
c. ( C l_{2}(g)+S_{2} O_{3}^{2-} rightarrow S O_{4}^{2-}+S+C l )
D. None of the above
11
314Q. 17 The reaction Cl, (g) + 20H(aq) → CLO- (aq) + Cl(aq) + H20(1)
represents the process of bleaching. Identify and name the species that
bleaches the substances due to its oxidising action.
Thinking Process
Write the oxidation number of each element above its symbol, and then identify the
bleaching reagent by observing the change in oxidation number.
11
315Which of the following is the strongest reducing agent in aqueous medium?
( mathbf{A} cdot M g )
в. ( N a )
( c cdot L i )
D. ( C a )
11
316Balance the following equation.
( boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{I}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
A ( cdot 2 I O_{4}^{-}+14 I^{-}+16 H^{+} rightarrow 8 I_{2}+8 H_{2} O )
B . ( 2 I O_{4}^{-}+14 I^{-}+4 H^{+} rightarrow 3 I_{2}+8 H_{2} O )
c. ( I O_{4}^{-}+7 I^{-}+8 H^{+} rightarrow 4 I_{2}+4 H_{2} O )
D. None of these
11
317Which of the following is disproposination reaction?
A ( cdot C a C O_{3}+2 H^{+} rightarrow C a^{2+}+H_{2} O+C O_{2} )
B . ( 2 mathrm{CrO}_{4}^{2-}+2 mathrm{H}^{+} rightarrow mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+mathrm{H}_{2} mathrm{O} )
c. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O )
D. ( C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O )
11
318The oxidation state of the underlined
element in the given compound is:
( C_{12} H_{22} O_{11} )
A ( .+5 )
( B cdot+4 )
( c cdot 0 )
D. none of these
11
319Match the reaction in list 1 with their
type in list 2
11
320The reaction ( Z n O+C rightarrow Z n+C O ) is
an example of a
A. Combination reaction
B. Reduction-oxidation reaction
c. Displacement reaction
D. Decomposition Reaction
11
321( a C u^{2+}(a q)+b I^{-}(a q) rightarrow c C u I(s)+d I_{2}(s) )
When the equation above is balanced and
all coefficients are reduced to lowest
whole-number terms, what will be the
coefficient for ( I^{-} ) ?
( mathbf{A} cdot mathbf{1} )
B. 2
( c cdot 3 )
( D cdot 4 )
( E cdot 5 )
11
322The number of moles of ( C r_{2} O_{7}^{2-} ) needed
to oxidize 0.136 equivalent of ( N_{2} H_{5}^{+} )
through the reaction ( N_{2} H_{5}^{+}+ ) ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-} rightarrow boldsymbol{N}_{2}+boldsymbol{C r}^{3+}+boldsymbol{H}_{2} boldsymbol{O}, ) is :
A . 0.236
B. 0.087
c. 0.136
D. 0.488
11
323The oxidation state of oxygen of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) in the final products when it reacts with
( boldsymbol{A} boldsymbol{s}_{2} boldsymbol{O}_{3} ) is :
( mathbf{A} cdot mathbf{0} )
B.
( c cdot-1 )
D. – –
11
324Which of the following is not a redox reaction?
A ( cdot C a C O_{3} rightarrow C a O+C O_{2} )
в. ( O_{2}+2 H_{2} longrightarrow 2 H_{2} O )
c. ( N a+H_{2} O longrightarrow N a O H+frac{1}{2} H_{2} )
D. ( M n C l_{3} longrightarrow M n C l_{2}+frac{1}{2} C l_{2} )
11
325What is the oxidation number of Cl in
( H C l O ) and ( H C l O_{2} ? )
11
326( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{O} boldsymbol{H}^{-}(boldsymbol{H} boldsymbol{o} boldsymbol{t}) rightarrow(boldsymbol{P})+ )
( (Q) ;(P)+(Q)+H^{+} rightarrow B r_{2} )
( (P) ) gives yellow precipitate with
( A g N O_{3},(P) ) and ( (Q) ) are:
A. ( B r^{-}, B r O^{-} )
B. ( B r^{-}, B r O_{3} )
c. ( B r O^{-}, B r O_{3}^{-} )
D. ( B r O^{-}, B r O 4 )
11
327The oxidation state of the most
electronegative element in the products
of the reaction between ( B a O_{2} ) and
( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} ) are
A. 0 and -1
B. -1 and -2
c. -2 and 0
D. -2 and +1
11
328Balance the following redox reactions in acidic medium :
[
Z n+N O_{3}^{-} longrightarrow Z n^{2+}+N_{2}
]
A ( cdot 5 Z n+2 N O_{3}^{-}+12 H^{+} rightarrow 5 Z n^{2+}+N_{2}+3 H_{2} O )
B . ( 5 Z n+2 N O_{3}^{-}+12 H^{+} rightarrow 5 Z n^{2+}+N_{2}+6 H_{2} O )
( mathrm{c} cdot 5 Z n+2 N O_{3}^{-}+6 H^{+} rightarrow 3 Z n^{2+}+N_{2}+6 H_{2} O )
D. None of these
11
329In the redox reaction given below:
( boldsymbol{x} boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{y} boldsymbol{A} boldsymbol{s}_{2} boldsymbol{S}_{3}+boldsymbol{z} boldsymbol{H}_{2} boldsymbol{O} rightarrow )
( boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{3-}+boldsymbol{N} boldsymbol{O}+boldsymbol{S} boldsymbol{O}_{4}^{2-}+boldsymbol{H}^{+} )
What is the value of ( frac{x}{z} ? )
11
33011. A double salt KHC204.H_C204.2H20 is 0.2 N
acid. Thus, it is
(a) 0.267 N as reducing agent
(b) 0.6 M as an acid
(c) 0.067 M as a reducing agent
(d) 0.067 M as an acid
11
331In which of the following, sulphur has the highest oxidation state?
This question has multiple correct options
( A cdot S O_{2} )
в. ( S O_{3} )
c. ( H_{2} S O_{4} )
D. ( H_{2} S_{S} )
11
332Balance the following reaction.
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{C}_{2} boldsymbol{H}_{4} boldsymbol{O}+boldsymbol{H}^{+} rightarrow )
( boldsymbol{C}_{2} boldsymbol{H}_{4} boldsymbol{O}_{2}+boldsymbol{C} boldsymbol{r}^{3+} )
A ( cdot C r_{2} O_{7}^{2-}+3 C_{2} H_{4} O+8 H^{+} rightarrow 3 C_{2} H_{4} O_{2}+2 C r^{3+}+ )
( 4 H_{2} O )
B . ( C r_{2} O_{7}^{2-}+C_{2} H_{4} O+8 H^{+} rightarrow 3 C_{2} H_{4} O_{2}+5 C r^{3+}+H_{2} O )
C. ( C r_{2} O_{7}^{2-}+4 C_{2} H_{4} O+4 H^{+} rightarrow C_{2} H_{4} O_{2}+2 C r^{3+}+ )
( 4 H_{2} O )
D. None of these
11
333( C u^{+} ) undergoes disproportionation to
( C u ) and ( C u^{2+} )
If true enter 1 , else enter 0 .
( A )
11
334The balanced equation in basic
medium is :
( boldsymbol{S}_{2} boldsymbol{O}_{4}^{2-}+boldsymbol{A} boldsymbol{g}_{2} boldsymbol{O} stackrel{O H^{-}}{rightarrow} boldsymbol{A} boldsymbol{g}+boldsymbol{S} boldsymbol{O}_{3}^{2-} )
A ( cdot S_{2} O_{4}^{2-}+A g_{2} O+2 O H^{-} rightarrow 2 A g+2 S O_{3}^{2-}+H_{2} O )
B. ( S_{2} O_{4}^{2-}+2 A g_{2} O+2 O H^{-} rightarrow 2 A g+S O_{3}^{2-}+H_{2} O )
( mathbf{c} cdot 2 S_{2} O_{4}^{2-}+3 A g_{2} O+2 O H^{-} rightarrow 2 A g+2 S O_{3}^{2-}+H_{2} O )
D. none of these
11
335The species reduce in the following
reaction is :
( boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{3} boldsymbol{C} boldsymbol{O} rightarrow boldsymbol{2} boldsymbol{F} boldsymbol{e}+boldsymbol{3} boldsymbol{C} boldsymbol{O}_{2} )
A . ( F e )
в. ( C O )
( c cdot C O_{2} )
D. ( F e_{2} O_{3} )
11
336Find the sum of average oxidation
number of ( S ) in ( H_{2} S O_{5} ) (peroxy
monosulphuric acid) and ( N a_{2} S_{2} O_{3} )
(sodium thiosulphate)
11
337In the following reaction ( : boldsymbol{C r}(boldsymbol{O H})_{3}+ )
( boldsymbol{O H}^{-}+boldsymbol{I O}_{3}^{-} rightarrow boldsymbol{C r} boldsymbol{O}_{4}^{2-}+boldsymbol{H}_{2} boldsymbol{O}+ )
( boldsymbol{I}^{-}: )
A ( cdot I O_{3} ) – is oxidising agent
B. ( C r(O H)_{3} ) is oxidised
C. ( 6 e^{-} ) are being taken per iodine atom
D. all of these
11
338Q19. Identify the oxidant and the reductant in the following reaction.
N,H.(g) + Clo, (aq) → NO(g) + Cl(aq)
11
339Out of the halogens, which one is the most powerful oxidizing agent?
A. bromine
B. fluorine
c. iodine
D. chlorine
11
340Estimate the cell potential of a Daniel cell having ( 1.0 M Z n^{++} ) and originally having ( 1.0 M C u^{++} ) after sufficient
( N H_{3} ) has been added to the cathode
compartment to make ( N H_{3} )
concentration ( 2.0 M ) at equilibrium.
( operatorname{Given} boldsymbol{K}_{f} ) for ( left[boldsymbol{C u}left(boldsymbol{N} boldsymbol{H}_{3}right)_{4}right]^{2+}=mathbf{1} times )
( 10^{12}, E^{o} ) for the reaction, ( Z n+ )
( boldsymbol{C u}^{2+} longrightarrow Z boldsymbol{n}^{2+}+boldsymbol{C u} quad mathbf{1 . 1} boldsymbol{V} ) (Take
( frac{mathbf{2 . 3 0 3} boldsymbol{R} boldsymbol{T}}{boldsymbol{F}}=mathbf{0 . 0 6} log mathbf{6 . 2 5}=mathbf{0 . 8} mathbf{)} )
11
3410.5 Thiosulphate reacts differently with iodine
ate reacts differently with iodine and bromine in the reactions
given below
250 + Iz 50% + 25
S203 + 2Br2 + 5H20 – 2503 + 2Br + 10H*
Which of the following statements justifies the above dual behaviour of
thiosulphate?
(a) Bromine is a stronger oxidant than iodine
(b) Bromine is a weaker oxidant than iodine
(c) Thiosulphate undergoes oxidation by bromine and reduction by iodine in these
reactions
(d) Bromine undergoes oxidation and iodine undergoes reduction in these reactions
11
342Choose the redox reaction from the
following.
( mathbf{A} cdot C u+2 H_{2} S O_{4} rightarrow C u S O_{4}+S O_{2}+2 H_{2} O )
B ( cdot B a C l_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+2 H C l )
( mathbf{c} cdot 2 N a O H+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+2 H_{2} O )
( mathbf{D} cdot K N O_{2}+H_{2} S O_{4} rightarrow 2 H N O_{2}+K_{2} S O_{4} )
11
343The oxidation state of phoshorus varies
from
A. -1 to +1
B . -3 to +3
( mathbf{c} cdot-3 ) to +5
D. -5 to +1
11
344The reaction is balanced if ( 5 H_{2} O_{2}+ )
( boldsymbol{x} boldsymbol{C l} boldsymbol{O}_{2}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{x} boldsymbol{C l}^{-}+boldsymbol{y} boldsymbol{O}_{2}+ )
( 6 H_{2} O )
The value of ( y ) is :
11
345Write formulas for the following compounds. Tin (IV) oxide11
346Identify the pair of binary corresponds in which nitrogen exhibits the lowest
and the highest oxidation state.
A. ( N H_{3}, N O_{2} )
в. ( N_{3} H, N_{2} O_{5} )
c. ( N_{2}, H N O_{3} )
D. ( N_{2} O, N_{2} O_{5} )
11
347Explain Displacement reaction with examples11
348What coefficients are required to balance the following equation?
( boldsymbol{F} boldsymbol{e}+boldsymbol{O}_{2} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{O} )
( mathbf{A} cdot 2,1,2 )
B. 1,1,1
c. 4,2,4
D. 2,1,1
11
349Corrosion of iron is :
( A cdot ) redox process
B. neutrilization process
C . precipitation process
D. none of the above
11
350( Z n+H_{2} S O_{4} rightarrow ) a gas
If we bring a burning splinter near the gas produced in the given reaction, it burns with a pop sound. The gas is:
( A cdot O_{2} )
в. ( N_{2} )
( mathrm{c} cdot mathrm{H}_{2} )
D. ( C O_{2} )
11
351Match the reactions in column I with
the molar ratio of their respective oxidants and reductant in column II.
11
352How many substances have underlined
atoms of different nature?
( N a_{2} S_{4} O_{6}, N a_{2} S_{2} O_{3}, C a O C l_{2}, N_{2} H_{4} O_{3} )
A. 7
B. 5
( c cdot 4 )
D. 8
11
353In the formation of electrovalent
compound ( M g C l_{2} ) name the substance that is oxidized and is reduced.
11
354The redox process involves the complete transfer of electrons in the formation in
ionic bonds or partial transfer or shift of electrons in the formation of covalent
bonds.
If true enter 1 , else enter 0 .
( A )
11
355An element forms two oxides containing respectively 53.33 and 36.36 percent of oxygen. These figures illustrate the law of
A. Conservation of mass
B. Constant proportions
c. Reciprocal proportions
D. Multiple proportions
11
356Which of the following compounds have zero oxidation state at carbon?
This question has multiple correct options
A. ( C_{6} H_{12} O_{6} )
в. нсоон
c. нсно
D. ( C H_{4} )
11
357( N a O H+H_{2} S O_{4} rightarrow N a_{2} S O_{4}+H_{2} O )
Balance the given chemical equation
11
358Which of the following represents a correctly balanced half-reaction?
A ( cdot C l_{2}+2 e^{-} rightarrow C l^{-} )
B ( cdot 2 e+F e rightarrow F e^{2+} )
c. ( O_{2} rightarrow 2 e^{-}+2 O^{2} )
D. ( A l^{3+} rightarrow A l+3 e^{-} )
E ( cdot 2 H^{+}+2 e^{-} rightarrow H_{2} )
11
359Identify redox reaction among the following:
A. acid-base neutralization
B. precipitation reaction
c. metal displacement reaction
D. all the above
11
360Volume of ( 0.1 mathrm{M} K M n O_{4}, ) required to
oxidise completely ( 50 mathrm{ml} ) of ( 0.5 mathrm{M} ) ferrous oxalate solution in acidic
medium will be:
A . ( 100 mathrm{mL} )
B . ( 120 mathrm{mL} )
( c .150 mathrm{mL} )
D. ( 200 mathrm{mL} )
11
361Q2. What is a redox couple?11
362In the reaction ( 2 A g+2 H_{2} S O_{4} rightarrow )
( A g_{2} S O_{4}+2 H_{2} O+S O_{2} ) sulphuric acid
acts as:
A. an oxidising agent
B. a reducing agent
c. a catalyst
D. an acid as well as oxidant
11
363When ( S O_{2} ) is passed in a solution of
potassium iodate, the oxidation state of iodine changes from:
A . +5 to 0
B. +5 to -1
c. -5 to 0
D. -7 to -1
11
364In the following reaction which element is oxidized?
( boldsymbol{M} boldsymbol{g}(boldsymbol{s})+boldsymbol{C l}_{2}(boldsymbol{g}) longrightarrow boldsymbol{M} boldsymbol{g} boldsymbol{C l}_{2}(boldsymbol{s}) )
( mathbf{A} cdot M g )
в. ( C l_{2} )
( mathrm{c} cdot M g^{+} )
D. ( C l^{-} )
11
365( B r_{2} rightarrow B r O_{3}^{-}+B r^{-}(text {acidic }) ) is a
balanced equation.
If true enter 1 , else enter 0 .
( A )
11
366What is incorrectly matched?
( mathbf{A} cdot C s B r_{3} rightleftharpoons C s^{oplus}+B r_{3}^{ominus} rightleftharpoons C s^{oplus}+B r^{ominus}+B r_{2} )
B ( cdot I_{4} O_{9} rightleftharpoons I^{3}+3left(I O_{3}right)^{ominus} )
( mathbf{c} cdot A g B r O_{3} rightleftharpoons A g^{oplus} B r_{3}^{ominus} )
( mathbf{D} cdot I_{2} O_{4} rightleftharpoons I O_{2}^{oplus}+I O_{2}^{ominus} )
11
367Q6. (a) Arrange the following in order of increasing O.N of iodine:
1,, HI, HIO, KIO, ICI.
(b) Identify the oxidant and reductant in the following redox reaction:
2KMnO4 + Cl2KCl + 2KMnO
ta
TL
11
368Q. 22 Calculate the oxidation number of phosphorus in the following species.
(a) HPO-
(6) PO3-
11
369Which of the following oxidation numbers is not correctly matched?
A ( cdot P ) in ( N a H_{2} P O_{4}=+5 )
B. ( N i ) in ( left[N i(C N)_{6}right]^{4-}=+2 )
( mathbf{c} cdot P ) in ( M g_{2} P_{2} O_{7}=+6 )
D. ( C r ) in ( left(N H_{4}right)_{2} C r_{2} O_{7}=+6 )
11
370Q.10 Identify disproportionation reaction
(a) CH4 + 202 → CO2 + 2H,0
(b) CH4 + 4Cl2 → CCIA + 4HCI
(c) 2F + 20H2F+OF+
HO
(d) 2NO, + 2OH- NO2 + NO3 + H2O
11
371Consider the reaction: ( boldsymbol{F e}+boldsymbol{H}_{2} boldsymbol{O} rightarrow )
( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}+boldsymbol{H}_{2} )
If the number of electrons lost or gained
during the changes is ( x ). Then, the value
of ( x ) is :
11
372A qualitative analysis test for ( M n^{2+} )
involves its oxidation to ( M n O_{4}^{-} ) in
acidic solution by sodium bismuthate,
( N a B i O_{3} . ) The bisulphate ion is reduced
to ( B i^{3 i} . ) What is a balanced equation for
this test?
A ( cdot B i O_{3}^{-2}+M n^{2+}+H^{+} rightarrow M n O_{4}^{-}+B i^{3+}+H_{2} O )
B. ( 5 B i O_{3}^{-}+2 M n^{2+}+7 H^{+} rightarrow 2 M n O_{4}^{-}+5 B i^{3+}+7 O H )
C. ( 5 B i O_{3}^{-}+2 M n^{2+}+14 H^{+} rightarrow 2 M n O_{4}^{-}+5 B i^{3+}+7 H_{2} O )
D. None of these
11
373Which of the following examples does not represent disproportionation?
A ( cdot M n O_{2}+4 H C l rightarrow M n C l_{2}+C l_{2}+2 H_{2} O )
в. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} )
c. ( 4 K C l O_{3} rightarrow 3 K C l O_{4}+K C l )
D. ( 3 C l_{2}+6 N a O H longrightarrow 5 N a C l+N a C l O_{3}+3 H_{2} O )
11
374In an experiment, 20 g of vanadium ( (V) ) oxide (molar mass ( =182 ) g/mol) was
reduced by excess of zinc dust in acidic solution to vanadium
(II) ions. If the
required number of moles of iodine to
reoxidise vanadium
(II) to ( V O^{2+} ) is
( 22 times 10^{-x}, ) then what is the value of ( x ? )
11
375Consider the following reaction,
( mathbf{5} boldsymbol{H}_{mathbf{2}} boldsymbol{O}_{mathbf{2}}+boldsymbol{x} boldsymbol{C l} boldsymbol{O}_{mathbf{2}}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{x} boldsymbol{C l}^{-}+ )
( boldsymbol{y} boldsymbol{O}_{2}+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O} . ) The reaction is balanced
if
A ( . x=5, y=2 )
в. ( x=2, y=5 )
c. ( x=4, y=10 )
D. ( x=5, y=5 )
11
376Which compound amongst the following has the highest oxidation
number of ( M n ? )
A. ( K M n O_{4} )
в. ( K_{2} M n O_{4} )
( mathrm{c} cdot M n O_{2} )
D. ( M n_{2} O_{3} )
11
377Which of the following is not a redox reaction?
A. ( M g+N_{2} rightarrow M g_{3} N_{2} )
B . ( M n O_{4}^{-}+C_{2} O_{4}^{2-} rightarrow M n^{2+}+C O_{2} )
c. ( C u S O_{4}+K I rightarrow 2 C u I+I_{2}+K_{2} S O_{4} )
D. ( A g C l+N H_{3} rightarrowleft[A gleft(N H_{3}right)_{2}right] C l )
11
378Balance the following in basic medium:
( boldsymbol{A s O}_{3}^{3+}+boldsymbol{M n O}_{4}^{-} rightarrow boldsymbol{A} boldsymbol{s} boldsymbol{O}_{4}^{3-}+boldsymbol{M n O}_{2} )
A ( cdot 3 A s O_{3}^{3+}+2 M n O_{4}^{-}+H_{2} O rightarrow 3 A s O_{4}^{3-}+2 M n O_{2}+ )
( 2 O H^{-} )
B. ( 3 A s O_{3}^{3+}+2 M n O_{4}^{-}+4 H_{2} O rightarrow 3 A s O_{4}^{3-}+3 M n O_{2}+ )
( 2 O H^{-} )
( mathrm{c} cdot 3 A s O_{3}^{3+}+4 M n O_{4}^{-}+3 H_{2} O rightarrow 3 A s O_{4}^{3-}+2 M n O_{2}+ )
( 4 O H^{-} )
D. None of these
11
379( 2 P b O+C rightarrow 2 P b+C O_{2} ) is an
example of
A. oxiation reaction
B. reduction reaction
c. redox reaction
D. none
11
380Q. 9 The largest oxidation number exhibited by an element depends on its
outer electronic configuration. With which of the following outer
electronic configurations the element will exhibit largest oxidation
number?
(a) 3d 452 (b) 3d 452 (c) 3d 4s’ (d) 3d 4s
11
381Which of the followings are redox titration?
A. Complexometric titration
B. Iodometric titration
c. Acid-base titration
D. Back titration
E. All of these
11
382What coefficient is needed for fluorine
to balance the following equation? ( boldsymbol{L} boldsymbol{i}+boldsymbol{F}_{2} rightarrow boldsymbol{L} boldsymbol{i} boldsymbol{F} )
( mathbf{A} cdot mathbf{0} )
B.
( c cdot 2 )
D. 3
11
383For the reaction between ( M n O_{4}^{-} ) and
( C_{2} O_{4}^{-} ) in basic solution, the unbalanced equation is as follows:
( M n O_{4}^{-}+C_{2} O_{4}^{2-} longrightarrow M n O_{2}(s)+ )
( boldsymbol{C O}_{3}^{2-} )
In a balanced equation, the number of
( O H^{-} ) ions on the right is :
11
384In which of the following, the oxidation number of oxygen has been arranged in increasing order?
A. ( B a O_{2}<K O_{2}<O_{3}<O F_{2} )
в. ( O F_{2}<K O_{2}<B a O_{2}<O_{3} )
c. ( B a O_{2}<O_{3}<O F_{2}<K O_{2} )
D. ( K O_{2}<O F_{2}<O_{3}<B a O_{2} )
11
385( A l+M n O_{4}^{-} rightarrow A l(O H)_{4}^{-}+M n O_{2} )
For this reaction, element ( X ) is reduced
and element Y is oxidised. Then ( X ) and
( Y ) are respectively:
A. ( A l ) and ( M n )
B. ( M n ) and ( A l )
c. ( A l ) and ( A l )
D. Mn and ( M n )
11
386Write the overall reaction taking place
in Daniel Cell.
11
387The cell reaction ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2+}(boldsymbol{a q})+ )
( mathbf{1 4} boldsymbol{H}^{+}(boldsymbol{a q})+boldsymbol{6} boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a q}) rightarrow )
( mathbf{6} F e^{3+}(boldsymbol{a} boldsymbol{q})+mathbf{2} boldsymbol{C} boldsymbol{r}^{3+}(boldsymbol{a} boldsymbol{q})+mathbf{7} boldsymbol{H}_{2} boldsymbol{O}(l) )
best represented by:
A ( cdot P t(s)left|F e^{2+}(a q), F e^{3+}(a q) | C r_{2} O_{7}^{2+}(a q), C r^{3+}(a q)right| P t(s) )
B . ( P t(s)left|C r_{2} O_{7}^{2+}(a q), C r^{3+}(a q) | F e^{3+}(a q), F e^{2+}(a q)right| P t(s) )
C. ( F e^{2+}(a q)left|F e^{3+}(a q) | C r_{2} O_{7}^{2+}(a q)right| C r^{3+}(a q) )
D. ( C r_{2} O_{7}^{2+}(a q)left|C r^{3+}(a q) | F e^{3+}(a q)right| F e^{2+}(a q) )
11
388Select the correct alternative.
In the reaction of ( Z n+F e S O_{4} rightarrow )
( Z n S O_{4}+F e )
A. zn gets oxidized
B. Fe gets oxidized
c. zn is oxidized in agent
D. zn and Fe both get oxidized
11
389The oxidation number of chlorine is
maximum in
A . ( H O C l )
в. ( C l_{2} O_{6} )
c. ( K C l O_{4} )
D. ( N a C l O_{3} )
11
390Which type of reaction produces heat and light?
A. Endothermic
B. Phytochemical
c. Reduction
D. Exothermic
11
391The reaction: ( 3 C l O^{-} rightarrow C l O_{3}^{-}+2 C l^{-} )
is an example of
A. Oxidation reaction
B. Reduction reaction
c. Disproportionation reaction
D. Decomposition reaction
11
392How many mL of ( 0.3 mathrm{M} K_{2} C r_{2} O_{7}(text { acidic }) )
is required for complete oxidation of 5
( mathrm{mL} ) of ( 0.2 mathrm{M} ) Sn ( C_{2} mathrm{O}_{4} ) solution.
(Round off to 1 decimal place)
11
39307. What is salt bridge?11
394What is the reaction called when
oxidation and reduction take place simultaneously? Explain with one example.
11
395State whether the given statement is
true or false:
Neutralisation is a double
displacement reaction
A. True
B. False
11
396Which indicator we prefer to use in
iodometric titration?
A. Starch
B. Phenolphthalein
c. 1,10 phenathroline
D. All of the above
11
397Number of peroxide bonds in ( K_{3} C r O_{8} )
is 4
If true enter 1 , else enter 0 .
( A )
11
398Which of the following reactions is/ are
not intermolecular redox reaction?
This question has multiple correct options
( mathbf{A} cdot P b O_{2}+H_{2} O rightarrow P b O+H_{2} O_{2} )
B ( cdot 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} )
( mathbf{C} cdotleft(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+4 H_{2} O )
D. ( N H_{4} N O_{2} rightarrow N_{2}+2 H_{2} O )
11
399Balance the following redox reactions:
[
boldsymbol{I}_{2}(boldsymbol{s})+boldsymbol{O} boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) longrightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}(boldsymbol{a} boldsymbol{q})+
]
( boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) )
( mathbf{A} cdot I_{2}(s)+5 O C l^{-}(a q)+H_{2} O(l) longrightarrow 2 I O_{3}^{-}(a q)+ )
[
5 C l^{-}(a q)+2 H^{+}(a q)
]
B ( cdot I_{2}(s)+5 O C l^{-}(a q)+2 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ )
[
4 C l^{-}(a q)+2 H^{+}(a q)
]
( mathbf{c} cdot I_{2}(s)+3 O C l^{-}(a q)+4 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ )
( 4 C l^{-}(a q)+2 H^{+}(a q) )
( mathbf{D} cdot I_{2}(s)+5 O C l^{-}(a q)+7 H_{2} O(l) longrightarrow I O_{3}^{-}(a q)+ )
( 5 C l^{-}(a q)+2 H^{+}(a q) )
11
4005. Which ordering of compounds is according to the
decreasing order of the oxidation state of nitrogen?
(a) HNO, NO, NHẠCl, N,
(b) HNO2, NO, N, NH,CI
(c) HNO, NHCl, NO, N,
(d) NO, HNO, NHẠCl, N,
11
401( C N^{ominus} ) ion is oxidised by a powerful
oxidising agent to ( N O_{3}^{ominus} ) and ( C O_{2} ) or
( C O_{3}^{2-} ) depending on the acidity of the
reaction mixture.
( boldsymbol{C N}^{ominus} longrightarrow boldsymbol{C O}_{2}+boldsymbol{N O}_{3}^{ominus}+boldsymbol{H}^{oplus}+boldsymbol{n} e^{-} )
What is the number ( (n) ) of electrons
involved in the process?
11
402The oxidation reaction always takes place with a reduction reaction. Why is isolated oxidation reaction not
possible?
11
403Q. 20 Nitric acid is an oxidising agent and reacts with PbO but it does not
react with Pb0,. Explain why?
11
404The oxidation state of the underlined
element in the given compound is:
( boldsymbol{N} boldsymbol{a}_{2}left[underline{boldsymbol{F}} e(boldsymbol{C} boldsymbol{N})_{5} boldsymbol{N} boldsymbol{O}right] )
( A cdot-2 )
( B .+2 )
( c cdot+3 )
D. none of these
11
405Assertion
The oxidation state of ( S ) in ( H_{2} S_{2} O_{8} ) is 6
Reason
Maximum oxidation state of ( S ) is 6
because the maximum oxidation state
of an element is its number of valence
electron.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
406Chlorine is used to purify drinking water. Excess of chlorine is harmful. The
excess of chlorine is removed by treating with sulphur dioxide. Present a balanced equation for the redox change taking place in water
11
407The oxidation number of the nitrogen atom in the ammonium ion is :
( A cdot+3 )
( B .+2 )
( c cdot+1 )
( D cdot-2 )
E. – –
11
408Balance the following equation by ion electron method.
( M n O_{4}^{-}+H^{+}+H_{2} O_{2} rightarrow M n^{2+}+ )
( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{O}_{2} )
11
409Titration curves for ( 0.1 mathrm{M} ) solutions of
three weak acids ( H A_{1}, H A_{2} ) ans ( H A_{3} )
with ionization constants ( boldsymbol{K}_{1}, boldsymbol{K}_{2} ) and
( K_{3} ) respectively are plotted in the figure.which of the following is/are
true?
( mathbf{A} cdot K_{2}=left(K_{1}+K_{3}right) / 2 )
B . ( K_{1}K_{2} )
D. ( K_{2}>K_{3} )
11
410A number which is assigned to each
atom or ion in a compound which explains its degree of oxidation is called:
A. oxidation degree
B. oxidation number
c. oxidation state
D. both ( B ) and ( C )
11
41142 DIN
Q13. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the
following reactions.
(a) 2AgBr(s) + CH 0,(aq) —>2Ag(s) + 2HBr(aq) + CH,0, (aq)
(b) HCHO) + 2[AgNH,), (aq) + 3OH (aq) »
2Ag(s) + HCOO (aq) + 4NH, (aq) + 2H2O(1)
(c) HCHOI) + 2Cu2+ (aq) + 50H(aq) → Cu,O(s) + HCOO (aq) + 3H2O(1)
(d) N,H.(I) + 2H20 (1) ► N.(g) + 4H2O(1)
(e) Pb(s) + PbO (s) + 2H,SO, aq) 2PbSO4(s) + 2H20(1)
11
412Bleaching powder ( left(C a O C l_{2}right) ) has two types of chlorine atoms with oxidation
number of +1 and ( -1 . ) It can be
represented as:
A ( cdot C a^{2+}left(C l O_{2}^{-}right) C l^{-} )
в. ( C a^{2+}left(C l O_{3}^{-}right) C l^{-} )
c. ( C a^{2+}left(C l O^{+}right) C l^{-} )
D. ( C a^{2+}left(C l O^{-}right) C l^{-} )
11
413Given ( 4 N H_{3}(g)+5 O_{2}(g) rightarrow )
( mathbf{4} boldsymbol{N} boldsymbol{O}(boldsymbol{g})+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) )
The above reaction is an example of:
(i) displacement reaction
(ii) combination reaction
(iii) redox reaction
(iv) neutralisation reaction
A ( . ) (i) and (iv)
B. (ii) and (iii)
c. (i) and (iii)
D. (iii) and (iv)
11
414Balance the following equation by ion electron method.
( Z n+B r O_{4}^{-}+O H^{-}+H_{2} O rightarrow )
( left[boldsymbol{Z n}(boldsymbol{O H})_{4}right]^{2-}+boldsymbol{B r}^{-} )
11
415The oxidation state of ( mathrm{Mn} ) in ( boldsymbol{K}_{mathbf{2}} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{boldsymbol{4}} )
is:
( A cdot+5 )
( B cdot+4 )
( c cdot+7 )
( D cdot+6 )
11
416Ag, SO, + 2H,0 + SOZ
4. On the reaction
2Ag + 2H, SO
sulphuric acid acts as
(a) an oxidizing agent
(C) a catalyst
The Qyidation in
(b) a reducing agent
(d) an acid as well as an oxidant
5
11
417Oxidation means
(gain/loss) of ( O_{2} ) and reduction means
gain of hydrogen.
11
4180.28 Match the items in Column I with relevant items in Column II.
Column 1
Column II
A. Tons having positive charge
1. +7
B. The sum of oxidation number of 2 -1 oth
all atoms in a neutral molecule
с. Oxidation number of hydrogen
3 +1 O
ion (HT)
D O xidation number of fluorine in
NaF
E lons having negative charge 5. Cation
Anion
11
419The ratio of oxygen atom having -2 and
-1 oxidation numbers in ( S_{2} O_{8}^{2-} ) is
three
If true enter 1 , else enter 0
A.
11
420Which reaction does not represent autoredox or disproportionation?
A ( cdot C l_{2}+2 O H^{-} rightarrow C l^{-}+C l O^{-}+H_{2} O )
B. ( 2 H_{2} O_{2} rightarrow 2 H_{2} O+O_{2} )
( mathbf{c} cdot 2 C u^{+} rightarrow C u^{+2}+C u )
D. ( left(N H_{4}right)_{2} C r_{2} O_{7} longrightarrow N_{2}+C r_{2} O_{3}+4 H_{2} O )
11
421Arrange the following in the order of increasing oxidation number of
nitrogen: ( N H_{3}, N_{3} H, N_{2} O, N O, N_{2} O_{5} )
11
422Assertion
( F_{2} ) undergoes disproportionation
reaction.
Reason
Fluorine shows both positive and
negative oxidation states.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
423Explain how ( Z n+2 A g N O_{3} rightarrow 2 A g+ )
( Z nleft(N O_{3}right)_{2} ) is a redox reaction.
11
424Match the compounds given in column I with oxidation states of carbon given in column II and mark the apropriate
choice.
( (A) )
(B) The the ( begin{array}{llll}text { Column I } & & text { Column II } \ & & \ C_{6} H_{12} O_{6} & text { (i) } & +3 \ & C H C l_{3} & text { (ii) } & -3 \ & C H_{3} C H_{3} & text { (iii) } & +2 \ & (C O O H)_{2} & text { (iv) } & 0end{array} )
(c)
(D)
( A )
( (A) rightarrow(text { iv }),(B) rightarrow(text { iii }),(C) rightarrow(text { ii }),(D) rightarrow(i) )
B. ( (A) rightarrow(text { i }),(B) rightarrow(text { ii }),(C) rightarrow(text { iii }),(D) rightarrow(text { iv }) )
C. ( (A) rightarrow(text { ii }),(B) rightarrow(text { iii }),(C) rightarrow(text { iv }),(D) rightarrow(i) )
( D cdot(A) rightarrow(text { iii }),(B) rightarrow(text { ii }),(C) rightarrow(i),(D) rightarrow(text { iv }) )
11
425Which of the one is not true about redox
reactions?
A. Share of electrons
B. Transfer of electrons
c. Gain of oxygen
D. Loss of Hydrogen
11
426Assertion
Oxidation involves loss of electrons and
reduction involves gain of electrons.
Reason
The overall reaction in which oxidation
and reduction occurs simultaneously is called redox reaction.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
427Arrange the following in increasing
order of oxidation state of ( N i )
( boldsymbol{K}_{2}left[boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{N})_{4}right], boldsymbol{K}_{2}left[boldsymbol{N} boldsymbol{i} boldsymbol{F}_{6}right], boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{O})_{4} )
A ( cdot N i(C O)_{4}, K_{2}left[N i(C N)_{4}right], K_{2}left[N i F_{6}right] )
B . ( K_{2}left[N i(C N)_{4}right], N i(C O)_{4}, K_{2}left[N i F_{6}right] )
c. ( N i(C O)_{4}, K_{2}left[N i F_{6}right], K_{2}left[N i(C N)_{4}right] )
D. ( K_{2}left[N i F_{6}right], K_{2}left[N i(C N)_{4}right], K_{2}left[N i(C N)_{4}right]^{prime} )
11
428What is the oxidising agent in the following reaction? ( mathbf{2} boldsymbol{F} boldsymbol{e}_{boldsymbol{a} boldsymbol{q}}^{mathbf{2}+}+boldsymbol{C l}_{mathbf{2}(boldsymbol{g})} rightarrow mathbf{2} boldsymbol{F} boldsymbol{e}_{(boldsymbol{a q})}^{mathbf{3}+}+mathbf{2} boldsymbol{C l}_{(boldsymbol{a} boldsymbol{q})}^{-} )
A ( cdot F e^{2} )
в. ( C l_{2} )
( mathrm{c} cdot F e^{3} )
D. ( C l^{-} )
11
42909. Consider the reactions:
(a) 6CO2(8) 6H2O(l) CH4,06(s) + 60,(8) (b) 03(8) + H,0,1)→ H2O(l) +202(8)
Why it is more appropriate to write these reactions as:
(a) 6CO2(8) + 12H,O(1) CH20c(s) + 6H2O(l) + 60 (8)
(6) 03(8) + H,0,1) → H2O(1) + 0,(g) + O. (8)
Also suggest a technique to investigate the path of above (a) and (b) redox reactions.
11
430Find the oxidation state of bromine in
( mathrm{HBrO}_{3} )
( A cdot-3 )
B . –
( c cdot 1 )
( D .3 )
E. 5
11
431Determine the change in oxidation
number of sulphur in ( H_{2} S ) and ( S O_{2} ) respectively in the following reaction.
( 2 H_{2} S+S O_{2} rightarrow 2 H_{2} O+3 S )
A .0,+2
в. +2,-4
c. -2,+2
( mathbf{D} cdot+4,0 )
11
432Justify that the following reactions are
redox reactions.
( mathbf{A} cdot C u O(s)+H_{2}(g) rightarrow C u(s)+H_{2} O(g) )
B ( cdot F e_{2} O_{3}(s)+3 C O(g) rightarrow 2 F e(s)+3 C O_{2}(g) )
( mathbf{c} cdot 4 B C l_{3}(g)+3 L i A l H_{4}(s) rightarrow 2 B_{2} H_{6}(s)+3 L i C l(s)+ )
( 3 A l C l_{3}(s) )
D ( cdot 2 K(s)+F_{2}(g) rightarrow 2 K^{+} F^{-}(s) )
11
433In the reaction: ( S_{2} O_{8}^{2-}+2 I^{-} rightarrow )
( 2 S O_{4}^{2-}+I_{2} )
A. oxidation of iodide into iodine takes place
B. reduction of iodine into iodide takes place
c. both oxidation and reduction of iodine takes place
D. none of the above
11
434A balanced chemical equation is in accordance with:
A. Avogadro’s Law
B. Law of constant proportion
c. Law of conservation of mass
D. Law of gaseous volumes
11
435[
begin{array}{c}
begin{array}{c}
O \
C
end{array}-H \
H-C_{1}^{prime} O-H \
H
end{array}
]
Write oxidation No. of each ( C ) atom.
11
436The oxidation number of ( P t ) in
( left[boldsymbol{P t}left(boldsymbol{C}_{2} boldsymbol{H}_{4}right) boldsymbol{C l}_{3}right]^{-} ) is :
11
437Write balanced chemical equation for
the following. Action of ozone on hydrogen peroxide.
11
438Balance the following equation:
( boldsymbol{K} boldsymbol{C l} boldsymbol{O}_{3}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{K} boldsymbol{H} boldsymbol{S} boldsymbol{O}_{4}+ )
( boldsymbol{H} boldsymbol{C l O}_{4}+boldsymbol{C l O}_{2} )
A ( cdot 3 K C l O_{3}+3 H_{2} S O_{4} rightarrow 3 K H S O_{4}+H C l O_{4}+2 C l O_{2}+ )
( H_{2} O )
в. ( K C l O_{3}+5 H_{2} S O_{4} rightarrow 3 K H S O_{4}+3 H C l O_{4}+2 C l O_{2}+ )
( 3 H_{2} O )
c. ( 3 K C l O_{3}+4 H_{2} S O_{4} rightarrow 3 K H S O_{4}+2 H C l O_{4}+ )
( 2 C l O_{2}+H_{2} O )
D. None of these
11
439Find the oxidation number of elements
in each case.
( S ) in ( N a_{2} S_{2} O_{3}, S_{4}, S_{8} ) and ( N a_{2} S_{2} O_{7} )
( mathbf{A} cdot+2,0,0,+6 )
B. +1,1,0,+5
c. 0,0,1,+4
D. None of these
11
440Determine the oxidation state of the
underlined element in ( underline{I} C l )
A ( .+1 )
B. +4
( c cdot+2 )
D. +3
11
441( ln F e C r_{2} O_{4}, ) the oxidation number of ( f e )
and Cr are:
( A cdot+2 ) and +3
B. 0 and +2
( c cdot+2 ) and +6
D. 2 and
11
442For joining railway tracks, ferric oxide is reacted with aluminium to produce aluminium oxide and iron. The balanced
chemical equation for the given reaction is ( boldsymbol{F e}_{2} boldsymbol{O}_{3(x)}+boldsymbol{2} boldsymbol{A} boldsymbol{l}_{(x)} rightarrow )
Ferricoxide
( begin{array}{cc}boldsymbol{A} boldsymbol{l}_{2} boldsymbol{O}_{boldsymbol{3}(boldsymbol{x})} & boldsymbol{+} boldsymbol{2} boldsymbol{F} boldsymbol{e}_{(boldsymbol{x})} \ text {Aluminium oxide} & text {Iron}end{array} )
Which of the following substances is oxidized in the given reaction?
A ( cdot A l_{2} O_{3} )
в. ( F e_{2} O_{3} )
( c . A l )
D. ( F e )
11
443Balance the following equation by ion electron method.
( boldsymbol{P}_{4}+boldsymbol{O H}^{-}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}^{-}+boldsymbol{P H}_{3} )
11
444Cen when no current 10ws uvugu ce
Q16. Calculate the oxidation number of Cr in [Cr (
HO)Jion.
11
445What sorts of informations can you
draw from the following reaction?
( (boldsymbol{C N})_{2}(boldsymbol{g})+mathbf{2 O H}^{-}(boldsymbol{a q}) rightarrow )
( boldsymbol{C N}^{-}(boldsymbol{a q})+boldsymbol{C N O ^ { – }}(boldsymbol{a q})+boldsymbol{H}_{2} boldsymbol{O}(l) )
11
446What are the oxidation number of the
underlined elements in each of
the following and how do you rationalise your results?
( boldsymbol{K} underline{boldsymbol{I}}_{mathbf{3}} )
11
447Which of the following statement(s) is/are true?
This question has multiple correct options
A. All reactions are oxidation and reduction reactions.
B. Oxidising agent is itself reduced.
c. oxidation and reduction always go side by side
D. Oxidation number during reduction decreases.
11
448In a galvanic cell, the electrons flow
from:
A. anode to cathode through the solution
B. cathode to anode through the solution
C. anode to cathode through the external circuit
D. cathode to anode through the external circuit
11
4492. Oxalic acid H,C,0, reacts with permanganate on
according to the balanced equation given below. How
many milliliter of 0.0154 M KMnO solution is required
to react 25.0 mL of 0.0208 MH,C,0, solution?
5H_C20_(aq) + 2MnO2 +6H*(aq) →
2Mn2+(aq) + 10CO2(g) + 8H2O(1)
(a) 13.5 mL
(b) 18.5 mL
(c) 33.8 mL
(d) 84.4 mL
11
450Write balanced chemical equation for
the reaction of calcium oxide with
water?
11
451The number of redox reactions from the
following equations are:
a. ( boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{F} boldsymbol{e}^{3+} longrightarrow boldsymbol{F} boldsymbol{e}^{2+}+boldsymbol{S} downarrow+boldsymbol{H}^{oplus} )
b. ( boldsymbol{I}^{ominus}+boldsymbol{I} boldsymbol{O}_{3}^{ominus}+boldsymbol{H}^{oplus} longrightarrow boldsymbol{I}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
c. ( boldsymbol{B} boldsymbol{i}(boldsymbol{s})+boldsymbol{N} boldsymbol{O}_{3}^{ominus}+boldsymbol{H}^{oplus} longrightarrow boldsymbol{N} boldsymbol{O}_{2}+ )
( B i^{3+}+H_{2} O )
( mathbf{d .} boldsymbol{I}^{ominus}+boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O} longrightarrow boldsymbol{I}_{2}+stackrel{ominus}{boldsymbol{O}} boldsymbol{H} )
e. ( boldsymbol{C u}(boldsymbol{s})+boldsymbol{A} boldsymbol{u}^{oplus} longrightarrow boldsymbol{A} boldsymbol{u}(boldsymbol{s})+boldsymbol{C} boldsymbol{u}^{2+} )
11
452Calculate the equilibrium constant for the redox reaction at ( 25^{circ} mathrm{C}, S r_{(s)}+ ) ( M g_{(a q)}^{2+} rightarrow S r_{(a q)}^{2+}+M g_{(s)}, ) that occurs
in a galvanic cell. ( boldsymbol{E}_{M g^{2+} / M g}^{o}=-2.37 mathrm{V} )
and ( boldsymbol{E}_{boldsymbol{S r}^{2}+/ boldsymbol{S} boldsymbol{r}}^{o}=-boldsymbol{2} . boldsymbol{8} boldsymbol{9} boldsymbol{V} )
A ( cdot 2.69 times 10^{15} )
В. ( 2.69 times 10^{17} )
D. ( 3.69 times 10^{15} )
11
453Aqueous solutions of magnesium
chloride and silver nitrate are mixed to
form solid silver chloride and aqueous
magnesium nitrate.The balanced net ionic equation contains which of the
following terms?
( mathbf{A} cdot A g_{(a q)}^{+} )
B. ( M g_{(a q)}^{2+} )
c. ( N O_{3(a q)}^{-} )
D. ( 2 N O_{3(a q)}^{-} )
E ( .3 A g C l_{s} )
11
454Why can ( M n O_{2} ) be reduced by ‘ ( A l^{prime} ) and not by carbon?11
455Which one is the oxidising agent in the reaction given below? ( mathbf{2} boldsymbol{C r} boldsymbol{O}_{mathbf{4}}^{2-}+mathbf{2} boldsymbol{H}^{+} rightarrow boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+boldsymbol{H}_{2} boldsymbol{O} )
A . ( H^{+} )
в. ( C r_{2} O_{7}^{-2} )
( c cdot C r^{2} )
D. None
11
456Write the following equation in ionic form.
( M n O_{2}+4 H C l rightarrow M n C l_{2}+2 H_{2} O+ )
( C l_{2} )
11
457Write the stoichiometric coefficient for
the following reaction:
( boldsymbol{x} boldsymbol{I}_{2}+boldsymbol{y} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{z} boldsymbol{I}^{-}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} )
B. ( x-(3), y-(2), z-(3) )
( c cdot x-(3), y-(6), z-(5) )
( D cdot x-(3), y-(3), z-(3) )
11
458Select the incorrect statement for
developing of an exposed camera film involving the reaction.
A. Hydroquinol acts as reductant.
B. ( A g^{+} ) acts as oxidant.
C. Hydroquinol and AgBr undergoes redox change
D. It involves intramolecular change.
11
459Four ( C l_{2} ) molecules undergo a loss and
gain of 6 mole of electrons to form two
oxidation states of ( C l ) in auto redox
change. What are the ( +v e ) and ( -v e )
oxidation states of ( C l ) in the change:
A ( cdot C l^{5+}, C l^{circ} )
в. ( C l^{7+}, C l^{-} )
( mathbf{c} cdot C l^{3+}, C l^{circ} )
D. ( C l^{3+}, C l^{-} )
11
460The following reaction is balanced if ( boldsymbol{X}+boldsymbol{Y} ) is
( mathbf{5} boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{X} boldsymbol{C l} boldsymbol{O}_{2}+mathbf{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow )
( boldsymbol{X} boldsymbol{C l}^{-}+boldsymbol{Y} boldsymbol{O}_{2}+boldsymbol{6} boldsymbol{H}_{2} boldsymbol{O} )
11
461Identify the redox reaction taking place
in a beaker.
( left.mathbf{A} cdot Z n_{(} sright)+C u_{(a q)}^{2+} rightarrow Z n_{(a q)}^{2++}+C u(s) )
B. ( left.C u(s)+2 A g_{(a q)}^{+} rightarrow C u_{(a q)}^{2+}+2 A g_{(} sright) )
C ( left.cdot C u_{(} sright)+Z n_{(a q)}^{2+} rightarrow Z n(s)+C u_{(a q)}^{2+} )
( left.text { D. }left.2 A g_{(} sright)+C u_{(a q)}^{2+} rightarrow 2 A g_{(a q)}^{+}+C u_{(} sright) )
11
462Write balanced net ionic equation for the following reactions in acidic solution:
( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{N} boldsymbol{O}_{3}^{-}+boldsymbol{N} boldsymbol{O}(boldsymbol{g}) )
A ( cdot H N O_{2}(a q) rightarrow H N O_{3}^{-}+2 N O(g)+H_{2} O )
B ( cdot 2 H N O_{2}(a q) rightarrow 2 H N O_{3}^{-}+2 N O(g)+2 H_{2} O )
( mathrm{c} cdot 3 mathrm{HNO}_{2}(a q) rightarrow mathrm{NO}_{3}^{-}+2 mathrm{NO}(g)+mathrm{H}_{2} mathrm{O}+mathrm{H}^{+} )
D. None of the above
11
463Given are two figures of Daniell cell(X) and (Y). Study the figures and mark the incorrect statement from the following.
A . In fig( ( (x) ) ) electrons flow from ( Z n ) rod to ( C u ) rod hence current flows from ( C u ) to ( Z nleft(E_{text {ext}}1.1 mathrm{V}right) )
( c . ln operatorname{fig}(x), Z n ) dissolves at anode and ( C u ) deposits at cathode
D. In fig ( ( gamma ) ), ( Z n ) is deposited at ( C u ) and ( C u ) is deposited at ( z_{n} )
11
464Which of the following changes
represents a disproportional
reaction(s)?
( mathbf{A} cdot C l_{2}+2 O H^{-} rightarrow C l O^{-}+C l^{-}+H_{2} O )
B. ( C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O )
( mathbf{C} cdot 2 H C u C l_{2} frac{text {dilution with}}{text {water}} C u+C u^{2+}+4 C l^{-}+2 H^{+} )
D. All of the above
11
465Which of the following is a redox
reaction:
A ( cdot 2 operatorname{Na}left[A g(C N)_{2}right]+Z n rightarrow N a_{2}left[operatorname{Zn}(C N)_{4}right]+2 A g )
в. ( B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} )
c. ( N_{2} O_{5}+H_{2} O rightarrow 2 H N O_{3} )
D. ( A g N O_{3}+K I longrightarrow A g I+K N O_{3} )
11
466Assertion
The only way to get ( F_{2} ) from ( F^{-} ) is to oxidise electrolytically
Reason
The recovery of halogens from their halides requires an oxidation process.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
467( boldsymbol{F} e^{2+} rightarrow boldsymbol{F} e^{3+}+boldsymbol{e}^{-} ; boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{5} boldsymbol{e}^{-} rightarrow )
( M n^{2+}, ) the ratio of stoichiometric
coefficient of ( F e^{2+} ) and ( M n O_{4}^{-} ) in the balanced redox reaction is:
A .1: 5
B. 5: 1
c. 2: 3
( D cdot 6: 1 )
11
468Calculate the oxidation number:
(i) ( M o ) in ( left(N H_{4}right)_{2} M o O_{4} )
(ii) ( N i ) in ( N i(C N)_{4}^{2-} )
11
469In the given reaction,
( mathbf{2} boldsymbol{K}_{mathbf{4}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{6}right](boldsymbol{a} boldsymbol{q})+boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) longrightarrow )
( mathbf{2} boldsymbol{K}_{mathbf{3}}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right](boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{K} boldsymbol{O} boldsymbol{H}(boldsymbol{a} boldsymbol{q}) )
Which of the following processes takes place?
A. Oxidation due to removal of potassiummm
B. Oxidation due to removal of iron
c. Reduction due to removal of potassium
D. Oxidation due to removal of electronegative element
11
470Assertion
Oxidation number of chromium in
( boldsymbol{C r} boldsymbol{O}_{5} ) is ( +boldsymbol{6} )
Reason
Oxidation number of each oxygen atom
in ( C r O_{5} ) is -2
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
4713. Which of the following is most powerful oxidizing agent in the following
(a) o
(b) KMnO (C) H,02
(d) K,Cr,
11
472Given reaction ( boldsymbol{H} boldsymbol{C} boldsymbol{H} boldsymbol{O} rightarrow boldsymbol{C} boldsymbol{H}_{3} boldsymbol{O} boldsymbol{H}+ )
( H C O O^{-} ) is an example of
A. intermolecular redox change
B. intramolecular redox change
c. disproportionation or auto redox
D. none of these
11
473Assertion
Following reaction is a
disproportionation reaction:
( boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{2} boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{B} boldsymbol{r} boldsymbol{O}^{-}+boldsymbol{B} boldsymbol{r}^{-}+ )
( 2 H_{2} O )
Reason
( B r_{2} ) is oxidized to ( B r O^{-} ) as well as
reduced to ( B r^{-} )
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
474toppr
Q туре your question
reactions that are physically separated. So that the electrons must travel
through a wire from the reducing agent to the oxidizing agent.

The reducing agent loses electrons and is oxidized in a reaction that takes
place at an electrode is called the anode. The oxidizing agent gains electrons and is reduced in a reaction
that takes at an electrode is called the
cathode.

To maintain a net zero charge in each compartment, there is a limited flow of ions through a salt bridge. For example, in a car battery the reducing agent is oxidized by the following reaction, which involves a lead
( (P b) ) anode and sulfuric acid ( left(H_{2} S O_{4}right) )
Lead sulfate ( left(P b S O_{4}right), ) protons ( (H) )
and electrons ( left(e^{-}right) ) are produced
At the cathode, the below reaction
occurs :
( boldsymbol{P b O}_{2}+boldsymbol{H}_{2} boldsymbol{S O}_{4}+mathbf{2 H}^{+}+boldsymbol{2} boldsymbol{e}^{-} rightarrow )
PbSO ( _{-} 4+2 H_{-} 20 $ $ )
At the anode, the below reaction occurs
( boldsymbol{P b}+boldsymbol{H}_{2} boldsymbol{S O}_{4} rightarrow boldsymbol{P b S O}_{4}+boldsymbol{2} boldsymbol{H}^{+}+boldsymbol{2} boldsymbol{e}^{-} )
Electrons are produced by a chemical reaction that takes place at the:
A. anode
B. cathode
c. lead oxide electrode
D. oxidizer
E. salt bridge,

11
475Loss of an electron is called :
A. reduction
B. oxidation
c. ( A ) or ( B )
D. none of the above
11
476Which of the following is/are correct
about blue per chromate?
This question has multiple correct options
A. It has two peroxide bonds.
B. It has four oxygen atoms having oxidation number -1.
C ( . ) It reacts with ( H_{2} S O_{4} ) to give oxygen
D. It acts as oxidant as well as reductant.
11
477( boldsymbol{H}_{2}+boldsymbol{C l}_{2} rightarrow boldsymbol{H} boldsymbol{C l} ) The above reaction is
an example of which of the following reaction?
A. Combination reaction
B. Decomposition reaction
c. Displacement reaction
D. Double displacement reaction
11
478Q4. Fluorine reacts with ice and results in the change:
HO(s) + F.(g) HF(g) + HOF(8)
Justify that this reaction is a redox reaction.
TATO N
1
bolo baye
11
479Reaction occurring in lead storage battery is a kind of:
A. disproportionation
B. comproportionation
c. oxidation
D. reduction
11
480( boldsymbol{S} boldsymbol{O}_{2} ) reduces ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-} ) to ( boldsymbol{C r}^{2+} ). The
change in oxidation number of ( boldsymbol{C r} ) is:
11
481HOCl( (a q) ) is the molecule that kills bacteria wen chlorine is added to water
The following reaction produces this
molecule
( boldsymbol{C l}_{2}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}(l) rightleftharpoons boldsymbol{H} boldsymbol{O} boldsymbol{C l}(boldsymbol{a} boldsymbol{q})+ )
( boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q})+boldsymbol{C l}^{-}(boldsymbol{a} boldsymbol{q}) )
Which statement about this reaction is
correct?
A. Chlorine is both oxidised and reduced
B. Chlorine is oxidised but not reduced
c. Hydrogen is both oxidised and reduced
D. Hydrogen is oxidised but not reduced
11
482Identify disproportionation reaction
A. ( C H_{3}+2 O_{2} rightarrow C O_{2}+2 H_{2} O )
в. ( C H_{4}+4 C l_{2} rightarrow C C l_{4}+4 H C l )
c. ( 2 F_{2}+2 O H^{-} rightarrow 2 F^{-}+O F_{2}+H_{2} O )
D. ( 2 N O_{2}+2 O H^{-} rightarrow N O_{2}^{-}+N O_{3}^{-}+H_{2} O )
11
483Out of the following redox reactions ( boldsymbol{I} cdot boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} stackrel{Delta}{rightarrow} boldsymbol{N}_{2} boldsymbol{O}+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O} )
III.N ( boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{2} stackrel{Delta}{rightarrow} boldsymbol{N}_{2}+mathbf{2} boldsymbol{H}_{2} boldsymbol{O} )
IIII.PCl( _{5} stackrel{Delta}{rightarrow} P C l_{3}+C l_{2} )
disproportionation is not shown in:
A . I and II
B. II and III
c. I and III
D. I, II and III
11
484Statement I: The ( A l^{3+} ) ion needs to be
reduced to form aluminum metal.
Statement II: Reduction is a gain of
electrons.
A. Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement
B. Both Statement I and Statement II are correct, but Statement II is not the correct explanation of Statement I.
c. Statement I is correct, but Statement II is incorrect
D. Statement I is incorrect, but Statement II is correct
11
485( boldsymbol{A l}+boldsymbol{N} boldsymbol{O}_{mathbf{2}}^{-} rightarrow boldsymbol{A l}(boldsymbol{O} boldsymbol{H})_{4}^{-}+boldsymbol{N} boldsymbol{H}_{3} )
The oxidizing agent for this reaction
is
A . ( A l )
в. ( N )
( c cdot O )
D. both ( A ) and ( B )
11
486Which of the following species are oxidised and reduced in the following (unbalanced) reaction?
( boldsymbol{C N}^{-}+boldsymbol{O C l}^{-} longrightarrow boldsymbol{N}_{2}+boldsymbol{H} boldsymbol{C O}_{3}^{-}+ )
( C l^{-} )
A. oxidized- ( C, N ) in ( C N^{-} ) “, reduced ( -O C l^{-} )
B. Oxidized- ( N, C N^{-}, H C O_{3}^{-} ; N_{2} ) reduced ( -C O C l^{-} )
C. oxidized- ( C, N, H C O_{3}^{-} ; N_{2} ) reduced ( -O C l^{-}, C N^{-} )
D. None of these
11
487Photographic paper is developed with
alkaline hydroquinone.
Select the correct answer.
A. Hydroquinone is the oxidant
B. ( A g^{+} ) is the oxidant
C ( . B r^{-} ) is the oxidant
D. ( A g^{+} ) is the reductant
11
488Give equations for the decomposition of a metallic
¡] chloride
ii] nitrate with conc. ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} )
11
489Q10. (a) Calculate the oxidation number of
(i) C in CH,COOH (ii) S in 5,062
(b) Give one example of disproportionation reaction.
11
490Consider the following reaction, taking
place in a container fitted with a movable piston.
( 2 S O_{2}(g)+O_{2}(g) rightarrow 2 S O_{3}(g) )
Suppose we place two moles each of
( boldsymbol{S O}_{2} ) and ( boldsymbol{O}_{2} ) in the reaction vessel at
( 25^{circ} mathrm{C}, ) and adjust the volume to give a
total pressure of 1.0 atm. The reaction
is ignited by a spark, and goes to completion. The temperature is
returned to ( 25^{circ} mathrm{C} )
Which of the following best describes this system after reaction is complete?
( A cdot S O_{2} ) is limiting. The volume of the system remains the same
B. Neither reactant is limiting. The volume of the system decreases
C. ( S O_{2} ) is limiting. The volume of the system decreases.
D. ( O_{2} ) is limiting. The volume of the system remains the same
11
491The oxidation number of Na in NaCl:
A. 0
B. – –
( c cdot+1 )
D. 2
( E cdot+2 )
11
492Which of the following is not a disproportionation reaction?
( N H_{4} N O_{3} stackrel{Delta}{longrightarrow} N_{2} O+H_{2} O )
II. ( boldsymbol{P}_{4} stackrel{Delta}{longrightarrow} boldsymbol{P} boldsymbol{H}_{3}+boldsymbol{H} boldsymbol{P} boldsymbol{O}_{2}^{ominus} )
III. ( boldsymbol{P C l}_{5} stackrel{boldsymbol{Delta}}{longrightarrow} boldsymbol{P C l}_{3}+boldsymbol{C l}_{2} )
IV. ( boldsymbol{I} boldsymbol{O}_{3}^{ominus}+boldsymbol{I}^{ominus} longrightarrow boldsymbol{I}_{2} )
A . ।, ॥
B. I, III, IV
c. ॥, IV
D. ।, II
11
493The ( p H ) of a ( 10 m l ) aqueous solution of ( H C l ) is ( 4 . ) The amount of water to be
added to this solution in order to
change its ( p H ) from 4 to 5 is?
A. ( 30 m )
в. ( 60 mathrm{ml} )
( c .90 m l )
D. ( 120 m l )
11
494( 2 C u I rightarrow C u+C u I_{2}, ) the reaction is :
A. redox
B. neutralisation
c. displacement
D. none of the above
11
495Find the oxidation number of elements
in each case:
( C r ) in
( boldsymbol{C r} boldsymbol{O}_{2} boldsymbol{C l}_{2}, boldsymbol{N} boldsymbol{a}_{2} boldsymbol{C r}_{3} boldsymbol{O}_{10}, boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3} ) and
( left[boldsymbol{C r} boldsymbol{O}_{8}right]^{3-} )
A. +6,+6,+3,+5
В. +5,+6,+3,+4
( mathbf{c} cdot+4,+6,+2,+5 )
D. None of the above
11
496The decomposition of ( K C I O_{3} ) to ( K C l )
and ( O_{2} ) on heating is an example of :
A. intermolecular redox change
B. intramolecular redox change
c. disproportionation or auto redox change
D. none of the above
11
497Reduction reaction is:
A. addition of electron
B. decrease in oxidation state of element
C . addition of hydrogen
D. all of these
11
498An oxidation number can be:
A . positive
B. negative
c. zero
D. all of these
11
499Which of the following have been arrange in order of decreasing oxidation number of sulphur? This question has multiple correct options
A ( cdot N a_{2} S_{4} O_{6}>H_{2} S_{2} O_{7}>N a_{2} S_{2} O_{3}>S_{8} )
в. ( S O_{2}^{+}>S O_{4}^{2-}>S O_{3}^{2-}>H S O_{4} )
c. ( H_{2} S O_{5}>H_{2} S O_{3}>S C l_{2}>H_{2} S )
D. ( H_{2} S O_{4}>S O_{2}>H_{2} S>H_{2} S_{2} O_{8} )
11
500Bromine reacts with the hot aqueous
alkali to give bromide and bromate. What is the change that is brought
about in the oxidation state of bromine
to bromate?
A ( .-1 ) to +5
B. 0 to +5
( c cdot 0 ) to +7
D. None of these
11
501( boldsymbol{C H}_{4}+boldsymbol{O}_{2} rightarrow boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is:
A. combustion reaction
B. redox Reaction
c. both ( A ) and ( B )
D. none of the above
11
502Fill in the blanks.
Sulphur ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) to
produce nitrogen dioxide.
11
503Which of the following is/are reduction reaction ?
A. Hydrogenation of alkene and alkyne
B. Ozonolysis with ( O_{3} / Z n )
c. Halogenation of alkene
D. All of these
11
504The oxidation state(s) of ( C l ) in ( C a O_{2} C l_{2} )
(bleaching powder) is/are:
( A cdot+1 ) only
B. – – ‘ only
( c cdot+1 ) and -1
D. none of these
11
505Formulate a call for each of the
following reactions; ( S n^{2+}(a q)+2 A g C l(s) longrightarrow S n^{4+}(a q)+ )
( 2 A g(s)+2 C l^{-}(a q) )
( M g(s)+B r_{2}(l) longrightarrow M g^{2+}(a q)+ )
( 2 B r^{-}(a q) )
11
506The balanced equation in acidic
medium is :
( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}+boldsymbol{S} boldsymbol{b}_{2} boldsymbol{O}_{5} stackrel{boldsymbol{H}^{+}}{rightarrow} boldsymbol{S b} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{3} )
A ( cdot 3 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+6 H^{+} 3 H_{2} O rightarrow 4 S b O+6 H_{2} S O_{3} )
B . ( 2 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+6 H^{+} 3 H_{2} O rightarrow 4 S b O+4 H_{2} S O_{3} )
( mathrm{c} cdot 3 S_{2} O_{3}^{2-}+2 S b_{2} O_{5}+4 H^{+} 2 H_{2} O rightarrow 4 S b O+2 H_{2} S O_{3} )
D. none of these
11
507What is the oxidation number of ( M n ) in
( M n O_{2} ? )
( A cdot+2 )
B. +4
( c cdot-2 )
D. –
11
508dic medium are required
12. Equal moles of K Cr,0, in acidic medium
for oxidation of by 1 mole of
(a) FeSO3
(b) FeS204
(c) Fe (SO2)3
(d) Al2(SO3)2
11
509In the reaction,
( boldsymbol{X}+boldsymbol{I}_{2}+mathbf{2} boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{S} boldsymbol{n} boldsymbol{C l}_{4}+mathbf{2 H I} )
The correct option regarding ( X ) is/are:
A. It is an strong reducing agent
B. It is an angular molecule
C. It is used as a reagent in test of ( H g^{2+} ) radical
D. All of the above
11
510Consider the following reaction.
[
left.right|_{mathbf{C H O}} ^{mathbf{C H O}}+left.mathbf{O H}^{-} longrightarrowright|_{mathbf{C H}_{2} mathbf{O H}} ^{mathbf{O O}^{-}}
]
A. It is not a disproportionation reaction
B. It is intramolecular redox reaction
C. ( O H^{-} ) is reducing as well as oxidising agent
D. ( (C H O)_{2} ) is a reducing as well as oxidising agent
11
511How many gram of ( K M n O_{4} ) is
contained in 4 litre of ( 0.05 N ) solution.
The ( K M n O_{4} ) is to used as an oxidant in
acid medium ( left(M_{W}=158right): )
A. ( 1.58 g )
B. ( 15.8 g )
c. ( 6.32 g )
D. ( 31.6 g )
11
512Of the following acids, the one that is strongest is :
A. ( H B r O_{4} )
в. НОС l
c. ( H N O_{2} )
D. ( H_{3} P O_{3} )
11
513Which statement is correct about the
following reaction?
( mathrm{ZnO}+mathrm{CO} rightarrow mathrm{Zn}+mathrm{CO}_{2} )
A. zno is being oxidized
B. co is being reduced
( mathrm{C} cdot mathrm{CO}_{2} ) is being oxidized
D. zno is being reduced
11
514The reduced product formed when
chlorine reacts with ( boldsymbol{H}_{2} boldsymbol{S} ) :
A . ( N a C l )
в. ( C u )
c. ( operatorname{Fe}left(O H_{3}right) )
D. ( H C l )
11
515( H_{2} S_{2} O_{8} ) and ( H_{2} S O_{5} ) both have +6
oxidation state of sulphur. It is due to
the:
A. presence of peroxy group
B. presence of superoxo group
c. presence of neutral group
D. presence of ozone
11
516( boldsymbol{C l O}_{3}^{-}+boldsymbol{C l}^{-} rightarrow boldsymbol{C l}_{2}+boldsymbol{C l O}_{2} )
Which of the following is correct for this reaction:
A. Its a disproportion reaction
B. ( C l ) is both oxidised and reduced
c. ( C l ) is both reducing and oxydising agent
D. All of these
11
517Which of the statements about the
reaction below are incorrect?
( 2 P b O(s)+C(s) rightarrow 2 P b(s)+C O_{2}(g) )
(a) Lead is getting reduced.
(b) Carbon dioxide is getting oxidised.
(c) Carbon is getting oxidised.
(d) Lead oxide is getting reduced.
A ( cdot(a) ) and ( (b) )
B. (a) and (c)
( c cdot(a),(b) ) and ( (c) )
D. All
11
518In the following (unbalanced) reaction:
( boldsymbol{I}^{-}+boldsymbol{O}_{3} longrightarrow boldsymbol{O}_{2}+boldsymbol{I}_{2} )
What is oxidising agent?
( A cdot O_{3} )
B . ( I^{-} )
c. None
D. Both
11
519Give a clear idea about how
( M n O_{4}^{-}, C r O_{4}^{2-}, C r_{2} O_{7}^{2-} ) changes its
oxidation state when it is in the acidic,
basic and neutral medium.
11
520Oxidation number of the nitrogen atom
in ( H N O_{3} ) is :
A . –
B. +1
( c cdot 0 )
( D cdot+4 )
( mathrm{E} cdot+5 )
11
521The balanced equation in basic
medium is :
( boldsymbol{C l O}_{2}+boldsymbol{S b O}_{2}^{-} rightarrow boldsymbol{C l O}_{2}^{-}+boldsymbol{S b}(boldsymbol{O H})_{6}^{-} )
A ( cdot 2 C l O_{2}+S b O_{2}^{-}+2 O H^{-}+2 H_{2} O rightarrow 2 C l O_{2}^{-}+ )
( S b(O H)_{6} )
B . ( 2 C l O_{2}+5 S b O_{2}^{-}+2 O H^{-}+3 H_{2} O rightarrow 2 C l O_{2}^{-}+ )
( 2 S b(O H)_{6} )
( mathrm{c} cdot 2 mathrm{ClO}_{2}+mathrm{SbO}_{2}^{-}+3 mathrm{OH}^{-}+4 mathrm{H}_{2} mathrm{O} rightarrow 2 mathrm{ClO}_{2}^{-}+ )
( 3 S b(O H)_{6} )
D. None of these
11
522Addition of silver nitrate to sodium
chloride solution causes preciptation of silve chloride. This is an example reaction
11
523An oxidation process involves:
A. increase in oxidation number
B. Decrease in oxidation number
c. Addition of electrons
D. Removal of electronegative element
11
524Balance the following equation in basic medium by ion-electron method and oxidation number methods and identify
the oxidising agent and the reducing
agent
( boldsymbol{C l}_{2} boldsymbol{O}_{7}(boldsymbol{g})+boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{C l O}_{2}^{-}(boldsymbol{a q})+ )
( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{H}^{+} )
11
525The metals undergoing disproportionation are
A. sn
B. Na
( c cdot c u )
D. ( c a )
11
526In the reaction of ( Z n+F e S O_{4} rightarrow )
( Z n S O_{4}+F e )
A. zn gets oxidized
B. Fe gets oxidized
c. zn is oxidizing agent
D. zn and Fe both get oxidized
11
527Match the Column-I with Column-II.11
528Which of the following is incorrect
about ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ? )
A ( . ) It can be prepared from ( K_{2} C r O_{4} )
B. It is used in redox titrations
c. It is stable in both acid & base
D. It is orange in colour
11
529The complete balanced equation is:
( boldsymbol{C l}_{2}+boldsymbol{I O}_{3}^{-}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
A ( cdot C l_{2}+I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O )
в. ( 4 C l_{2}+I O_{3}^{-}+4 O H^{-} rightarrow I O_{4}^{-}+C l^{-}+H_{2} O )
c. ( C l_{2}+I O_{3}^{-}+3 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O )
D. none of these
11
530Q.14 The exhibition of various oxidation states by an element is also related
to the outer orbital electronic configuration of its atom. Atom (s)
having which of the following outermost electronic configurations will
exhibit more than one oxidation state in its compounds.
(2) 35′
(b) 3d 452 (c) 3d24s? (d) 3s 3p
11
531Balance the following equation by
oxidation number method.
( boldsymbol{F} boldsymbol{e}_{2}left(boldsymbol{S} boldsymbol{O}_{4}right)_{3}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{3}+boldsymbol{H}_{2} boldsymbol{O} rightarrow )
( boldsymbol{F} boldsymbol{e} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} )
11
532( y=8 )
( y=4 )
( y )
11
533What is the atomic number of the
following elements
Potassium iodide, lodine is
11
534Find the oxidation number of nitrogen in each case:
( N ) in ( N H_{3}, N H_{2} O H, N a N_{3} ) and
( N H_{4} N O_{2} )
( mathbf{A} cdot_{-3,-1,-frac{1}{3},+3 &-3} )
B. ( _{-3,-2,-frac{1}{3},+1} )
D. None of the above
11
535Identify ( X ) in the equation given below.
( boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{3}+boldsymbol{S O}_{2}+boldsymbol{H}_{2} boldsymbol{O} rightarrow boldsymbol{F} boldsymbol{e} boldsymbol{C l}_{2}+ )
( boldsymbol{H} boldsymbol{C l}+boldsymbol{X} )
A ( . H_{2} S )
в. ( S O_{3} )
c. ( H_{2} S O_{4} )
D. ( H_{2} S O_{3} )
11
536In balancing the reaction ( boldsymbol{x} boldsymbol{Z} boldsymbol{n}+ ) ( N O_{3}^{-}+y H^{+} rightarrow x Z n^{2+}+N H_{4}^{+}+ )
( z H_{2} O, x, y ) and ( z ) are respectively:
A .4,10,3
в. 3,8,3
( mathrm{c} cdot 3,10,3 )
D. 4,3,10
11
537Which of the following does not define reduction?
A. Gain of electron and addition of hydrogen
B. Removal of oxygen
c. Decrease in oxidation state
D. Removal of electron, removal of hydrogen, addition of oxygen and increase in oxidation state
11
538Zinc granules are added in excess to ( mathbf{5 0 0} boldsymbol{m L} ) of ( mathbf{1 . 0} boldsymbol{M} ) nickel nitrate solution
at ( 25^{circ} C ) until the equilibrium is reached. If the standard reduction
potentials of ( Z n^{2+} / Z n ) and ( N i^{2+} / N i )
are -0.75 and -0.24 volt respectively
find out the concentration of ( N i^{2+} ) ions
in solution at equilibrium.
11
539( B r_{2}+H_{2} O_{2} rightarrow ) (in acidic medium)
Complete the reaction.
11
540In a reaction, 4 mol of electrons are
transferred to one mol of ( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} ) when it acts as an oxidant. The possible reduction product is :
A. 0.5 mol ( N_{2} )
B. 0.5 mol ( N_{2} ),
c. 1 mol ( N O_{2} )
D. 1 mol ( N H_{3} )
11
541( K M n O_{4} ) is acidified for redox
titrations by:
A. ( H C l )
в. ( H N O_{3} )
c. ( H_{2} S O_{4} )
D. any of these
11
542( 2 K_{2} C r_{2} O_{7}+8 H_{2} S O_{4} rightarrow 2 K_{2} S O_{4}+ )
( 2 C r_{2}left(S O_{4}right)_{3}+8 H_{2} O+3 O_{2} )
Is the above reaction correct?
A. True
B. False
11
543Q21. In the reaction
M,O, + 4HCI
which species is oxidised.
M.CI+ CI+
11
544A mixed solution of potassium hydroxide and sodium carbonate required ( 15 mathrm{mL} ) of ( frac{N}{20} H C l ) solution when titrated with phenolphthalein as an indicator. But the same amount of
the solution when titrated with methyl orange as an indicator required ( 25 mathrm{ml} ) of
the same acid. The amount of ( K O H )
present in the solution is :
A. ( 0.014 mathrm{g} )
B. ( 0.14 mathrm{g} )
c. ( 0.028 mathrm{g} )
D. ( 1.4 mathrm{g} )
11
545( mathbf{3} N_{2} H_{4}+2 B r O_{3}-3 N_{2}+ )
( 2 B r^{-}+6 H_{2} O )
The above reaction shows:
A. intermolecular redox
B. auto-redox
C. intramolecular redox
D. either of these
11
546Identify the substance oxidised, reduced, oxidising agent and reducing
agent for each of the following reactions
( boldsymbol{P b}_{(s)}+boldsymbol{P b O}_{2(s)}+mathbf{2 H}_{2} boldsymbol{S O}_{4(a q)} rightarrow )
( 2 P b S O_{4(s)}+2 H_{2} O_{(l)} )
11
547When ( K M n O_{4} ) acts as an oxidising
agent and forms ( M n^{+2}, ) the number of
electrons transferred per molecule of
( K M n O_{4} ) is :
11
548The oxidation number of Cr is +6
in

This question has multiple correct options
A ( cdot operatorname{Fe} C r_{2} O_{4} )
в. ( K C r O_{3} C l )
c. ( C r O_{5} )
D. ( left[C r(O H)_{4}right]^{-} )

11
549Assign oxidation number to the
underlined element in ( boldsymbol{H}_{4} underline{boldsymbol{P}}_{2} boldsymbol{O}_{7} )
11
550The complete balanced equation is:
( boldsymbol{C u}+boldsymbol{N} boldsymbol{O}_{3}^{-}+ldots . rightarrow boldsymbol{C u}^{2+}+boldsymbol{N} boldsymbol{O}_{2}+ )
A ( cdot C u+4 H^{+}+2 N O_{3}^{-} rightarrow C u^{2+}+2 N O_{2}+2 H_{2} O )
B . ( C u+6 H^{+}+N O_{3}^{-} rightarrow C u^{2+}+2 N O_{2}+2 H_{2} O )
c. ( C u+4 H^{+}+2 N O_{3}^{-} rightarrow 2 C u^{2+}+N O_{2}+2 H_{2} O )
D. none of these
11
551Which of the following not represents redox reactions?
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{2} stackrel{theta}{boldsymbol{O}} boldsymbol{H} longrightarrow boldsymbol{2} boldsymbol{C r} boldsymbol{O}_{4}^{2-}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
II. ( Z n+C u S O_{4} longrightarrow Z n S O_{4}+C u )
III. ( 2 M n O_{4}^{ominus}+3 M n^{2+}+4 stackrel{theta}{O} H longrightarrow )
( mathbf{5} M n O_{2}+2 H_{2} O )
IV. ( 2 C u^{oplus} longrightarrow C u+C u^{2+} )
( A )
в. ।, ॥
c. ॥ा, ।॥
D. ॥, ॥I, IV
11
552Which of the following is not a redox reaction?
A ( cdot 2 N O+O_{2} rightarrow 2 N O_{2} )
в. ( C l_{2}+H_{2} O rightarrow H C l+H C l O )
( mathrm{c} cdot 2 mathrm{Cr} mathrm{O}_{4}^{2-}+2 mathrm{H}^{+} rightarrow mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+mathrm{H}_{2} mathrm{O} )
D. ( M n O_{4}^{-}+8 H^{+} rightarrow M n^{2+}+4 H_{2} O )
11
553The oxidation number of phosphorus in ( boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} boldsymbol{P} boldsymbol{O}_{2}right)_{2} ) is:
( A cdot+3 )
B. +2
( c cdot+1 )
D. –
11
554Which of the following is/are redox reactions?
This question has multiple correct options
A. ( B a O_{2}+H_{2} S O_{4} rightarrow B a S O_{4}+H_{2} O_{2} )
в. ( 2 B a O+O_{2} rightarrow 2 B a O_{2} )
( mathbf{c} cdot 2 K C I O_{3} rightarrow 2 K C l+3 O_{2} )
D. ( S O_{2}+2 H_{2} S rightarrow 2 H_{2} O+3 S )
11
555tion)
08. (a) Balance the following equation by oxidation number method or by.com
method,
MnO, Fe2+ → Mn2+ + Fe3+ acidic medium
(b) Consider the cell,
Zn | Zn2+ (aq) || Cu2+(aq)| Cu
The standard electrode potentials are E° Zn2+/Zn = -0.76 V; E° Cu-T/Cu = +0.34 write
down the cell reaction.
11
556Balance the following equation by ion electron method.
( M n O_{4}^{2-}+H_{2} O rightarrow M n O_{4}^{-}+O H^{-}+ )
( M n O_{2} )
11
557Which one of the following is not a redox reaction?
A. ( C a C O_{3} rightarrow C a O+C O_{2} )
В. ( 2 H_{2}+O_{2} longrightarrow 2 H_{2} O )
( ^{mathrm{c}} cdot_{N a+H_{2} O} rightarrow N a O H+frac{1}{2} H_{2} )
D. ( _{M n C l_{3}} rightarrow M n C l_{2}+frac{1}{2} C l_{2} )
11
558Oxidation number of ( N a ) in ( N a-H g )
amalgam is zero.
If true enter 1 , else enter 0 .
( A cdot 1 )
11
559Consider the following redox reaction:
( 2 S_{2} O_{3}^{2-}+I_{2} longrightarrow S_{4} O_{6}^{2-}+2 I^{ominus} )
This question has multiple correct options
A ( cdot S_{2} O_{3}^{2-} ) gets reduced to ( S_{4} O_{6}^{2} )
B. ( S_{2} O_{3}^{2-} ) gets oxidised to ( S_{4} O_{6}^{2} )
c. ( I_{2} ) gets reduced to ( I^{ominus} )
( mathbf{D} cdot I_{2} ) gets oxidised to ( I^{ominus} )
11
560Dissolution of ( C a H_{2} ) in water is an
auto-redox process.
If true enter 1 , else enter 0
( A )
11
561Consider the reactions:
( 2 S_{2} O_{3}^{2-}(a q)+I_{2}(s) longrightarrow S_{4} O_{6}^{2-}(a q)+ )
( 2 I^{-}(a q) )
( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(l) longrightarrow )
( mathbf{2} boldsymbol{S} boldsymbol{O}_{4}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{4} boldsymbol{B} boldsymbol{r}^{-}(boldsymbol{a} boldsymbol{q})+mathbf{1 0} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) )
Why does the same reductant
thiosulphate react differently with iodine and bromine?
11
562Dvide the following redox equations into oxidation half equation and reduction half equation.
( boldsymbol{a}) boldsymbol{P}_{(s)}+boldsymbol{P} boldsymbol{O}_{4(a q)}^{3} boldsymbol{H} boldsymbol{P} boldsymbol{O}_{3(a q)}^{2} )
( boldsymbol{b}) boldsymbol{H} boldsymbol{N} boldsymbol{O}_{2(a q)} longrightarrow boldsymbol{N} boldsymbol{O}_{3(a q)}^{-}+boldsymbol{N} boldsymbol{O}_{(g)} )
( boldsymbol{c}) boldsymbol{I} boldsymbol{O}_{boldsymbol{3}(boldsymbol{a q})}^{-}+boldsymbol{R e}_{(s)} longrightarrow boldsymbol{R e} boldsymbol{O}_{4(boldsymbol{a q})}+boldsymbol{I}_{(a q)} )
11
563The reaction of white phosphorus with
aqueous ( N a O H ) gives phosphine along with another phosphorus containing compound. The reaction type, the oxidation states of phosphorus in phosphine and the other product are, respectively:
A. redox reaction; -3 and -5
B. redox reaction; +3 and +5
c. disproportionation reaction; -3 and +1
D. disproportionation reaction; -3 and +3
11
564Which compound amongst the following has the highest oxidation
number for ( M n ? )
( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} ) and
( boldsymbol{M} boldsymbol{n}_{2} boldsymbol{O}_{3} )
11
565(a) Draw the labelled diagram of Daniell cell.
(b) Write the half-reactions of oxidation
and reduction taking place on electrodes.
11
566Assertion
The alkali metals are strong oxidizing
agents.
Reason
The one electron in their valence shell is
easily lost.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is incorrect but Reason is correct
D. Both Assertion and Reason are incorrect
11
567Write the following equation in ionic form:
a) ( M n O_{2}+4 H C l rightarrow M n C l_{2}+ )
( mathbf{2} boldsymbol{H}_{mathbf{2}} boldsymbol{O}+boldsymbol{C} boldsymbol{l}_{mathbf{2}} )
b) ( 2 N a H C O_{3}+H_{2} S O_{4} rightarrow )
( N a_{2} S O_{4}+H_{2} O+C O_{2} )
A ( cdot ) a) ( M n O_{2}+4 H^{+}+4 C l^{-} rightarrow M n^{2+}+2 C l^{-}+2 H_{2} O+ )
( C l_{2} )
b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ )
( S O_{4}^{2-}+2 H_{2} O+C O_{2} )
B. a) ( 2 M n O_{2}+8 H^{+}+4 C l^{-} rightarrow 2 M n^{2+}+2 C l^{-}+ )
( 4 H_{2} O+C l_{2} )
b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ )
( S O_{4}^{2-}+2 H_{2} O+C O_{2} )
c. a) ( M n O_{2}+4 H^{+}+3 C l^{-} rightarrow M n^{2+}+C l^{-}+2 H_{2} O+ )
( C l_{2} )
b) ( 2 N a^{+}+2 H C O_{3}^{-}+2 H^{+}+S O_{4}^{2-} rightarrow 2 N a^{+}+ )
( S O_{4}^{2-}+2 H_{2} O+C O_{2} )
D. None of these
11
568Consider the following reaction:
( boldsymbol{H} boldsymbol{C H O}+mathbf{2}left[boldsymbol{A} boldsymbol{g}left(boldsymbol{N} boldsymbol{H}_{3}right)_{2}right]^{+}+boldsymbol{3} boldsymbol{O} boldsymbol{H}^{-} rightarrow )
( mathbf{2 A g}+boldsymbol{H C O O}^{-}+mathbf{4 N H}_{mathbf{3}}+mathbf{2 H}_{mathbf{2}} boldsymbol{O} )
Which of the following statements
regarding oxidation and reduction is
correct?
( mathbf{A} cdot H C H O ) is oxidised to ( H C O O^{-} ) and ( left[A gleft(N H_{3}right)_{2}right]^{+} ) is reduced to ( A g )
B. ( H C H O ) is reduced to ( H C O O^{-} ) and ( left[A gleft(N H_{3}right)_{2}right]^{+} ) is oxidised to ( A g )
( mathbf{C} cdotleft[A gleft(N H_{3}right)_{2}right]^{+} ) is reduced to ( A g ) while ( O H^{-} ) is oxidised to ( H C O O^{-} )
( mathbf{D} cdotleft[A gleft(N H_{3}right)_{2}right]^{+} ) is oxidised to ( N H_{3} ) while ( H C H O ) is reduced to ( H_{2} O )
11
5690.30 Assertion (A) In the reaction between potassium permanganate and
potassium iodide, permanganate ions act as oxidising agent.
Reason (R) Oxidation state of manganese changes from +2 to +7 during
the reaction.
(a) Both A and Rare true and R is the correct explanation of A
(b) Both A and Rare true but is not the correct explanation of A
(c) A is true but R is false
(d) Both A and R are false
11
570Which of the following is a redox reaction?
A . Reaction of ( H_{2} S O_{4} ) with ( N a O H )
B. In atmosphere, formation of ( O_{3} ) from ( O_{2} ) by lightening
c. Formation of oxides of nitrogen from nitrogen and oxygen by lightening
D. Evaporation of ( H_{2} O )
11
57117. In the balance chemical reaction,
10, +al+bH – CH2O + dl,
a, b, c and d respectively correspond to:
(a) 5,6,3, 3
(b) 5,3,6,3
(c) 3,5, 3,6
(d) 5, 6, 5,5
11
572is a degradation phenomenon in which the electrons in a plastic are so strongly attracted to
oxygen atoms.
A. Oxidation
B. Reduction
c. Hydrolysis
D. Polymerization
11
573Identify the true statement regarding
Daniel cell:
A. zinc ions flows across salt bridge
B. ( K^{+} ) ions move from salt bridge to ( C u / C u^{+2} ) half cell
C. Oxidation takes place at copper electrode
D. Flow of current takes place from copper electrode to zinc electrode
11
574A redox reaction is one in which:
A. both the substance are reduced.
B. both the substance are oxidised.
C. one substance is reduced and other is oxidised.
D. all of the above.
11
575Balance the following in basic medium:
( boldsymbol{F} boldsymbol{e}_{3} boldsymbol{O}_{4}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-} rightarrow boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} )
A ( cdot 6 F e_{3} O_{4}+2 M n O_{4}^{-}+H_{2} O rightarrow 9 F e_{2} O_{3}+2 M n O_{2} )
( 2 O H^{-} )
B. ( 6 F e_{3} O_{4}+4 M n O_{4}^{-}+H_{2} O rightarrow 9 F e_{2} O_{3}+5 M n O_{2}+ )
( O H^{-} )
( mathrm{c} cdot 6 mathrm{Fe}_{3} mathrm{O}_{4}+mathrm{MnO}_{4}^{-}+mathrm{H}_{2} mathrm{O} rightarrow 9 mathrm{Fe}_{2} mathrm{O}_{3}+3 mathrm{MnO}_{2}+ )
( 2 O H^{-} )
D. None of these
11
576Q8. What is meant by reducing agent? Name the best reducing agent.11
577The change in the oxidation number of
the underlined nitrogen atom in the following chemical reactions are :
a. Nitrous acid ( left(H underline{N} O_{2}right) ) reduces
( M n O_{4}^{ominus} ) in acid solution
b. Nitrous acid ( left(H underline{N} O_{2}right) ) oxidises ( I^{ominus} ) to
( I_{2} ) in acid solution.
( A cdot(a)+3 ) to +5
( (b)+3 t 0+2 )
B. (a) +3 to +6
( (b)+3 t 0+2 )
( c cdot(a)+3 t a+5 )
( (b)+3 t 0+1 )
D. ( (a)+3 ) to +2
( (b)+3 t 0+5 )
11
578In the given reaction, ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7}+ )
( boldsymbol{X} boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{Y} boldsymbol{S} boldsymbol{O}_{2} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+ )
( boldsymbol{C r}_{2}left(boldsymbol{S O}_{4}right)_{3}+boldsymbol{Z H}_{2} boldsymbol{O} . ) Find ( mathbf{X}, mathbf{Y} ) and ( mathbf{Z} )
11
579In a chemical reaction, oxidation is
always accompanied by reduction
If true enter 1 , else enter 0 .
( A )
11
580Which of the following is a disproportionation reaction?
A ( cdot C u_{2} O+2 H^{+} rightarrow C u+C u^{2+}+H_{2} O )
B ( cdot 2 C r O_{4}^{2-}+2 H^{+} rightarrow C r_{2} O_{7}^{2-}+H_{2} O )
( mathrm{c} cdot mathrm{CaCO}_{3}+2 mathrm{H}^{+} rightarrow mathrm{Ca}^{2+}+mathrm{H}_{2} mathrm{O}+mathrm{CO}_{2} )
D. ( C r_{2} O_{7}^{2-}+2 O H^{-} rightarrow 2 C r O_{4}^{2-}+H_{2} O )
11
581Which of the following behaves as both oxidising and reducing agents?
A. ( H_{2} S O_{4} )
в. ( S O_{4} )
c. ( H_{2} )
D. ( H N O_{3} )
11
582The value of ( n ) in the following reaction
is :
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{n} e^{-}+mathbf{1 4 H}^{+} rightarrow boldsymbol{2 C r}^{3+}+ )
( mathbf{7} boldsymbol{H}_{mathbf{2}} boldsymbol{O} )
11
58310. In which of the following reactions, equivalent mass
the underlined is equal to molar mass?
(a) Cl2 + 20H- CH- + CIO +H2O
(b) 2HCHO + OH-HCOO- + CH,OH
(C) 2MnO – MnO2 + MnO,
(d) 2KCIO3 -> 2KCI + 302
11
584The ion ( A^{n+} ) is oxidised to ( A O_{3}^{-} ) by
( M n O_{4}^{-} ) changing to ( M n^{2+} ) in acid
medium. Given that ( 2.68 times 10^{-3} ) mole of
( A^{n+} ) required ( 1.61 times 10^{-3} ) mole ( M n O^{-} )
What is the value of n?
11
585Q3. Consider a voltaic cell constructed with the following substances:
Cr+ (aq) + 3e Cr(s)
MnO4 (aq) + SH+ (aq) + 5e – Mr** (aq) + 4H,O(1)
E° = -0.74 V
E° = +1.51 V
(a) Which substances are oxidised and reduced in this cell?
(b) Which are the negative and positive electrode?
.
11
586Assertion
When an electric current is passed through an aqueous solution of sodium chloride, sodium ions move towards cathode and chloride ions move towards
anode.
Reason
Cathode is a negatively charged electrode and therefore attracts ( boldsymbol{N} boldsymbol{A}+ )
ions. Anode is a positively charged
electrode and therefore attracts ( C l- )
ions
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
587In the following reaction:
( boldsymbol{A}^{+}+boldsymbol{B} rightarrow boldsymbol{A}+boldsymbol{B}^{+} )
oxidizing agent is:
A ( . A^{+} )
в. ( B )
c. Both of them
D. None of them
11
588The redox reaction ( Z n(s)+ )
( boldsymbol{P b C l}_{2}(boldsymbol{a q}) longrightarrow boldsymbol{P b}(boldsymbol{s})+boldsymbol{Z n C l}_{2}(boldsymbol{a q}) )
can be represented as following half equations ( : Z n(s) longrightarrow Z n^{2+}(a q)+ )
( 2 e^{-}(text {oxidation }) ) and ( P b^{2+}(a q)+ )
( 2 e^{-} longrightarrow P b(s)(text { reduction }) )
If true enter 1 , else enter 0 .
( A )
11
589A molecule is reduced means it:
A. loses electron.
B. gains proton
c. loses proton and electrons
D. gains electron.
11
590In balancing the half reaction, ( S_{2} O_{3}^{2-} rightarrow S(s), ) the number of electrons
that must be added on the left is :
11
591Balance the following equation by ion electron method:
( boldsymbol{H} boldsymbol{g} boldsymbol{S}+boldsymbol{C l}^{-}+boldsymbol{H}^{+}+boldsymbol{N} boldsymbol{O}_{3}^{-} rightarrow )
( boldsymbol{H} boldsymbol{g} boldsymbol{C l}_{4}^{2-}+boldsymbol{S}+boldsymbol{N} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{O} )
11
592Complete the following ionic equation:
( mathbf{3} M n O_{4}^{2-}+4 H^{+} rightarrow )
11
593Which of the following arrangements represent increasing oxidation number of the central atom?
A ( cdot C r O_{2}^{-}, C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-} )
B . ( C l O_{3}^{-}, C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-} )
c. ( C r O_{2}^{-}, C l O_{3}^{-}, M n O_{4}^{-}, C r O_{4}^{2-} )
D. ( C r O_{4}^{2-}, M n O_{4}^{-}, C r O_{2}^{-}, C l O_{3}^{-} )
11
594The oxidation states exhibited by
hydrogen in its various molecular forms/compounds are :
A . – – ‘ only
B. zero only
( c cdot+1,-1 ) and 0
D. +1 only
11
595What coefficient of ( A g N O_{3} ) is required to
balance the following equation?
( C u+A g N O_{3} rightarrow C uleft(N O_{3}right)_{2}+A g )
( mathbf{A} cdot mathbf{0} )
B. 1
c. 2
D. 3
11
596When zinc reacts with very dilute
( H N O_{3}, ) the oxidation state of nitrogen
changes from:
A. +5 to +1
B. +5 to -3
( c cdot+5 t o+4 )
D. +5 to +3
11
597Metals exhibit ….. oxidation states in
their compounds.
A. Positive
B. Negative
c. Neutral
D. none of these
11
5981. Among the following molecules, in which does bromine show the maximum oxidation
number?
(a) Hg, (Bro,), (b) Br-a (c) KBrO
(d) Br₂
itinaxidotion number in their
11
599When potassium chloride and lead ( (I I) ) nitrate react in an aqueous solution, which of the following terms will be present in the balanced molecular
equation?
A ( cdot P b C l_{s} )
B ( cdot P b_{2} C l_{(s)} )
( mathbf{c} cdot K N O_{3(a q)} )
D. ( 2 K N O_{3(a q)} )
E ( cdot 2 K C l_{2(s)} )
11
600( ln K H, ) the oxidation number of
hydrogen is:
A ( .+2 )
B. +1
c. 0
D. –
E. -2
11
60111. A substance which gets oxidised, during a redox reaction,
is known as
(a) oxidizing agent
(b) reducing agent
c) either oxidising or reducing agent
(d) None of the above
11
602The number of moles of ( K_{2} C r_{2} O_{7} ) that
will be needed to react with one mole of
( H_{2} S ) in acidic medium is :
A ( cdot frac{1}{6} )
B. ( frac{1}{3} )
( c cdot frac{2}{5} )
D. ( frac{2}{3} )
11
603Which of the following equations is a
balanced one?
( mathbf{A} cdot 5 B i O_{3}^{-}+22 H^{+}+M n^{2+} rightarrow 5 B i^{3+}+7 H_{2} O+M n O_{4}^{-} )
B. ( 5 B i O_{3}^{-}+14 H^{+}+2 M n^{2+} rightarrow 5 B i^{3+}+7 H_{2} O+2 M n O_{4}^{-} )
( mathbf{c} cdot 2 B i O_{3}+4 H^{+}+M n^{2+} rightarrow 2 B i^{3+}+2 H_{2} O+M n O_{4}^{-} )
D. ( 6 B i O_{3}^{-}+12 H^{+}+3 M n^{2+} rightarrow 6 B i^{3+}+6 H_{2} O+3 M n O_{4}^{-} )
11
604A redox reaction simply involves the transfer of electrons from reductant to
oxidant
If true enter 1 , else enter 0 .
( A )
11
605A dilute ferrous sulphate solution was
gradually added to the beaker
containing acidified potassium
permanganate solution. The light purple colour of the solution fades and finally disappears. Which of the following is the correct explanation for the observation?
( mathbf{A} cdot K M n O_{4} ) is an oxidising agent, it oxidises ( F e S O_{4} )
B. ( F e S O_{4} ) acts as an oxidising agent and oxidises ( K M n O_{4} )
C. The colour disappears due to dilution; no reaction is involved
D. ( K M n O_{4} ) is an unstable compound and decomposes in presence of ( F e S O_{4} ) to a colourless compound
11
606Give the oxidation state of underlined.
( N a_{2} S_{4} O_{6} )
11
607Q4. (a) Give two important functions of salt bridge.
(b) Balance the following equation by oxidation number method:
Fe2+ + Cr, 02- + H–> Fe3+ + Cr3+ + H2O
11
608“Reaction of potassium iodide solution
with lead nitrate solution” is the
example of :
This question has multiple correct options
A. Chemical replacement reaction
B. Neutralisation reaction
c. Precipitation reaction
D. Chemical double decomposition reaction
11
609Oxidation number of ( S ) in ( left(C H_{3}right)_{2} S ) is
( mathbf{A} cdot mathbf{0} )
B. +1
( c .-2 )
D. +3
11
610The number of electrons required to balance the given equation is
( N O_{3}^{-}+4 H^{+}+e^{-} longrightarrow 2 H_{2} O+N O )
( mathbf{A} cdot mathbf{5} )
B. 2
( c cdot 3 )
D.
11
611Which of the following is/are disproportionation reaction(s)? This question has multiple correct options
A ( cdot 2 C C l_{3} C H O+N a O H rightarrow C C l_{3} C O O N a+ )
( C C l_{3} C H_{2} O H )
в. ( N H_{4} N O_{3} rightarrow N_{2} O+2 H_{2} O )
c. ( 2 K C l O_{3} rightarrow 2 K C l+3 O_{2} )
D. ( 5 C l_{2}+6 O H^{-} rightarrow C l O_{3}^{-}+5 C l^{-}+3 H_{2} O )
11
612The role of fluorspar (CaF,) which is added in small
quantities in the electrolytic reduction of alumina
dissolved in fused cryolite (Na AlF,) is:
(a) as a catalyst
(b) to make the fused mixture very conducting
(c) to increase the temperature of the melt
(d) to decrease the rate of oxidation of carbon at the anode
11
613Q. 49 Why in the redox titration of KMnO4 vs oxalic acid, we heat oxalic acid
solution before starting the titration?
ne As we know with inerne
11
614Oxalic acid dihydrate, ( boldsymbol{H}_{2} boldsymbol{C}_{2} boldsymbol{O}_{4} )
( 2 H_{2} O(s) ) is often used as a primary
reagent to standardise sodium
hydroxide solution. Which of these facts are reasons to choose this substance as
a primary standard?
I. It is diprotic.
II. It is a stable compound that can be weighed directly in air.
III. It is available in pure form.
A. III only
B. I and II only
c. ॥ and III only
D. I. II and III
11
615Oxidation of NO in air produces:
в. ( N_{2} O_{3} )
( c cdot N O_{2} )
D. ( N_{2} O_{5} )
11
616The oxidation state of ( A, B, ) and ( C ) in a
compound are +2,+5 and -2 respectively. The compound is :
( mathbf{A} cdot A_{2}(B C)_{2} )
B ( cdot A_{2}(B C)_{3} )
( mathbf{c} cdot A_{3}left(B C_{4}right)_{2} )
D. ( A_{2}left(B C_{4}right)_{3} )
11
617Assertion
Lower parts of the ship or bridge is
coated with tar.
Reason
It is to increase rusting.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is
not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Assertion is incorrect but Reason is correct
11
618The oxidation state of oxygen of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) in the final products when it reacts with ( C l O_{3}^{ominus} ) is :
( mathbf{A} cdot mathbf{0} )
B.
( c cdot-1 )
D. – –
11
619Select redox reaction from the following
A ( . Z n+C u S O_{4} rightarrow Z n S O_{4}+C u )
в. ( C a O+2 H C l rightarrow C a C l_{2}+H_{2} O )
c. ( N a O H+2 H C l rightarrow N a C l_{2}+H_{2} O )
D. ( C a C O_{3} rightarrow C a O+C O_{2} )
11
620The substance oxidized and the
oxidizing agent in the following reaction are respectively:
( Z n+H_{2} S O_{4} rightarrow Z n S O_{4}+H_{2} )
A. zinc atoms and hydrogen ions
B. zinc ions and hydrogen atoms
c. hydrogen ions and zinc atoms
D. hydrogen atoms and zinc ions
11
621The following intramolecular redox
reaction shows a loss and gain of how much electrons?
( left(N H_{4}right)_{2} C r_{2} O_{7} rightarrow N_{2}+C r_{2} O_{3}+ )
( 4 H_{2} O )
A. Six
B. Seven
c. Eight
D. None of these
11
622Find oxidation number of Magnese in
( boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} )
11
623Select the species having zero oxidation state at the underlined elements.
This question has multiple correct options
( mathbf{A} cdotleft(C H_{3}right)_{2} S O )
B. ( underline{C}_{12} mathrm{H}_{22} mathrm{O}_{11} )
c. ( H_{2} S O_{3} )
D. ( underline{N}_{2} H_{4} )
11
624When zinc is added to ( C u S O_{4} ) solution,
copper is precipitated because :
A ( cdot C u^{+2} ) is reduced
B. ( C u^{+2} ) is oxidised
c. ( C u S O_{4} ) is ionized
D. ( C u S O_{4} ) is hydrolysed
11
625In which of the following processes is nitrogen oxidized?
A ( cdot N H_{4}^{oplus} rightarrow N_{2} )
B ( . N O_{3}^{ominus} longrightarrow N O )
( mathrm{c} cdot mathrm{NO}_{2} longrightarrow mathrm{NO}_{2}^{circ} )
D. ( N O_{3}^{ominus} longrightarrow N H_{4}^{oplus} )
11
626Is the following reaction is a redox
reaction?
( boldsymbol{B} boldsymbol{a} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4} rightarrow boldsymbol{B} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O}_{2} )
11
627Q. 15 Identify the correct statements with reference to the given reaction
PA +30H + 3H,0 PH2 + 3H,POZ
(a) Phosphorus is undergoing reduction only
(b) Phosphorus is undergoing oxidation only
(c) Phosphorus is undergoing oxidation as well as reduction
(d) Hydrogen is undergoing neither oxidation nor reduction
11
628Consider the given reaction.
This question has multiple correct options
A. It is disproportionation reaction.
B. It is intramolecular redox reaction
C. ( O H^{-} ) is a reducing as well as oxidising agent
D. ( C H O-C H O ) is a reducing as well as oxidising agentt
11
629Balance the following equations by ion
electron method:
( boldsymbol{C l}_{2}+boldsymbol{I O}_{3}^{-}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
11
630The oxidation number of ( C ) in
( boldsymbol{C H}_{4}, boldsymbol{C H}_{3} boldsymbol{C l}, boldsymbol{C H}_{2} boldsymbol{C l}_{2}, boldsymbol{C H} boldsymbol{C l}_{3} ) and
( C C l_{4} ) are respectively :
в. +2,+4,0,-4,-2
c. -4,-2,0,+2,+4
D. -2,-4,0,+4,+2
11
631The sum of the oxidation number of the
carbon atoms in ( C H_{3} C H O ) is:
A . -2
B. +2
( c .-4 )
D. –
11
632Which of the following reactions takes place at anode?
A. Reduction
B. Oxidation
c. Decomposition
D. Dissolution
11
633The oxidation state of iron in the
coordination sphere of prussian blue is:
( A cdot+2 )
B. 0
( c cdot+1 )
D. +3
11
634For the galvanic cell, ( boldsymbol{C u}left|boldsymbol{C u}^{2+} | boldsymbol{A} boldsymbol{g}^{+}right| boldsymbol{A} boldsymbol{g} )
Which of the following observations is
not correct?
A. Cu acts as anode and Ag acts as cathode
B. Ag electrode loses mass and Cu electrode gains mass
C. Reaction at anode, ( C u rightarrow C u^{2+}+2 e^{-} )
D. copper is more reactive than silver
11
635Write balanced net ionic equation for
the following reactions in acidic
solution.
[
begin{array}{l}
boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{A l}(boldsymbol{s}) rightarrow boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{a} boldsymbol{q})+ \
boldsymbol{A l}^{3+}(boldsymbol{a} boldsymbol{q})
end{array}
]
( mathbf{A} cdot S_{4} O_{6}^{2-}(a q)+6 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ )
[
6 A l^{3+}(a q)+6 H_{2} O
]
( mathbf{B} cdot 2 S_{4} O_{6}^{2-}(a q)+6 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ )
[
2 A l^{3+}(a q)+6 H_{2} O
]
( mathbf{c} cdot S_{4} O_{6}^{2-}(a q)+5 A l(s)+20 H^{+} rightarrow 4 H_{2} S(a q)+ )
[
3 A l^{3+}(a q)+6 H_{2} O
]
D. None of the above
11
636The sum of the coefficients in the
balanced equation of ( boldsymbol{C o}+boldsymbol{N} boldsymbol{i}^{2+} rightarrow )
( boldsymbol{C o}^{boldsymbol{3}+}+boldsymbol{N} boldsymbol{i}, ) is:
A . 5
B. 2
( c cdot 3 )
D. 10
E . 13
11
637In reduction of dichromate by ( boldsymbol{F} boldsymbol{e}(boldsymbol{I} boldsymbol{I}) )
the number of electrons involved per
chromium atoms is:
( A cdot 2 )
B. 3
( c cdot 4 )
D.
11
638The complete balanced equation is:
( M n O_{2}+H_{2} O_{2} rightarrow M n O_{4}^{-}+H_{2} O )
(Basic medium)
A ( cdot 3 mathrm{H}_{2} mathrm{O}_{2}+2 mathrm{MnO}_{2}+2 mathrm{OH}^{-} rightarrow 2 mathrm{MnO}_{4}^{-}+4 mathrm{H}_{2} mathrm{O} )
B. ( 3 H_{2} O_{2}+M n O_{2}+3 O H^{-} rightarrow 2 M n O_{4}^{-}+5 H_{2} O )
( mathrm{c} cdot mathrm{H}_{2} mathrm{O}_{2}+2 mathrm{MnO}_{2}+mathrm{OH}^{-} rightarrow 2 mathrm{MnO}_{4}^{-}+4 mathrm{H}_{2} mathrm{O} )
D. none of these
11
639A reaction in which there is a transfer of
electrons from one reactant to another
is called a (combustion/redox) reaction.
11
6400.01 mole of ( N a_{2} C_{2} O_{4} ) dissolve in
alkaline solution. This solution is
titrated with ( mathrm{V} mathrm{ml} ) 0.1 ( boldsymbol{M} boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} )
solution. Find out ( V )
A .200
в. ( frac{200}{3} )
c. 40
D. ( frac{100}{3} )
11
641Which one of the following statements
is not correct?
A. Oxidation number of ( sin left(N H_{4}right)_{2} S_{2} O_{8} ) is +6
B. Oxidation number of 0 s in ( O s O_{4} ) is +8
C. Oxidation number of ( sin H_{2} S O_{5} ) is +8
Dexidation number of 0 in ( K O_{2} ) is ( -frac{1}{2} )
11
642A solution contains ( boldsymbol{F e}^{+2}, boldsymbol{F e}^{+mathbf{3}} ) and ( boldsymbol{I}^{-} )
ions. This solution was treated with
iodine at ( 35^{circ} mathrm{C} ). Then the favourable
redox reaction is:
(Given that ( boldsymbol{E}_{boldsymbol{F} e^{+3} / boldsymbol{F} e^{+2}}^{boldsymbol{o}}= )
( left.+mathbf{0 . 7 7 V} ; quad boldsymbol{E}_{I_{2} / I^{-}}^{o}=mathbf{0 . 5 3 6} boldsymbol{V}right) )
A ( . I_{2} ) will be reduced to ( I^{-} )
B. there will be no redox reaction
c. ( I^{-} ) will be oxidised to ( I_{2} )
D. ( F e^{+} ) will be oxidised to ( F e^{+3} )
11
643de ion according to
18. Bleaching powder reacts with iodide ion
the following unbalanced equation:
OCI + I +
H 12 + CI+H,0
A 0.6000 g sample of bleaching powder re
35.24 mL of 0.1084 N Na S203 to titrate the libe
iodine. The percentage of Cl in the sample is
(a) 22.58% C1 (b) 5.15% CI
(c) 11.29% C1 (d) 45.16% C1
11
644When an atom reacts chemically and gains one or more electrons, it is said to have been?
A. Catalyzed
B. Oxidized
c. Reduced
D. Decomposed
11
645Oxidation number of ( mathrm{P} ) in ( boldsymbol{P}_{2} boldsymbol{O}_{7}^{4-} ) is :
( A cdot+3 )
( B cdot+4 )
( c cdot+5 )
( D cdot+6 )
11
646Using the standard half-cell potential listed, calculate the equilibrium constant for the reaction:
( boldsymbol{C o}(s)+mathbf{2} boldsymbol{H}^{+}(boldsymbol{a q}) longrightarrow boldsymbol{C o}^{2+}(boldsymbol{a q})+ )
( boldsymbol{H}_{2}(boldsymbol{g}) quad boldsymbol{a t} quad boldsymbol{2} boldsymbol{9} boldsymbol{8} boldsymbol{K} )
( boldsymbol{C o}^{2+}(boldsymbol{a q})+boldsymbol{2 e}-longrightarrow boldsymbol{C o}(boldsymbol{s}) boldsymbol{E}^{0}= )
( -0.277 V )
A ( cdot 2.3 times 10^{9} )
B . ( 4.8 times 10^{4} )
C ( .4 .8 times 10^{7} )
D. ( 4.8 times 10^{11} )
11
647Arrange the following in increasing
order of oxidation states of ( M n )
( boldsymbol{K}_{2} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}, boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4} )
11
648( H_{2} S O_{4} ) cannot be used to dry up ( H_{2} S )
because it oxidises ( H_{2} S ) to ( S O_{2} ) and ( S )
If true enter 1 , else enter 0 .
A.
11
649Iron
(III) oxide on heating with carbon
monoxide gas form solid iron and liberates carbon dioxide gas. This is a:
A. precipitation reaction
B. double decomposition reaction
c. synthesis reaction
D. redox reaction
11
650The ratio of coefficient of
( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}, boldsymbol{F} boldsymbol{e}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2} ) and ( boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} ) in
the following redox equation, ( boldsymbol{F e}+ )
( boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3} rightarrow boldsymbol{F} boldsymbol{e}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3}+ )
( H_{2} O ) in the balanced form will be?
A .10: 1: 4
B . 10: 4: 1
c. 4: 10: 1
D. 4: 1: 10
11
651The passage of electricity in the Daniell cell when ( Z n ) and ( C u ) electrodes are
connected is from:
A. ( C u ) to ( Z n ) in the cell
B. ( C u ) to ( Z n ) outside the cell
c. ( Z n ) to ( C u ) outside the cell
D. ( Z n ) to ( C u ) in the cell
11
652The decomposition of ( K C l O_{3} ) on
heating is an example of:
11
653In substance ( M gleft(H X O_{3}right), ) the oxidation number of ( X ) is :
( mathbf{A} cdot mathbf{0} )
B. +2
( c cdot+3 )
D. +4
11
654What is the oxidation state of sulphur in the following.
a) ( boldsymbol{S F}_{mathbf{6}} )
b) ( N a_{2} S_{2} O_{3} )
11
6555. The reaction of white phosphorus with aqueous NaOH
gives phosphine along with another phosphorus
containing compound. The reaction type, the oxidation
states of phosphorus in phosphine and the other product
are respectively:
(a) redox reaction; -3 and -5
(b) redox reaction; +3 and +5
(c) disproportionation reaction; -3 and +1
(d) disproportionation reaction; -3 and +3
11
656The reaction given below is interpreted
as:
( boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{C l}_{2}(boldsymbol{g}) rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}(boldsymbol{g})+boldsymbol{S}(boldsymbol{s}) )
A. ( H_{2} S ) is getting oxidized and ( C l_{2} ) is getting reduced
B. ( H_{2} S ) is getting reduced and ( C l_{2} ) is getting oxidized
c. only ( H_{2} S ) is oxidized
D. Both ( H_{2} S ) and ( C l_{2} ) are reduced
11
657Equivalent weight of ( boldsymbol{H}_{3} boldsymbol{P} boldsymbol{O}_{2} ) when it
disproportionates into ( P H_{3} ) and
( H 3 P O_{3}(text { mol. wt. }=M) ) is :
( mathbf{A} cdot M )
в. ( frac{M}{2} )
c. ( frac{M}{4} )
D. ( frac{3 M}{4} )
11
658The oxidation numbers of phosphorus in ( B aleft(H_{2} P O_{2}right)_{2} ) and xenon in
( N a_{4} X e O_{6} ) respectively are:
( A cdot+3 ) and +4
B. +2 and +6
( c cdot+1 ) and +8
D. -1 and -6
11
659In the reaction given below, identify the specie undergoing oxidation and reduction
( boldsymbol{H}_{2} boldsymbol{S}(boldsymbol{g})+boldsymbol{C l}_{2} rightarrow boldsymbol{2} boldsymbol{H} boldsymbol{C l}(boldsymbol{g})+boldsymbol{S}(boldsymbol{s}) )
11
660The value of ( n ) in the equation, ( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+mathbf{1 4} boldsymbol{H}^{+}+boldsymbol{n} boldsymbol{e}^{-} rightarrow boldsymbol{2} boldsymbol{C r}^{boldsymbol{3}+}+ )
( mathbf{7} H_{2} O ) is:
( A cdot 2 )
B. 3
( c cdot 4 )
D. 6
11
6612.
Assertion : A cation is formed after the removal of electrons.
Reason: An element always looses one electron to form
cation.
11
662Oxidation numbers of ( M n ) in its
compounds ( M n C l_{2}, M n(O H)_{3} )
( M n O_{2} ) and ( K M n O_{4} ) respectively are:
( A cdot+2,+4,+7,+3 )
B. +2,+3,+4,+7
( c cdot+7,+3,+2,+4 )
( D cdot+7,+4,+3,+2 )
11
663Which is not a disproportionation
reaction?
( A )
B.
[
begin{array}{l}
mathrm{CHO} \
mathrm{COOH}
end{array}+mathrm{OH}^{-} longrightarrow begin{array}{l}
mathrm{CH}_{2} mathrm{OH} quad mathrm{COO}^{-} \
mathrm{COO}^{-}+mid \
mathrm{COO}^{-}
end{array}
]
c. ( N a H+H_{2} O longrightarrow N a O H+H_{2} )
D. All of the above
11
664A decomposition reaction taking place
due to passage of electric current is
called
11
665When an alkali metal is reacted with
hydrogen then metallic hydride is formed. In this reaction:
A. hydrogen is oxidized
B. hydrogen is reduced
c. hydrogen is neither oxidised nor reduced
D. hydrogen is oxidized as well as reduced
11
666DL
2. Which of the following halogens do not exhibit a positive oxidation number in their
compounds?
(a) F
(6) Br
(c) 1
(d) ai
3. TAZbioboru
11
667( H_{2} O_{2} ) oxidises ( M n O_{2} ) to ( M n O_{4}^{-} ) in
basic medium. ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) and ( boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2} ) react
in the molar ratio of ( x: y . ) What is the
value of ( boldsymbol{x}+boldsymbol{y} ? )
11
668Type of redox reaction that occur in
volcanic eruptions is:
A. disproportionation
B. comproportionation
c. reduction
D. both ( A ) and ( B )
11
669What is the correct representation of
reaction occurring when HCl is heated
with ( M n O_{2} ? )
( mathbf{A} cdot M n O_{4}^{-}+5 C l^{-}+8 H^{+} rightarrow M n^{2+}+5 C l^{-}+5 H_{2} O )
B. ( M n O_{2}+2 C l^{-}+4 H^{+} rightarrow M n^{2+}+C l_{2}+2 H_{2} O )
( mathbf{c} cdot 2 M n O_{2}+4 C l^{-}+8 H^{+} rightarrow 2 M n^{2+}+2 C l_{2}+4 H_{2} O )
D. ( M n O_{2}+4 H C l rightarrow M n C l_{4}+C l_{2}+H_{2} O )
11
670Balance the following equations by ion electron method:
( boldsymbol{I}_{2}+boldsymbol{O H}^{-} rightarrow boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{I}^{-}+boldsymbol{H}_{2} boldsymbol{O} )
11
671Write balanced redox reactions of the
following:
( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) ) reduces ( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}(boldsymbol{a} boldsymbol{q}) ) to
green coloured ( C r^{3+}(a q) ) in acidic
medium.
A ( cdot C r_{2} O_{7}^{2-}+3 H_{2} O_{2}+8 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+7 H_{2} O )
B . ( C r_{2} O_{9}^{2-}+3 H_{2} O_{2}+4 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+7 H_{2} O )
c. ( C r_{2} O_{7}^{2-}+3 H_{2} O_{2}+8 H^{+} rightarrow 2 C r^{3+}+3 O_{2}+9 H_{2} O )
D. None of these
11
672Justify that the following reactions are
redox reactions:
( boldsymbol{C u O}(boldsymbol{s})+boldsymbol{H}_{2}(boldsymbol{g}) rightarrow boldsymbol{C u}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g}) )
11
673When P reacts with caustic soda, the
products are ( boldsymbol{P H}_{3} ) and ( boldsymbol{N a H}_{2} boldsymbol{P O}_{2} . ) The
reaction is an example of
A. Oxidation
B. Reduction
c. Both oxidation and reduction
D. Neutralisation
11
674In the reaction ( : boldsymbol{C l}_{2}+boldsymbol{O H}^{-} rightarrow boldsymbol{C l}^{-}+ )
( boldsymbol{C l O}_{boldsymbol{4}}^{-}+boldsymbol{H}_{2} boldsymbol{O} ? )
A. Chlorine is oxidised
B. Chlorine is reduced
C. Chlorine is oxidised as well as reduced
D. Chlorine is neither oxidised nor reduced
11
675In the following reaction:
( mathbf{3} boldsymbol{B} boldsymbol{r}_{2}+boldsymbol{6} boldsymbol{C} boldsymbol{O}_{3}^{2-}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} rightarrow mathbf{5} boldsymbol{B} boldsymbol{r}^{-}+ )
( boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}^{-}+boldsymbol{6} boldsymbol{H} boldsymbol{C} boldsymbol{O}_{3}^{-} )
This question has multiple correct options
A. bromine is oxidised and carbonate is reduced
B. bromine is oxidised
c. bromine is neither oxidised nor reduced
D. bromine is reduced
11
676What is an example of a single replacement reaction?
A. ( A+X rightarrow A X )
в. ( A X rightarrow A+X )
c. ( A+B X rightarrow A X+B )
D. ( A X+B Y rightarrow A Y+B X )
E . ( A+X rightarrow B+Y )
11
677State whether the following conversions are oxidation or reduction?
( boldsymbol{P b O}_{2}+boldsymbol{S O}_{2} rightarrow boldsymbol{P b S O}_{4} )
11
678The volume of ( C O_{2} ) produced at STP by
decomposition of ( 4.2 g ) of ( N a H C O_{3} )
according to the reaction:
( 2 N a H C O_{3} rightarrow N a_{2} C O_{3}+H_{2} O+C O_{2} )
( mathbf{A} cdot 150 mathrm{m} )
B. ( 569 mathrm{ml} )
c. ( 1.68 L )
D. ( 5.6 L )
11
679Statement: Reducing agents are mostly non-metals while oxidizing agents are
mostly metals.

State whether the given statement is
true or false.
A. True
B. False

11
680Oxidation number of nitrogen in which among the oxides of nitrogen is the lowest?
A. Nitric oxide
B. Nitrous oxide
c. Nitrogen dioxide
D. Dinitrogen trioxide
11
681In redox reaction:
A. energy is absorbed.
B. energy is released.
C. transfer of electrons takes place between species.
D. catalyst increases the rate of reaction.
11
6828. Which of the following are not redox reactions?
(a) Mg + N2 – Mg3N2
(6) K[Fe (CN).] + H2SO, +H,
O K ,SO, + CO + FeSO, + (NH2)2SO4
(c) 12 + 3Cl2 → ICI,
(d) CuSO4 + NH3-> [Cu (NH3)4] SO,
TABichana
11
683The oxidation number of ( C r ) is +6 in :
This question has multiple correct options
A ( cdot operatorname{Fe} C r_{2} O_{4} )
в. ( K C r O_{3} C l )
( mathrm{c} cdot mathrm{Cr} mathrm{O}_{5} )
( mathrm{D} cdotleft[mathrm{Cr}(mathrm{OH})_{4}right]^{8} )
11
684( 20 m L ) solution of ( 0.1 ~ M ) ferrous
sulphate was completely oxidised using a suitable oxidising agent. What is the number of electrons exchanged?
A. ( 1.204 times 10^{22} )
в. 193
c. 1930
D. ( 1.204 times 10^{2} )
11
685UL WJ ILUJUIL WUL
JUPUL llais uererly WILL DI, du
Q15. Justify giving reactions that among halogens, fluorine is the best oxidant and among hydrohalic
compounds, Iydroiodic acid is the best reductant.
11
686Write the balanced equations for the reaction occurring when gold is dissolved in aqua regia.
A ( cdot 2 A u+3 H N O_{3}+11 H C l rightarrow 2 H A u C l_{4}+3 N O C l+ )
( 6 H_{2} O )
B . ( 2 A u+3 H N O_{3}+13 H C l rightarrow 2 H A u C l_{4}+2 N O C l+ )
( 8 H_{2} O )
c. ( 2 A u+5 H N O_{3}+11 H C l rightarrow 2 H A u C l_{4}+2 N O C l+ )
( 8 H_{2} O )
D. None of these
11
687Which of the following is not an
intermolecular redox reaction?
( mathbf{A} cdot M g C O_{3} longrightarrow M g O+C O_{2} )
B. ( O_{2}+2 H_{2} longrightarrow 2 H_{2} O )
( mathbf{c} cdot K+H_{2} O longrightarrow K O H+(1 / 2) H_{2} )
D. ( M n B r_{3} longrightarrow M n B r_{2}+(1 / 2) B r_{2} )
11
68810ml of ( N H_{4} C l, 20 mathrm{ml} ) of ( N / 2 H_{2} S O_{4} )
and ( 30 mathrm{ml} ) of ( N / 3 H N O_{3} ) are mixed together and volume made to one litre.
Normality of resulting solution is:
A. ( 30 N / 100 )
в. ( N / 10 )
c. ( N / 20 )
D. ( N / 40 )
11
689In the reaction,
( mathbf{3} boldsymbol{C u} boldsymbol{O}+mathbf{2 N H}_{3} longrightarrow boldsymbol{N}_{2}+mathbf{3} boldsymbol{H}_{2} boldsymbol{O}+ )
( mathbf{3} C u )
the change of ( N H_{3} ) to ( N_{2} ) involves:
A . Loss of 6 electrons per mole of ( N_{2} )
B. Loss of 3 electrons per mole of ( N_{2} )
c. Gain of 6 electrons per mole of ( N_{2} )
D. Gain of 3 electrons per mole of ( N_{2} )
11
690In the following reaction ( P b ) undergoes:
( boldsymbol{P b}(s)+boldsymbol{P b O}_{2}(boldsymbol{s})+mathbf{2} boldsymbol{H}_{2} boldsymbol{S O}_{4}(boldsymbol{a q}) rightarrow )
( 2 P b S O_{4}(s)+2 H_{2} O(l) )
A. disproportionation
B. comproportionation
c. reduction
D. oxidation
11
691Which of the following reactions does not involve oxidation-reduction?
This question has multiple correct options
A ( cdot 2 R b+2 H_{2} O rightarrow 2 R b O H+H_{2} )
в. ( 2 C u I_{2} rightarrow 2 C u I+I_{2} )
c. ( N H_{4} C l+N a O H rightarrow N a C l+N H_{3}+H_{2} O )
D. ( _{4 K C N}+F e(C N)_{2} rightarrow K_{4}left[F e(C N)_{6}right] )
11
692Assertion
In the reaction,
( left.left.2 C u_{2} O_{(s)}+C u_{2} S_{(} sright) rightarrow 6 C u_{(} sright)+ )
( boldsymbol{S} boldsymbol{O}_{2(boldsymbol{g})} )
copper acts as a reductant and sulphur
acts as an oxidant
Reason
The given reaction is not a redox
reaction
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is
not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
693Following reaction describes the rusting
of iron.
( 4 F e+3 O_{2} rightarrow 4 F e^{3+}+6 O^{2-} )
Which one of the following statement is (are) correct?
This question has multiple correct options
A. This is an example of a oxidation reaction
B. Metallic iron is oxidised to ( F e^{3} )
c. ( F e^{3+} ) is an oxidizing agent
D. Metallic iron is a strong reducing agent
11
694When phosphorus reacts with caustic
soda, the products are ( P H_{3} ) and
( N a H_{2} P O_{2} . ) This reaction is an example
of.
A. Oxidation
B. Reduction
c. Disproportionation
D. None of these
11
695Assertion
In the process of drying dishes with a towel, the wetting agent is the dish and the drying agent is the towel
Reason
The wetting agent gets wet during the
process.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
696Which is not a disproportionation
reaction?
( A )
B.
[
begin{array}{ll}
text { CHO } & text { CH }_{2} text { OH } quad text { COO }^{-} \
text {COOH } & text { COO }^{-}+mid
end{array}
]
c. ( N a H+H_{2} O rightarrow N a O H+H_{2} )
D. All of the above
11
697( boldsymbol{A}: mathbf{2} boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{C H} boldsymbol{O}+boldsymbol{K} boldsymbol{O H} longrightarrow )
( boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{C O O K}+boldsymbol{C}_{6} boldsymbol{H}_{5} boldsymbol{C H}_{2} boldsymbol{O H} )
( boldsymbol{B}: mathbf{3} boldsymbol{C l}_{2}+boldsymbol{6} boldsymbol{K O H} longrightarrow mathbf{5} boldsymbol{K} boldsymbol{C l}+ )
( boldsymbol{K} boldsymbol{C l O}_{3}+boldsymbol{3} boldsymbol{H}_{2} boldsymbol{O} )
Select the correct statement.
A. Both are redox reactions
B. Both are disproportionation reaction
c. ( A ) is a disproportionation reaction and ( B ) is a redox reaction
D. ( A ) is a redox reaction and ( B ) is a disproportionation reaction.
11
6981.
Find the value of x in NaxBO,
11
699What are the conditions for a species to
act as a donor and an acceptor during dative bond formation?
11
700In the following reaction, the correct
statements are:
( M g+2 H^{+} rightarrow M g^{2+}+H_{2} )
1. ( M g ) is a reducing agent, ( H^{+} ) is an oxidising agent
2. ( M g ) is oxidising agent, ( H^{+} ) is a reducing agent.
A. only 1
B. only 2
c. both
D. none
11
701Which of the following behaves as both oxidizing and reducing agents?
A. ( H_{2} S O_{4} )
в. ( S O_{2} )
c. ( H_{2} )
D. ( H N O_{3} )
11
702( boldsymbol{C u O}+boldsymbol{H}_{2} rightarrow boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C u} )
Above reaction is an example of :
A. redox reaction
B. synthesis reaction
c. neutralisation
D. analysis reaction
11
703Which of the following is/are disproportionation reactions?
This question has multiple correct options
( ^{mathbf{A}} cdot_{H_{2}} O_{2} rightarrow H_{2} O+frac{1}{2} O_{2} )
B . ( H N O_{3}+H C l rightarrow N O+C l_{2}+H_{2} O )
c. ( 3 C l O^{-} rightarrow C l O_{3}^{-}+2 C l^{-} )
D. ( C l_{2}+H_{2} O rightarrow H C l+H C l O )
11
704Assertion
Conversion of potassium ferrocyanide to potassium is an oxidation process.
Reason Oxidation is the additon of oxygen 1 electronegative element to a substance or removal of hydrogen / electropositive element from a substance.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
705What is the oxidation number of
underlined element?
[
boldsymbol{B} boldsymbol{a}left(boldsymbol{H}_{2} underline{boldsymbol{P}} boldsymbol{O}_{2}right)_{2}
]
11
706Balance the following redox reaction in basic medium.
( boldsymbol{C l}_{2}+boldsymbol{I} boldsymbol{O}_{3}^{-}+boldsymbol{O H}^{-} longrightarrow boldsymbol{I} boldsymbol{O}_{4}^{-}+boldsymbol{C l}^{-} )
A ( cdot C l_{2}+I O_{3}^{-}+3 O H^{-} rightarrow I O_{4}^{-}+5 C l^{-}+H_{2} O )
B. ( C l_{2}+I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+2 C l^{-}+H_{2} O )
c. ( C l_{2}+2 I O_{3}^{-}+2 O H^{-} rightarrow I O_{4}^{-}+5 C l^{-}+H_{2} O )
D. None of the above
11
707When Magnesium is burnt in air, a
white ash remain as left over. What is
this?
( mathbf{A} cdot M g O_{2} )
в. ( M g O )
c. ( M g )
D. ( M g_{3} O )
11
708For the redox reaction
( M n O_{4}^{ominus}+C_{2} O_{4}^{2-}+H^{oplus} longrightarrow M n^{2+}+ )
( boldsymbol{C O}_{2}+boldsymbol{H}_{2} boldsymbol{O} )
the correct coefficients of the reactions
for the balanced reaction are:
( begin{array}{lll}text { A. } M n O_{4}^{ominus} & C_{2} O_{4}^{2-} & H^{oplus}end{array} )
( 2 quad 5 quad 16 )
B. ( M n O_{4}^{ominus} quad C_{2} O_{4}^{2-} quad H^{oplus} )
( 16 quad 5 quad 2 )
( begin{array}{lll}text { c. } M n O_{4}^{ominus} & C_{2} O_{4}^{2-} & H^{oplus}end{array} )
16
D. ( M n O_{4}^{ominus} quad C_{2} O_{4}^{2-} quad H^{oplus} )
11
709Which of the following is a redox
reaction?
( mathbf{A} cdot H_{2} S O_{4} ) with ( N a O H )
B. In atmosphere, ( O_{3} ) from ( O_{2} ) by lightning
C. Nitrogen oxides form nitrogen and oxygen by lightning
D. Evaporation of ( H_{2} O )
11
710Identify the type of reaction taking place in ( boldsymbol{F e}+boldsymbol{C u S O}_{4} rightarrow boldsymbol{C u}+boldsymbol{F e} boldsymbol{S O}_{4} )
A. Redox reaction
B. Displacement reaction
c. Neutralization reaction
D. Precipitation reaction
11
711The reaction, ( Z n^{2+}(a q)+2 e^{-} rightarrow Z n(s) )
is:
A. oxidation
B. reduction
c. redox reduction
D. none of the above
11
712What is the sum of oxidation numbers
of all the carbon atoms except that
attached to ( -C H O ) group in
( boldsymbol{C}_{boldsymbol{6}} boldsymbol{H}_{boldsymbol{5}} boldsymbol{C} boldsymbol{H} boldsymbol{O} ? )
A . -6
B. -5
c. -4
D. – –
11
713Name the reducing agent in the following:
( mathbf{3} M n O_{2}+4 A l rightarrow 3 M n+2 A l_{2} O_{3} )
( mathbf{A} cdot M n )
B. ( A l )
( mathrm{c} cdot M n O_{2} )
D. ( A l_{2} O_{3} )
11
714The above reaction is a type of intramolecular disproportionation reaction.
If true enter 1 , else enter 0 .
[
underbrace{mathrm{CHO}}_{mathrm{CHO}} stackrel{mathrm{OH}^{-}}{longrightarrow} underbrace{mathrm{COO}^{-}}_{mathrm{CH}_{2} mathrm{OH}}
]
( A )
11
715In the reaction, ( C l_{2}+O H^{-} rightarrow C l^{-}+ )
( C l O_{4}^{-}+H_{2} O, ) chlorine is?
A. Oxidised
B. Reduced
c. Oxidised as well as reduced
D. Neither oxidised nor reduced
11
716Reaction of magnesium ribbon with dilute sulphuric acid to form magnesium sulphate and hydrogen is a combination reaction.
A. True
B. False
11
717Match the reactions in column I with
their respective characteristics given in column II.
11
718Identify disproportionation reaction.
( mathbf{A} cdot C H_{4}+2 O_{2} rightarrow C O_{2}+2 H_{2} O )
( mathbf{B} cdot C H_{4}+4 C l_{2} rightarrow C C l_{4}+4 H C l )
( mathbf{c} cdot 2 F_{2}+2 O H^{-} rightarrow 2 F^{-}+O F_{2}+H_{2} O )
D. ( 2 N O_{2}+2 O H^{-} rightarrow N O_{2}^{-}+N O_{3}^{-}+H_{2} O )
11
719Complete and balance the following
compound ( boldsymbol{C a}_{mathbf{5}}left(boldsymbol{P O}_{4}right)_{3} boldsymbol{F}+boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+ )
( boldsymbol{H}_{2} boldsymbol{O} stackrel{boldsymbol{H} e a t}{rightarrow}-ldots-ldots-+boldsymbol{C} boldsymbol{a} boldsymbol{S} boldsymbol{O}_{4} )
( 2 H_{2} O+_{-}-_{-}– )
11
720The number of electrons required to balance the following equation is:
( N O_{3}^{-}+4 H^{+}+e^{-} rightarrow 2 H_{2} O+N O )
( mathbf{A} cdot mathbf{5} )
B. 4
( c .3 )
D. 2
11
721Assertion
Oxidation is the gain of oxygen.
Reason

Reduction is the loss of oxygen.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect

11
722Question 22. What is meant by ‘disproportionation’? Give two examples
of disproportionation reaction in aqueous solution.
11
723Consider a titration of potassium
dichromate solution with acidified
Mohr’s salt solution using diphenylamine as indicator. The number of moles of Mohr’s salt required per mole of dichromate is:
A . 3
B. 4
c. 5
D. 6
11
724Number of moles of ( boldsymbol{K}_{2} boldsymbol{C r}_{2} boldsymbol{O}_{7} ) reduced
by one mole of ( S n^{2+} ) ions is :
A ( cdot frac{1}{3} )
B. 3
( c cdot frac{1}{6} )
D. 6
11
725How many grams of ( 70 % ) concentrated nitric acid solution should be used to
prepare ( 250 mathrm{mL} ) of ( 2.0 mathrm{M} ? )
A ( cdot 45.0 mathrm{g} ) conc. ( mathrm{H} mathrm{NO}_{3} )
B. 90.0 g conc. H ( mathrm{NO}_{3} )
c. 70.0 conc. ( H N O_{3} )
D. 54.0 g conc. H NO
11
726( 2 K(s)+F_{2}(g) rightarrow 2 K^{+} F^{-}(s) ) is a type
of reaction.
A. disproportionation
B. combustion
c. corrosion
D. redox
11
72732. Browning of paper in ola
books is caused by
(1) frequent use
(2) lack of aeration
(3) collection of dust
(4) oxidation of cellulose
11
728Choose the correct options –
A. Reaction between lead nitrate and potassium iodide is double decomposition reaction.
B. Reaction between copper oxide and hydrogen is redox reaction.
C. Reactions in which heat is absorbed are called exothermic reactions
D. Both (A) and (B).
11
729Formation of calcium oxide and carbon
dioxide by heating limestone is an example of double decomposition reaction.
A. True
B. False
11
730Statement 1: Oxidation and reduction
occur together Statement 2: In redox reactions,
electrons must be gained and lost.
A. Both Statement 1 and Statement 2 are correct and Statement 2 is the correct explanation of Statement 1
B. Both Statement 1 and Statement 2 are correct and Statement 2 is not the correct explanation of Statement 1.
c. statement 1 is correct but statement 2 is not correct
D. Statement 1 is not correct but Statement 2 is correct
E. Both the Statement 1 and Statement 2 are not correct
11
731Sulphur dioxide bleaches colouring matter by
A. dehydration
B. oxidation
c. decomposition
D. reduction
11
732Assign oxidation numbers to each atom
in ( boldsymbol{N} boldsymbol{H}_{mathbf{4}} boldsymbol{N} boldsymbol{O}_{2} )
A. ( N=4,-4 ; H=1 ; O=-2 )
B. ( N=-3 ; H=1 ; O=3 )
c. ( N=-1 ; H=1 ; O=-2 )
11
733In the reaction, ( 4 C r O_{5}+6 H_{2} S O_{4} rightarrow )
( 2 C r_{2}left(S O_{4}right)_{3}+6 H_{2} O+7 O_{2}, ) which
statement is wrong?
A. It is a disproportionation reaction.
B. It is an intramolecular redox reaction
c. ( C r O_{5} ) acts as oxidant and reductant both.
D. cracts as oxidant and 0 acts as reductant
11
734Balance the following equations.
(i) ( boldsymbol{K} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}+boldsymbol{H} boldsymbol{C l} rightarrow boldsymbol{K} boldsymbol{C l}+ )
( M n C l_{2}+H_{2} O+C l_{2} )
(ii) ( boldsymbol{N} boldsymbol{H}_{3}+boldsymbol{O}_{3} rightarrow boldsymbol{N} boldsymbol{O}+boldsymbol{H}_{2} boldsymbol{O} )
11
735Before: ( C u O+ ) porcelain boat ( =62.869 g )
( C a C l_{2}+U-t u b e=80.483 g )
After:Porcelain boat+contents =
( 54.869 g )
CaCl ( _{2}+ ) U-tube ( =89.483 mathrm{g} )
Reactions: ( Z n(s)+2 H C l(a q) rightarrow )
( Z n C l_{2}(a q)+H_{2}(g) ) then ( H_{2}(g)+ )
( boldsymbol{C u} boldsymbol{O}(boldsymbol{s}) rightarrow boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{g})+boldsymbol{C u}(boldsymbol{s}) )
What type of reaction occurred in the
porcelain boat?
A . Electrolysis
B. Double displacement
c. Reduction and oxidation
D. Decomposition or analysis
E. Combination or synthesis
11
736The oxidation number of ( S ) in ( N a_{2} S_{4} O_{6} )
is :
A . +2.5
B. +2 and +3 (two ( S ) have +2 and other two have +3 )
( mathrm{c} cdot+2 ) and +3 (three ( S ) have +2 and one ( S ) has +3
D. +5 and 0 (two S have +5 and the other two ( S ) have 0 )
11
737Identify tthe compounds which are reduced and oxidised in the following
reaction.
( mathbf{3} N_{2} boldsymbol{H}_{4}+mathbf{2} boldsymbol{B} boldsymbol{r} boldsymbol{O}_{3}^{-} rightarrow mathbf{3} boldsymbol{N}_{2}+mathbf{2} boldsymbol{B} boldsymbol{r}^{-}+ )
( mathbf{6} boldsymbol{H}_{2} boldsymbol{O} )
A ( cdot N_{2} H_{4} ) is oxidised and ( B r O_{3}^{-} ) is reduced
B. ( B r O_{3}^{-} ) is oxidised and ( N_{2} H_{4} ) is reduced
C. ( B r O_{3}^{-} ) is both reduced and oxidised
D. This is not a redox reaction
11
738Number of which two chemical species will be same in the given procedure?
A. ( M n O_{2} )
в. ( I_{2} )
c. ( I^{-} )
D. ( S_{2} O_{3}^{2} )
11
739Consider the following ( boldsymbol{E}^{0} ) values:
( boldsymbol{E}_{boldsymbol{F} boldsymbol{e}^{3+} / boldsymbol{F} e^{2+}}^{boldsymbol{0}}=boldsymbol{0 . 7 7 V} )
( E_{S n^{2+} / S n}^{0}=-0.14 V )
Under standard conditions the potential
for the reaction, is:
( boldsymbol{S} boldsymbol{n}(boldsymbol{s})+boldsymbol{2} boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2} boldsymbol{F} boldsymbol{e}^{2+}(boldsymbol{a} boldsymbol{q})+ )
( boldsymbol{S} boldsymbol{n}^{2+}(boldsymbol{a} boldsymbol{q}) )
A . ( 0.91 mathrm{V} )
B. 1.40V
c. ( 1.68 v )
D. 0.63v
11
740Hydrogen sulphide gets reduced to sulphur.
A . True
B. False
11
741When a piece of magnesium ribbon is placed in a beaker of copper sulfate solution, which one of the following is most likely to happen?
A. A vigorous reaction immediately takes place, with the release of a lot of heat
B. The blue colour of the copper sulfate solution gets darker
c. The blue colour of the copper sulfate solution gets lighter.
D. The magnesium catches fire
11
742Oxidation number is ( mathrm{S} ) in ( left(C H_{3}right)_{2} S O ) is :
A. zero
B. +1
( c cdot+2 )
( D cdot+3 )
11
743The oxidation state of iodine in ( boldsymbol{H}_{4} boldsymbol{I} boldsymbol{O}_{mathbf{6}}^{-} )
is?
( A cdot+7 )
B. –
( c .+5 )
D. +1
11
744The permanganate ion is an excellent oxidizing agent in aqueous solutions.
When the half reaction, ( M n O_{4}^{-}+ )
( boldsymbol{H}^{+}+boldsymbol{e}^{-} rightarrow boldsymbol{M} boldsymbol{n} boldsymbol{O}_{2}+boldsymbol{H}_{2} boldsymbol{O} ) is
balanced, the correct coefficients for the species involved are:
A. 1,4,4,1,2
B. 1,4,2,1,2
c. 1,4,3,1,2
D. 1,4,1,1,2
11
74509. Identify the substance oxidised, reduced, oxidising agent and reducing agent for each of the
following reactions,
(a) 2AgBr(s) + C,H,O, (aq) — 2Ag(s) + 2HBr(aq) + C.H.O.(aq)
(6) HCHOW) + 2[Ag(NH2).1 (aq) + 3OH (ag)
Ag(s) + HCOO (aq) + 4NH (aq) + 2H,01)
(c) NH4) + 2H,0,0) – Ng(g) + 4H,O)
11
746Which of the following represent redox reactions?
( mathrm{Cr}_{2} mathrm{O}_{7}^{2-}+2^{ominus} boldsymbol{O} boldsymbol{H} longrightarrow 2 boldsymbol{C r} boldsymbol{O}_{4}^{2-}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
II. ( Z n+C u S O_{4} longrightarrow Z n S O_{4}+C u )
III. ( 2 M n O_{4}^{ominus}+3 M n^{2+}+4 stackrel{theta}{O} H longrightarrow )
( mathbf{5} M n O_{2}+2 H_{2} O )
IV. ( 2 C u^{oplus} longrightarrow C u+C u^{2+} )
A . ।, । ।
в. ।, ॥
c. ॥ा, ।ा
D. ॥, ॥I, IV
11
747Solid calcium oxide was taken in a
container and water was added slowly
to it-
(i) State two observations made in the
experiment.
(ii) Write the name and the chemical
formula.
11
74810. In the ethylene molecule the two carbon atoms have the oxidation numbers.
(a) -1, -1 (6) -2,-2
(c) -1, -2 2 (d) +2,2
5 d)
11
749( 10=0 )
( alpha )
( alpha )
( alpha )
11
750Assertion
The two Fe atoms in ( F e_{3} O_{4} ) have
different oxidation numbers.
Reason
( F e^{2+} ) ions decolourise ( K M n O_{4} )
Solution.
A. Both Assertion and Reason are correct and Reason is
the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
C. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
751Consider the reactions:
( mathbf{2} S_{2} O_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{I}_{2}(boldsymbol{s}) rightarrow boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-}(boldsymbol{a} boldsymbol{q})+ )
( 2 I^{-}(a q) )
( boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-}(boldsymbol{a} boldsymbol{q})+boldsymbol{2} boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+boldsymbol{5} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) rightarrow )
( mathbf{2} boldsymbol{S} boldsymbol{O}_{mathbf{4}}^{mathbf{2}-}(boldsymbol{a} boldsymbol{q})+boldsymbol{4} boldsymbol{B} boldsymbol{r}^{-}(boldsymbol{a} boldsymbol{q})+mathbf{1 0} boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) )
Why does the same reductant,
thiosulphate react differently with iodine and bromine?
11
752Which of the reactants act as oxidant or
reductant if any:
( boldsymbol{C a}+boldsymbol{C l}_{2} rightarrow boldsymbol{C a} boldsymbol{C l}_{2} )
A ( cdot C l_{2} )
в. ( C a )
c. Both of these
D. None of these
11
753( boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{A} boldsymbol{X}+boldsymbol{B} boldsymbol{Y} longrightarrow boldsymbol{H} boldsymbol{A}+boldsymbol{O} boldsymbol{Y}+ )
( boldsymbol{X}_{2} boldsymbol{B} )
In the above-unbalanced redox
reaction, the oxidation number of ( boldsymbol{X} ) is
-2 and neither ( X ) nor water is involved
in the redox process. If the above reaction is balanced with
the smallest whole-number
coefficients, the sum of the
stoichiometric coefficients of all the
compounds is :
( A cdot 9 )
B. 8
( c .7 )
D. 6
11
754Q7. Suggest a list of substances where carbon can exhibit oxidation states from
nitrogen from -3 to +5.
4 to +4 and
11
755What is the oxidation number of
underlined element?
[
underline{I} C l_{3}
]
11
756Match the reactions in list I with the
number of electrons that participate in list II.
11
757Which one of the following substances is a good oxidising agent?
A. coke
B. water
c. Hydrogen peroxide
D. sulphur dioxide
11
758Match the Column-I with Column-II.11
759During the oxidation of arsenite ion, ( A s O_{3}^{3-}, ) to arsenate ion, ( A s O_{4}^{3-}, ) in alkaline medium, the number of moles of hydroxide ions consumed per mole of arsenite ion is
( A cdot 2 )
B. 3
( c cdot 2 / 3 )
D. 3/2
11
760Identyfy oxidation and reduction process for the reaction-
( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{s})+boldsymbol{F}_{2}(boldsymbol{g}) rightarrow boldsymbol{H} boldsymbol{F}(boldsymbol{g})+boldsymbol{H} boldsymbol{O} boldsymbol{F}(boldsymbol{g}) )
11
761( boldsymbol{H} boldsymbol{C l}(boldsymbol{a} boldsymbol{q})+boldsymbol{Z} boldsymbol{n}(boldsymbol{s}) rightarrow boldsymbol{Z} boldsymbol{n} boldsymbol{C l}_{2}(boldsymbol{a q})+ )
( boldsymbol{H}_{2}(boldsymbol{g}) )
In the reaction above, which term best
describes the role of ( boldsymbol{H} boldsymbol{C l}(boldsymbol{a} boldsymbol{q}) ? )
A. Bronsted acid
B. Oxidizing agent
c. Reducing agent
D. Precipitate
E. Cathode
11
762The non-metals undergoing disproportionation
are
This question has multiple correct options
( A cdot P_{4} )
в. ( C l_{2} )
( c cdot I_{2} )
D.
11
763Choose the correct option regarding change in oxidation number of the underlined atom in the following
conversion.
( boldsymbol{H}_{2} underline{boldsymbol{S}} boldsymbol{O}_{5}+boldsymbol{2} boldsymbol{K} boldsymbol{I} rightarrow boldsymbol{K}_{2} boldsymbol{S} boldsymbol{O}_{4}+boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{I}_{2} )
( A cdot 2 )
B. 3
( c )
D. No Change
11
764In which of the following reactions have the underlined substance been
reduced?
A. Carbonmonoxide + copperoxide ( rightarrow ) carbondioxide ( + ) Carbon
copper
в. ( frac{text { Copperoxide }}{text { water }}+ ) hydrochloricacid ( rightarrow ) copperchloride ( + )
c. Hydrogen( + )ironoxide( rightarrow )iron ( + )water
D. ( underline{S t e a m}+ )iron ( rightarrow ) ironoxide ( + )hydrogen
11
765The addition of oxygen to a substance is called
A. oxidation
B. reduction
c. synthesis
D. none of these
11
766Dichloroacetic acid ( left(boldsymbol{C H} boldsymbol{C l}_{2} boldsymbol{C O}_{2} boldsymbol{H}right) ) is
oxidized to ( C O_{2}, H_{2} O ) and ( C l_{2} ) by 1.2 equivalents of an oxidizing agent. Same amount of the acid can neutralize ‘X’
moles of ( N H_{2} ) to give ammonium
dichloroacetate.’ ( X^{prime} ) is
A. 0.4
B. 0.3
( c cdot 0.2 )
D. 0.1
11
767Which of the following are primary standard?
This question has multiple correct options
A . Oxalic acid
B. Potassium permanganate
c. Potassium dichromate
D. Sodium hydroxide
11
768Q5. Write the O.N of all the atoms for the following well known oxidants?
(i) KMnO, (ii) K,Cr,0, (iii) KCIO,
11
769In acid medium, the standard reduction
potential of ( N O ) converted to ( N_{2} O ) is
( mathbf{1 . 5 9} boldsymbol{V} ). Its standard potential in alkaline
medium would be:
A. ( -1.59 V )
В. ( -0.764 V )
c. ( 0.764 V )
D. ( 0.062 V )
11
770In a balanced equation, ( boldsymbol{H}_{2} boldsymbol{S} boldsymbol{O}_{4}+ )
( boldsymbol{x} boldsymbol{H} boldsymbol{I} rightarrow boldsymbol{H}_{2} boldsymbol{S}+boldsymbol{y} boldsymbol{I}_{2}+boldsymbol{z} boldsymbol{H}_{2} boldsymbol{O}, ) the values
of ( x, y ) and ( z ) are respectively:
A. ( x=3, y=5, z=2 )
в. ( x=4, y=8, z=5 )
c. ( x=8, y=4, z=4 )
D. ( x=5, y=3, z=1 )
11
771When hydrogen sulphide gas is passed through a blue
solution of copper sulphate, a black precipitate of copper
sulphide is formed. This is an example of?
(a) combination reaction
(b) displacement reaction
(c) decomposition reaction
(d) double decomposition reaction
11
772In cyanide method, silver metal is
obtained as given in the following
reaction:
( mathbf{2} boldsymbol{K}left[boldsymbol{A} boldsymbol{g}(boldsymbol{C} boldsymbol{N})_{2}right]+boldsymbol{Z} boldsymbol{n} longrightarrow )
( boldsymbol{K}_{2}left[boldsymbol{Z} boldsymbol{n}(boldsymbol{C} boldsymbol{N})_{4}right]+boldsymbol{2} boldsymbol{A} boldsymbol{g} )
In this :
A. ( A g ) has been oxidised and ( Z n ) has been reduced
B. ( A g^{+} ) has been reduced and ( Z n ) has been oxidised
c. both the metals have been oxidised
D. both the metals have been reduced
11
773In redox reactions, oxidation state of oxidising agent and reducing agent respectively
A. Increases and decreases
B. Decreases and increases
c. Increases and remains same
D. Decreases and remains same
11
774From the given reactions which is a
redox reaction?
This question has multiple correct options
( mathbf{A} cdot C u O(s)+H_{2}(g) rightarrow C u(s)+H_{2} O(l) )
B ( cdot 2 C u(s)+O_{2}(g) rightarrow 2 C u O(s) )
( mathbf{c} cdot C(s)+2 H_{2}(g) rightarrow C H_{4}(g) )
D. ( 4 A l(s)+3 O_{2}(g) rightarrow 2 A l_{2} O_{3}(s) )
11
775Carbon and oxygen combine to form two oxides, carbon monoxide and carbon
dioxide in which the ratio of the weights of carbon and oxygen is respectively 12: 16 and 12: 32
These figures illustrate the:
A. Law of multiple proportions
B. Law of reciprocal proportions
c. Law of conservation of mass
D. Law of constant proportions
11
776Q.8 Which of the following arrangements represent increasing oxidation
number of the central atom ?
(a) Cro, CIOZ, Croa. MnO4 (b) CIO3, Croa. Mno. Croz
(c) Croz, CIO3, MnO,, Cro (d) Croa. Mnoz, CrO2, CIO
11
777When ( C u O ) reacts with hydrogen, ( dots )……. is
reduced.
A. ( C u O )
в. ( H_{2} )
c. ( C u )
D. ( H_{2} O )
11
778Why do fireflies glow at night?
A. Fireflies contain an organic compound.
B. Chemical reaction involves emission of visible light.
C. Fireflies produce two chemicals which mix with each other and oxygen.
D. All of the above.
11
779One mole of ( N_{2} H_{4} ) loses 10 moles of
electrons to form a new compound ( boldsymbol{A} )
Assuming that all the nitrogen appears in the new compound, what is the oxidation state of nitrogen in ( A ) ? [There is no change in the oxidation state of hydrogen ( ] )
A ( .+1 )
B. -3
( c cdot+3 )
D. +5
11
780Give half cell equation of Daniel cell takes place at cathode.11
781Which of the following reaction is an example of a redox reaction?
A. ( X e F_{2}+P F_{5} rightarrow[X e F]^{+}+P F_{6} )
в. ( X e F_{6}+H_{2} O rightarrow X e O F_{4}+2 H F )
c. ( X e F_{6}+2 H_{2} O rightarrow X e O_{2} F_{2}+4 H F )
D. ( X e F_{4}+O_{2} F_{2} rightarrow X e F_{6}+O_{2} )
11
782Balance the following equations by
oxidation number method.
( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{C l} boldsymbol{O}_{2}+boldsymbol{O} boldsymbol{H}^{-} rightarrow boldsymbol{C l}^{-}+boldsymbol{O}_{2}+ )
( boldsymbol{H}_{2} boldsymbol{O} )
11
783One gas bleaches the colour of flowers by reduction while the other gas by
oxidation. The two gases are,
respectively:
A ( cdot cos 2 l_{2} )
в. ( H_{2} S & B r_{2} )
( mathrm{c} cdot operatorname{SO}_{2} & C l_{2} )
D. ( N H_{3} & S O_{3} )
11
784“Nitric oxide reacts with oxygen to form reddish brown nitrogen dioxide gas”” Choose the correct equation for the
above reaction
A ( cdot 2 N O+O_{2} rightarrow 2 N O_{2} )
в. ( N_{2} O+O_{2} rightarrow N O_{2}+N O )
C. ( N a N O_{3} stackrel{text {heat}}{longrightarrow} 2 mathrm{NaNO}_{2}+mathrm{O}_{2} )
D. ( 2 N O_{3}+O_{2} rightarrow 2 N O_{2}+2 O_{2} )
11
785Other things being equal, the EMF of a Daniell cell may be increased by
A. Keeping low temperature
B. Using large copper electrodes
c. using large zinc electrodes
D. Decreasing concentration of ( C u^{2+} ) ions
11
786mpounds exchange their
(a A
The reactions in which two compounds
radicals to form two new compounds are called
(a) displacement reaction
(b) decomposition reaction
(c) double displacement reaction
(d) isomerisation reaction
ronction and tell thiob
11
787In calcium hypophosphite, oxidation number of phosphorus is
( mathbf{A} cdot mathbf{0} )
B. +1
( c cdot+3 )
D. + 5
11
788Which of the following half-reactions is correctly balanced?
A ( cdot M n O_{4}^{-} rightarrow M n^{2+}+4 H_{2} O )
B. ( C u+2 A g^{+} rightarrow 2 A g+C u^{2+} )
( mathbf{c} cdot H_{2}+O H^{-} rightarrow 2 H_{2} O )
( mathbf{D} cdot P b^{2+}+2 e^{-} rightarrow P b )
E ( cdot 2 F^{-}+2 e^{-} rightarrow F_{2} )
11
789Assertion
Moles of KMnO4 required for oxidation of Fe2 in acidic and basic medium will
be different.
Reason
Final oxidation state to which M will be
reduced will be different in case of
acidic and basic medium.
A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion
B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
c. Assertion is correct but Reason is incorrect
D. Both Assertion and Reason are incorrect
11
790Oxidation state of carbon in ( boldsymbol{C} boldsymbol{H} boldsymbol{C l}_{3} ) is :
( A cdot+1 )
( B .+2 )
( c cdot+4 )
D. – –
11
79117. The number of moles of Mohr’s salt required per mole
of dichromate ion is:
(a) 3
(b)
4
2
(c) 5
(d) 6
11
792Which of the following has least tendency in +3 oxidation state to show disproportionation reaction.
A . ( N )
в. ( P )
( c . B i )
D. ( S b )
11
793Which of the following is a dispropprtonation reaction?
A ( cdot C a C O_{3}+2 H^{+} rightarrow C a^{2+}+C O_{2} )
B ( cdot 2 C r O_{4}^{2-}+rightarrow C r_{2} O_{7}^{2+} H_{2} O )
c. ( C r_{2} O_{4}^{2-}+rightarrow 2 C r O_{4}^{2-}+H_{2} O )
D. ( C u_{2} O+2 H^{+} rightarrow C u^{2+}+H_{2} O )
11
794( ldots B r O_{3}^{-}(a q)+ldots B r^{-}(a q)+ )
( ldots boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) rightarrow ldots boldsymbol{B} boldsymbol{r}_{2}(boldsymbol{l})+ldots boldsymbol{H}_{2} boldsymbol{O} )
After balancing the above equation.
What is the ratio of coefficient ( B r O_{3}^{-} ) to
( B r^{-} ? )
A .1: 5
B. 1: 3
( c cdot 1: 2 )
D. 1:
E. 2: 3
11
795Which of the following is not a redox reaction?
A. ( C a C O_{3} rightarrow C a O+C O_{2} )
в. ( O_{2}+2 H_{2} rightarrow 2 H_{2} O )
c. ( _{N a+H_{2} O rightarrow N a O H+frac{1}{2} H_{2}} )
D. ( M n C l_{3} rightarrow M n C l_{2}+frac{1}{2} C l_{2} )
11
796Q. 18 Mn0% undergoes disproportionation reaction in acidic medium but Mno
does not. Give reason.
11
797In the following redox reaction:
( boldsymbol{Z} boldsymbol{n}(boldsymbol{s})+boldsymbol{N} boldsymbol{O}_{boldsymbol{3}}^{-}(boldsymbol{a} boldsymbol{q})+boldsymbol{H}^{+}(boldsymbol{a} boldsymbol{q}) longrightarrow )
( Z n^{2+}(a q)+N H_{4}^{+}(a q) )
( Z n(s) ) and ( N O_{3}^{-}(a q) ) respectively are
respectively:
A. oxidant and reductant
B. reductant and oxidant
c. both oxidant
D. both reductant
11
798Find the oxidation number of Ni in
( left[boldsymbol{N} boldsymbol{i}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-} )
11
799( boldsymbol{x} boldsymbol{N a O H}+boldsymbol{H}_{2} boldsymbol{S O}_{4} rightarrow boldsymbol{N a}_{2} boldsymbol{S O}_{4}+ )
( boldsymbol{y} boldsymbol{H}_{2} boldsymbol{O} . ) Balance the given chemical
equation and find the value of ( x ) and ( y )
A .2,1
в. 2,2
c. 2,3
D. 1,2
11
800In the following reaction:
( boldsymbol{x} boldsymbol{Z} boldsymbol{n}+boldsymbol{y} boldsymbol{H} boldsymbol{N} boldsymbol{O}_{3}(boldsymbol{d} boldsymbol{i} l) longrightarrow )
( boldsymbol{a} boldsymbol{Z} boldsymbol{n}left(boldsymbol{N} boldsymbol{O}_{3}right)_{2}+boldsymbol{b} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{c} boldsymbol{N} boldsymbol{H}_{4} boldsymbol{N} boldsymbol{O}_{3} )
What is the sum of the coefficients
( (a+b+c) ? )
11
801Excess of KI reacts with ( C u S O_{4} )
solution and then ( N a_{2} S_{2} O_{3} ) solution is
added to it. Which of the statement is
incorrect for this reaction?
A ( cdot C u_{2} I_{2} ) is formed
B. ( C u I_{2} ) is formed
c. ( N a_{2} S_{2} O_{3} ) is oxidised
D. Evolved ( I_{2} ) is reduced
11
802( boldsymbol{H}_{2} boldsymbol{O}_{2}+boldsymbol{O}_{3} rightarrow boldsymbol{H}_{2} boldsymbol{O}+mathbf{2} boldsymbol{O}_{2}, ) in this
reaction
A. ( H_{2} O_{2} ) is bleached
B. ( H_{2} O_{2} ) is oxidised
C. ( H_{2} O_{2} ) is dehydrated
D. ( H_{2} O_{2} ) is neither oxidised nor reduced
11
803( M n O_{4}^{2-}(1 text { mole }) ) in neutral aqueous medium disproportionate to
A ( cdot 2 / 3 ) mole ( M n O_{4}^{-} ) and ( 1 / 3 ) mole ( M n O_{2} )
B . 1/3 mole ( M n O_{4}^{-} ) and ( 2 / 3 ) mole ( M n O_{2} )
( mathrm{c} cdot 1 / 3 ) mole of ( M n_{2} O_{7} ) and ( 1 / 3 ) mole of ( M n O_{2} )
D. ( 2 / 3 ) mole of ( M n_{2} O_{7} ) and ( 1 / 3 ) mole of ( M n O_{2} )
11
804Iron is extracted from iron oxide using
carbon monoxide as shown.
iron oxide ( + ) carbon monoxide ( rightarrow ) iron ( + )
carbon dioxide
Which statement is correct?
A. Carbon monoxide is oxidised to carbon dioxide
B. Carbon monoxide is reduced to carbon dioxide
C. Iron is oxidised to iron oxide
D. Iron oxide is oxidised to iron
11
805Which of the following is not a redox
reaction?
A. Burning of candle
B. Rusting of iron
c. Dissolving a saltin water
D. Dissolving Zn in dil. ( H_{2} S O_{4} )
11
806From the periodic table select three possible non-metals which can show disproportionation reaction.11
807Redox indicators are substances that
undergo a colour change at specific
A ( . p H )
B. electrode potential
c. both ( A ) and ( B )
D. none of them
11
808Which of the following is not a disproportionation reaction?
A ( cdot 2 P h C H O quad A l(O E t)_{3}, P h C O O C H_{2} P h )
c. ( N a H+H_{2} O longrightarrow N a O H+H_{2} )
D. All
11
809Which of the following statements is
wrong?
A. Acidified ( K M n O_{4} ) solution decolourises on the addition of sodium oxalate
B. In the reaction between ( B r_{2} ) and ( C s I, B r_{2} ) is an oxidising agent and ( C s I ) is a reducing agent
c. In the reaction ( 2 K_{2} S_{2} O_{3}+I_{2} rightarrow 2 K I+K_{2} S_{4} O_{6} ), the
change in the oxidation number of ( S ) is 0.5
D. ( C ) has the same oxidation number in both ( C H_{4} ) and
( C O_{2} )
11
810When phosphorus reacts with caustic
soda, the products are ( P H_{3} ) and
( N a H_{2} P O_{2} . ) This reaction is an example
of
A. Oxidation
B. Reduction
c. Oxidation and reduction (Redox)
D. Neutralization
11
811Q13. Calculate the oxidation number of sulphur in H.So, and Na SO4
A
TO
11
812The oxidation number of Phosphorus in
( M g_{2} P_{2} O_{7} ) is:
( A cdot+3 )
( B .+2 )
( c cdot+5 )
( D cdot-3 )
11
813If true enter 1 , else enter 0 .
Following reaction is disproportionation
reaction:
( N H_{4}^{+}+N O_{3}^{-} longrightarrow N_{2} O+2 H_{2} O )
( A )
11
814Balance the following equations in acidic medium by both oxidation number and ion electron methods and
identify the oxidants and the
reductants :
( M n O_{4}^{-}(a q)+C_{2} H_{2} O_{4}(a q) rightarrow )
( M n^{2+}(a q)+C O_{2}(g)+H_{2} O(l) )
11
815What is the oxidation state of chlorine
in hypochlorous acid?
( A cdot+1 )
B. +3
( c .+5 )
( D cdot+7 )
11
816Which of the following pairs of elements show similar set of oxidation state?
A. ( O^{16}, O^{18} )
в. ( N a, K )
c. ( C, B e )
D. ( Z n, R b )
11
817If a substance gains oxygen during a reaction, it is being oxidized. If it loses oxygen, it is being reduced. Oxidation and Reduction always take place together, so that if one substance is oxidized, another is reduced. Using this idea, say which substance is oxidised and which substance is reduced in each
reaction
¡) ( M g+O_{2} rightarrow 2 M g O )
( (s) )
( (s) )
ii) ( Z n O+C rightarrow Z n+C O )
iii) ( F e_{2} O_{3}+3 C O rightarrow 2 F e+3 C O_{2} )
iv) ( C r_{2} O_{3}+2 A l rightarrow 2 C r+A l_{2} O_{3} )
11
818In balancing the half reaction:
( S_{2} O_{3}^{2-} rightarrow S(s), ) the number of electrons
that must be added is :
A. 2 on the right
B. 2 on the left
c. 3 on the right
D. 4 on the left
11
819The oxidation number of sulphur in the
sulphur molecule ( left(S_{8}right) ) is :
11
820All combustion reactions are oxidation-
reduction reactions.
If true enter 1 , else enter 0 .
( A )
11
821Which of the statements about the
reaction below are incorrect?
( 2 P b O(s)+C(s) rightarrow 2 P b(s)+C O_{2}(g) )
(a) Lead is getting reduced.
(b) Carbon dioxide is getting oxidised
(c) Carbon is getting oxidised.
(d) Lead oxide is getting reduced
A ( cdot(a) ) and ( (b) )
B. (a) and (c)
( c cdot(a),(b) ) and ( (c) )
D. All
11
822is not
1.
Multip
Column I
Column II
A. C+02 → CO2 +heat (p) Exothermic
B. CaCO, A + CaO +CO, (q) Combination
CN2+O2 → 2NO
(r) Endothermic
D. HCI+NH,OH →
(s) Decomposition
NH,C1+H,O+12.3kJ.
heat
not
on
11
823Explain daniel cell with cell diagram, representation and process taking place in the cell.11
8247. The oxidation number of carbon is zero in
(a) HCHO (b) CH.CI, (c)
(e) all of the above
H₂O,
(d) CH2
11
825The reaction used to join railway tracks involves reducing agent:
( A cdot A )
в. Мв
( c cdot c )
D. co
11
826Formation of ( S O_{3} ) from ( S O_{2} ) and ( O_{2} ) is a
reaction.
11
827Q20. Write four informations about the reaction:
(CN),(8) + 2OH(aq) CN (aq) + CNO (aq) + H2O(l)
11
828How much electric charge is required to oxidise:
(a) 1 mole of ( H_{2} O ) to ( O_{2} ) and
(b) 1 mole of ( F e O ) to ( F e_{2} O_{3} )
11
829( boldsymbol{C u O}(boldsymbol{s})+boldsymbol{H}_{2}(boldsymbol{g}) rightarrow boldsymbol{C u}(boldsymbol{s})+boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) )
In this reaction, is reduced.
A. copper oxide
B. copper
c. hydrogen
D. water
11
830The no. of cells which may be
constructed with different ( E_{c e l l}^{o} ) values
for the reaction
( boldsymbol{F} boldsymbol{e}+boldsymbol{2} boldsymbol{F} boldsymbol{e}^{boldsymbol{3}+} rightarrow boldsymbol{3} boldsymbol{F} boldsymbol{e}^{2+} boldsymbol{i} boldsymbol{s} )
11
831UU
5. The oxidation number of the carboxylic carbon atom in CH,COOH is
(a) +2
(6) + 4
(c) +1
(d) +3
11
832The ( C l^{-} ) ion is formed, when ( ^{prime} C l^{prime} ) atom
loses an electron.
A. True
B. False
11
833Which of the following reactions is not oxidation-reduction reaction?
( mathbf{A} cdot H oplus+O H^{ominus} rightarrow H_{2} O )
B ( cdot frac{1}{2} H_{2}+frac{1}{2} C l_{2} rightarrow H C l )
( mathrm{c} cdot mathrm{CaCO}_{3} rightarrow mathrm{CaO}+mathrm{CO}_{2} )
D. ( A ) and ( C )
11
834What is redox reaction? Explain with one example.11
835Balance the following equations:
( boldsymbol{C r}_{2} boldsymbol{O}_{7}^{2-}+boldsymbol{I}^{-}+boldsymbol{H}^{+} rightarrow boldsymbol{C r}^{3+}+boldsymbol{I}_{2}+ )
( H_{2} O )
( mathbf{A} cdot C r_{2} O_{7}^{2-}+6 I^{-}+14 H^{+} rightarrow 2 C r^{3+}+3 I_{2}+7 H_{2} O )
B. ( C r_{2} O_{7}^{2-}+I^{-}+14 H^{+} rightarrow 2 C r^{3+}+3 I_{2}+7 H_{2} O )
( mathbf{c} cdot C r_{2} O_{7}^{2-}+6 I^{-}+7 H^{+} rightarrow 2 C r^{3+}+I_{2}+7 H_{2} O )
D. None of these
11
836Select the strongest oxidant oxoanion and weakest oxidant oxanion among
the following:
( boldsymbol{V} boldsymbol{O}_{4}^{3-}, boldsymbol{C r} boldsymbol{O}_{4}^{2-}, boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{2-}, boldsymbol{F} boldsymbol{e} boldsymbol{O}_{4}^{2-} )
A. Strongest: ( F e O_{4}^{2-} ; ) weakest ( : V O_{4}^{3} )
B. Strongest: ( V O_{4}^{3-} ); weakest: ( F e O_{4}^{2} )
c. Both are equally strong
D. None of these
11
837In the reaction ( rightarrow )
( M N O_{2}+4 H C L rightarrow M n C l_{2}+ )
( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}+boldsymbol{C} boldsymbol{l}_{2} )
(a) name the compound (i) oxidised
(ii) reduced
(b) define oxidation of reduction on its
basis.
11
838Oxidation number and covalency of
sulphur in ( S_{8} ) molecule respectively are
( mathbf{A} cdot 6 & 8 )
B. ( 0 & 8 )
c. ( 0 & 2 )
D. ( 6 & 2 )
11
839In a conjugate pair of reductant and oxidant, the reductant has:
A. lower ox. no
B. higher ox. no
( c . ) same ox. no
D. either of these
11
840Fill up the table from the given choice.
Element Oxidation number
-2 in most compounds
(i) in Oxygen ( quad H_{2} O_{2} ) and
(ii) in ( O F_{2} )
Halogen
– 1 for
(iii) in all its compounds
(iv) in most of its compounds Hydrogen
(v)in binary metallic hydrides
Sulphur
(vi) in all sulphides
( mathbf{A} cdot(i)+1(i i)+1(i i i) C l(i v)+1(v)-1(v i)+2 )
B. ( (i)-1(i i)+2(i i i) F(i v)+1(v)-1(v i)-2 )
( mathbf{c} cdot(i)-1(i i)+1(i i i) F(i v)+1(v)+2(v i)+2 )
D. ( (i)+1(i i)+2(i i i) C l(i v)+1(v)+1(v i)+6 )
11
841The value of ( ^{prime} n^{prime} ) in the reaction is:
( boldsymbol{C r}_{2} boldsymbol{O}_{mathbf{7}}^{2-}+mathbf{1 4} boldsymbol{H}^{+}++boldsymbol{n} boldsymbol{F} boldsymbol{e}^{2+} rightarrow )
( 2 C r^{3+}+n F e^{3+}+7 H_{2} O )
( A cdot 2 )
B. 3
( c cdot 6 )
D.
11
8421113
ICU (113)41 04
4
9. Which one among the following is not example of autoredox reaction
(a) P, + OHH , PO, + PH, (b) H,
O H ,O + O2
(c) S, 0,2- 0,2 +S
(d) AgCI + NH, Āg (NH3)2] CI
10
11
843Which of the these are
disproportionation reactions?
I. ( 2 mathrm{C}_{6} mathrm{H}_{5} mathrm{CHO}-^{mathrm{A}left(mathrm{CC}_{2} mathrm{H}_{5}right)_{3}} mathrm{C}_{6} mathrm{H}_{5} mathrm{COOCH}_{2} mathrm{C}_{6} mathrm{H}_{5} )
III. ( mathrm{Cl}_{2}+2 mathrm{OH}^{-} longrightarrow mathrm{Cl}^{-}+mathrm{ClO}^{-}+mathrm{H}_{2} mathrm{O} )
IV. ( 2 mathrm{KClO}_{3} longrightarrow 2 mathrm{KCl}+3 mathrm{O}_{2} )
( mathbf{A} cdot ) ।, ॥।, ॥ ॥
в. ॥, IV
c. ॥, ॥ा, । v
D. I, IV
11
844Which of the following reaction
equation is wrongly labeled?
( mathbf{A} cdot F e+C r^{3+} rightarrow F e^{3+}+C r(r e d o x) )
B ( cdot K B r+H_{2} O rightarrow H B r+K O H ) (hydrolysis)
( mathbf{c} cdot C H_{4}+2 O_{2} rightarrow C O_{2}+2 H_{2} O ) (combustion)
D. ( C H_{4}+C l_{2} rightarrow C H_{3} C l+H C l ) (addition)
E ( cdot C O_{2}+H_{2} O rightarrow H_{2} C O_{3} ) (synthesis)
11
845Find the oxidation number of elements
in each case.
( O ) in ( O_{2}, O_{3}, O F_{2} ) and ( B a O_{2} )
в. 0,0,+2,+1
c. 0,0,+1,0
D. None of the above
11
846Enzyme catalysed reaction of ( boldsymbol{H}_{2} boldsymbol{O}_{2} ) is a disproportionation redox process. If true enter 1 , else enter 0 .
( A )
11
847Permanganate ion reacts with bromide
ion in basic medium to give
magnesium dioxide and bromate ion.Write the balanced ionic equation
for the reaction.
11
848Write balanced redox reactions of the
following:
4 moles of ( S n^{2+}(a q) ) reduces ( I O_{4}^{-} ) to
( boldsymbol{I}^{-}(boldsymbol{a} boldsymbol{q}) )
A ( cdot 4 S n^{2+}+I O_{4}^{-}+8 H^{+} rightarrow 6 S n^{4+}+I^{-}+4 H_{2} O )
B . ( 4 S n^{2+}+I O_{8}^{-}+8 H^{+} rightarrow 4 S n^{4+}+I^{-}+4 H_{2} O )
c. ( 4 S n^{2+}+I O_{4}^{-}+8 H^{+} longrightarrow 4 S n^{4+}+I^{-}+4 H_{2} O )
D. none of these
11
849heat
Column I
A. C+0, → CO,
B. H2S+ Cl2 → 2HCI + S
C. 12+H2S → 2HI + S
D. H2 + Cl2 → 2HC1
Column II
(p) Displacement
(q) Oxidation
(r) Combination
(s) Reduction
11
850Determine the. oxidation state of
chromium in the finfll product formed by the reaction between KI and acidified potassium dichromate solution.
( A cdot+3 )
( B .+2 )
( c cdot+1 )
( D ldots-3 )
11
851Which of the reactants act as oxidant or
reductant if any:
( 2 C u S O_{4}+S O_{2}+2 K B r+2 H_{2} O rightarrow )
( 2 C u B r+2 H_{2} S O_{4}+K_{2} S O_{4} )
A ( . C u S O_{4} )
в. ( S O_{2} )
c. Both of these
D. None of these
11
852Indicate in each reaction which one is
oxidised or reduced if any:
( mathbf{2} N boldsymbol{a}_{2} boldsymbol{S}+mathbf{4} boldsymbol{H} boldsymbol{C l}+boldsymbol{S} boldsymbol{O}_{3} rightarrow mathbf{4} boldsymbol{N} boldsymbol{a} boldsymbol{C l}+ )
( 3 S+2 H_{2} O )
In the above reaction, which one of the following is oxidised?
A ( cdot N a_{2} S )
в. ( H C l )
c. ( N a C l )
D. None of these
11
853( boldsymbol{C N}^{-} longrightarrow boldsymbol{C N O}^{-} )
The number of electrons that must be
added in balancing the half reaction is:
( mathbf{A} cdot mathbf{0} )
B. 1 on the right
c. 1 on the left
D. 2 on the right
11
854Latha dropped some crystals of
( K M n O_{4} ) in a beaker of water and
observing to know what happens.What
is the phenomenon that occurs in the experiment?
11
855Balance the following equation.
( boldsymbol{F} boldsymbol{e} boldsymbol{S}_{2}+boldsymbol{O}_{2} rightarrow boldsymbol{F} boldsymbol{e}_{2} boldsymbol{O}_{3}+boldsymbol{S} boldsymbol{O}_{2} )
11
856Determine the standard reduction
potential for the half reaction.
[
boldsymbol{C l}_{2}+mathbf{2} e^{-} rightarrow mathbf{2} boldsymbol{C l}^{-}
]
Given: ( boldsymbol{P t}^{2+}+mathbf{2} boldsymbol{C l}^{-} rightarrow boldsymbol{P t}+ )
[
begin{array}{l}
boldsymbol{C l}_{2}, boldsymbol{E}_{c e l l}=-mathbf{0 . 1 5} boldsymbol{V} \
boldsymbol{P t}^{2+}+boldsymbol{2} e^{-} rightarrow boldsymbol{P t}, boldsymbol{E}=1.20 boldsymbol{V}
end{array}
]
11
857Using electron-transfer concept, identify the oxidant and reductant in
the following redox reactions.
(a) ( Z n(s)+2 H^{+}(a q) longrightarrow )
( Z n^{2+}(a q)+H_{2}(g) )
(b) ( 2left[F e(C N)_{6}right]^{3-}(a q)+2 O H^{-}(a q)+ )
( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2}left[boldsymbol{F} e(boldsymbol{C} boldsymbol{N})_{6}right]^{4-}(boldsymbol{a} boldsymbol{q})+ )
( mathbf{2} boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) )
(c) ( 2left[F e(C N)_{6}right]^{3-}(a q)+2 O H^{-}(a q)+ )
( boldsymbol{H}_{2} boldsymbol{O}_{2}(boldsymbol{a} boldsymbol{q}) rightarrow boldsymbol{2}left[boldsymbol{F} boldsymbol{e}(boldsymbol{C} boldsymbol{N})_{boldsymbol{6}}right]^{4-}(boldsymbol{a} boldsymbol{q})+ )
( boldsymbol{O}_{2}(boldsymbol{g})+boldsymbol{2} boldsymbol{H}_{2} boldsymbol{O}(l) )
11
858An excess of ( A g N O_{3} ) is added to
( 100 m L ) of a ( 0.01 M ) solution of
dichlorotetraaquachromium (III) chloride. The number of moles of ( A g C l ) precipitated would be:
A. 0.001
B. 0.002
c. 0.003
D. 0.01
11
859Which of the reactants act as oxidant or
reductant if any:
( 2 I^{-}+H_{2} O_{2} rightarrow 2 O H^{-}+I_{2} )
( mathbf{A} cdot H_{2} O_{2} )
B . ( I^{-} )
c. Both of these
D. None of these
11
860The species that undergo(es) disproportionation in alkaline medium is/are:
This question has multiple correct options
A ( cdot C l_{2} )
B . ( M n O_{4}^{2} )
( c cdot N O_{2} )
D. ( C l O_{4}^{-} )
11
861In which of the following, iron is present
in its lowest oxidation state?
A ( cdot ) FeSO( _{4} cdot 7 mathrm{H}_{2} ) O
в. ( F e(C O)_{5} )
( mathrm{c} . F e_{e, 94} mathrm{O} )
D. ( F e_{3} O_{4} )
11
862In the reaction: ( boldsymbol{I}_{2}+2 boldsymbol{S}_{2} boldsymbol{O}_{3}^{2-} rightarrow boldsymbol{2} boldsymbol{I}^{-}+ )
( boldsymbol{S}_{4} boldsymbol{O}_{6}^{2-} )
A ( cdot I_{2} ) is a reducing agent
B . ( I_{2} ) is an oxidising agent
c. ( S_{2} O_{3}^{2-} ) is a reducing agent
D. ( S_{2} O_{3}^{2-} ) is an oxidising agent
11
863For the redox reaction:
( boldsymbol{x} boldsymbol{M} boldsymbol{n} boldsymbol{O}_{4}^{-}+boldsymbol{y} boldsymbol{H}_{2} boldsymbol{C}_{2} boldsymbol{O}_{4}+boldsymbol{z} boldsymbol{H}^{+} rightarrow )
( boldsymbol{m} boldsymbol{M} boldsymbol{n}^{2+}+boldsymbol{n} boldsymbol{C} boldsymbol{O}_{2}+boldsymbol{p} boldsymbol{H}_{2} boldsymbol{O} )
The values of ( x, y, m ) and ( n ) are:
A. 10,2,5,2
В. 2,5,2,10
c. 6,4,2,5
D. 3,5,2,10
11
864( boldsymbol{C}_{4} boldsymbol{H}_{10}(boldsymbol{g})+boldsymbol{O}_{2}(boldsymbol{g}) rightarrow boldsymbol{C} boldsymbol{O}_{2}(boldsymbol{g})+ )
( boldsymbol{H}_{2} boldsymbol{O}(boldsymbol{l}) )
Find the coefficient of ( C O_{2} ), when the
above equation is balanced using the lowest whole-number terms?
( A cdot 4 )
B. 2
( c cdot 13 )
D. 10
E. 8
11
865Many grain products, including cereals and others that identify themselves as a ‘source of iron’ list something called reduced iron’ among the ingredients. To which of the following would the term reduced iron’ most likely be referring?
A. Compounds containing iron (III) ions
B. Compounds containing iron (II) ions
c. Iron metal
D. oxides of iron
11
866Calculate the oxidation number of the
underlined elements.
a. ( underline{P H}_{3} )
b. ( underline{S} O_{2} )
( boldsymbol{H} underline{boldsymbol{N}} boldsymbol{O}_{3} )
d. ( boldsymbol{H}_{3} underline{boldsymbol{P}} boldsymbol{O}_{mathbf{4}} )
( begin{array}{llll}text { A. } text { a. }-3 ; & text { b. }+4 ; & text { c. }+5 ;end{array} ) +5
В. а. ( -3 ; quad ) b. ( +2 ; quad ) с. ( +5 ; )
d. +5
c. a. ( -3 ; ) b. +4
c. +5 +4
D. None of these
11
867Which statement below is
incorrect regarding balanced
equations?
A. ( C+O_{2} rightarrow C O_{2} ) is balanced and is a synthesis reaction
B. ( C a C O_{3} rightarrow C a O+C O_{2} ) is balanced and is a
decomposition reaction
C ( . N a+C l_{2} rightarrow N a C l ) is not balanced but demonstrates a
synthesis reaction
D. ( K I+P bleft(N O_{3}right)_{2} rightarrow P b I_{2}+K N O_{3} ) is balanced and is a
single replacement reaction
E ( cdot 2 H_{2} O rightarrow 2 H_{2}+O_{2} ) is balanced and demonstrates a
redox reaction
11
868Hydrochloric acid solution ( A ) and ( B ) have a concentration of ( 0.5 N ) and ( 0.1 N )
respectively. The volume of solutions ( boldsymbol{A} )
and ( B ) required to make 2 litres of
( mathbf{0 . 2} mathbf{N} mathbf{H} mathbf{C l} ) are:
A. 0.5 Lof ( A+1.5 ) Lof ( B )
B. 1.5 Lof ( A+0.5 ) Lof ( B )
c. 1.0 Lof ( A+1.0 ) Lof ( B )
D. 0.75 Lof ( A+1.25 ) Lof ( B )
11
869Q5. What is the oxidation state of Ni in Ni (CO) ?11

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