Redox Reactions Test

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Redox Reactions Test - 5

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Weekly Quiz Competition

Question 1
1 / -0

All combustion reactions, which make use of elemental dioxygen, as well as other reactions involving elements other than dioxygen are

A
disproportionation reactions

B
displacement reactions

C
decomposition reactions

D
Combination reaction

Solution

A combination reaction (also known as a synthesis reaction) is a reaction where two or more elements or compounds (reactants) combine to form a single compound (product). Such reactions may be represented by equations of the following form: X + Y → XY.
Question 2
1 / -0

In the reaction HAsO₂ + Sn²⁺ As + Sn⁴⁺ + H₂O, the oxidising agent is

A
Sn²⁺

B
Sn⁴⁺

C
As

D
HAsO₂
Question 3
1 / -0

Acidified KMnO₄ oxidises oxalic acid to CO₂. What volume (in litres) of 10^-4 M KMnO₄ is required to completely oxidise 0.5 L of 10^-2 M oxalic acid in acidic medium?

A
125

B
1250

C
200

D
20
Question 4
1 / -0

The standard values of A, B and C are +0.68 V, -2.54 V and -0.50 V, respectively. Which of the following statements is correct in context to the given data?

A
C can be reduced by both A and B.

B
A is the strongest reducing agent.

C
B can be reduced by A, but not by C.

D
B can be oxidised by both A and C.
Question 5
1 / -0

Which of the following reactions involves both oxidation and reduction?

A
NaBr + HCl NaCl + HBr

B
HBr + AgNO₃ AgBr + HNO₃

C
H₂ + Br₂ 2HBr

D
Na₂O + H₂SO₄ Na₂SO₄ + H₂O
Question 6
1 / -0

The oxidation number of oxygen in most compounds is

A
4

B
1

C
-2

D
-3

Solution

Oxygen is the most electronegative element. Oxygen have 6 electrons in its outermost shell and to gain noble gas configuration oxygen have to take 2 more electrons.
Question 7
1 / -0

Equivalent mass of oxidising agent in the reaction SO₂ + 2H₂S 3S + 2H₂O is

A
32 g

B
64 g

C
16 g

D
8 g
Question 8
1 / -0

The highest value of oxidation number changes from 1 to 7

A
In alkaline earth metals

B
the first three groups

C
across the third period in the periodic table

D
in the atoms of transition elements

Solution

The highest value of oxidation number exhibited by an atom of an element generally increases across the period in the periodic table.
Question 9
1 / -0

For Zn²⁺/Zn = - 0.76 V, Cl₂/Cl^- = 1.36 V, H⁺/1/2H₂ = 0 V and Fe³⁺/Fe²⁺ = 0.77 V, the increasing order of strengths as a reducing agent is

A
Cl^-, Zn, H₂, Fe³⁺

B
H₂, Zn, Fe³⁺, Cl^-

C
Cl^-, Fe³⁺, Zn, H₂

D
Cl^-, Fe³⁺, H₂, Zn
Question 10
1 / -0

_{^{Consider the reaction between potassium permanganate and a metal sulphite represented as follows.}}

Which of the following options about the process is correct?

A
1 mole of potassium permanganate oxidises 5 moles of the metal sulphite.

B
There is a net transfer of 5 electrons in the reaction.

C
20 mL of 0.5M KMnO₄ solution can neutralise 10 mL of 0.25 M metal sulphite.

D
50 mL of KMnO₄ can oxidise a 20 mL equimolar solution of the metal sulphite.
Question 11
1 / -0

The oxidation number of sulphur in H₂S₂O₈ is

A
+ 6

B
+ 8

C
+ 2

D
+ 7
Question 12
1 / -0

The oxidation number of phosphorus in HP₂O₇⁻ ion is

A
+ 3

B
+ 5

C
+ 6

D
+ 7
Question 13
1 / -0

KMnO₄ is a strong oxidising agent in the acidic medium. To provide acidic medium, H₂SO₄ is used instead of HCl. This is because

A
H₂SO₄ is a stronger acid than HCl

B
HCl is oxidised by KMnO₄ to Cl₂

C
H₂SO₄ is a dibasic acid

D
rate of reaction is faster in the presence of H₂SO₄
Question 14
1 / -0

What would happen when a small quantity of H₂O₂ is added to a solution of FeSO₄?

A
An electron is gained by Fe²⁺.

B
An electron is lost by Fe²⁺.

C
The colour disappears.

D
H₂ is evolved.
Question 15
1 / -0

Formation of coloured solution is possible when metal ion in the compound contains

A
unpaired electrons

B
lone pair of electrons

C
negative ionic state

D
paired electrons

Solution

Color in complex arises due to the presence of unpaired electrons in the system when complex reaction takes place.
Question 16
1 / -0

The standard reduction potentials of Fe⁺²/Fe and Cu⁺²/Cu electrodes are -0.44 and 0.34 volts, respectively.
Which of the following statements is true?

A
Copper will reduce Fe⁺² ions.

B
Iron will reduce Cu²⁺ ions.

C
Iron will oxidise copper metal.

D
Cu⁺² ions will reduce Fe⁺² ions.
Question 17
1 / -0

The oxidation potential values of A, B, C and D are -0.03 V, +0.108 V, -0.07 V and +0.1 V, respectively. The non-spontaneous cell reaction takes place between

A
A (anode) and B (cathode)

B
B (anode) and D (cathode)

C
D (anode) and A (cathode)

D
B (anode) and C (cathode)

E
A (anode) and C (cathode)
Question 18
1 / -0

In which of the following reactions does H₂O₂ act as a reducing agent?

A
2FeCl₂ + 2HCl + H₂O₂ → 2FeCl₃ + 2H₂O

B
Cl₂ + H₂O₂ → 2HCl + O₂

C
2Hl + H₂O₂ → 2H₂O + l₂

D
H₂SO₃ + H₂O₂ → H₂SO₄ + H₂O
Question 19
1 / -0

The E^oM³⁺/M²⁺values for Cr, Mn, Fe and Co are -0.41, +1.57, +0.77 and +1.97 V, respectively. For which of these metals is the change in oxidation state from +2 to +3 the easiest?

A
Cr

B
Mn

C
Fe

D
Co
Question 20
1 / -0

Aurous chloride and auric chloride are written as Au(l)Cl and Au(lll)Cl₃.The roman numeral in parenthesis after the symbol of the metal in the molecular formula represents the

A
basic character

B
oxidation number

C
electronegativity

D
Ionic state

Solution

The roman number represents the oxidation number/oxidation state of an element.It is popularly known as Stock notation given by the german scientist Alfred stock.

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Redox Reactions Test - 5

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Redox Reactions Test - 5

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Question 1

disproportionation reactions

displacement reactions

decomposition reactions

Combination reaction

Solution

Question 2

Sn2+

Sn4+

As

HAsO2

Question 3

125

1250

200

20

Question 4

C can be reduced by both A and B.

A is the strongest reducing agent.

B can be reduced by A, but not by C.

B can be oxidised by both A and C.

Question 5

NaBr + HCl NaCl + HBr

HBr + AgNO3 AgBr + HNO3

H2 + Br2 2HBr

Na2O + H2SO4 Na2SO4 + H2O

Question 6

4

1

-2

-3

Solution

Question 7

32 g

64 g

16 g

8 g

Question 8

In alkaline earth metals

the first three groups

across the third period in the periodic table

in the atoms of transition elements

Solution

Question 9

Cl-, Zn, H2, Fe3+

H2, Zn, Fe3+, Cl-

Cl-, Fe3+, Zn, H2

Cl-, Fe3+, H2, Zn

Question 10

1 mole of potassium permanganate oxidises 5 moles of the metal sulphite.

There is a net transfer of 5 electrons in the reaction.

20 mL of 0.5M KMnO4 solution can neutralise 10 mL of 0.25 M metal sulphite.

50 mL of KMnO4 can oxidise a 20 mL equimolar solution of the metal sulphite.

Question 11

+ 6

+ 8

+ 2

+ 7

Question 12

+ 3

+ 5

+ 6

+ 7

Question 13

H2SO4 is a stronger acid than HCl

HCl is oxidised by KMnO4 to Cl2

H2SO4 is a dibasic acid

rate of reaction is faster in the presence of H2SO4

Question 14

An electron is gained by Fe2+.

An electron is lost by Fe2+.

The colour disappears.

Sn²⁺

Sn⁴⁺

HAsO₂

HBr + AgNO₃ AgBr + HNO₃

H₂ + Br₂ 2HBr

Na₂O + H₂SO₄ Na₂SO₄ + H₂O

Cl^-, Zn, H₂, Fe³⁺

H₂, Zn, Fe³⁺, Cl^-

Cl^-, Fe³⁺, Zn, H₂

Cl^-, Fe³⁺, H₂, Zn

20 mL of 0.5M KMnO₄ solution can neutralise 10 mL of 0.25 M metal sulphite.

50 mL of KMnO₄ can oxidise a 20 mL equimolar solution of the metal sulphite.

H₂SO₄ is a stronger acid than HCl

HCl is oxidised by KMnO₄ to Cl₂

H₂SO₄ is a dibasic acid

rate of reaction is faster in the presence of H₂SO₄

An electron is gained by Fe²⁺.

An electron is lost by Fe²⁺.

H₂ is evolved.

Copper will reduce Fe⁺² ions.

Iron will reduce Cu²⁺ ions.

Cu⁺² ions will reduce Fe⁺² ions.

2FeCl₂ + 2HCl + H₂O₂ → 2FeCl₃ + 2H₂O

Cl₂ + H₂O₂ → 2HCl + O₂

2Hl + H₂O₂ → 2H₂O + l₂

H₂SO₃ + H₂O₂ → H₂SO₄ + H₂O