Electrochemistry Test

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Electrochemistry Test - 2

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following statements is correct?

A
The equivalent conductance of both strong and weak electrolytes decreases with dilution.

B
The equivalent conductance of strong electrolytes increases with dilution, while that of weak electrolytes decreases with dilution.

C
The equivalent conductance of strong electrolytes decreases with dilution, while that of weak electrolytes increases with dilution.

D
The equivalent conductance of both strong and weak electrolytes increases with dilution.
Question 2
1 / -0

The potential of the cell Pt | H₂(g, 1 atm)H⁺ (0.01 M) || OH^–(10^–6 M)|H₂(g, 1 atm)| Pt at 298 K will be

A
– 0.236 V

B
0.236 V

C
– 0.472 V

D
0.472 V
Question 3
1 / -0

A solution is 0.1 M in each of Pb²⁺ and Fe²⁺ ions. If powders of lead and iron are added in this solution, which of the following facts comes out to be true?

A
More of Fe and Pb²⁺ ions are formed.

B
More of Pb and Fe²⁺ ions are formed.

C
Concentrations of Pb²⁺ and Fe²⁺ ions are increased.

D
Concentrations of Pb²⁺ and Fe²⁺ ions are decreased.
Question 4
1 / -0

A cell utilises the reaction Zn (s) + 2H⁺(aq) → Zn ²⁺ (aq) + H₂ (g). Addition of H₂SO₄to the cathode compartment will

A
lower E and shift equilibrium to the left

B
lower E and shift equilibrium to the right

C
increase E and shift equilibrium to the right

D
increase E only
Question 5
1 / -0

Two Faraday of electricity is passed through a solution of CuSO₄. The mass of copper deposited at the cathode is
(Atomic mass of Cu = 63.5 amu)

A
0 g

B
63.5 g

C
2 g

D
127 g
Question 6
1 / -0

The standard free energy change of the reaction Cu²⁺ + Sn(s) → Cu(s) + Sn²⁺ (Given: E° = 0.48 V) is

A
– 31.8 kJmol^–1

B
– 62.1 kJmol^–1

C
– 79.2 kJmol^–1

D
– 92.64 kJmol^–1
Question 7
1 / -0

The unit of conductance is

A
Ω

B
Ω^-1

C
Ω^-1 cm^-1

D
Ω^-1 cm^-2 mol^-1
Question 8
1 / -0

Electrolytic cell uses electrical energy to bring about

A
`spontaneous chemical reactions

B
non-spontaneous chemical reactions

C
spontaneous nuclear reactions

D
non-spontaneous nuclear reactions

Solution

Electrolytic cell drives a non- spontaneous redox chemical reaction by application of electrical energy
Question 9
1 / -0

Resistivity is defined as

A
inverse of resistance

B
inverse of conductance

C
inverse of conductivity

D
inverse cell constant

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Electrochemistry Test - 2

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Electrochemistry Test - 2

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Question 1

The equivalent conductance of both strong and weak electrolytes decreases with dilution.

The equivalent conductance of strong electrolytes increases with dilution, while that of weak electrolytes decreases with dilution.

The equivalent conductance of strong electrolytes decreases with dilution, while that of weak electrolytes increases with dilution.

The equivalent conductance of both strong and weak electrolytes increases with dilution.

Question 2

– 0.236 V

0.236 V

– 0.472 V

0.472 V

Question 3

More of Fe and Pb2+ ions are formed.

More of Pb and Fe2+ ions are formed.

Concentrations of Pb2+ and Fe2+ ions are increased.

Concentrations of Pb2+ and Fe2+ ions are decreased.

Question 4

lower E and shift equilibrium to the left

lower E and shift equilibrium to the right

increase E and shift equilibrium to the right

increase E only

Question 5

0 g

63.5 g

2 g

127 g

Question 6

– 31.8 kJmol–1

– 62.1 kJmol–1

– 79.2 kJmol–1

– 92.64 kJmol–1

Question 7

Ω

Ω-1

Ω-1 cm-1

Ω-1 cm-2 mol-1

Question 8

`spontaneous chemical reactions

non-spontaneous chemical reactions

spontaneous nuclear reactions

non-spontaneous nuclear reactions

Solution

Question 9

inverse of resistance

inverse of conductance

inverse of conductivity

inverse cell constant

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More of Fe and Pb²⁺ ions are formed.

More of Pb and Fe²⁺ ions are formed.

Concentrations of Pb²⁺ and Fe²⁺ ions are increased.

Concentrations of Pb²⁺ and Fe²⁺ ions are decreased.

– 31.8 kJmol^–1

– 62.1 kJmol^–1

– 79.2 kJmol^–1

– 92.64 kJmol^–1

Ω^-1

Ω^-1 cm^-1

Ω^-1 cm^-2 mol^-1