Nernst Equation and its Applications NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Nernst Equation and its Applications MCQ Questions


7.
For the Daniell cell with [Zn²⁺] = 0.1 M and [Cu²⁺] = 1.0 M, E°_cell = 1.10 V. The cell EMF at 298 K is approximately:
A.
1.16 V
B.
1.10 V
C.
1.13 V
D.
1.07 V
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ANSWER :
C. 1.13 V
8.
If [Zn²⁺] = [Cu²⁺] in a Daniell cell, E_cell at 298 K is:
A.
Zero
B.
Less than E°_cell
C.
Greater than E°_cell
D.
Equal to E°_cell
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ANSWER :
D. Equal to E°_cell
9.
In a Daniell cell at 298 K, increasing [Cu²⁺] (other things equal) causes the EMF to:
A.
Remain unchanged
B.
Decrease
C.
Increase
D.
Become zero
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ANSWER :
C. Increase
10.
For the Daniell cell, the EMF becomes zero when:
A.
[Cu²⁺] = 0
B.
[Zn²⁺] = 0
C.
[Zn²⁺]/[Cu²⁺] = K_c (the equilibrium constant)
D.
[Zn²⁺] = [Cu²⁺]
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ANSWER :
C. [Zn²⁺]/[Cu²⁺] = K_c (the equilibrium constant)
11.
The relation between standard cell potential E°_cell and equilibrium constant K at 298 K is:
A.
log K = (0.0591 × n)/E°_cell
B.
log K = (n × E°_cell)/0.0591
C.
log K = (n × 0.0591)/E°_cell
D.
log K = E°_cell/(0.0591 × n)
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ANSWER :
B. log K = (n × E°_cell)/0.0591
12.
For a cell reaction with E°_cell = 0.295 V and n = 2 at 298 K, the equilibrium constant K is approximately:
A.
10¹⁰
B.
10²
C.
10
D.
10⁵
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ANSWER :
A. 10¹⁰