Relationship between Cell Potential and Gibbs Energy Change NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Relationship between Cell Potential and Gibbs Energy Change MCQ Questions


7.
If a cell reaction has ΔG° > 0, then E°_cell is:
A.
Equal to nF
B.
Negative
C.
Zero
D.
Positive
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ANSWER :
B. Negative
8.
A cell reaction is spontaneous if:
A.
E°_cell < 0 and ΔG° > 0
B.
E°_cell > 0 and ΔG° < 0
C.
E°_cell > 0 and ΔG° > 0
D.
E°_cell = 0 and ΔG° = 0
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ANSWER :
B. E°_cell > 0 and ΔG° < 0
9.
The cell reaction at equilibrium is characterised by:
A.
ΔG > 0, E_cell > 0
B.
ΔG = 0, E_cell = 0
C.
ΔG < 0, E_cell > 0
D.
ΔG° = 0, E°_cell = 0
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ANSWER :
B. ΔG = 0, E_cell = 0
10.
For a cell reaction with E°_cell = 1.10 V and n = 2, ΔG° at 298 K is approximately:
A.
−212 kJ mol⁻¹
B.
+212 kJ mol⁻¹
C.
−424 kJ mol⁻¹
D.
−106 kJ mol⁻¹
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ANSWER :
A. −212 kJ mol⁻¹
11.
If E°_cell = 0.34 V for Cu²⁺/Cu vs SHE (n = 2), the standard Gibbs energy change for Cu²⁺ + H₂ → Cu + 2H⁺ is approximately:
A.
+65.6 kJ mol⁻¹
B.
−131.2 kJ mol⁻¹
C.
−65.6 kJ mol⁻¹
D.
−32.8 kJ mol⁻¹
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ANSWER :
C. −65.6 kJ mol⁻¹
12.
Given Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s) with E°_cell = 1.56 V, ΔG° at 298 K is approximately:
A.
+301 kJ mol⁻¹
B.
−602 kJ mol⁻¹
C.
−151 kJ mol⁻¹
D.
−301 kJ mol⁻¹
😑 View Answer Rough Work Error
ANSWER :
D. −301 kJ mol⁻¹