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


13.
If E°_cell = 0.0591 V and n = 1 at 298 K, ΔG° is approximately:
A.
−0.6 kJ mol⁻¹
B.
−5.7 kJ mol⁻¹
C.
+5.7 kJ mol⁻¹
D.
−11.4 kJ mol⁻¹
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ANSWER :
B. −5.7 kJ mol⁻¹
14.
If ΔG° = −193 kJ mol⁻¹ for a cell reaction with n = 2 at 298 K, E°_cell is approximately:
A.
+2.00 V
B.
+0.50 V
C.
+0.25 V
D.
+1.00 V
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ANSWER :
D. +1.00 V
15.
For a cell with n = 1 and ΔG° = −96.485 kJ mol⁻¹, E°_cell is:
A.
+1.00 V
B.
+1.50 V
C.
+2.00 V
D.
+0.50 V
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ANSWER :
A. +1.00 V
16.
The maximum work that can be obtained from the Daniell cell (E°_cell = 1.10 V, n = 2) per mole of cell reaction is:
A.
−106 kJ
B.
+106 kJ
C.
+212 kJ
D.
−212 kJ
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ANSWER :
C. +212 kJ
17.
The three quantities ΔG°, E°_cell, and K are related by:
A.
ΔG° = −nFE°_cell = +RT ln K
B.
ΔG° = +nFE°_cell = +RT ln K
C.
ΔG° = −nFE°_cell = −RT ln K
D.
ΔG° = −F/E°_cell = −RT ln K
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ANSWER :
C. ΔG° = −nFE°_cell = −RT ln K
18.
The relation between E°_cell and equilibrium constant K at 298 K is:
A.
E°_cell = −(0.0591/n) log K
B.
E°_cell = 0.0591 × n × log K
C.
E°_cell = (0.0591/n) log K
D.
E°_cell = (n/0.0591) log K
😑 View Answer Rough Work Error
ANSWER :
C. E°_cell = (0.0591/n) log K