Nernst Equation and its Applications NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Nernst Equation and its Applications MCQ Questions


13.
The standard Gibbs energy change ΔG° is related to E°_cell by:
A.
ΔG° = nE°_cell/F
B.
ΔG° = −F E°_cell/n
C.
ΔG° = −nFE°_cell
D.
ΔG° = nFE°_cell
😑 View Answer Rough Work Error
ANSWER :
C. ΔG° = −nFE°_cell
14.
ΔG° is related to equilibrium constant K by:
A.
ΔG° = −RT ln K
B.
ΔG° = nF/ln K
C.
ΔG° = −RT/ln K
D.
ΔG° = RT ln K
😑 View Answer Rough Work Error
ANSWER :
A. ΔG° = −RT ln K
15.
For a cell reaction with E°_cell = 0.0591 V and n = 1 at 298 K, K equals:
A.
100
B.
0.1
C.
10
D.
1
😑 View Answer Rough Work Error
ANSWER :
C. 10
16.
A concentration cell consists of:
A.
Two different electrodes in the same electrolyte
B.
Two electrodes in molten salt
C.
Two different electrodes in different electrolytes
D.
Two identical electrodes dipped in solutions of the same electrolyte at different concentrations
😑 View Answer Rough Work Error
ANSWER :
D. Two identical electrodes dipped in solutions of the same electrolyte at different concentrations
17.
For a Cu | Cu²⁺ (c₁) || Cu²⁺ (c₂) | Cu concentration cell at 298 K, the EMF is:
A.
E_cell = E°_cell + (0.0591/2) log (c₂/c₁)
B.
E_cell = (0.0591/2) log (c₁/c₂)
C.
E_cell = (0.0591/2) log (c₂/c₁)
D.
E_cell = (0.0591) log (c₂/c₁)
😑 View Answer Rough Work Error
ANSWER :
C. E_cell = (0.0591/2) log (c₂/c₁)
18.
In a Cu concentration cell with c_cathode = 1.0 M and c_anode = 0.01 M Cu²⁺ at 298 K, the EMF is approximately:
A.
0.0296 V
B.
0.0591 V
C.
0.118 V
D.
0.0886 V
😑 View Answer Rough Work Error
ANSWER :
B. 0.0591 V