Nernst Equation and its Applications NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Nernst Equation and its Applications MCQ Questions


1.
The Nernst equation for a general electrode reaction Mⁿ⁺ + ne⁻ → M at 298 K (using log) is:
A.
E = E° + (0.0591/n) log [Mⁿ⁺]
B.
E = E° − (0.0591/n) log (1/[Mⁿ⁺])
C.
E = E° + (RT/nF) ln (1/[Mⁿ⁺])
D.
E = E° − (0.0591/n) log [Mⁿ⁺]
😑 View Answer Rough Work Error
ANSWER :
B. E = E° − (0.0591/n) log (1/[Mⁿ⁺])
2.
The Nernst equation at 298 K for the cell reaction with reaction quotient Q is:
A.
E_cell = E°_cell + (0.0591/n) log Q
B.
E_cell = E°_cell × log Q
C.
E_cell = E°_cell − (0.0591/n) ln Q
D.
E_cell = E°_cell − (0.0591/n) log Q
😑 View Answer Rough Work Error
ANSWER :
D. E_cell = E°_cell − (0.0591/n) log Q
3.
The factor 0.0591 V in the Nernst equation arises from:
A.
F/RT at 298 K
B.
(RT/F) × 2.303 at 298 K
C.
RT/F at 298 K
D.
RT/F at 273 K
😑 View Answer Rough Work Error
ANSWER :
B. (RT/F) × 2.303 at 298 K
4.
In the Nernst equation E_cell = E°_cell − (0.0591/n) log Q, 'n' represents:
A.
Number of moles of electrolyte
B.
Avogadro's number
C.
Number of electrons transferred in the balanced cell reaction
D.
Number of ions in solution
😑 View Answer Rough Work Error
ANSWER :
C. Number of electrons transferred in the balanced cell reaction
5.
The Nernst equation in the form E = E° − (RT/nF) ln Q is valid:
A.
Only at equilibrium
B.
At any temperature
C.
Only at 298 K
D.
Only for standard conditions
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ANSWER :
B. At any temperature
6.
For the Daniell cell Zn|Zn²⁺(aq)||Cu²⁺(aq)|Cu, the Nernst equation at 298 K is:
A.
E_cell = E°_cell − (0.0591/2) log {[Zn²⁺]/[Cu²⁺]}
B.
E_cell = E°_cell + (0.0591/2) log {[Zn²⁺]/[Cu²⁺]}
C.
E_cell = E°_cell − (0.0591/2) log {[Cu²⁺]/[Zn²⁺]}
D.
E_cell = E°_cell − (0.0591) log {[Zn²⁺]/[Cu²⁺]}
😑 View Answer Rough Work Error
ANSWER :
A. E_cell = E°_cell − (0.0591/2) log {[Zn²⁺]/[Cu²⁺]}