Electrochemical Cells (Electrolytic and Galvanic Cells, Different Types of Electrodes,...) NEET Questions

Physical Chemistry - Redox Reactions and Electrochemistry

Electrochemical Cells (Electrolytic and Galvanic Cells, Different Types of Electrodes,...) MCQ Questions


13.
The cell potential of a galvanic cell becomes zero when:
A.
The salt bridge is removed
B.
The cell reaches equilibrium
C.
Pure metals are used as electrodes
D.
The cell is opened in an open circuit
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ANSWER :
B. The cell reaches equilibrium
14.
Which type of electrode is the SHE classified as?
A.
Metal-insoluble salt electrode
B.
Gas electrode
C.
Metal-metal ion electrode
D.
Redox electrode
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ANSWER :
B. Gas electrode
15.
An example of a metal-metal insoluble salt-anion electrode is:
A.
Calomel electrode (Hg | Hg₂Cl₂ | Cl⁻)
B.
Pt | Fe²⁺, Fe³⁺ electrode
C.
Zinc electrode (Zn | Zn²⁺)
D.
Standard hydrogen electrode (Pt, H₂ | H⁺)
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ANSWER :
A. Calomel electrode (Hg | Hg₂Cl₂ | Cl⁻)
16.
The Nernst equation for a half-cell M^n+ + ne⁻ → M at 298 K is:
A.
E = E° + 0.0591 × n × log [M^n+]
B.
E = E° − (0.0591/n) log [M^n+]
C.
E = E° − (0.0591/n) log (1/[M^n+])
D.
E = E° + (0.0591/n) log (1/[M^n+])
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ANSWER :
C. E = E° − (0.0591/n) log (1/[M^n+])
17.
For the cell reaction: Zn + Cu²⁺ → Zn²⁺ + 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 × log ([Zn²⁺]/[Cu²⁺])
D.
E(cell) = E°(cell) − (0.0591/2) log ([Cu²⁺]/[Zn²⁺])
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ANSWER :
B. E(cell) = E°(cell) − (0.0591/2) log ([Zn²⁺]/[Cu²⁺])
18.
The relationship between standard cell potential E°(cell) and equilibrium constant K at 298 K is:
A.
log K = E°cell × n × 0.0591
B.
log K = (0.0591 × E°cell)/n
C.
log K = (n × E°cell)/0.0591
D.
ln K = E°cell × n/0.0591
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ANSWER :
C. log K = (n × E°cell)/0.0591