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,...)

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
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