Questions on Standard Cell Potentials
Standard Cell Potentials – Multiple Choice Questions
Questions
1. What does the standard cell potential (E°cell) represent?
A) The amount of charge in a cell
B) The maximum current a cell can provide
C) The voltage of an electrochemical cell under standard conditions
D) The heat released during a redox reaction
E) The resistance of an electrochemical cell
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2. Standard conditions for measuring E°cell include all of the following EXCEPT:
A) 1 M solution concentration
B) 298 K temperature
C) 1 atm pressure for gases
D) Presence of a catalyst
E) Use of a standard hydrogen electrode
3. The E°cell of a voltaic cell is always:
A) Negative
B) Zero
C) Positive
D) Variable
E) Dependent only on temperature
4. Which formula is used to calculate standard cell potential?
A) E°cell = E°oxidation − E°reduction
B) E°cell = E°cathode − E°anode
C) E°cell = I × R
D) E°cell = Q × V
E) E°cell = ΔG / nF
5. A cell has E°cathode = +0.80 V and E°anode = –0.76 V. What is E°cell?
A) +0.04 V
B) –1.56 V
C) +1.56 V
D) –0.04 V
E) 0.00 V
6. A positive E°cell value indicates that the redox reaction is:
A) At equilibrium
B) Spontaneous
C) Nonspontaneous
D) Reversible
E) Exothermic
7. Which of the following half-cells would make the best oxidizing agent?
A) E° = –0.76 V
B) E° = –1.66 V
C) E° = +0.00 V
D) E° = +0.80 V
E) E° = –0.13 V
8. The more positive the E° value of a reduction half-reaction, the:
A) Weaker the oxidizing agent
B) Stronger the reducing agent
C) More favorable the reduction
D) More stable the reactant
E) Lower the voltage
9. Which pair of electrodes would produce the highest E°cell?
A) Cu²⁺/Cu and Zn²⁺/Zn
B) Fe²⁺/Fe and Zn²⁺/Zn
C) Ag⁺/Ag and Mg²⁺/Mg
D) H⁺/H₂ and Ni²⁺/Ni
E) Pb²⁺/Pb and Fe³⁺/Fe²⁺
10. What is the standard potential of the SHE (Standard Hydrogen Electrode)?
A) –1.00 V
B) +1.00 V
C) +0.76 V
D) 0.00 V
E) –0.76 V
11. In a galvanic cell, which half-cell has the higher potential?
A) The anode
B) The cathode
C) The salt bridge
D) The one with the more negative E°
E) The one producing gas
12. Which of the following changes will NOT affect the standard cell potential?
A) Changing temperature to 350 K
B) Increasing reactant concentrations
C) Increasing pressure of gases
D) Using non-standard concentrations
E) Swapping electrodes but keeping half-reactions the same
13. The standard cell potential is related to Gibbs free energy change by which equation?
A) ΔG° = E°cell × T
B) ΔG° = –nFE°cell
C) ΔG° = nFE°cell
D) ΔG° = RT ln K
E) ΔG° = Q/V
14. Which factor determines the spontaneity of a redox reaction in an electrochemical cell?
A) Current
B) Resistance
C) E°cell sign
D) Molarity
E) Salt bridge material
15. The half-cell with the more negative standard reduction potential functions as:
A) The cathode
B) The oxidizing agent
C) The reducing agent
D) The standard reference
E) The salt bridge
16. A voltaic cell with a positive E°cell value will:
A) Not function without external power
B) Spontaneously produce electrical energy
C) Be used in electrolysis
D) Need a catalyst to start
E) Always contain silver
17. When writing a cell diagram, which electrode is written on the left?
A) Cathode
B) Salt bridge
C) Oxidizing agent
D) Anode
E) Hydrogen electrode
18. Which component completes the circuit in a voltaic cell?
A) Electrodes
B) Voltmeter
C) Salt bridge
D) Battery
E) Light bulb
19. If E°cell is negative, the cell reaction is:
A) Spontaneous
B) Reversible
C) Nonspontaneous
D) At equilibrium
E) Electrolytic and galvanic
20. What happens to E°cell if both half-cell potentials increase equally by 0.20 V?
A) E°cell doubles
B) E°cell decreases
C) E°cell remains the same
D) E°cell becomes zero
E) E°cell becomes negative
Answers with Explanations
1. C – E°cell is the voltage under standard conditions.
2. D – Catalysts are not part of standard conditions.
3. C – A positive E°cell indicates a spontaneous voltaic reaction.
4. B – E°cell = E°(cathode) − E°(anode).
5. C – E°cell = 0.80 – (–0.76) = 1.56 V.
6. B – A positive E°cell indicates a spontaneous reaction.
7. D – The most positive reduction potential = best oxidizing agent.
8. C – A higher E° means the reduction is more favorable.
9. C – Ag⁺/Ag (+0.80 V) and Mg²⁺/Mg (–2.37 V): E°cell = 3.17 V (very high).
10. D – SHE is defined as 0.00 V.
11. B – The cathode has the higher potential (where reduction occurs).
12. E – Swapping electrodes reverses sign but not the difference between them.
13. B – ΔG° = –nFE°cell, linking free energy and voltage.
14. C – The sign of E°cell indicates spontaneity.
15. C – The more negative half-cell donates electrons = reducing agent.
16. B – Voltaic cells with positive E°cell are spontaneous.
17. D – The anode (oxidation) is written on the left.
18. C – A salt bridge maintains electrical neutrality.
19. C – A negative E°cell means the reaction is nonspontaneous.
20. C – If both increase equally, the difference remains the same.
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