Electrochemical cells and cell potentials Quiz
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5 questions, one answer each
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1. In a cell diagram, which half-cell is written on the left?
- A. The one where oxidation occurs (negative electrode)
- B. The one where reduction occurs
- C. The one with the more positive E°
- D. The one with the higher concentration
2. What is E°cell for a cell made from Ni²⁺|Ni (−0.25 V) and Ag⁺|Ag (+0.80 V)?
- A. +0.55 V
- B. +1.05 V
- C. −1.05 V
- D. +2.10 V
3. Which species is the strongest reducing agent?
- A. Cu (E° of Cu²⁺|Cu = +0.34 V)
- B. Ag (E° of Ag⁺|Ag = +0.80 V)
- C. Cl⁻ (E° of Cl₂|Cl⁻ = +1.36 V)
- D. Mg (E° of Mg²⁺|Mg = −2.37 V)
4. The Ag⁺ concentration in an Ag⁺|Ag half-cell is lowered to 0.10 mol dm⁻³. What happens to its electrode potential?
- A. It becomes less positive, as the equilibrium shifts left
- B. It becomes more positive, as the equilibrium shifts right
- C. It stays the same, as E° is a constant
- D. It becomes exactly 0.00 V
5. What is E°cell for 2Ag⁺ + Cu → 2Ag + Cu²⁺, given E°(Ag⁺|Ag) = +0.80 V and E°(Cu²⁺|Cu) = +0.34 V?
- A. +1.26 V
- B. +0.92 V
- C. +0.46 V
- D. −0.46 V