Electrochemistry - Electrochemical Cells, EMF

Grade 12 Chemistry — Electrochemistry - Electrochemical Cells, EMF: 25 practice questions with instant scoring and explanations.

1. An electrochemical cell converts:
2. In a galvanic cell, oxidation occurs at:
3. In an electrolytic cell, oxidation occurs at:
4. The electrode potential of standard hydrogen electrode (SHE) is taken as:
5. The standard cell potential (E°cell) is given by:
6. A cell with E°cell > 0 is:
7. A cell with E°cell < 0 is:
8. For the reaction 2H⁺ + 2e⁻ → H₂, E° =:
9. For the reaction Zn²⁺ + 2e⁻ → Zn, E° = −0.76 V. For Zn → Zn²⁺ + 2e⁻, E° =:
10. The relationship between E°cell and ΔG° is:
11. Faraday constant (F) equals:
12. For a spontaneous reaction at 298 K, ΔG° is:
13. The relationship between E°cell, K, and temperature is:
14. In a galvanic cell, the anode is the:
15. In a galvanic cell, the cathode is the:
16. The EMF (electromotive force) of a cell is also called:
17. When E° is expressed at standard conditions (298 K, 1 M, 1 atm), it is called:
18. The direction of electron flow in external circuit is from:
19. The Daniell cell has E°cell =:
20. For the cell Mg | Mg²⁺ || Cu²⁺ | Cu with E°(Mg²⁺/Mg) = −2.37 V and E°(Cu²⁺/Cu) = 0.34 V, E°cell =:
21. The relationship between cell potential and concentration (Nernst equation) is:
22. When a cell reaches equilibrium, E =:
23. The number of electrons transferred in the reaction 2MnO₄⁻ + 16H⁺ + 10e⁻ → 2Mn²⁺ + 8H₂O is:
24. For maximum work output, a cell should operate:
25. An ideal cell has internal resistance of: