Electrochemical cells electrode potentials Nernst equation and fuel cells - One Line Questions

1. The standard reduction potential of Cu²⁺/Cu is +0.34 V and that of Zn²⁺/Zn is -0.76 V. The standard cell potential (E°_cell) for the reaction Zn + Cu²⁺ → Zn²⁺ + Cu is: — +1.10 V
2. If a half-reaction has a standard reduction potential of +0.80 V, it is more likely to be reduced than a half-reaction with a standard reduction potential of: — +0.34 V
3. What is the standard electrode potential for the reduction of H⁺ to H₂ (SHE - Standard Hydrogen Electrode)? — 0.00 V
4. In a hydrogen-oxygen fuel cell, what is the overall reaction? — 2H₂ + O₂ → 2H₂O
5. What is the unit of electrode potential? — Volt
6. Reduction occurs at which electrode in an electrochemical cell? — Cathode
7. In an electrochemical cell, which electrode is the site of oxidation? — Anode
8. If the reaction quotient Q is very large, the electrode potential E will be: — Significantly lower than E°
9. Which of the following is NOT a factor affecting electrode potential? — Color of the solution
10. At 298 K, the Nernst equation can be simplified to: — E = E° - (0.0591/n) log Q
11. What is the Nernst equation for a single electrode at 298 K? — E = E° - (RT/nF) ln Q
12. What is the relationship between the cell potential (E_cell) and the standard cell potential (E°_cell) at non-standard conditions? — E_cell = E°_cell - (RT/nF) ln Q
13. The standard cell potential (E°_cell) of a galvanic cell is calculated as: — E°_cathode - E°_anode
14. The relationship between E°_cell and K at 298 K is given by: — E°_cell = (0.0591/n) log K
15. The potential difference that drives the flow of electrons in the external circuit is called: — Cell potential (EMF)
16. In a fuel cell, the electrodes are typically made of: — Platinum or other catalytic materials
17. Which species is reduced at the cathode of a hydrogen-oxygen fuel cell (alkaline electrolyte)? — O₂
18. What is the main advantage of using fuel cells over conventional combustion engines? — Reduced pollution and higher efficiency
19. If the concentration of products is higher than reactants (Q > 1), the electrode potential (E) will: — Decrease
20. For the reaction Mⁿ⁺ + ne⁻ → M, if the concentration of Mⁿ⁺ increases, the electrode potential (E) will: — Increase
21. The electromotive force (EMF) of a fuel cell is generally: — Dependent on the type of fuel and oxidant
22. Electrode potential is an intensive property. What does this mean? — It does not depend on the amount of substance.
23. What happens to the electrode potential of a metal when its cation concentration in solution decreases? — It increases
24. Which of the following is a disadvantage of hydrogen as a fuel in fuel cells? — It is difficult to store and transport.
25. Which of the following is a characteristic of a fuel cell that makes it environmentally friendly? — Its primary emission is water.
26. Which of the following is a characteristic of a galvanic cell? — It converts chemical energy into electrical energy.
27. What is the equilibrium constant (K) for a redox reaction when E_cell = 0? — K = 1
28. Which of the following is a common fuel used in fuel cells? — Hydrogen
29. If Q < 1 in the Nernst equation, the term -(RT/nF) ln Q will be: — Positive
30. In an electrolytic cell, the anode is connected to the: — Positive terminal of the power supply
31. If E°_cell is positive, the reaction is: — Spontaneous under standard conditions
32. Which species is oxidized at the anode of a hydrogen-oxygen fuel cell? — H₂
33. The Nernst equation is essential for understanding: — How electrode potentials change with concentration
34. Which of the following statements about electrode potentials is correct? — Oxidation potential is the negative of the reduction potential for the same electrode.
35. In an electrolytic cell, the cathode is connected to the: — Negative terminal of the power supply
36. A fuel cell that uses molten carbonate as an electrolyte operates at high temperatures. This is typically a: — Solid Oxide Fuel Cell (SOFC)
37. The Nernst equation can be used to calculate the cell potential under conditions of: — Non-standard temperature and pressure
38. A fuel cell is a type of electrochemical cell that: — Converts chemical energy from a fuel into electrical energy
39. What is the primary component of the electrolyte in many alkaline hydrogen-oxygen fuel cells? — Potassium hydroxide solution
40. The Nernst equation relates the electrode potential to: — Standard electrode potential and reaction quotient
41. Which of the following statements is true for a spontaneous redox reaction in an electrochemical cell? — The cell potential (E_cell) is positive
42. What does 'n' represent in the Nernst equation? — The number of electrons transferred in the redox reaction
43. What is the standard electrode potential (E°)? — The potential of an electrode at standard conditions (298 K, 1 atm, 1 M concentration)
44. What is the role of electrons in the external circuit of an electrochemical cell? — They flow from the anode to the cathode.
45. What is the primary function of an electrochemical cell? — To generate electrical energy from chemical reactions
46. What is the main reason for using catalytic electrodes in fuel cells? — To increase the rate of electrochemical reactions
47. What is the purpose of the salt bridge in a galvanic cell? — To complete the internal circuit by allowing ion migration
48. In the Daniell cell (Zn | Zn²⁺ || Cu²⁺ | Cu), what is the cathode reaction? — Cu²⁺(aq) + 2e⁻ → Cu(s)
49. Consider the Daniell cell: Zn(s) | Zn²⁺(aq) || Cu²⁺(aq) | Cu(s). What is the anode reaction? — Zn(s) → Zn²⁺(aq) + 2e⁻
50. The Nernst equation is derived from which thermodynamic relationship? — ΔG = -nFE_cell
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