Electrochemistry - Nernst Equation, Conductance

Grade 12 Chemistry — Electrochemistry - Nernst Equation, Conductance: 25 practice questions with instant scoring and explanations.

1. The Nernst equation at 298 K in log form is:
2. At equilibrium in Nernst equation, E = 0, therefore:
3. Conductance (G) is measured in:
4. Specific conductance (κ) has units of:
5. The relationship between conductance (G) and resistance (R) is:
6. The relationship between specific conductance (κ) and resistivity (ρ) is:
7. Molar conductance (Λm) is defined as:
8. The relationship between specific conductance and molar conductance is:
9. Strong electrolytes show molar conductance that:
10. Weak electrolytes show molar conductance that:
11. The limiting molar conductance (Λ°m) is the molar conductance at:
12. Kohlrausch's law states that Λ°m for an electrolyte =:
13. For the electrolyte AB₂, Λ°m = λ°A + 2λ°B. This is:
14. The ionic strength (I) of a solution is defined as:
15. Debye-Hückel theory explains:
16. The relationship between degree of dissociation (α) and molar conductance is:
17. For a weak electrolyte, Ka can be calculated from:
18. The conductivity of water is due to:
19. At 298 K, the relationship between E and log Q in Nernst equation is linear because:
20. The cell potential increases as Q:
21. For the half-reaction with n = 2, a 10-fold increase in [Red]/[Ox] changes E by:
22. Equivalent conductance (Λ) is related to molar conductance (Λm) by:
23. The conductivity of a solution increases with:
24. The degree of ionization of a weak electrolyte is calculated using:
25. The equivalent conductance is related to molar conductance by: