Conductance in electrolytic solutions, Kohlrausch's law, electrochemical cells, electrode potentials, Nernst equation, relationship between cell potential and Gibbs energy - One Line Questions

1. At 298 K, if E°cell is 0.1 V, the equilibrium constant K for the cell reaction will be approximately: — 10^10
2. Standard electrode potential (E°) is measured at: — 298 K temperature, 1 atm pressure, and 1 M concentration
3. In electrolysis, the electrode connected to the negative terminal of the external battery is called the: — Cathode
4. In an electrochemical cell, reduction occurs at the: — Cathode
5. Which of the following is a typical application of Kohlrausch's law? — Determining solubility product
6. In electrolysis, the electrode connected to the positive terminal of the external battery is called the: — Anode
7. In an electrochemical cell, oxidation occurs at the: — Anode
8. Kohlrausch's law states that the molar conductivity of an electrolyte at infinite dilution is the sum of the contributions of its: — Cations and anions
9. The molar conductivity of a weak electrolyte approaches a finite value at infinite dilution due to: — Complete dissociation
10. The electrode potential of a half-cell depends on: — All of the above
11. The Nernst equation can be used to calculate the electrode potential under non-standard conditions, specifically when: — Any of the above
12. At 298 K, the Nernst equation can be simplified to: — E = E° - (0.0591/n)log([Products]/[Reactants])
13. The Nernst equation for a single electrode reaction M^n+ + ne- → M is: — E = E° + (RT/nF)ln([M^n+]/[M])
14. The cell potential (Ecell) of an electrochemical cell is given by: — E_cathode - E_anode
15. The equilibrium constant (K) of a cell reaction is related to the standard cell potential (E°cell) by: — E°cell = (RT/nF)ln(K)
16. Which of the following is a primary example of an electrochemical cell? — Dry cell battery
17. A galvanic cell is an example of a(n): — Electrochemical cell
18. If the reaction quotient (Q) is greater than the equilibrium constant (K), the reaction will proceed in the: — Reverse direction
19. Conductance (G) is related to cell constant (G*) and conductivity (κ) by: — G = κ * (l/A)
20. If the concentration of product is higher than reactants, the electrode potential will: — Decrease
21. Which of the following statements is INCORRECT regarding electrode potential? — It depends on the amount of electrode material.
22. Which type of ions have higher molar conductivity at infinite dilution? — Smaller hydrated ions
23. The cell constant (G*) of a conductivity cell is defined as the ratio of: — Length (l) to the area of cross-section (A)
24. An electrochemical cell converts chemical energy into: — Electrical energy
25. Molar conductivity (Λm) is defined as conductivity (κ) divided by: — Molarity (C)
26. In a concentration cell, the cell potential arises due to the difference in: — Concentration of the electrolyte
27. Which of the following factors does NOT affect the conductance of an electrolytic solution? — Pressure applied to the solution
28. A positive cell potential (Ecell > 0) indicates that the reaction is: — Spontaneous
29. What is the SI unit of conductivity? — Siemens per meter (S/m)
30. Faraday's constant (F) represents the charge of: — One mole of electrons
31. The conductance of a solution is the reciprocal of its: — Resistance
32. The standard cell potential (E°cell) is the difference between: — Standard cathode potential and standard anode potential
33. Kohlrausch's law is particularly useful for determining the limiting molar conductivity of: — Weak electrolytes
34. Electrode potential is an intensive property, meaning it is independent of: — Amount of substance
35. The Nernst equation relates the electrode potential (E) to the standard electrode potential (E°) and: — All of the above
36. The term 'standard' in standard electrode potential refers to standard conditions of: — Concentration only
37. A negative Gibbs energy change (ΔG < 0) for a cell reaction indicates: — The cell reaction is spontaneous
38. For a strong electrolyte, molar conductivity increases with dilution because: — The inter-ionic attraction decreases
39. An electrolytic cell requires an external source of: — Energy
40. At equilibrium, the cell potential (Ecell) is: — Zero
41. The limiting molar conductivity of a weak electrolyte can be determined using Kohlrausch's law by extrapolating the plot of Λm versus √C to: — Zero concentration
42. For a reversible electrochemical cell reaction, the relationship between cell potential (Ecell) and Gibbs energy change (ΔG) is: — ΔG = -nFEcell
43. The relationship between standard cell potential (E°cell) and standard Gibbs energy change (ΔG°) is given by: — ΔG° = -nFE°cell
44. The standard Gibbs energy change (ΔG°) is related to the equilibrium constant (K) by: — ΔG° = -RTln(K)
45. Which of the following statements is true for a spontaneous redox reaction? — ΔG° < 0 and E°cell > 0
46. Conductivity (κ) and resistivity (ρ) are related by: — κ = 1/ρ
47. Which of the following expressions correctly represents Kohlrausch's law for an electrolyte A_x B_y? — Λm°(A_x B_y) = xΛm°(A^y+) + yΛm°(B^x-)
48. According to Kohlrausch's law, Λm°(NaCl) is equal to: — Λm°(Na+) + Λm°(Cl-)
49. Which of the following units is equivalent to S/m? — mho/m
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