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

1. Which of the following statements is INCORRECT regarding electrode potential?
A) It depends on the concentration of ions.
B) It depends on temperature.
C) It depends on the amount of electrode material.
D) It is an intensive property.
2. At 298 K, if E°cell is 0.1 V, the equilibrium constant K for the cell reaction will be approximately:
A) 10^1
B) 10^10
C) 10^20
D) 10^0.1
3. For a reversible electrochemical cell reaction, the relationship between cell potential (Ecell) and Gibbs energy change (ΔG) is:
A) ΔG = -nFEcell
B) ΔG = nFEcell
C) ΔG = -nEcell/F
D) ΔG = nEcell/F
4. In a concentration cell, the cell potential arises due to the difference in:
A) Nature of electrodes
B) Concentration of the electrolyte
C) Temperature
D) Pressure
5. Which of the following is a typical application of Kohlrausch's law?
A) Calculating cell potential
B) Determining solubility product
C) Measuring electrode potential
D) Predicting reaction spontaneity
6. The molar conductivity of a weak electrolyte approaches a finite value at infinite dilution due to:
A) Complete dissociation
B) Partial dissociation
C) Inter-ionic attraction
D) Solvent effects
7. Faraday's constant (F) represents the charge of:
A) One electron
B) One mole of electrons
C) One proton
D) One mole of protons
8. A negative Gibbs energy change (ΔG < 0) for a cell reaction indicates:
A) The cell reaction is non-spontaneous
B) The cell reaction is spontaneous
C) The cell reaction is at equilibrium
D) The cell reaction requires external energy
9. The standard Gibbs energy change (ΔG°) is related to the equilibrium constant (K) by:
A) ΔG° = -RTln(K)
B) ΔG° = RTln(K)
C) ΔG° = -RT/ln(K)
D) ΔG° = RT/ln(K)
10. If the reaction quotient (Q) is greater than the equilibrium constant (K), the reaction will proceed in the:
A) Forward direction
B) Reverse direction
C) Will be at equilibrium
D) Will stop
11. The Nernst equation can be used to calculate the electrode potential under non-standard conditions, specifically when:
A) Concentrations are different from 1 M
B) Temperature is different from 298 K
C) Pressure is different from 1 atm
D) Any of the above
12. The term 'standard' in standard electrode potential refers to standard conditions of:
A) Temperature only
B) Pressure only
C) Concentration only
D) Temperature, pressure, and concentration
13. Electrode potential is an intensive property, meaning it is independent of:
A) Temperature
B) Concentration
C) Amount of substance
D) Pressure
14. Which of the following is a primary example of an electrochemical cell?
A) Electric heater
B) Electric motor
C) Dry cell battery
D) Incandescent bulb
15. In electrolysis, the electrode connected to the negative terminal of the external battery is called the:
A) Anode
B) Cathode
C) Electrode
D) Electrolyte
16. In electrolysis, the electrode connected to the positive terminal of the external battery is called the:
A) Cathode
B) Anode
C) Electrolyte
D) Electrode
17. Kohlrausch's law is particularly useful for determining the limiting molar conductivity of:
A) Strong electrolytes
B) Weak electrolytes
C) Metals
D) Semiconductors
18. Which type of ions have higher molar conductivity at infinite dilution?
A) Larger ions
B) Smaller hydrated ions
C) Ions with higher charge
D) Ions with lower charge
19. Conductance (G) is related to cell constant (G*) and conductivity (κ) by:
A) G = κ * (A/l)
B) G = κ / (A/l)
C) G = κ * (l/A)
D) G = κ / (l/A)
20. The cell constant (G*) of a conductivity cell is defined as the ratio of:
A) Length (l) to the area of cross-section (A)
B) Area of cross-section (A) to the length (l)
C) Resistance (R) to resistivity (ρ)
D) Conductivity (κ) to conductance (G)
21. Which of the following units is equivalent to S/m?
A) Ω·m
B) Ω/m
C) mho/m
D) mho·m
22. Conductivity (κ) and resistivity (ρ) are related by:
A) κ = 1/ρ
B) κ = ρ
C) κ = -1/ρ
D) κ = 1/√(ρ)
23. Which of the following statements is true for a spontaneous redox reaction?
A) ΔG° > 0 and E°cell < 0
B) ΔG° < 0 and E°cell > 0
C) ΔG° = 0 and E°cell = 0
D) ΔG° > 0 and E°cell > 0
24. The equilibrium constant (K) of a cell reaction is related to the standard cell potential (E°cell) by:
A) E°cell = (RT/nF)ln(K)
B) E°cell = -(RT/nF)ln(K)
C) E°cell = (nF/RT)ln(K)
D) E°cell = -(nF/RT)ln(K)
25. At equilibrium, the cell potential (Ecell) is:
A) Zero
B) Infinite
C) Equal to E°cell
D) Negative
26. The relationship between standard cell potential (E°cell) and standard Gibbs energy change (ΔG°) is given by:
A) ΔG° = -nFE°cell
B) ΔG° = nFE°cell
C) ΔG° = -nE°cell/F
D) ΔG° = nE°cell/F
27. A positive cell potential (Ecell > 0) indicates that the reaction is:
A) Non-spontaneous
B) Spontaneous
C) At equilibrium
D) Reversible
28. The standard cell potential (E°cell) is the difference between:
A) Standard anode potential and standard cathode potential
B) Standard cathode potential and standard anode potential
C) Standard electrode potentials of both electrodes
D) Standard reduction potentials of both electrodes
29. The cell potential (Ecell) of an electrochemical cell is given by:
A) E_cathode - E_anode
B) E_anode - E_cathode
C) E_cathode + E_anode
D) E_anode / E_cathode
30. If the concentration of product is higher than reactants, the electrode potential will:
A) Increase
B) Decrease
C) Remain unchanged
D) Become zero
31. At 298 K, the Nernst equation can be simplified to:
A) E = E° - (0.0591/n)log([Products]/[Reactants])
B) E = E° + (0.0591/n)log([Products]/[Reactants])
C) E = E° - (0.0591/n)log([Reactants]/[Products])
D) E = E° + (0.0591/n)log([Reactants]/[Products])
32. The Nernst equation for a single electrode reaction M^n+ + ne- → M is:
A) E = E° - (RT/nF)ln([M]/[M^n+])
B) E = E° + (RT/nF)ln([M^n+]/[M])
C) E = E° - (nF/RT)ln([M]/[M^n+])
D) E = E° + (nF/RT)ln([M^n+]/[M])
33. The Nernst equation relates the electrode potential (E) to the standard electrode potential (E°) and:
A) Temperature and pressure
B) Concentration of reactants and products
C) Number of electrons transferred
D) All of the above
34. Standard electrode potential (E°) is measured at:
A) 298 K temperature and 1 atm pressure
B) 298 K temperature and 1 M concentration
C) 298 K temperature, 1 atm pressure, and 1 M concentration
D) 0°C temperature and 1 atm pressure
35. The electrode potential of a half-cell depends on:
A) Concentration of ions
B) Temperature
C) Pressure
D) All of the above
36. An electrolytic cell requires an external source of:
A) Voltage
B) Current
C) Energy
D) Power
37. A galvanic cell is an example of a(n):
A) Electrolytic cell
B) Electrochemical cell
C) Concentration cell
D) Fuel cell
38. In an electrochemical cell, reduction occurs at the:
A) Anode
B) Cathode
C) External circuit
D) Electrode surface
39. In an electrochemical cell, oxidation occurs at the:
A) Cathode
B) Anode
C) Salt bridge
D) Electrolyte
40. An electrochemical cell converts chemical energy into:
A) Mechanical energy
B) Electrical energy
C) Thermal energy
D) Light energy
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:
A) Zero concentration
B) Infinite concentration
C) Zero conductivity
D) Infinite conductivity
42. Which of the following expressions correctly represents Kohlrausch's law for an electrolyte A_x B_y?
A) Λm°(A_x B_y) = xΛm°(A^y+) + yΛm°(B^x-)
B) Λm°(A_x B_y) = yΛm°(A^x+) + xΛm°(B^y-)
C) Λm°(A_x B_y) = xΛm°(A^y-) + yΛm°(B^x+)
D) Λm°(A_x B_y) = Λm°(A) + Λm°(B)
43. According to Kohlrausch's law, Λm°(NaCl) is equal to:
A) Λm°(Na+) + Λm°(Cl-)
B) Λm°(Na+) - Λm°(Cl-)
C) Λm°(Na) + Λm°(Cl)
D) Λm°(Na+) * Λm°(Cl-)
44. Kohlrausch's law states that the molar conductivity of an electrolyte at infinite dilution is the sum of the contributions of its:
A) Cations only
B) Anions only
C) Cations and anions
D) Electrons and holes
45. For a strong electrolyte, molar conductivity increases with dilution because:
A) The number of ions increases
B) The inter-ionic attraction decreases
C) The mobility of ions decreases
D) The volume of the solution decreases
46. Molar conductivity (Λm) is defined as conductivity (κ) divided by:
A) Molar mass
B) Molarity (C)
C) Molality (m)
D) Density
47. The conductance of a solution is the reciprocal of its:
A) Resistance
B) Resistivity
C) Conductivity
D) Molar conductivity
48. Which of the following factors does NOT affect the conductance of an electrolytic solution?
A) Nature of the electrolyte
B) Concentration of the electrolyte
C) Temperature of the solution
D) Pressure applied to the solution
49. What is the SI unit of conductivity?
A) Ohm meter (Ω·m)
B) Siemens per meter (S/m)
C) Ohm per meter (Ω/m)
D) Siemens meter (S·m)
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