IIT JEE Chemistry Practice Paper – Part 15 (Electrochemistry)

Q1. The standard electrode potential of Zn²⁺/Zn is –0.76 V and that of Cu²⁺/Cu is +0.34 V. The EMF of the cell Zn | Zn²⁺ || Cu²⁺ | Cu is:

a) 0.42 V
b) 1.10 V
c) 0.76 V
d) –1.10 V

Q2. The unit of molar conductivity is:

a) S m² mol^–1
b) S mol^–1
c) ohm^–1
d) S m mol^–1

Q3. Which of the following electrolytes shows the highest molar conductivity at infinite dilution?

a) NaCl
b) HCl
c) NH₄OH
d) CH₃COOH

Q4. In the electrolysis of molten NaCl, the product at the cathode is:

a) Na
b) Cl₂
c) NaOH
d) H₂

Q5. According to Kohlrausch’s Law, the molar conductivity of an electrolyte at infinite dilution is equal to:

a) Sum of equivalent conductivities of cation and anion at infinite dilution
b) Product of ionic mobilities
c) Square of ionic mobilities
d) None of these

Q6. The slope of a graph between log([oxidised]/[reduced]) and electrode potential (E) is related to:

a) Faraday’s constant
b) Nernst equation
c) Gibbs free energy
d) Cell constant

Q7. The conductance of a solution depends upon:

a) Nature of ions only
b) Concentration of ions only
c) Nature and concentration of ions, and temperature
d) Electrode potential

Q8. In a galvanic cell, the flow of electrons occurs from:

a) Cathode to anode
b) Anode to cathode
c) Salt bridge to anode
d) Salt bridge to cathode

Q9. During electrolysis, the amount of substance deposited on an electrode is proportional to:

a) Charge passed
b) Voltage applied
c) Temperature
d) Pressure

Q10. The relation between free energy change (ΔG) and EMF of the cell (E) is:

a) ΔG = –nFE
b) ΔG = nFE
c) ΔG = –RT lnK
d) ΔG = E/RT