Q1. A constant current was passed through a solution of AuCl₄⁻ ion between gold electrodes. After 10.0 minutes, the increase in mass of cathode was 1.314 g. The total charge passed through the solution is ___ ×10⁻² F. (Given: Atomic mass of Au = 197)

Q2. The emf of the cell Tl | Tl⁺(0.001 M) || Cu²⁺(0.01 M) | Cu is 0.83 V at 298 K. It can be increased by:

Q3. A metal surface of area 100 cm² is coated with nickel of thickness 0.001 mm. A current of 2 A is passed through Ni(NO₃)₂ solution. Find time required in seconds. (Given: density of Ni = 10 g mL⁻¹, molar mass = 60 g mol⁻¹, F = 96500 C mol⁻¹)

Q4. Number of alkanes obtained on electrolysis of a mixture of CH₃COONa and C₂H₅COONa is:

Q5. The amount of electricity (×10⁵ C) required for oxidation of 1 mol of H₂O to O₂ is:

Q6. Which equation correctly represents change of molar conductivity with concentration for a weak electrolyte?

Q7. How can a galvanic cell be converted into an electrolytic cell?

Q8. On charging a lead storage battery, oxidation state of Pb at anode and cathode respectively becomes:

Q9. For the reaction Fe²⁺ + Ag⁺ → Fe³⁺ + Ag, the standard cell potential is:

Q10. Aluminium chloride solution is electrolysed for 30 minutes using 2 A current. Amount of aluminium deposited is: