Chapter 2: Electrochemistry
Important Questions
1. The chemistry of corrosion of iron is essentially an electro-chemical phenomenon. Explain the reactions occurring during the corrosion of iron in the atmosphere.
2. Complete the following chemical equations:
(i) MnO4– + C2O42– + H+
(ii) 
(iii) 
3. Calculate the emf of the following cell at 298 K:
Given E0cell = +0.44V)
4. Express the relation between conductivity and molar conductivity of a solution held in a cell.
5. The conductivity of 0.20 M solution of KCl at 298 K is 0.025 S cm–1. Calculate its molar conductivity.
Sample Questions
1. Define the following terms:
(i) Molar conductivity (Λm)
(ii) Secondary batteries
2. Conductivity of 0.00241 M acetic acid solution is 7.896 × 10–5 S cm–1. Calculate its molar conductivity in this solution. If Δ0m for acetic acid be 390.5 S cm2 mol–1, what would be its dissociation constant?
3. What type of a battery is lead storage battery? Write the anode and the cathode reactions and the overall reactions occurring in a lead storage battery.
4. Calculate the time to deposit 1.5 g of silver at cathode when a current of 1.5 was passed through the solution of AgNO3. (Molar mass of
Ag = 108 g mol–1, 1F = 96500 C mol–1)
5. What type of cell is a lead storage battery? Write the anode and the cathode reactions and the overall cell reaction occurring in the use of a lead storage battery?
OR
Construct the redox equation from the two half cell reactions and predict if this reaction favours formation of reactants or product shown in the equation.