A cell, Ag | Ag⁺ || Cu²⁺ | Cu, initially contains 1 M Ag⁺ and 1 M Cu²⁺ ions. Calculate the change in the cell potential after the passage of 9.65 A current for 1 h.

Calculate the equilibrium constant for the reaction:
2Fe³⁺ + 3I^- $$\leftrightharpoons$$ 2Fe²⁺ + $$I_3^-$$. The standard reduction potentials in acidic conditions are 0.78 V and 0.54 V respectively for Fe³⁺ | Fe²⁺ and $$I_3^-$$ | I^- couples.

Find the solubility product of a saturated solution of Ag₂CrO₄ in water at 298 K if the emf of the cell Ag|Ag⁺ (satd. Ag₂CrO₄ soln.) || Ag⁺ (0.1 M) | Ag is 0.164 V at 298 K.

How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 8.0 hours at a current of 8.46 amperes? What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is 10.5 g/cm³