Question

Calculate the emf of the following cell at 298 K : Fe(s) | Fe²⁺ (0.01M) || H⁺(1M) | H₂(g) (1 bar), Pt(s). Given E°Cell = 0.44 V.

State Kohlrausch's law of independent migration of ions.

Calculate Δ_rG° and log Kc for the following cell : Ni(s) + 2 Ag⁺(aq) → Ni²⁺(aq) + 2Ag(s) Given that E°cell = 1.05V, 1F = 96,500 Cmol⁻¹.

The standard Gibbs energy (ΔrG°) for the following cell reaction is −300 kJ mol⁻¹: Zn(s) + 2Ag⁺(aq) → Zn²⁺(aq) + 2Ag(s). Calculate E°cell for the reaction. (Given: 1 F = 96500 mol⁻¹)