RE-NEET Chemistry Electrochemistry Class 12 Questions

The standard electrode potential (E°) for the half-cell reaction Fe³⁺ + e⁻ → Fe²⁺ at 298 K is (Given: E°(Fe³⁺/Fe) = -0.04 V and E°(Fe²⁺/Fe) = -0.44 V at 298 K)

For a salt XY, which is a strong electrolyte, the plot of Λₘ versus √C has a slope of^{-90}.0 S cm² mol⁻³/² L¹/² at 298 K. At 0.01 M concentration of XY, the value of Λₘ is 145.0 S cm² mol⁻¹. The limiting molar conductivity of Y⁻ ion (Λ⁰ᵧ⁻, in S cm² mol⁻¹) at 298 K will be (Given: Λ⁰ₓ⁺ = 74.0 S cm² mol⁻¹)

The standard cell potential of the following cell Zn|Zn²⁺ (aq)|Fe²⁺(aq)|Fe is 0.32 V. Calculate the standard Gibbs energy change for the reaction : Zn(s) + Fe²⁺(aq) → Zn²⁺(aq) + Fe(s) (Given : 1 F = 96487 C)