Question

Consider an electrochemical cell: A(s) | Aⁿ⁺ (aq, 2 M) || B²ⁿ⁺ (aq, 1 M) | B(s). The value of ΔH^θ for the cell reaction is twice that of ΔG^θ at 300 K. If the emf of the cell is zero, the ΔS^θ (in J K⁻¹ mol⁻¹) of the cell reaction per mole of B formed at 300 K is ____.
(Given: ln(2) = 0.7, R (universal gas constant) = 8.3 J K⁻¹ mol⁻¹. H, S and G are enthalpy, entropy and Gibbs energy, respectively.)

Answer 1

Answer: -11.62J mol^-1K^-1

Solution: