The standard electrode potential E o and its temperature coefficient dE dT for a cell are 2   V and - 5 ×10 - 4   V K - 1 at 300  K , respectively. The reaction is Zn s + Cu 2 + aq → Zn 2 + aq + Cu s . The standard reaction enthalpy Δ r H - at 300   K in m o l - 1 is [ Use R = 8 J K - 1 mol - 1 and F =96,500 C   mol - 1 ]

Step-by-step solution

Δ G = - nFE cell = - 2 × 96500 × 2 = - 386   kJ Δ S = nF dE dT = 2 × 96500 × - 5 × 10 - 4   J   degree   celcious - 1 = - 96 .5  J At 298  K , TΔ S = 298 × - 96 .5   J = - 28 .757   kJ At constant temperature T = 248   K and pressure, ΔG = ΔH - TΔ S ΔH = ΔG + TΔ S = - 386 - 28.757 = -414.75 ≃ -412.8