Solve this: The standard emf of the following cell: Cd(s)|CdCl2(aq) (0.10 M)||Cl-| AgCl(s)|Ag(s) In which the cell reaction is 2AgCl(s) + Cd(s) → 2Ag(s) +Cd2+ + 2Cl-(aq) is 0.6915 V at 100 C and 0.6753 V at 250C. The ∆ H of reaction at 250C is (A) -192.5 kJ (B) -234.7 kJ (C) 123.5 kJ (D) -167.26 kJ Share with your friends Share 13 Shyama Charan Mandal answered this Dear Student, 1. The formula used is Gibbs Helmoltz equation : ∆G=∆H-T∆S2. From the data in question: ∆G1(283K) =-nFE∘=-2×96500×0.6195=11.96 kJ ∆G2(298K) = -nFE∘=-2×96500×0.6753=13.03 kJ3. Using equation 1 : 11.96 kJ = ∆H-283∆S ...(1)- 13.03 kJ =-∆H+298∆S ...(2)we get, ∆S =-572 JK-1 ∆H= 123.5 kJ Regards, 3 View Full Answer