Answer to Question #339315 in Physical Chemistry for Chinnu

Question

Consider the cell, Zn(s)|ZnCl2(0.0050 mol kg−1)|Hg2Cl2(s)|Hg(l), for which the cell reaction is Hg2Cl2(s) + Zn(s) → 2 Hg(l) + 2 Cl−(aq) + Zn2+(aq). The cell potential is +1.2272 V, E⦵(Zn2+,Zn) = −0.7628 V, and E⦵(Hg2Cl2,Hg) = +0.2676 V. (a) Write the Nernst equation for the cell. Determine (b) the standard cell potential, (c) ΔrG, ΔrG⦵, and K for the cell reaction, (d) the mean ionic activity and activity coefficient of ZnCl2 from the measured cell potential, and (e) the mean ionic activity coefficient of ZnCl2 from the Debye–Hückel limiting law. (f) Given that (∂Ecell/∂T)p = −4.52 × 10−4 V K−1, Calculate ΔrS and ΔrH.

Answer 1

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