d(ΔG)=−(ΔSreaction).dT ΔG=ΔH−TΔS ΔG=ΔH+T(d(ΔG)dT)P At 300 – InterviewSolution

1.	d(ΔG)=−(ΔSreaction).dT ΔG=ΔH−TΔS ΔG=ΔH+T(d(ΔG)dT)P At 300 K,ΔH for the reaction, Zn(S)+2AgCl(S)→ZnCl2(aq)+2Ag(S) is −218 kJ/mol while the e.m.f of the cell is 1.015 V. (dEdT)P of the cell is:
Answer» $d (Δ G) = - (Δ S_{reaction}) . d T$ $Δ G = Δ H - T Δ S$ $Δ G = Δ H + T {(\frac{d (Δ G)}{d T})}_{P}$ At $300 K, Δ H$ for the reaction, $Z n_{(S)} + 2 A g C l_{(S)} \to Z n C l_{2_{(a q)}} + 2 A g_{(S)}$ is $- 218 kJ/mol$ while the e.m.f of the cell is $1.015 V$ . ${(\frac{d E}{d T})}_{P}$ of the cell is:

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