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d(ΔG)=−(ΔSreaction).dT ΔG=ΔH−TΔS ΔG=ΔH+T(d(ΔG)dT)PAt 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: |
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Answer» 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: |
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