The cell potential (Ecell) of a reaction is related as ΔG=nF Ecell, where ΔG represents maximum useful electrical work. n = no. of moles of electrons exchanged during the reaction. For reversible cell reaction d(ΔG)=(ΔV)dp−(ΔS)dT At const. P, d(ΔG)=−(ΔS)dT At const. P, ΔG=ΔH−TΔS. (1) ∴ ΔG=ΔH+T(d(ΔG)ΔT)P. (2) (dEcelldT)p is known as temperature coefficient of the emf of the cell. At 300K, ΔH for the reaction Zn+2AgCl→ZnCl2+2Agis−218 kJ/mole while emf of the cell was 1.015V.(dEdT)p of the cell is

The cell potential (Ecell) of a reaction is related as ΔG=nF Ecell, w

1.	The cell potential (Ecell) of a reaction is related as ΔG=nF Ecell, where ΔG represents maximum useful electrical work. n = no. of moles of electrons exchanged during the reaction. For reversible cell reaction d(ΔG)=(ΔV)dp−(ΔS)dT At const. P, d(ΔG)=−(ΔS)dT At const. P, ΔG=ΔH−TΔS. (1) ∴ ΔG=ΔH+T(d(ΔG)ΔT)P. (2) (dEcelldT)p is known as temperature coefficient of the emf of the cell. At 300K, ΔH for the reaction Zn+2AgCl→ZnCl2+2Agis−218 kJ/mole while emf of the cell was 1.015V.(dEdT)p of the cell is
Answer» The cell potential $(E_{c e l l})$ of a reaction is related as $Δ G = n F E_{c e l l}$ , where $Δ G$ represents maximum useful electrical work. n = no. of moles of electrons exchanged during the reaction. For reversible cell reaction $d (Δ G) = (Δ V) d p - (Δ S) d T$ At const. P, $d (Δ G) = - (Δ S) d T$ At const. P, $Δ G = Δ H - T Δ S$ . (1) $∴ Δ G = Δ H + T {(\frac{d (Δ G)}{Δ T})}_{P}$ . (2) ${(\frac{d E_{c e l l}}{d T})}_{p}$ is known as temperature coefficient of the emf of the cell. At 300K, $Δ H$ for the reaction $Z n + 2 A g C l \to Z n C l_{2} + 2 A g i s - 218$ kJ/mole while emf of the cell was $1.015 V . {(\frac{d E}{d T})}_{p}$ of the cell is