Standard electrode potentials for a few half | vedclass

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(A) The relationship between standard Gibbs free energy change and standard cell potential is given by $\Delta G^0 = -nFE^0_{cell}$.For a cell to have

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$Zn \mid Zn^{2+}(1 \ M) \parallel Ag^{+}(1 \ M) \mid Ag$

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(A) The relationship between standard Gibbs free energy change and standard cell potential is given by $\Delta G^0 = -nFE^0_{cell}$.For a cell to have the most negative $\Delta G^0$,it must have the most positive $E^0_{cell}$ value.$E^0_{cell} = E^0_{cathode} - E^0_{anode}$.$A) \ E^0_{cell} = 0.80 - (-0.76) = 1.56 \ V; \Delta G^0 = -2 	imes F 	imes 1.56 = -3.12 \ F$$B) \ E^0_{cell} = -2.37 - (-0.76) = -1.61 \ V; \Delta G^0 = -2 	imes F 	imes (-1.61) = +3.22 \ F$$C) \ E^0_{cell} = -2.37 - 0.80 = -3.17 \ V; \Delta G^0 = -2 	imes F 	imes (-3.17) = +6.34 \ F$$D) \ E^0_{cell} = 0.80 - 0.34 = 0.46 \ V; \Delta G^0 = -2 	imes F 	imes 0.46 = -0.92 \ F$Comparing the values,option $(A)$ gives the most negative $\Delta G^0$.

Standard electrode potentials for a few half cells are mentioned below:
$E^0_{Cu^{2+}/Cu} = 0.34 \ V, E^0_{Zn^{2+}/Zn} = -0.76 \ V$
$E^0_{Ag^{+}/Ag} = 0.80 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$
Which one of the following cells gives the most negative value of $\Delta G^0$?

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Standard electrode potentials for a few half cells are mentioned below:$E^0_{Cu^{2+}/Cu} = 0.34 \ V, E^0_{Zn^{2+}/Zn} = -0.76 \ V$$E^0_{Ag^{+}/Ag} = 0.80 \ V, E^0_{Mg^{2+}/Mg} = -2.37 \ V$Which one of the following cells gives the most negative value of $\Delta G^0$?