For the reaction 2Fe^3+ + Sn^2+ -> 2Fe^2+ + Sn^4+ at 298 K, use E deg(Fe^3+/Fe^2+) = +0.77 V, E deg(Sn^4+/Sn^2+) = +0.15 V and F = 96500 C mol^-1. Delta G deg for the reaction as written is

JEE Main levelSingle correct optionDifficulty 2 of 3df065

For the reaction $2 Fe X^{3 +} + Sn X^{2 +} \to 2 Fe X^{2 +} + Sn X^{4 +}$ at 298 K, use $E^{\circ} (Fe X^{3 +} / Fe X^{2 +}) = + 0.77 V$ , $E^{\circ} (Sn X^{4 +} / Sn X^{2 +}) = + 0.15 V$ and $F = 96500 C mo l^{- 1}$ . $Δ G^{\circ}$ for the reaction as written is

E_{cell}^{\circ} = 0.77 - 0.15 = 0.62 V

and

n = 2

electrons are transferred.

Δ G^{\circ} = - n F E^{\circ} = - 2 \times 96500 \times 0.62 = - 119660 J \approx - 119.7 kJ