Cu(s) + Sn^(2+) (0.001M) -> Cu^(2+) (0.01M) + Sn(s) The Gibbs free energy change for the above reaction at 298 K is x x 10^(-1) kJ mol^(-1). The value of x is __________. [nearest integer] [Given : E_Cu^2 + /Cu^Theta = 0.34 V ; E_Sn^2 + /Sn^Theta = - 0.14 V ; F = 96500 C mol^(-1)]

Cu + Sn^+2 -> Cu^+2+ Sn( s) \ E_ cell ^° = E_ OX^°+ E_ Red ^° \ =-0.34-0.14 \ =-0.48 V \ E= E^°-(0.0591 / 2) log frac[ Cu^+2][ Sn^+2] \ = -0.48-0.0295 log 10 \ = -0.5095 V \ Delta G= - nFE \ =-2 x 96500 x -0.5095 J / mol \ =98333.5 x 10^-3 kJ / mol \ =983.3 x 10^-1 kJ / mol \ =983 x 10^-1 kJ / mol

Cus Sn2 0001M Cu2 001M Sns The Gibbs free energy change... | null (Chemistry)

\begin{aligned} \mathrm{Cu} &+\mathrm{Sn}^{+2} \longrightarrow \mathrm{Cu}^{+2}+\mathrm{Sn}(\mathrm{s}) \\\\ \mathrm{E}_{\text {cell }}^{\circ} &=\mathrm{E}_{\mathrm{OX}}^{\circ}+\mathrm{E}_{\text {Red }}^{\circ} \\\\ &=-0.34-0.14 \\\\ &=-0.48 \mathrm{~V} \\\\ \mathrm{E}=& ~\mathrm{E}^{\circ}-\frac{0.0591}{2} \log \frac{\left[\mathrm{Cu}^{+2}\right]}{\left[\mathrm{Sn}^{+2}\right]} \\\\ =&-0.48-0.0295 \log 10 \\\\ =&-0.5095 \mathrm{~V} \\\\ \Delta \mathrm{G}=&-\mathrm{nFE} \\\\ &=-2 \times 96500 \times-0.5095 \mathrm{~J} / \mathrm{mol} \\\\ &=98333.5 \times 10^{-3} \mathrm{~kJ} / \mathrm{mol} \\\\ &=983.3 \times 10^{-1} \mathrm{~kJ} / \mathrm{mol} \\\\ &=983 \times 10^{-1} \mathrm{~kJ} / \mathrm{mol} \end{aligned}

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