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Construct the cell corresponding to the reaction: \( 3 \mathrm{Cr}^{2+}(1 \mathrm{M}) \rightarrow 2 \mathrm{Cr}^{3+}(1 \mathrm{M})+\mathrm{Cr}(\mathrm{s}) \) and predict if the reaction is spontaneous. Also calculate the following \( \Delta H \) and \( \Delta S \) of the reaction at \( 25^{\circ} \mathrm{C} \).

Given \( E_{\mathrm{Cr}^{3} \cdot \mathrm{Cr}}^{0}=0.5 \mathrm{~V}, E_{\mathrm{Cr}^{3} \cdot \mathrm{Cr}^{2+}}^{0}=-0.41 \mathrm{~V} \) and \( \Delta G \) of the reaction at \( 35^{\circ} \mathrm{C}=-270.50 \mathrm{~kJ} \)
(A) \( \Delta H=-51.05 \mathrm{~kJ}, \Delta S=700 \mathrm{~kJ} \mathrm{~K}^{-1} \)
(B) \( \Delta H=-31.05 \mathrm{~kJ}, \Delta S=-700 \mathrm{~kJ} \mathrm{~K}^{-1} \)
(C) \( \Delta H=-51.05 \mathrm{~kJ}, \Delta S=706 \mathrm{~kJ} \mathrm{~K}^{-1} \)
(D) \( \Delta H=-53.05 \mathrm{~kJ}, \Delta S=706 \mathrm{~kJ} \mathrm{~K}^{-1} \)
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