List of top Chemistry Questions on Gibbs energy change and equilibrium asked in CBSE Class XII

The relationship between \( E^{o}_{(cell)} \) and \( \Delta_rG^{\ominus} \) is :

The relationship between \( \mathrm{E^{\circ}_{(cell)}} \) and \( \Delta_r G^{\ominus} \) is :

Consider the following reaction :
\( \text{Zn}_{(s)} + \text{Ag}_2\text{O}_{(s)} + \text{H}_2\text{O}_{(l)} \rightarrow \text{Zn}^{2+}_{(aq)} + 2\text{Ag}_{(s)} + 2\text{OH}^-_{(aq)} \)
Given : \( E^\circ_{\text{Ag}^+/\text{Ag}} = 0.80 \, \text{V} \), \( E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \, \text{V} \), \( 1 \, \text{F} = 96500 \, \text{C mol}^{-1} \).
\( \Delta_r G^\circ \) for the above reaction is :

Calculate \(\Delta_r G^{\circ}\) and \(\log K_C\) of the reaction.

\(\mathrm{2Cr(s) + 3Cd^{2+}(aq) \to 2Cr^{3+}(aq) + 3Cd(s)}\)

Given \(E^{\circ}_{\mathrm{Cr^{3+}/Cr}} = -0.74\) V, \(E^{\circ}_{\mathrm{Cd^{2+}/Cd}} = -0.40\) V

[R = 8.314 J \(\mathrm{K^{-1}\,mol^{-1}}\), F = 96500 C \(\mathrm{mol^{-1}}\)]

Calculate \(\Delta_r G^\circ\) and \(\log K_C\) of the reaction :
\(\mathrm{Fe^{2+}(aq) + Ag^+(aq) \longrightarrow Fe^{3+}(aq) + Ag(s)}\)
Given : \(E^\circ_{Ag^+/Ag} = 0.80\ \mathrm{V},\ E^\circ_{Fe^{3+}/Fe^{2+}} = 0.77\ \mathrm{V}\)
[\(R = 8.314\ \mathrm{J\ K^{-1}\ mol^{-1}},\ F = 96500\ \mathrm{C\ mol^{-1}}\)]