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Chemistry · PYQ NEET UG 2019(1)
हिन्दीFor the cell reaction, \( 2\text{Fe}^{3+}_{(\text{aq})} + 2\text{I}^-_{(\text{aq})} \longrightarrow 2\text{Fe}^{2+}_{(\text{aq})} + \text{I}_{2(\text{aq})} \) \( E^\circ_{\text{cell}} = 0.24\text{ V} \) at \( 298\text{ K} \). The standard Gibbs energy (\( \Delta_r G^\circ \)) of the cell reaction is ______.\n[Given that Faraday constant \( \text{F} = 96500\text{ C mol}^{-1} \)]
Correct answer · Option 4
\( -46.32\text{ kJ mol}^{-1} \)
Explanation
\( \Delta_r G^\circ = -nFE^\circ_{\text{cell}} \). Here \( n = 2 \), \( F = 96500 \), \( E^\circ_{\text{cell}} = 0.24 \). \( \Delta_r G^\circ = -2 \times 96500 \times 0.24 = -46320\text{ J mol}^{-1} = -46.32\text{ kJ mol}^{-1} \).
