MHT CET · Chemistry · Electrochemistry
Calculate \(\Delta \mathrm{G}^{\circ}\) for the cell:
\(\mathrm{Sn}_{(\mathrm{s})}\left|\operatorname{Sn}_{(\mathrm{IM})}^{++}\right|\left|\operatorname{Ag}_{(\mathrm{IM})}^{+}\right| \mathrm{Ag}_{(\mathrm{s})} \text { at } 25^{\circ} \mathrm{C}\) \(\left(\mathrm{E}_{\text {cell }}^{\circ}=0.90 \mathrm{~V}\right)\)
- A \(-173.7 \mathrm{~kJ}\)
- B \(-225.3 \mathrm{~kJ}\)
- C \(-100.2 \mathrm{~kJ}\)
- D \(-290.8 \mathrm{~kJ}\)
Answer & Solution
Correct Answer
(A) \(-173.7 \mathrm{~kJ}\)
Step-by-step Solution
Detailed explanation
\(\Delta \mathrm{G}^{\circ} =-\mathrm{nF}_{\text {cell }}^{\circ} \)
\( =-2 \times 96500 \times 0.90 \)
\( =-173700 \mathrm{~J} \)
\( =-173.7 \mathrm{~kJ}\)
\( =-2 \times 96500 \times 0.90 \)
\( =-173700 \mathrm{~J} \)
\( =-173.7 \mathrm{~kJ}\)
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