MHT CET · Chemistry · Electrochemistry
Calculate \(\Delta \mathrm{G}^{\circ}\) for the reaction \(\mathrm{Mg}_{(s)}+\mathrm{Sn}_{(\mathrm{aq})}^{++} \longrightarrow \mathrm{Mg}_{(\mathrm{mq})}^{++}+\mathrm{Sn}_{(s)}\) if \(\mathrm{E}_{\text {cell }}^0\) is \(2.23 \mathrm{~V}\).
- A \(-430.4 \mathrm{~kJ}\)
- B \(215.2 \mathrm{~kJ}\)
- C \(645.6 \mathrm{~kJ}\)
- D \(-860.8 \mathrm{~kJ}\)
Answer & Solution
Correct Answer
(A) \(-430.4 \mathrm{~kJ}\)
Step-by-step Solution
Detailed explanation
\(\begin{aligned} \Delta \mathrm{G}^{\circ} & =-\mathrm{nFE}_{\text {cell }}^{\circ} \\ & =-2 \times 96500 \times 2.23 \\ & =-430390 \mathrm{~J} \\ & =-430.4 \mathrm{~kJ}\end{aligned}\)
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