What is the standard free energy change for the cell, having following cell reaction? $2…

What is the standard free energy change for the cell, having following cell reaction? $2 \mathrm{Ag}_{(\mathrm{aq} .)}^{+}+\mathrm{Cd}_{(\mathrm{s})} \longrightarrow 2 \mathrm{Ag}_{(\mathrm{s})}+\mathrm{Cd}_{(\mathrm{aq})}^{2+}, \mathrm{E}^{\circ} \mathrm{cell}=1 \cdot 20 \mathrm{~V}$
  1. $-231 \cdot 6 \mathrm{~kJ}$
  2. $-160 \cdot 8 \mathrm{~kJ}$
  3. $-115 \cdot 8 \mathrm{~kJ}$
  4. $-260 \cdot 8 \mathrm{K} \mathrm{j}$

Solution

$2 \mathrm{Ag}_{(\mathrm{aq})}^{+}+\mathrm{Cd}_{(\mathrm{s})} \longrightarrow 2 \mathrm{Ag}_{(\mathrm{s})}+\mathrm{Cd}_{(\mathrm{aq})}^{2+}$ $\therefore \mathrm{n}=2$ $\Delta \mathrm{G}^{0}=-\mathrm{nFE}_{\mathrm{cell}}^{0}=-2 \times 96500 \times 1.20=-231600 \mathrm{~J}=-231.6 \mathrm{~kJ}$

Asked in: MHT CET 2020 (15 Oct Shift 2)

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