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  • For the reaction taking place in the cell: <img alt="\mathrm{Pt}(\mathrm{s})\left|\mathrm{H}_{2}(\mathrm{g})| \mathrm{H}^{+}(\mathrm{aq}) \| \mathrm{Ag}^{+}(\mathrm{aq})\right| \mathrm{Ag

For the reaction taking place in the cell:

\mathrm{Pt}(\mathrm{s})\left|\mathrm{H}_{2}(\mathrm{g})| \mathrm{H}^{+}(\mathrm{aq}) \| \mathrm{Ag}^{+}(\mathrm{aq})\right| \mathrm{Ag}(\mathrm{s})

\mathrm{E^{\circ}}_{\text {cell }}=+0.5332 \mathrm{~V}.

The value of \Delta_{f} \mathrm{G}^{\Theta} for the reaction given below is ____________\mathrm{kJ} \; \mathrm{mol}^{-1}.(in nearest integer)

Reaction:  \mathrm{\frac{1}{2}H_2 + Ag^+ \longrightarrow H^+ + Ag}

Option: 1

51


Option: 2

-


Option: 3

-


Option: 4

-


Answers (1)

best_answer

\begin{aligned} \mathrm{\Delta G^{\circ} =-n \; f \: E^{\circ} }\\ \end{aligned}

           \\ =-1 \times 96500 \times 0.5332\\ \\ =-51453 \: \mathrm{Jmol} ^{-1}\\ \\ =-51.453 \mathrm{~kJ} \mathrm{~mol}^{-1}

Answer is 51

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Riya

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