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Calculate the potential of the following cell reaction at \( 298 \mathrm{~K} \)
\[
\mathrm{Sn}^{4+}(1.05 \mathrm{M})+\mathrm{Zn}(\mathrm{s}) \rightarrow \mathrm{Sn}^{2+}(0.50 \mathrm{M})+\mathrm{Zn}^{2+}(2.0 \mathrm{M})
\]
\( \mathrm{P} \)
The standard potential \( \mathrm{E}^{\circ} \) of the cell is \( 0.89 \mathrm{~V} \). Whether the potential of the cell will increase or decrease, if the concentration of \( \mathrm{Sn}^{4+} \) is increased in the cell? \( \left(\mathrm{R}=8.314 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} ; \mathrm{F}=96,500 \mathrm{C} \mathrm{mol}^{-1}\right) \)
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