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An aqueous solution containing \( \mathrm{Na}^{+}, \mathrm{Sn}^{2+}, \mathrm{Cl} \& \mathrm{SO}_{4}^{2-} \) ions, all at unit concentration, is electrolysed between a silver anode and a platinum cathode. What changes occur at the electrodes when current is passed through the cell? Given:
\[
\begin{array}{l}
\mathrm{E}_{\mathrm{Ag}^{+} \mid \mathrm{Ag}}^{\mathrm{o}}=0.799 \mathrm{~V}, \\
\mathrm{E}_{\mathrm{Sn}^{2}+\mathrm{Sn}}^{\mathrm{os}}=-0.14 \mathrm{~V}, \mathrm{E}_{\mathrm{Cl}_{2} \mid \mathrm{CI}}^{\mathrm{o}}=1.36 \mathrm{~V}, \mathrm{E}_{\mathrm{S}_{2} \mathrm{O}_{\mathrm{g}}^{2-\mid} \mathrm{SO}_{4}^{2-}}^{\mathrm{o}}=2 \mathrm{~V}, \\
\mathrm{E}_{\mathrm{Sn}^{+} \mid \mathrm{Sn}^{2+}}^{\mathrm{o}}=0.13 \mathrm{~V}
\end{array}
\]
(a) \( \mathrm{Sn}^{2+} \) is reduced and \( \mathrm{Cl}^{-} \)is oxidized
(b) \( \mathrm{Ag} \) is oxidized and \( \mathrm{Sn}^{2+} \) is reduced
(c) \( \mathrm{Sn}^{2+} \) is reduced and \( \mathrm{Sn}^{2+} \) is oxidized
(d) \( \mathrm{H}^{+} \)is reduced and \( \mathrm{Sn}^{2+} \) is oxidized
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