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Comprehension
For the reaction: \( \operatorname{Ag}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \rightleftharpoons \operatorname{AgCl}(\mathrm{s}) \). Given
\begin{tabular}{lcc}
\cline { 2 - 3 } \( \mathbf{A g}^{+}+\mathrm{e}^{-} \rightarrow \mathbf{A g} ; E^{\circ}=\mathbf{0 . 8 0} \mathrm{V} \) & Species & \( \Delta G_{\mathrm{f}}^{0}(\mathbf{k J} / \mathbf{m o l}) \) at \( \mathbf{2 5}^{\circ} \mathbf{C} \) \\
\cline { 2 - 3 } \( \mathbf{Z n}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathbf{Z n} ; E^{\circ}=-\mathbf{0 . 7 6} \mathrm{V} \) & \( \mathrm{Ag}^{+}(\mathrm{aq}) \) & \( +77 \) \\
& \( \mathrm{Cl}^{-}(\mathrm{aq}) \) & \( -129 \) \\
\cline { 3 } & \( \mathrm{AgCl}(\mathrm{s}) \) & \( -109 \) \\
\hline
\end{tabular}
A quantity of \( 6.539 \times 10^{-2} \mathrm{~g} \) of metallic zinc is added to \( 100 \mathrm{ml} \) of saturated solution of \( \mathrm{AgCl} \). The value of \( \log \frac{\left[\mathrm{Zn}^{2+}\right]}{\left[\mathrm{Ag}^{+}\right]^{2}} \) is \( (\mathrm{Zn}=65.39) \)
(a) \( 5.288 \)
(b) \( 52.88 \)
(c) \( 528.8 \)
(d) \( 26.44 \)
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