Question

Consider the following electrochemical cell at

298 \mathrm{~K}

\begin{aligned} & {Ag}(s)\left|A g I(s)\left\|I^{-}(a q)\right\| Cl^{-}(a q)\right|\left|H g_2 Cl_2\right| H g(l) P t(s) \\ & {\left[\text {Given } E_{{Cl}^{-}\left|{Hg}_2 {C} l_2\right| {Hg}}^0=0.26 {~V} \cdot E_{{Ag}^{+} / {Ag}}^0=0.8 {~V}, K_{s p}({AgI})=10^{-16} \text { and } \frac{2.303 R T}{F}=0.06\right]} \\ \end{aligned}

The overall reaction occurring in the above all is

Accepted Answer

$\frac{1}{2} {Hg}_2 {Cl}_2(s)+{Ag}(s)+{I}^{-}({aq}) \rightarrow {Hg}(l)+{Cl}^{-}({aq})+{AgI}(s)$

Answer

${Ag}^{+}(a q)+I^{-}(a q) \rightarrow {AgI}(s)$

Answer

${Hg}_2^{2+}({aq})+{I}_2 {Cl}^{-}({aq}) \rightarrow {Hg}_2 {C l}_2(s)$

Answer

Cell reaction is not possible

NEET UG CHEMISTRY MCQ: ELECTRO CHEMISTRY

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