ABC26PH0415 · Electrochemistry

Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Nernst Cells · Exam: GATE 2005-2021 · Marks: 2 · Difficulty: Medium

Consider the electrochemical cell
\[ \mathrm{M(s)|MI_2(s)|MI_2(aq)|M(s)} \]
where 'M' is a metal. At 298 K, the standard reduction potential are
\[ \mathrm{E}^{\mathrm{o}}_{\mathrm{M^{2+}(aq)/M(s)}} = -0.12\,\mathrm{V},\ \mathrm{E}^{\mathrm{o}}_{\mathrm{MI_2(s)/M(s)}} = -0.36\,\mathrm{V} \text{ and the temperature coefficient is} \]
\[ \left(\frac{\partial \mathrm{E}^{\mathrm{o}}_{\mathrm{cell}}}{\partial \mathrm{T}}\right)_{\mathrm{P}} = 1.5 \times 10^{-4}\,\mathrm{V\,K^{-1}}. \]
At this temperature the standard enthalpy change for the overall cell reaction, $\Delta_{\mathrm{r}}\mathrm{H}^{\mathrm{o}}$, is ____ $\mathrm{kJ\,mol^{-1}}$. (Round off to two decimal place) (Faraday constant $\mathrm{F} = 96500\,\mathrm{C\,mol^{-1}}$)
Answer
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