Subject: Physical Chemistry · Chapter: Electrochemistry · Topic: Nernst Cells · Exam: JAM 2001-2022 · Marks: 2 · Difficulty: Medium
For a cell reaction, $\mathrm{Pb}(\mathrm{s})+\mathrm{Hg}_{2} \mathrm{Cl}_{2}(\mathrm{s}) \rightarrow \mathrm{PbCl}_{2}(\mathrm{s})+2 \mathrm{Hg}(l),\left(\frac{\partial \mathrm{E}}{\partial \mathrm{T}}\right)_{\mathrm{P}}$ is $1.45 \times 10^{-4} \mathrm{VK}^{-1}$. The entropy change (in $\mathrm{J} \mathrm{mol}^{-1} \mathrm{K}^{-1}$ ) for the reaction is ____ [Given: $1 \mathrm{F}=96500 \mathrm{C} \mathrm{mol}^{-1}$ ]
Answer
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