Question

The temperature coefficient of a cell whose operation is based on the reaction $Pb\left(s\right)+{HgCl}_2\left(aq\right)⟶{PbCl}_2\left(aq\right)+Hg\left(l\right)$ is :
${\left(\frac{dE}{dT}\right)}_p=1.5\ast {10}^{-4}V/K$ at 298 K
The change is entropy (in J/K mol) during the operation is :

• A. $8627$
• B. $57.9$
• C. $28.95$
• D. $14.475$

Answer 1

The correct option is C $28.95$

$\Delta S=nF\left(\frac{dE}{dT}\right)\Rightarrow 2\times 96500\times 1.5\times {10}^{-4}$
$\Rightarrow$ $28.95J/K-mol$ {Option (C)}