Chemistry - Electrochemistry Question with Solution | TestHub

$\begin{array}{rlrl}& {\mathrm{E}}_{\text{cell }}=-\frac{0.059}{1}\log \frac{{\left[{\mathrm{H}}^{+}\right]}_{\mathrm{a}}}{{\left[{\mathrm{H}}^{+}\right]}_{\mathrm{c}}}& & \end{array}$

$=-0.059\left({\mathrm{pH}}_{\mathrm{c}}-{\mathrm{pH}}_{\mathrm{a}}\right)$

$=-0.059(6-3)=-0.177\mathrm{V}$

$\because {\mathrm{E}}_{\text{cell }}$ is -ve , so reaction is non-spontaneous.