Chemistry - Electrochemistry Question with Solution | TestHub

$\begin{array}{ll}\text{Anodic Reaction}& \left[\mathrm{T}{\ell }_{(s)}\to {\mathrm{T}}^{+}{}_{(\mathrm{aq})}+{\mathrm{e}}^{-}\right]2\\ \text{Cathodic Reaction}& {\mathrm{Cu}}^{+2}{}_{(\mathrm{aq})}+2{\mathrm{e}}^{-}\to {\mathrm{Cu}}_{(\mathrm{s})}\\ \text{Overall Redox Reaction}& 2\mathrm{T}{\ell }_{(\mathrm{s})}+{\mathrm{Cu}}^{+2}{}_{(\mathrm{aq})}\to 2\mathrm{T}{\ell }_{(\mathrm{aq})}^{+}+{\mathrm{Cu}}_{(\mathrm{s})}\end{array}$ ${\mathrm{E}}_{\text{cell }}={\mathrm{E}}_{\text{cell }}^o-\frac{0.0591}{2}\log \frac{{\left[\mathrm{T}{\ell }^{+}\right]}^2}{\left[{\mathrm{Cu}}^{+2}\right]}$ ${\mathrm{E}}_{\text{cell }}$ increases by increasing concentration of $\left[{\mathrm{Cu}}^{+2}\right]$ ions.