Chemistry - Electrochemistry Question with Solution | TestHub

Cell reaction

${\mathrm{Cu}}^{2+}\left(\mathrm{aq}\right)+\mathrm{Zn}\rightleftharpoons \mathrm{Cu}\left(\mathrm{s}\right)+{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)$

$0.02\mathrm{M} 0.04\mathrm{M}$

$\left.E_{cell}^0=E_{C{u}^{2+}\mid Cu}^0-E_{Z{n}^{2+}\mid Zn}^0\right]$

$=0.34-(-0.75)=1.1 \mathrm{V}$

${\mathrm{E}}_{\mathrm{cell}}={\mathrm{E}}_{\mathrm{cell}}^0-\frac{0.059}{2}\log \frac{\left[{\mathrm{Zn}}^{2+}\right]}{\left[{\mathrm{Cu}}^{2+}\right]}$

$=1.1-\frac{0.059}{2}\log \left(\frac{0.04}{0.02}\right)$

$=1.1-0.03\log 2=1.1-0.03\times 0.30$

$=1.0915=1.09 \mathrm{V}=109\times {10}^{-2} \mathrm{V}$