Question

For the galvanic cell,
$Zn(s)+C{u}^{2+}(0.02M)\to Z{n}^{2+}(0.04M)+Cu(s)$
$E_{\text{cell }}=$ ____$\times 10^{-2}$(Nearest integer)
[Use : $E_{Cu/C{u}^{2+}}^0=-0.34V,E_{Zn/Z{n}^{2+}}^0=+0.76V,\frac{2.303RT}{F}=0.059V$ ]

Answer 1

Answer: 109

$Z{n}_{(s)}+\underset{0.02M}{C{u}_{(aq.)}^{+2}}\to \underset{0.04M}{Z{n}^{+2}}+Cu(s)$
Nernst equation $=F_{\text{cell }}=E_{\text{cell }}^{\circ }-\frac{0.059}{2}\log \frac{\left[2n^{+2}\right]}{\left[C{u}^{+2}\right]}$
$\Rightarrow E_{\text{cell }}\left[E_{\text{cell }}^{\circ }-E_{Z{n}^{+2}/Zn}^{\circ }\right]-\frac{0.059}{2}\log \frac{0.04}{0.02}$
$\Rightarrow E_{\text{cell }}[0.34-(-0.76)]-\frac{0.059}{2}{\log }^2$
$\Rightarrow E_{\text{cell }}1-1-\frac{0.059}{2}\times 0.3010$
$=1.0911=109.11\times 10^{-2}$
$=109$