$2 \mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{O}_{2}+4 \mathrm{H}^{\oplus}+4 \mathrm{e}^{-} ; \mathrm{E}_{\mathrm{red}}^{0}=1.23 \mathrm{V}$
$(\mathrm{R}=8.314 \;\mathrm{J} \mathrm{mol}^{-1} \mathrm{K}^{-1} ; \text { Temperature }=298 \;\mathrm{K} ;$ oxygen under std. atm. pressure of $1 \;bar$)
From nernst equation
$\mathrm{E}_{\text {cell }}=\mathrm{E}_{\text {cell }}^{0}-\frac{\mathrm{RT}}{\mathrm{nF}} \ln \mathrm{Q}$
at $1\; bar$ and $298 \mathrm{K}$
$\frac{2.303 \mathrm{RT}}{\mathrm{F}}=0.059$
$\mathrm{pH}=5 \Rightarrow\left[\mathrm{H}^{+}\right]=10^{-5} \mathrm{M}$
$\mathrm{E}_{\text {cell }}=1.23-\frac{0.059}{4} \log \left[\mathrm{H}^{+}\right]^{4}$
$\mathrm{E}_{\text {cell }}=1.23-\frac{0.059}{4} \log \left(10^{-5}\right)^{4}$
$=1.23+0.295=1.525 \mathrm{V}$
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$2X_2(s) + 3Y^{2+} (aq) \to 2X_2^{3+}(aq) + 3Y(s)$
$A_{(s)} + B^+ \to A^+ + B_{(s)} $; $\Delta H^o = -300\,kJ$ is $70\%$.
The standard electrode potential of cell is :- .................... $\mathrm{V}$