$(F = 96500 \,C\, mol^{-1})$
For the cell reaction,
\(2 \mathrm{Ag}^{+}+\mathrm{Cu} \rightarrow \mathrm{Cu}^{2+}+2 \mathrm{Ag}\)
\(\Delta E^{\circ}\) cell \(=+0.46 \mathrm{V}\)
\(\Delta \mathrm{G}^{\circ}=-2 \times 96500 \times 0.46\)
\(=-88780 \mathrm{J}\)
\(=-88.7 \mathrm{kJ}\)
\(=-89.0 \mathrm{kJ}\)
$M{g^{2 + }} + 2{e^ - } \to Mg(s);\,\,E = - 2.37\,V$
$C{u^{2 + }} + 2{e^ - } \to Cu(s);\,\,\,E = + 0.33\,V$
${Cu}({s})\left|{Cu}^{2+}({aq})(0.01 {M}) \| {Ag}^{+}({aq})(0.001 {M})\right| {Ag}({s})$ કોષ માટે ,કોષનો પોટેન્શિયલ $=.....\times 10^{-2} {~V}$
[ઉપયોગ : $\frac{2.303 {RT}}{{F}}=0.059$ ]
$Zn^{2+}(aq) + 2e^{-} $ $\rightleftharpoons$ $ Zn (s)$ , $E^o_{RP}= -0.762\, V$,
$Cr^{3+}(aq) + 3e^{-} $ $\rightleftharpoons$$ Cr(s)$, $E^o_{RP} = -0.740\, V$
$2H^{+}(aq) + 2e^{-} $$\rightleftharpoons$$ H_2(g)$, $E^o_{RP} = 0.00\,V$,
$Fe^{3+}_{(aq)} + 2e^{-} $$\rightleftharpoons$$ Fe^{2+}(aq)$ , $E^o_{RP} = 0.77 \,V$