For the reaction: H2 (1 bar) + 2AgCl(s) $\rightleftharpoons$ 2Ag(s) + 2H+ (0.1 M) + 2Cl− (0.1 M); ΔG

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For the reaction: H2 (1 bar) + 2AgCl(s) $\rightleftharpoons$ 2Ag(s) + 2H+ (0.1 M) + 2Cl− (0.1 M); ΔG0 = − 48,250 J at 25°C. The EMF of cell in which the given reaction takes place is

Accepted Answer

$\Delta G^{o} = - nF.E_{cell}^{o} \Rightarrow - 48250 = - 2 \times 96500 \times E_{cell}^{o}$

$\therefore E_{cell}^{o} = 0.25\text{ V} $$$\text{Now, }E_{cell} = E_{cell}^{o} - \frac{0.059}{2}.\log\frac{\left\lbrack H^{+} \right\rbrack^{2}\left\lbrack Cl^{-} \right\rbrack^{2}}{P_{H_{2}}} $$$= 0.25 - \frac{0.059}{2}.\log\frac{(0.1)^{2} \times (0.1)^{2}}{1} = 0.368\text{ V}$

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