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प्रश्न
Calculate emf of the following cell at 298 K:
Mg(s) | Mg2+(0.1 M) || Cu2+ (0.01) | Cu(s)
[Given Eocell = +2.71 V, 1 F = 96500 C mol–1]
उत्तर
The cell reaction can be represented as:
Mg(s) + Cu2+(aq.) → Mg2+(aq.) + Cu(s)
\[Given, \]
\[ E_{cell}^o = + 2 . 71 V\]
\[T = 298 K\]
\[\text{According to the Nernst equation:} \]
\[E = E_{cell}^o - \frac{0 . 0591}{2}\log\frac{[ {Mg}^{2 +} ]}{\left[ {Cu}^{2 +} \right]} = 2 . 71 - \frac{0 . 0591}{2}\log\frac{0 . 1}{0 . 01}\]
\[ = 2 . 71 - 0 . 0295 \log 10 = 2 . 71 - 0 . 0295\]
\[ = 2 . 6805 V\]
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