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प्रश्न
Calculate the e.m.f. of the following cell reaction at 298 K:
\[\ce{Mg_{(s)} + Cu{^{2+}} (0.0001 M) -> Mg{^{2+}} (0.001M) + Cu_{(s)}}\]
The standard potential (E°) of the cell is 2.71 V.
संख्यात्मक
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उत्तर
Given:
Cell reaction: \[\ce{Mg_{(s)} + Cu{^{2+}} (0.0001 M) -> Mg{^{2+}} (0.001M) + Cu_{(s)}}\]
Standard EMF, \[\ce{E{^{\circ}_{cell}}}\] = 2.71 V
Temperature (T) = 298 K
\[\ce{Q = \frac{Mg^{2+}}{Cu^{2+}}}\]
= \[\ce{\frac{10^{-3}}{10^{-4}}}\]
= 10
n = 2
\[\ce{E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} log Q}\] ...(Using the Nernst equation)
= \[\ce{2.71 - \frac{0.0591}{2} log 10}\]
= 2.71 − 0.02955 × 1 ...(log 10 = 1)
= 2.71 − 0.02955
= 2.680 V
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Galvanic Cells, Mechanism of Current Production in a Galvanic Cell; - Mechanism of Production of Electric Current in a Galvanic Cell
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