Assume a cell with the following reaction
\(\mathrm{Cu_{(s)} + 2Ag^{+}(1\times 10^{-3}\,M) \rightarrow Cu^{2+}(0.250\,M) + 2Ag_{(s)}}\)
\(E^{\Theta}_{cell} = 2.97\) V
\(E_{cell}\) for the above reaction is ______________ V. (Nearest integer)
[Given : log 2.5 = 0.3979, T = 298 K]
\(\mathrm{Cu_{(s)} + 2Ag^{+}(1\times 10^{-3}\,M) \rightarrow Cu^{2+}(0.250\,M) + 2Ag_{(s)}}\)
\(E^{\Theta}_{cell} = 2.97\) V
\(E_{cell}\) for the above reaction is ______________ V. (Nearest integer)
[Given : log 2.5 = 0.3979, T = 298 K]
Show Hint
Correct Answer: 3
Solution and Explanation
Nernst equation at 298 K: \(E = E^{\Theta} - \dfrac{0.0591}{n}\log Q\)
\(\log Q = \log 2.5 + 5 = 5.3979\)
\(E = 2.97 - \dfrac{0.0591}{2}\times 5.3979 = 2.97 - 0.02955\times 5.3979 = 2.97 - 0.1595 = 2.81\) V
Nearest integer = 3
Answer: 3
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