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Question
Represent the cell in which the following reaction takes place.The value of E˚ for the cell is 1.260 V. What is the value of Ecell?
\[\ce{2Al (s) + 3Cd^{2+} (0.1M) -> 3Cd (s) + 2Al^{3+} (0.01M)}\]
Solution
Al(s) /Cd2+ (0.1M) // Al3+ (0.01M) /Cd(s)
\[\ce{2Al(s) + 3Cd^{2+} (0.1M) -> 3Cd (s) + 2Al^{3+} (0.01M)}\]
Ecell = E°cell `(- 0.059)/n log [Al^(3+}]^2/([Cd^(2+)]^3`
Ecell = `1.26 - 0.059/6 log (0.01)^2/(0.1)^3`
= `1.26 - 0.059/6 (- 1)`
= 1.26 + 0.009
= 1.269 V
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