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Calculate the e.m.f. and DeltaG for the ...

Calculate the e.m.f. and `DeltaG` for the cell reaction at 298 K:
`Mg_((s))"/"Mg_((0.1M))^(2+)"//"Cu_((0.01M))^(2+)"/"Cu_((s))`
Given `E_("cell")^(@) = -2.71V`
`1F=96,500C`

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the electromotive force (e.m.f.) and the Gibbs free energy change (ΔG) for the given cell reaction at 298 K. ### Step 1: Identify the half-reactions The cell reaction is: \[ \text{Mg}_{(s)} + \text{Cu}^{2+}_{(0.01M)} \rightarrow \text{Mg}^{2+}_{(0.1M)} + \text{Cu}_{(s)} \] The half-reactions are: 1. Oxidation at the anode: ...
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