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Calculate the reduction potential for th...

Calculate the reduction potential for the following half cells at `25^@C`
`Mg|Mg^(2+) (1 times 10^-4 M), E_(Mg,Mg^(2+))^@=+2.36V`

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To calculate the reduction potential for the half-cell reaction \( \text{Mg} | \text{Mg}^{2+} (1 \times 10^{-4} \, \text{M}) \) at \( 25^\circ C \), we will use the Nernst equation. The standard reduction potential for the half-cell reaction is given as \( E^\circ_{\text{Mg}, \text{Mg}^{2+}} = +2.36 \, \text{V} \). ### Step-by-Step Solution: 1. **Identify the Reaction**: The half-cell reaction can be written as: \[ \text{Mg} \rightarrow \text{Mg}^{2+} + 2e^- ...
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