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Calculate the reduction potential for th...

Calculate the reduction potential for the following half cells at `25^@C`
`Cl_2|Cl^(-)(2 times 10^-5 M), E_(Cl_2,Cl^-)^@=+1.36V`

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To calculate the reduction potential for the half-cell reaction of \( \text{Cl}_2 \) to \( \text{Cl}^- \) at a concentration of \( 2 \times 10^{-5} \, \text{M} \) and given that the standard reduction potential \( E^\circ_{\text{Cl}_2/\text{Cl}^-} = +1.36 \, \text{V} \), we will use the Nernst equation. ### Step-by-Step Solution: 1. **Identify the half-reaction**: The half-reaction for the reduction of chlorine gas to chloride ions is: \[ \text{Cl}_2 + 2e^- \rightarrow 2\text{Cl}^- ...
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The standard reduction potential for the half-cell reaction, Cl_2 + 2e^(-) to 2Cl^(-) will be (Pt^(2+)+2Cl^(-)to Pt + Cl_2 , E_"cell"^@=-0.15 V , Pt^(2+) + 2e^(-) to Pt, E^@=1.20 V)