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(10Cl^(-)(aq) + 2MnO(4)^(-)(aq) + 16H^(+...

`(10Cl^(-)(aq) + 2MnO_(4)^(-)(aq) + 16H^(+)(aq) rightarrow 5Cl_(2)(g) + 2Mn^(2+) + 8H_2O)(l)`
The value of `E^(@)` for this reaction at `25^(@)C` is 0.15 V. What is the value of K for this reaction?

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To find the equilibrium constant \( K \) for the given reaction, we can use the Nernst equation. The Nernst equation relates the standard cell potential (\( E^\circ \)) to the equilibrium constant (\( K \)) at a given temperature. ### Step-by-Step Solution: 1. **Write the Nernst Equation**: The Nernst equation can be expressed as: \[ E = E^\circ - \frac{0.0591}{n} \log K ...
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