Calculate the equilibrium constant of the reaction `:`
`Cu(s)+2Ag(aq) hArrCu^(2+)(aq) +2Ag(s)`
`E^(c-)._(cell)=0.46V`

Explanation

To calculate the equilibrium constant (K) for the reaction:

\[ \text{Cu(s)} + 2\text{Ag}^+(aq) \rightleftharpoons \text{Cu}^{2+}(aq) + 2\text{Ag(s)} \]

given that the standard cell potential (\(E^{\circ}_{cell}\)) is 0.46 V, we can use the Nernst equation. The Nernst equation in its simplified form for equilibrium conditions is:

\[ E_{cell} = E^{\circ}_{cell} - \frac{0.0591}{n} \log K \]

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