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 (Kc) for the reaction:

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

with a given standard cell potential \( E^\circ_{cell} = 0.46 \, V \), we can use the Nernst equation in the form:

\[
E^\circ_{cell} = \frac{0.0591}{n} \log K_c
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