Find the equilibrium constant for the reaction
`Cu^(2+)+ 1n^(2+) Cu^(+) + 1n^(3+)`
Given that `E_(CU^(2+)//CU^(+))^(@) = 0.15V, E_(In^(2+)//1n^(+)) = -0.4V`
`E_(1n^(3+)//1n^(+))^(@) = - 0.42V`

Explanation

To find the equilibrium constant for the reaction

\[ \text{Cu}^{2+} + \text{In}^{2+} \rightleftharpoons \text{Cu}^{+} + \text{In}^{3+} \]

we will use the provided standard electrode potentials and the Nernst equation.

### Step 1: Identify the half-reactions and their standard potentials

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