Calculate the equilibrium constant for the reaction :
`Fe(s)Cd^(2+)(aq)harrFe^(2+)(aq)+Cd(s)`
`("Given" E_(cd^(2+)//Cd)^(@)=-0.40 V, E_(Fe^(2+)//Fe)^(@)=-0.44 V)`

Explanation

To calculate the equilibrium constant for the reaction:

\[ \text{Fe}(s) + \text{Cd}^{2+}(aq) \rightleftharpoons \text{Fe}^{2+}(aq) + \text{Cd}(s) \]

we will follow these steps:

### Step 1: Identify the half-reactions and their standard reduction potentials.
- The reduction potential for cadmium is given as:
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