An excess of liquid mercury is added to an acidified solution of ` 1 xx 10^(-3) M Fe^(3+)` . It is found that 5% of `Fe^(3+)` remains at equilibrium at `25^@C` . Calculate `E_(Hg^(2+)) , Hg^+)^@` assuming that the only reaction that occurs is
`2Hg + 2Fe^(3+) to Hg_2^(2+) + 2Fe^(2+)`

Explanation

To solve the problem step by step, we will follow the reaction and the equilibrium conditions given in the question.

### Step 1: Understand the Reaction
The reaction given is:
\[ 2 \text{Hg} + 2 \text{Fe}^{3+} \rightarrow \text{Hg}_2^{2+} + 2 \text{Fe}^{2+} \]

### Step 2: Initial Concentration of \( \text{Fe}^{3+} \)
The initial concentration of \( \text{Fe}^{3+} \) is given as:
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