Calculate the charge on mercurous ion and its magnetic moment. `EMF` of the cell given below is `0.0295V` at `25^(@)C`.
`Pt, Hg(l)|{:(0.01 M mercurous),(nitrate solution),(i n 0.1 M HNO_(3)):}||{:(0.1 M mercurous),(nitrate solution i n),(0.1 M HNO_(3)):}|Hg(l),Pt`

Explanation

To solve the problem of calculating the charge on the mercurous ion and its magnetic moment, we can follow these steps:

### Step 1: Identify the cell reaction and apply the Nernst equation
The given cell is:
\[ \text{Pt, Hg(l)} | \{0.01 \, \text{M mercurous}, \text{nitrate solution}, \text{in} \, 0.1 \, \text{M HNO}_3\} || \{0.1 \, \text{M mercurous}, \text{nitrate solution in} \, 0.1 \, \text{M HNO}_3\} | \text{Hg(l), Pt} \]

The half-reaction for the reduction of mercurous ion (Hg\(_2^{2+}\)) is:
\[ \text{Hg}_2^{2+} + 2e^- \rightarrow 2\text{Hg} \]
...