(a) How many mole of mercury will be produced by electrolysing 1.0 M Hg `(NO_(3))_(2)` solution with a current of 2.00 A for 3 hours? [Hg`(NO_(3))_(2) = 200.6 g mol^(-1)`].
(b) A voltaic cell is set up at `25^(@)`C with the following half-cells `Al^(3+)` (0.001M) and `Ni^(2+)` (0.50M). Write an equation for the reaction that occurs when the cell generates an electric current and determine the cell potential.
(Given : `E_(Ni^(2+)//Ni)^(2)=- 0.25 V,E_(Al^(3+)//Al)^(@)= - 1.66V`)

Explanation

### Step-by-Step Solution

**(a)** To find out how many moles of mercury will be produced by electrolyzing a 1.0 M Hg(NO₃)₂ solution with a current of 2.00 A for 3 hours, we can use Faraday's laws of electrolysis.

1. **Convert Time to Seconds:**
\[ \text{Time} = 3 \text{ hours} \times 3600 \text{ seconds/hour} = 10800 \text{ seconds} \]
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