40 mL of 0.125 M of `NiSO_(4)` solution is electrolysed by a current of 0.05 amp for 40 minutes. (i) Write the equation for the reactions occurring at each electrode. (ii) How many coulombs of electricity passed through the solution ? (iii) How many grams of the product deposited on the cathode ? (iv) How long will the same current have to pass through the solution to remove completely the metal ions from the solution ? (v) At the end of electrolysis how many grams of the product would appear at the anode ?

Explanation

To solve the given problem step by step, we will address each part of the question systematically.

### Step 1: Write the equations for the reactions occurring at each electrode.

**At the Cathode (Reduction):**
Nickel ions (\(Ni^{2+}\)) are reduced to nickel metal (\(Ni\)):
\[ Ni^{2+} + 2e^- \rightarrow Ni \]

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