A solution of `Ni(NO_(3))_(2)` is electrolysed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?

Options

A. 0.15
B. 0.05
C. `(0.20)`
D. `(0.10)`

Explanation

To determine how many moles of nickel (Ni) will be deposited at the cathode when a solution of Ni(NO₃)₂ is electrolyzed using 0.1 Faraday of electricity, we can follow these steps:

### Step 1: Understand the Electrolysis Reaction
The electrolysis of nickel(II) nitrate (Ni(NO₃)₂) involves the reduction of nickel ions (Ni²⁺) at the cathode. The half-reaction can be represented as:
\[ \text{Ni}^{2+} + 2e^- \rightarrow \text{Ni} \]
This equation shows that 2 moles of electrons are required to deposit 1 mole of nickel.

### Step 2: Calculate the Amount of Electricity Required
...