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 solve the problem of how many moles of Ni will be deposited at the cathode during the electrolysis of a Ni(NO₃)₂ solution 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 at the cathode can be written as:
\[ \text{Ni}^{2+} + 2e^- \rightarrow \text{Ni} \]

### Step 2: Determine the Amount of Charge Supplied
We are given that 0.1 Faraday of electricity is supplied. A Faraday (1 F) is the amount of electric charge required to deposit one mole of a monovalent ion. For divalent ions like Ni²⁺, it will require 2 Faradays to deposit one mole of Ni.
...