Calculate the strength of the current required to deposit 1.2 g magnesium from molten `MgCl_(2) ` in hour .
`[1F= 96,500Cmol^(-1), ("atomic mass"): Mg =24.0 u]`

Explanation

To solve the problem of calculating the strength of the current required to deposit 1.2 g of magnesium from molten MgCl₂ in one hour, we can follow these steps:

### Step 1: Determine the electrochemical equivalent (Z)
The electrochemical equivalent (Z) can be calculated using the formula:
\[ Z = \frac{\text{Molecular weight}}{\text{n-factor} \times F} \]
Where:
- Molecular weight of Mg = 24 g/mol
- n-factor for MgCl₂ = 2 (since 2 electrons are required to deposit 1 mole of Mg)
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