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 calculate 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: Write the reduction half-reaction
The reduction of magnesium ions in molten MgCl₂ can be represented by the following half-reaction:
\[ \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg (s)} \]

### Step 2: Determine the moles of magnesium to be deposited
To find the number of moles of magnesium (Mg) that corresponds to 1.2 g, we use the molar mass of magnesium, which is 24.0 g/mol:
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