Given, the enthalpy of formation of `MgCl_((s))` is `-125 kJ mol^(-1)` and the entahpy of formation of `MgCl_(2(s))` is`-642kJ mol^(-1)`. Predict whether `MgCl` will undergo disproportionnation or not? If yes, calculate the enthalpy of disproportion.

Explanation

To determine whether `MgCl` will undergo disproportionation and to calculate the enthalpy of disproportionation, we will follow these steps:

### Step 1: Write the formation reactions
The enthalpy of formation for `MgCl` and `MgCl2` can be represented by their respective formation reactions:

1. For `MgCl`:
\[
\text{Mg (s)} + \frac{1}{2} \text{Cl}_2 (g) \rightarrow \text{MgCl (s)} \quad \Delta H_1 = -125 \, \text{kJ/mol}
...