# Question #a2593

Aug 18, 2016

${\text{Mg"_ ((s)) + "H"_ (2(g)) -> "MgH}}_{2 \left(s\right)}$

#### Explanation:

Magnesium metal will react with hydrogen gas at very high pressures and at high temperatures to form magnesium hydride, ${\text{MgH}}_{2}$.

The balanced chemical equation that describes this synthesis reaction looks like this

${\text{Mg"_ ((s)) + "H"_ (2(g)) -> "MgH}}_{2 \left(s\right)}$

You can also think of this reaction as being an example of a redox reaction. Here magnesium metal is being oxidized by hydrogen gas which acts as a reducing agent.

Similarly, hydrogen is being reduced by magnesium which acts as an oxidizing agent.