Question

Complete and balance the following equation :

$3\mathrm{Mg}+{\mathrm{N}}_2\to \mathrm{\_\_\_\_\_\_\_}$

Answer 1

When magnesium ribbon burns even in the absence of oxygen and in the presence of nitrogen, which is not a supporter of combustion.

The reaction gives magnesium nitride.

$\underset{\mathrm{Magnesium}}{3\mathrm{Mg}\left(\mathrm{s}\right)}+\underset{\mathrm{Nitrogen}}{{\mathrm{N}}_2\left(\mathrm{g}\right)}\stackrel{\mathrm{Burn}}{\to }\underset{\mathrm{Magnesium}\mathrm{nitride}}{{\mathbf{Mg}}_{\mathbf{3}}{\mathbf{N}}_{\mathbf{2}}\mathbf{\left(}\mathbf{s}\mathbf{\right)}}$

• Here, the equation is already balanced as we have an equal number of atoms on both sides of the equation.
• This is an example of a combination reaction.
• A reaction in which two or more reactants combine to form a single product is known as a combination reaction.