Question

106 State the type of reaction taking place. Also balance the equation.

$\mathrm{Mg}{\left(\mathrm{OH}\right)}_2\to \mathrm{MgO}+{\mathrm{H}}_2\mathrm{O}$

Answer 1

Step 1:- List the number of atoms of a different element present in the unbalanced equation

The given chemical equation is as follows:

$\mathrm{Mg}{\left(\mathrm{OH}\right)}_2\to \mathrm{MgO}+{\mathrm{H}}_2\mathrm{O}$

Element	Number of atoms in reactant	Number of atom in product
Mg	1	1
O	2	2
H	2	2

Step 2:- Write the balanced chemical equation

Since, the number of atoms of all the elements in the equation are equal on both the sides thus, the chemical equation is said to be balanced. $\underset{\mathbf{Magnesium}\mathbf{}\mathbf{hydroxide}}{\mathbf{Mg}{\mathbf{\left(}\mathbf{OH}\mathbf{\right)}}_{\mathbf{2}}}\mathbf{\to }\underset{\mathbf{Magnesium}\mathbf{}\mathbf{oxide}}{\mathbf{MgO}}\mathbf{+}\underset{\mathbf{Water}}{{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}$

Step 3:- Identify the type of reaction

Decomposition reaction is the reaction in which one reactant breaks down into two or more products. Here, in the given reaction, Magnesium hydroxide is decomposed into Magnesium oxide (MgO) and water (H₂O).

Therefore,$\underset{\mathbf{Magnesium}\mathbf{}\mathbf{hydroxide}}{\mathbf{Mg}{\mathbf{\left(}\mathbf{OH}\mathbf{\right)}}_{\mathbf{2}}}\mathbf{\to }\underset{\mathbf{Magnesium}\mathbf{}\mathbf{oxide}}{\mathbf{MgO}}\mathbf{+}\underset{\mathbf{Water}}{{\mathbf{H}}_{\mathbf{2}}\mathbf{O}}$ is a decomposition reaction.