Balance the following chemical equation and identify the type of chemical reaction.
$\underset{}{HgO (s)} \overset{∆}{\to} Hg (l) + O_{2} (g)$

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Solution

Balanced equation: the chemical equation in which the number of atoms of each element on the reactant side as well as the product side is equal are known as a balanced equation.
Balancing the following chemical equation:
$\underset{mercuric oxide}{HgO (s)} \overset{∆}{\to} \underset{mercury}{Hg (l)} + \underset{oxygen}{O_{2} (g)}$
Steps to Balance the chemical equation:
Count the number of atoms of each element on either side. Now first balance the compound with the maximum number of atoms
A number of atoms of each element on the reactant side:
Hg=1 O=1
A number of atoms of each element on the product side:
Hg=1 O=2
Thus one oxygen is extra on the product side so we will multiply the reactant side by 2, and on the product side we will multiply Hg by 2 now the reaction is balanced.
$\underset{}{2 HgO (s)} \overset{∆}{\to} 2 Hg (l) + O_{2} (g)$
Decomposition reaction: a reaction in which a compound breaks down into two or more simple compounds on heating is called a decomposition reaction.
$XY \to X + Y$
Thus this reaction is an example of a decomposition reaction as mercuric oxide breaks down to give mercury and oxygen.

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