Question

Balance the following equation:

$\mathrm{Al}{\left(\mathrm{OH}\right)}_3\stackrel{∆}{\to }{\mathrm{Al}}_2{\mathrm{O}}_3+{\mathrm{H}}_2\mathrm{O}$

Answer 1

Balanced chemical equation: A balanced chemical equation represent the equation in which the number of atom of each element is equal on both the reactant and product side.

Given reaction: $\underset{\mathrm{Aluminium}\mathrm{hydroxide}}{\mathrm{Al}{\left(\mathrm{OH}\right)}_3}\stackrel{∆}{\to }\underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3}+\underset{\mathrm{Water}}{{\mathrm{H}}_2\mathrm{O}}$

Balancing of chemical reaction:

Step 1: Writing the number of atoms on each reactant and product side

Element	Number of atoms on the reactant side	Number of atoms on the product side
Al	1	2
O	3	4
H	3	2

Aluminum (Al), Hydrogen (H), and Oxygen (O) are unbalanced in the above chemical reaction.

Step 2: Balancing of the Aluminium atoms

Multiply the Aluminium hydroxide by 2 on the reactant side.

$\underset{\mathrm{Aluminium}\mathrm{hydroxide}}{2\mathrm{Al}{\left(\mathrm{OH}\right)}_3}\stackrel{∆}{\to }\underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3}+\underset{\mathrm{Water}}{{\mathrm{H}}_2\mathrm{O}}$

Step 3: Balancing the other unbalanced atoms

Now, the Hydrogen and Oxygen atoms are unbalanced. So, multiply water on the product side by 3.

$\underset{\mathrm{Aluminium}\mathrm{hydroxide}}{2\mathrm{Al}{\left(\mathrm{OH}\right)}_3}\stackrel{∆}{\to }\underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3}+\underset{\mathrm{Water}}{3{\mathrm{H}}_2\mathrm{O}}$

Element	Number of atoms on the reactant side	Number of atoms on the product side
Al	2	2
O	6	6
H	6	6

All the elements have an equal number of atoms.

Thus, the balanced chemical equation is $\underset{\mathrm{Aluminium}\mathrm{hydroxide}}{2\mathrm{Al}{\left(\mathrm{OH}\right)}_3}\stackrel{∆}{\to }\underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3}+\underset{\mathrm{Water}}{3{\mathrm{H}}_2\mathrm{O}}$.