Question

How would you balance: $\mathrm{Al}+{\mathrm{Fe}}_2{\mathrm{O}}_3\to {\mathrm{Al}}_2{\mathrm{O}}_3+\mathrm{Fe}$

Answer 1

Balancing the Chemical equation:

• When we balance chemical equations, we want the same number of each sort of atom on both sides of the equation.
• Only the coefficients are changed. The numbers in front of the molecule are called coefficients.
• Subscripts should never be changed.
• Metals must be balanced first, followed by nonmetals such as oxygen and hydrogen (hydrogen is not involved in this scenario).
• The unbalanced chemical reaction provided is

$\underset{\mathrm{Aluminium}}{\mathrm{Al}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\left(\mathrm{III}\right)\mathrm{oxide}}{{\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)}\to \underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}$

• It is a single displacement redox process in which Aluminium ($\mathrm{Al}$) and Iron ($\mathrm{Fe}$) swap places.
• As there are two Aluminium atoms on the right side, we must put a $2$ before the Aluminium on the left side.
• Second, the Iron must be balanced. As shown on the left, there are two Iron atoms in ${\mathrm{Fe}}_2{\mathrm{O}}_3$, thus a $2$ must be inserted on the right side to balance them.
• Finally, the oxygens must be balanced, but in this case, they are already at $3$ on each side, therefore the equation is now balanced.
• Thus, the balanced chemical reaction is:

$\underset{\mathrm{Aluminium}}{2\mathrm{Al}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\left(\mathrm{III}\right)\mathrm{oxide}}{{\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)}\to \underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)}+2\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}$