Question

Balance the equation $\mathrm{Al}+\mathrm{FeO}\to {\mathrm{Al}}_2{\mathrm{O}}_3+\mathrm{Fe}$

Answer 1

$\mathrm{Al}+\mathrm{FeO}\to {\mathrm{Al}}_2{\mathrm{O}}_3+\mathrm{Fe}$

Step 1: Count the number of atoms of each element on both the sides

Number of atoms of each element on LHS,

Aluminium(Al) = 1 atom, Iron(Fe) = 1 atom, Oxygen(O) = 1 atom

Number of atoms of each element on RHS,

Aluminium(Al) = 2 atoms, Iron(Fe) = 1 atom, Oxygen(O) = 3 atoms

We can see that there is an extra atom of Oxygen and aluminium in RHS.

Step 2:

Multiply the Aluminium by 2

$2\mathrm{Al}\left(\mathrm{s}\right)+\mathrm{FeO}\left(\mathrm{s}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+\mathrm{Fe}\left(\mathrm{s}\right)$

• Now on LHS, we have Al = 2 atoms, Fe = 1 atom, Oxygen = 1 atom
• On RHS, we have Al = 2 atoms, Fe = 1 atom, O = 3 atoms

Step 3:

Multiply the Iron oxide (FeO) by 3

$2\mathrm{Al}\left(\mathrm{s}\right)+3\mathrm{FeO}\left(\mathrm{s}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+\mathrm{Fe}\left(\mathrm{s}\right)$

• Now on LHS, we have Al = 2 atoms, Fe = 3 atom, Oxygen = 3 atom
• On RHS, we have Al = 2 atoms, Fe = 1 atom, O = 3 atoms

Step 4:

Multiply Iron by 3

$2\mathrm{Al}\left(\mathrm{s}\right)+3\mathrm{FeO}\left(\mathrm{s}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3\mathrm{Fe}\left(\mathrm{s}\right)$

• Now on LHS, we have Al = 2 atoms, Fe = 3 atom, Oxygen = 3 atom
• On RHS, we have Al = 2 atoms, Fe = 3 atom, O = 3 atoms

Now, the number of atoms of each element is the same on both sides and the equation is said to be balanced.

Therefore, the balanced chemical equation is $2\mathrm{Al}\left(\mathrm{s}\right)+3\mathrm{FeO}\left(\mathrm{s}\right)\to {\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3\mathrm{Fe}\left(\mathrm{s}\right)$