# al + fe2 o3

Open in App

Solution

## 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 tát 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: $\underset{\mathrm{Aluminium}}{2\mathrm{Al}\left(\mathrm{s}\right)}+\underset{\mathrm{Iron}\left(\mathrm{III}\right)\mathrm{oxide}}{{\mathrm{Fe}}_{2}{\mathrm{O}}_{3}\left(\mathrm{s}\right)}\to \underset{\mathrm{Aluminium}\mathrm{oxide}}{{\mathrm{Al}}_{2}{\mathrm{O}}_{3}\left(\mathrm{s}\right)}+2\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}$

Bạn đang xem: al + fe2 o3 Xem thêm: địa 10 cánh diều bài 9

Suggest Corrections 25

Join BYJU'S Learning Program