Question

How do you balance:$Al+F{{e}_{2}}{{O}_{3}}?A{{l}_{2}}{{O}_{3}}+Fe?$

Answer 1

Hint: we need to balance a chemical equation as we need to follow the “law of conservation of mass “and so the number of elements involved in a chemical reaction should remain the same at reactant and product side.

Complete answer:
Before we start the question let us some understand some terms first:
Law of conservation of mass: it states that that mass can neither be created nor be destroyed in a chemical reaction. Therefore, every reaction follows the “law of conservation of mass.
Any chemical reaction needs to be balanced, as it is only rearrangement of atoms. Atoms are neither created nor can be destroyed in a chemical reaction. Therefore, chemical reaction needs to balance to follow the law of conservation of mass.
We are using an algebraic balancing method. This method of balancing chemical equations involves assigning algebraic variables as stoichiometric coefficients to each species in the unbalanced chemical equation.
As given in the chemical equation we first try to balance the metal atom i.e., (Al and Fe) and then we start balancing the oxygen atom and at last we balance the hydrogen atom (if present any).
So, we first multiply Al by $2$ as there $2$ atoms of Al present in product side, then we balance Fe by multiplying $2$in product side, and then we see both reactant and product side get balanced (i.e., containing same number of atoms).
So, our balanced reaction becomes:$2Al+F{{e}_{2}}{{O}_{3}}\to A{{l}_{2}}{{O}_{3}}+2Fe$.

Note:
We should always balance the chemical reaction as we have to follow the law of conservation of mass. To balance always start with balancing metal first then oxygen / carbon terms then at last hydrogen atom.