Balance the following reactions: $\mathrm{Fe}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{Fe}}_3{\mathrm{O}}_4+{\mathrm{H}}_2\uparrow$

 

A balanced equation is one in which the number of atoms of each element on the reactant and product sides is equal. It always obeys the rule of conservation of mass and maintains electrical neutrality. The law of conservation of mass holds that mass cannot be generated or destroyed.

According to the rule of conservation of mass, during a chemical reaction, the mass must always be constant and unchanging. Since all of the elements and compounds in a balanced equation are present in equal proportions on both sides of the reaction, this means that the mass of the entire process is conserved. So, in light of the concept of conservation of mass, we may state that a balanced chemical equation is also balanced.

A balanced equation is an equation in which the number of atoms of each element is equal on the reactant side and product side.

First, we balance the number of iron atoms, we get,

$3\mathrm{Fe}+{\mathrm{H}}_2\mathrm{O}\to {\mathrm{Fe}}_3{\mathrm{O}}_4+{\mathrm{H}}_2$

By balancing, the number of hydrogen and oxygen atoms, we get the balanced chemical equation is:

$3\mathrm{Fe}+4{\mathrm{H}}_2\mathrm{O}\to {\mathrm{Fe}}_3{\mathrm{O}}_4+4{\mathrm{H}}_2$

Hence option (A) is correct.