Question

Balance the following equation:
$...Fe+...{{H}_{2}}O\to ...F{{e}_{3}}{{O}_{4}}+...{{H}_{2}}$

Answer 1

Hint: A chemical equation without the stoichiometric coefficient is called as unbalance. These stoichiometric coefficients tell us the amount of each element present in the reaction.

Complete step by step answer: A balanced chemical equation tells us about the exact amount of element present in the compounds and taking part in the chemical reaction. The numerical values written before the compounds are called as their stoichiometric coefficient.
We are given a chemical reaction with an unknown amount of the elements involved, as the equation is not balanced. To balance the chemical equation, we have to write the quantities of elements present in the reactants and products, before the symbols of the elements.
So, in the reaction, $...Fe+...{{H}_{2}}O\to ...F{{e}_{3}}{{O}_{4}}+...{{H}_{2}}$, we have been given, no value for Fe in the reactant and 3 Fe in the product, so we have to write 3 before Fe in the reactant side. Now, given is ${{H}_{2}}O$ , which has O and H, 4 oxygen are present on the product side, so 4 is to be written before ${{H}_{2}}O$, now 8 hydrogen are at the reactant while 2 in the product, so 4 has to be written before ${{H}_{2}}$ in the product. The amount of $F{{e}_{3}}{{O}_{4}}$ is balanced and no value is written before it. So, the balanced equation becomes,
$3\,Fe+4\,{{H}_{2}}O\to F{{e}_{3}}{{O}_{4}}+4\,{{H}_{2}}$
Hence, the equation is balanced.

Note: The reaction of iron (Fe) with water is actually occurring in moisture, with the oxidation of iron that yields rust. It is an example of rusting that occurs in nature.