Question

Balance the equation

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

Answer 1

Steps in Balancing a Chemical Equation:

• First, count each type of atom in reactants and products present in the reaction, if the same number of each atom appears on both sides of the arrow then the reaction is balanced.
• If not, then place coefficients, as needed, in front of the symbols or formulas to increase the number of atoms or molecules of the substances. (try to use the smallest coefficients possible).
• Change only the coefficients, never change the subscripts in chemical formulas changing subscripts changes the substances involved in the reaction.
• Repeat this until the equation is balanced.

Balancing the reaction:

• The given chemical reaction is

$\underset{\mathrm{Iron}}{\mathrm{Fe}\left(\mathrm{s}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Ferrous}\mathrm{oxide}}{\mathrm{FeO}\left(\mathrm{s}\right)}$

• The number of Iron atoms presents on the product side and reactant side is equal.
• But the number of Oxygen atoms on the product side and reactant side are not equal.
• Therefore, increase the number of moles of Iron on the reactant side from one to two.
• So that, increase the number of moles of Ferric oxide in the product becomes one to two
• That is:

$\underset{\mathrm{Iron}}{2\mathrm{Fe}\left(\mathrm{s}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Ferrous}\mathrm{oxide}}{2\mathrm{FeO}\left(\mathrm{s}\right)}$

• Now here the number of Iron and Oxygen atoms on both sides is equal.

Therefore, the balanced chemical equation is $\underset{\mathrm{Iron}}{2\mathrm{Fe}\left(\mathrm{s}\right)}+\underset{\mathrm{Oxygen}}{{\mathrm{O}}_2\left(\mathrm{g}\right)}\to \underset{\mathrm{Ferrous}\mathrm{oxide}}{2\mathrm{FeO}\left(\mathrm{s}\right)}$