Question

When iron rusts, solid iron reacts with gaseous oxygen to form solid iron(iii) oxide. part a write a balanced chemical equation for this reaction?

Answer 1

The balanced chemical reaction for rusting of iron is $\boxed{{\text{4Fe}}\left(s\right)+3{{\text{O}}_2}\left(g\right)\to2{\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}\left(s\right)}$ .

Further explanation:

The chemical reaction that contains an equal number of atoms of the different elements in the reactant as well as in the product side is known as a balanced chemical reaction. The chemical equation is required to be balanced to follow the Law of the conservation of mass.

Rusting of iron occurs when impure iron comes in contact with water, oxygen, and other oxidants. The extent of rusting increases in seawater due to the presence of salt in it. Rust consists of hydrated iron oxides and iron oxide-hydroxides.

The steps to balance a chemical reaction are as follows:

Step 1: Complete the reaction and write the unbalanced symbol equation.

In the rusting reaction, Fe reacts with ${{\text{O}}_2}$ to form ${\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}$ . The physical state of Fe is solid, ${{\text{O}}_2}$  is gas, ${\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}$ is solid. The unbalanced chemical equation is as follows:

${\text{Fe}}\left(s\right)+{{\text{O}}_2}\left(g\right)\to{\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}\left(s\right)$

Step 2: Then we write the number of atoms of all the different elements that are present in a chemical reaction in the reactant side and product side separately.

⦁ On reactant side,

Number of iron atoms is 1.

Number of oxygen atoms is 2.

⦁ On product side,

Number of iron atoms is 2.

Number of oxygen atoms is 3.

Step 3: Initially, we try to balance the number of other atoms of elements except for carbon, oxygen, and hydrogen by multiplying with some number on any side. To balance the number of iron atoms, multiply Fe by 2. Now the reaction is,

$\boxed{\text{2}}{\text{Fe}}\left(s\right)+{{\text{O}}_2}\left(g\right)\to{\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}\left(s\right)$

Step 4: After this, we balance the number of atoms of carbon and then hydrogen atom followed by oxygen atoms. To balance the number of oxygen atoms, multiply  ${{\text{O}}_{\text{2}}}$ by 3, Fe by 2 and ${\text{F}}{{\text{e}}_{\text{2}}}{{\text{O}}_{\text{3}}}$  by 2. Now the reaction is,

$\boxed{\text{4}}{\text{Fe}}\left(s\right)+\boxed3{{\text{O}}_2}\left(g\right)\to\boxed2{\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}\left(s\right)$

Step 5: So the balanced chemical equation is given as follows:

${\text{4Fe}}\left(s\right)+3{{\text{O}}_2}\left(g\right)\to2{\text{F}}{{\text{e}}_2}{{\text{O}}_{\text{3}}}\left(s\right)$

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Answer details:

Grade: High School

Subject: Chemistry

Chapter: Chemical reaction and equation

Keywords: balanced chemical reaction, rusting of iron, Fe, O2, Fe2O3, solid, gas, 2, 3, 4, iron atoms, oxygen atoms, reactant side, product side, 4 Fe, 3 O2, 2 Fe2O3.

Answer 2

The balanced chemical equation for the reaction between the iron and oxygen to produce iron (iii) oxide is:

4Fe(s) + 3O₂(g) —> 2Fe₂O₃(s)

Chemical equation is a representation of chemical reaction with symbols and formula of the reactants and products taking part in the reaction.

All chemical equation must be balanced in order to validate the law of conservation of matter which states that matter can neither be created nor destroyed during a chemical reaction but can be transferred from one form to another.

NOTE: An unbalanced equation simply means matter has been created or destroyed.

The equation for the reaction between iron and oxygen to produce iron (iii) oxide is given below:

Fe(s) + O₂(g) —> Fe₂O₃(s)

The above equation can be balance as follow:

Fe(s) + O₂(g) —> Fe₂O₃(s)

There are 2 atoms of O on the left side and 3 atoms on the right side. It can be balance by writing 3 before O₂ and 2 before Fe₂O₃ as shown below:

Fe(s) + 3O₂(g) —> 2Fe₂O₃(s)

There are 4 atoms of Fe on the right side and 1 atom on the left side. It can be balance by writing 4 before Fe as shown below:

4Fe(s) + 3O₂(g) —> 2Fe₂O₃(s)

Therefore, the balanced equation for the reaction between iron and oxygen to produce iron (iii) oxide is

4Fe(s) + 3O₂(g) —> 2Fe₂O₃(s)

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