Answered

At Westonci.ca, we provide reliable answers to your questions from a community of experts. Start exploring today! Get quick and reliable solutions to your questions from a community of seasoned experts on our user-friendly platform. Get quick and reliable solutions to your questions from a community of experienced experts on our platform.

Select the correct answer.

Iron reacts with atmospheric oxygen to form iron oxide or ferric oxide. Look at the chemical equation for this reaction:

[tex]\[ \text{Fe} + \text{O}_2 \rightarrow \text{Fe}_2\text{O}_3 \][/tex]

This equation is unbalanced. Which of the following is the correct balanced equation for this reaction?

A. [tex]\[ 4 \text{Fe} + 3 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \][/tex]

B. [tex]\[ 3 \text{Fe} + 4 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \][/tex]

C. [tex]\[ 2 \text{Fe} + 4 \text{O}_2 \rightarrow 3 \text{Fe}_2\text{O}_3 \][/tex]

D. [tex]\[ 3 \text{Fe} + 3 \text{O}_2 \rightarrow 4 \text{Fe}_2\text{O}_3 \][/tex]

E. [tex]\[ 4 \text{Fe} + 4 \text{O}_2 \rightarrow 3 \text{Fe}_2\text{O}_3 \][/tex]

Sagot :

GinnyAnswer
To balance the chemical equation for the reaction of iron with atmospheric oxygen to form iron(III) oxide (ferric oxide), let us start with the unbalanced equation provided:

[tex]\[ \text{Fe} + \text{O}_2 \rightarrow \text{Fe}_2\text{O}_3 \][/tex]

### Step-by-Step Balancing

#### Step 1: Count the Number of Atoms of Each Element
First, we'll count the number of iron (Fe) and oxygen (O) atoms on both sides of the unbalanced equation.

- Reactants:
- Iron (Fe) atoms: 1
- Oxygen (O) atoms: 2

- Products:
- Iron (Fe) atoms: 2
- Oxygen (O) atoms: 3

#### Step 2: Balance Iron (Fe) Atoms
To balance the number of Fe atoms on both sides, we need to have the same number of Fe atoms in the reactants and in the products. Since Fe appears as a single atom on the reactant side and as part of \(\text{Fe}_2\text{O}_3\) on the product side, we can place a coefficient of 4 in front of Fe on the reactant side, giving us:

[tex]\[ 4 \text{Fe} + \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \][/tex]

- Reactants:
- Iron (Fe) atoms: 4
- Oxygen (O) atoms: 2

- Products:
- Iron (Fe) atoms: 4 (since there are 2 \(\text{Fe}_2\text{O}_3\) molecules, and each contains 2 Fe atoms)
- Oxygen (O) atoms: 6 (since there are 2 \(\text{Fe}_2\text{O}_3\) molecules, and each contains 3 O atoms)

#### Step 3: Balance Oxygen (O) Atoms
To balance the number of O atoms, we now see that we have 2 O atoms on the reactant side and 6 O atoms on the product side. To balance this, we need to place a coefficient of 3 in front of \(\text{O}_2\) on the reactant side, giving us:

[tex]\[ 4 \text{Fe} + 3 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \][/tex]

- Reactants:
- Iron (Fe) atoms: 4
- Oxygen (O) atoms: 6 (since there are 3 \(\text{O}_2\) molecules, and each contains 2 O atoms)

- Products:
- Iron (Fe) atoms: 4
- Oxygen (O) atoms: 6

Now the equation is balanced, with 4 Fe atoms and 6 O atoms on both the reactant and product sides.

### Conclusion
The balanced chemical equation for the reaction of iron with oxygen to form iron(III) oxide is:

[tex]\[ 4 \text{Fe} + 3 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \][/tex]

Thus, the correct answer is:

A. [tex]\( 4 \text{Fe} + 3 \text{O}_2 \rightarrow 2 \text{Fe}_2\text{O}_3 \)[/tex]
Thanks for using our service. We're always here to provide accurate and up-to-date answers to all your queries. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. Stay curious and keep coming back to Westonci.ca for answers to all your burning questions.