Let's figure out the number of carbon dioxide (CO₂) and water (H₂O) molecules produced during the oxidation of butene (C₄H₈).
The given unbalanced chemical equation is:
[tex]\[ C_4H_8 + 6 O_2 \rightarrow CO_2 + H_2O \][/tex]
The quantities provided are as follows:
- For each molecule of butene (C₄H₈), 6 molecules of oxygen (O₂) are required.
Now, let’s balance the equation step by step:
1. Balancing Carbon Atoms:
- Butene (C₄H₈) has 4 carbon atoms, so we need 4 molecules of CO₂ to balance the carbon atoms.
[tex]\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + H_2O \][/tex]
2. Balancing Hydrogen Atoms:
- Butene (C₄H₈) has 8 hydrogen atoms. Each molecule of water (H₂O) provides 2 hydrogen atoms, so we need 4 molecules of H₂O to balance the hydrogen atoms.
[tex]\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + 4H_2O \][/tex]
3. Balancing Oxygen Atoms:
- We now have on the right side: [tex]\( 4 \times \text{CO}_2 = 4 \times 2 = 8 \text{ oxygen atoms} \)[/tex] and [tex]\( 4 \times \text{H}_2\text{O} = 4 \times 1 = 4 \text{ oxygen atoms} \)[/tex].
- In total, there are [tex]\( 8 + 4 = 12 \text{ oxygen atoms} \)[/tex] on the product side.
- To balance this on the reactant side, each molecule of O₂ provides 2 oxygen atoms, so [tex]\( 6 \times O_2 \)[/tex] provides 12 oxygen atoms, matching the product side.
Thus, the balanced equation is:
[tex]\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + 4H_2O \][/tex]
From the balanced equation, we observe that for each molecule of butene (C₄H₈) that reacts, 4 molecules of carbon dioxide (CO₂) and 4 molecules of water (H₂O) are produced.
Therefore, the answer to the question is:
Four carbon dioxide molecules and four water molecules.
