To determine the correct number of molecules of carbon dioxide (CO₂) and water (H₂O) produced during the oxidation of butene (C₄H₈), we must balance the given chemical equation:
\[ C_4H_8 + 6O_2 \rightarrow CO_2 + H_2O \]
Here, the left side of the equation shows 1 molecule of butene (C₄H₈) and 6 molecules of oxygen (O₂), whereas the right side lists carbon dioxide (CO₂) and water (H₂O) molecules without specified quantities.
Step-by-step balancing the equation:
1. **Balance the carbons**:
Butene (C₄H₈) has 4 carbons. Therefore, we need 4 molecules of CO₂ to balance the carbon atoms.
\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + H_2O \]
2. **Balance the hydrogens**:
Butene (C₄H₈) has 8 hydrogens. Therefore, we need 4 molecules of H₂O (since each H₂O molecule has 2 hydrogens) to balance the hydrogen atoms.
\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + 4H_2O \]
3. **Balance the oxygens**:
From the right side, we now have:
- 4 molecules of CO₂ contributing \(4 \times 2 = 8\) oxygen atoms
- 4 molecules of H₂O contributing \(4 \times 1 = 4\) oxygen atoms
The total oxygen atoms on the right side is \(8 + 4 = 12\).
On the left side, we have 6 molecules of O₂ providing \(6 \times 2 = 12\) oxygen atoms. The oxygens are balanced.
The fully balanced equation is:
\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + 4H_2O \]
Thus, for each molecule of C₄H₈ that reacts, 4 molecules of CO₂ and 4 molecules of H₂O are produced.
Therefore, the correct answer is:
B. Four carbon dioxide molecules and four water molecules
Consider the unbalanced equation for the oxidation of butene:
\[ C_4H_8 + 6O_2 \rightarrow CO_2 + H_2O \]
For each molecule of \[ C_4H_8 \] that reacts, how many molecules of carbon dioxide and water are produced?
A. Two carbon dioxide molecules and two water molecules
B. Four carbon dioxide molecules and four water molecules
C. Two carbon dioxide molecules and four water molecules
D. Four carbon dioxide molecules and two water molecules
1 answer
1 answer