To determine the products formed during the combustion of one molecule of [tex]\( C_4H_8 \)[/tex], we first need to refer to the balanced chemical equation for its combustion. The balanced equation for the combustion of butene ([tex]\( C_4H_8 \)[/tex]) is:
[tex]\[ C_4H_8 + 6O_2 \rightarrow 4CO_2 + 4H_2O \][/tex]
Let's break down what this equation tells us:
1. One molecule of [tex]\( C_4H_8 \)[/tex] reacts with six molecules of [tex]\( O_2 \)[/tex] (oxygen).
2. This reaction produces four molecules of [tex]\( CO_2 \)[/tex] (carbon dioxide).
3. Additionally, the reaction produces four molecules of [tex]\( H_2O \)[/tex] (water).
Therefore, for each molecule of [tex]\( C_4H_8 \)[/tex] that reacts:
- Number of carbon dioxide ([tex]\( CO_2 \)[/tex]) molecules produced: 4
- Number of water ([tex]\( H_2O \)[/tex]) molecules produced: 4
Thus, the correct response to the question is:
#### For each molecule of [tex]\( C_4H_8 \)[/tex] that reacts:
- Four molecules of carbon dioxide are produced.
- Four molecules of water are produced.
So, the correct choice is:
Four carbon dioxide molecules and four water molecules.
