consider the unbalanced equation for the oxidation of butene.\nc₄h₈ + 6o₂ → co₂ + h₂o\nfor each molecule of…

consider the unbalanced equation for the oxidation of butene.\nc₄h₈ + 6o₂ → co₂ + h₂o\nfor each molecule of c₄h₈ that reacts, how many molecules of carbon dioxide and water are produced?\no two carbon dioxide molecules and two water molecules\no four carbon dioxide molecules and four water molecules\no two carbon dioxide molecules and four water molecules\no four carbon dioxide molecules and two water molecules

consider the unbalanced equation for the oxidation of butene.\nc₄h₈ + 6o₂ → co₂ + h₂o\nfor each molecule of c₄h₈ that reacts, how many molecules of carbon dioxide and water are produced?\no two carbon dioxide molecules and two water molecules\no four carbon dioxide molecules and four water molecules\no two carbon dioxide molecules and four water molecules\no four carbon dioxide molecules and two water molecules

Answer

Explanation:

Step1: Balance the chemical equation

$C_4H_8 + 6O_2\rightarrow4CO_2 + 4H_2O$

Step2: Analyze the stoichiometric coefficients

From the balanced equation, for 1 molecule of $C_4H_8$ reacting, 4 molecules of $CO_2$ and 4 molecules of $H_2O$ are produced.

Answer:

four carbon dioxide molecules and four water molecules