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

We start with (C_{4}H_{8}+6O_{2}\rightarrow CO_{2}+H_{2}O). For carbon - atoms, there are 4 carbon atoms in (C_{4}H_{8}), so we need 4 moles of (CO_{2}) on the product side. For hydrogen - atoms, there are 8 hydrogen atoms in (C_{4}H_{8}), so we need 4 moles of (H_{2}O) on the product side. The balanced equation is (C_{4}H_{8}+6O_{2}\rightarrow4CO_{2}+4H_{2}O).

Answer:

four carbon dioxide molecules and four water molecules