Question

According to the given equation, how many molecules of O₂ are required to react with 4.71 moles C₄H₁₀?

2C₄H₁₀+13O₂-->8CO₂+10H₂O
Use 6.022 x 1023 mol for Avogadro's number.
Select the correct answer below:
a.1.84 × 102 molecules
b. 2.08 x 10s molecules
c.3.67 × 1025 molecules
d.none of the above

Answer 1

Approximately 1.85 × 10²µ molecules of O₂ are required to react with 4.71 moles of C₄H₁₀, which is not one of the options provided.

Step-by-step explanation:

To determine how many molecules of O₂ are required to react with 4.71 moles of C₄H₁₀, we first need to know the balanced chemical equation for the combustion of butane (C₄H₁₀). The balanced equation is:

2 C₄H₁₀ + 13 O₂ → 8 CO₂+ 10 H₂O

This equation shows that 2 moles of butane react with 13 moles of oxygen. To find the number of moles of O₂ required for 4.71 moles of C₄H₁₀, we set up a proportion:

(4.71 moles C₄H₁₀) x (13 moles O₂ / 2 moles C₄H₁₀) = 30.715 moles O₂

Now we convert moles of O₂ to molecules using Avogadro's number:

30.715 moles O₂ x (6.022 × 10²³ molecules/mol) ≈ 1.85 × 10²µ molecules O₂

So, approximately 1.85 × 10²µ molecules of O₂ are required to react with 4.71 moles of C₄H₁₀. Therefore, the correct answer is none of the above.