Question

the combustion of propane (c3hg) in the presence of excess oxygen yields co2 and h2o: c3h8 (g) + 5o2 (g) → 3co2 (g) + 4h2o (g) when 2.5 mol of o2 are consumed in their reaction, ______ mol of co2 are produced. 5.0 3.0 2.5 6.0 1.5

Explanation:

Step1: Determine mole ratio

From the balanced equation \(C_{3}H_{8}(g)+5O_{2}(g)\to3CO_{2}(g)+4H_{2}O(g)\), the mole ratio of \(O_{2}\) to \(CO_{2}\) is \(5:3\).

Step2: Set up proportion

Let \(x\) be the moles of \(CO_{2}\) produced. Using the mole ratio \(\frac{5\space mol\space O_{2}}{3\space mol\space CO_{2}}=\frac{2.5\space mol\space O_{2}}{x}\).
Cross - multiply: \(5x = 3\times2.5\).

Step3: Solve for \(x\)

\(x=\frac{3\times2.5}{5}\).
\(x = 1.5\).

Answer:

1.5