Question

Butane, C4H10, is the gas burned in disposable lighters. How many moles of oxygen are needed to burn 5.0 mol of butane in a lighter to produce carbon dioxide and water?

Unbalanced equation:

C4H10 + O2 -> CO2 + H2O


28 mol


32 mol


13 mol

Answer 1

32 mol

Step-by-step explanation:

Step 1: Write the balanced equation.

C₄H₁₀ + 6.5 O₂ → 4 CO₂ + 5 H₂O

Step 2: Establish the appropriate molar ratio.

The molar ratio of C₄H₁₀ to O₂ is 1:6.5

Step 3: Calculate the moles of oxygen needed to burn 5.0 mol of butane.

We use the molar ratio established in the previous step.

`5.0molC_4H_(10) * (6.5molO_2)/(1molC_4H_(10) ) = 32molO_2`