Propane (C₃H₈) burns in oxygen to form CO₂ and H₂O according to the following equation. How many grams of O₂ are required to burn 3.01 x 10²³ propane molecules?
C₃H₈ + 5 O₂ $\rightarrow$ 3 CO₂ + 4 H₂O

Question

Propane (C₃H₈) burns in oxygen to form CO₂ and H₂O according to the following equation. How many grams of O₂ are required to burn 3.01 x 10²³ propane molecules?
C₃H₈ + 5 O₂

\rightarrow

3 CO₂ + 4 H₂O

Quizplus · Accepted Answer

The balanced chemical equation shows that 1 molecule of propane reacts with 5 molecules of oxygen. Therefore, 3.01 x 10²³ molecules of propane will react with 5 x 3.01 x 10²³ = 1.505 x 10²⁴ molecules of oxygen. The molar mass of oxygen is 32 g/mol, so the mass of oxygen required is 1.505 x 10²⁴ molecules x (32 g/mol) / (6.022 x 10²³ molecules/mol) = 80.0 g.

Propane (C3H8) Burns in Oxygen to Form CO2 and H2O →\rightarrow→

Propane (C₃H₈) Burns in Oxygen to Form CO₂ and H₂O $\rightarrow$