Consider the commercial production of SO₃ via sulfur dioxide and oxygen:
SO₂ (g) + O₂ (g) → SO₃ (g)
If 5.3 L of sulfur dioxide and 4.7 L of oxygen are mixed, how much sulfur trioxide may be produced if all gases are at STP?

Question

Quizplus · Accepted Answer

At STP, volumes of gases in a chemical reaction are in the same ratio as their coefficients in the balanced equation. The equation is already balanced with a 2:1 ratio for $SO_2$ to $O_2$, producing 2 $SO_3$. Since $SO_2$ is the limiting reactant (5.3 L available), it will completely react and produce the same volume of $SO_3$ (5.3 L) because the mole ratio of $SO_2$ to $SO_3$ is 1:1.

Consider the Commercial Production of SO3 Via Sulfur Dioxide and Oxygen

Consider the Commercial Production of SO₃ Via Sulfur Dioxide and Oxygen