Use the following balanced equation: 2C₂H₆ + 7O₂ ---> 4CO₂ + 6H₂O

If 15 g of C₂H₆ react with 45 g of O₂, how many grams of water will be produced?

What is the excess reactant in the equation?

The theoretical yield is the maximum amount of product that can be formed in a chemical reaction based on the amount of limiting reactant.

LIMITING REACTANT OFTEN IS THE REACTANT YOU HAVE THE LEAST OF.

The amount of a product that is formed when the limiting reactant is fully consumed in a reaction is known as the theoretical yield.

The greatest amount of NH3 produced 3.2 moles of N2 and 5.4 moles of H2 is 3.6 moles of NH3. Which is the limiting reactant?

P₄ + 3O₂ --> P₄O₆ 
What is the limiting reactant is 12 moles of P₄ react with 15 moles of O₂?

In the reaction @@ ext{2H}_2 + ext{O}_2 ightarrow ext{2H}_2 ext{O} $$, if you start with 4 moles of$$ ext{H}_2 $$and 3 moles of$$ ext{O}_2@@, what is the limiting reactant?

Consider the reaction @@ ext{N}_2 + 3 ext{H}_2 ightarrow 2 ext{NH}_3 $$. If you have 5 moles of$$ ext{N}_2 $$and 12 moles of$$ ext{H}_2@@, which reactant is in excess?

In a chemical reaction, the reactant that determines the amount of product formed is called the limiting reactant.

For the reaction @@ ext{2SO}_2 + ext{O}_2 ightarrow ext{2SO}_3 $$, if 10 moles of$$ ext{SO}_2 $$react with 5 moles of$$ ext{O}_2@@, what is the limiting reactant?

In the reaction @@ ext{C}_3 ext{H}_8 + 5 ext{O}_2 ightarrow 3 ext{CO}_2 + 4 ext{H}_2 ext{O} $$, if 44 g of$$ ext{C}_3 ext{H}_8 $$react with 160 g of$$ ext{O}_2@@, what is the limiting reactant?

The limiting reactant is always the reactant that is present in the smallest amount by mass.

In the reaction @@ ext{4Fe} + 3 ext{O}_2 ightarrow 2 ext{Fe}_2 ext{O}_3 $$, if 20 moles of$$ ext{Fe} $$react with 10 moles of$$ ext{O}_2@@, what is the limiting reactant?

In a real-world application, why is it important to identify the limiting reactant in an industrial chemical process?