Limiting Reactants and Theoretical Yield

This video tutorial covers stoichiometry problems related to limiting and excess reactants. It explains how to balance chemical equations, identify limiting and excess reactants, and calculate percent yield. The tutorial uses examples involving nitrogen, hydrogen, and ammonia to demonstrate these concepts. Additionally, it provides a step-by-step guide to solving a problem involving propane and oxygen, emphasizing the importance of theoretical and actual yields in chemical reactions.

What is the first step in solving stoichiometry problems involving limiting and excess reactants?

• Write a balanced chemical equation

• Determine the actual yield

• Calculate the percent yield

• Identify the excess reactant

How do you determine the limiting reactant in a chemical reaction?

• By identifying the reactant with the highest molar mass

• By comparing the mass of reactants

• By calculating the percent yield

• By using the mole-to-coefficient ratio

What is the theoretical yield in a chemical reaction?

• The initial amount of reactants used

• The amount of excess reactant remaining

• The maximum amount of product that can be produced

• The amount of product actually obtained

How is percent yield calculated?

• By adding the actual yield to the theoretical yield

• By subtracting the excess reactant from the limiting reactant

• By dividing the theoretical yield by the actual yield and multiplying by 100%

• By dividing the actual yield by the theoretical yield and multiplying by 100%

In the example problem, what is the balanced equation for the combustion of propane?

• C3H8 + 5O2 → 3CO2 + 4H2O

• C3H8 + 6O2 → 3CO2 + 4H2O

• C3H8 + 4O2 → 3CO2 + 4H2O

• C3H8 + 3O2 → 3CO2 + 4H2O

What is the limiting reactant in the combustion of propane with oxygen?

• Propane

• Oxygen

• Carbon dioxide

• Water

How do you calculate the actual yield if the reaction efficiency is given?

• Divide the theoretical yield by the efficiency percentage

• Add the efficiency percentage to the theoretical yield

• Multiply the theoretical yield by the efficiency percentage

• Subtract the efficiency percentage from the theoretical yield

What is the theoretical yield of CO2 if 20g of propane reacts completely?

• 40g

• 60g

• 80g

• 100g

If 60g of oxygen is used, how much CO2 is theoretically produced?

• 80g

• 70g

• 49.5g

• 60g

How much excess propane remains after the reaction?

• 5g

• 3.5g

• 10g

• 7g