Theoretical Yield and Limiting Reactants

The video tutorial explains how to calculate the theoretical yield in chemical reactions by identifying the limiting reactant. It begins with an introduction to the concept of theoretical yield, followed by a step-by-step guide to finding the limiting reactant. The tutorial then demonstrates how to calculate the theoretical yield using proportions, specifically focusing on the production of water (H₂O) under ideal conditions. The video concludes with a summary of the process and key takeaways.

What is the theoretical yield in a chemical reaction?

• The actual amount of product obtained

• The maximum amount of product that can be formed

• The amount of reactants used

• The amount of excess reactant left

Why is it important to identify the limiting reactant in a reaction?

• It helps in identifying the excess reactant

• It is used to balance the chemical equation

• It controls the amount of product formed

• It determines the speed of the reaction

Which reactant is considered the limiting reactant?

• The reactant that is in excess

• The reactant that is not used in the reaction

• The reactant that is left over after the reaction

• The reactant that is completely consumed first

How do you calculate the theoretical yield using the limiting reactant?

• By using a proportion based on the balanced equation

• By estimating the amount of reactants

• By measuring the actual yield

• By using the excess reactant in calculations

What is the theoretical yield of H₂O if 2.9 moles of O₂ is the limiting reactant?

• 3.8 moles

• 2.9 moles

• 5.4 moles

• 1.0 mole