Understanding Yield in Chemical Reactions: Theoretical Yield, Actual Yield, and Percentage Yield

The video tutorial explains the concept of yield in chemical reactions, covering theoretical yield, actual yield, and percentage yield. It discusses factors that cause actual yield to be less than theoretical yield, such as incomplete reactions, reversible reactions, impurities, side reactions, and loss of chemicals. The tutorial also explains how to calculate percentage yield and provides example calculations to illustrate the concepts.

What is the yield of a reaction?

• The temperature at which the reaction occurs

• The speed of the reaction

• The mass of product formed

• The amount of reactants used

What does the theoretical yield represent in a chemical reaction?

• The speed at which the reaction occurs

• The actual amount of product obtained

• The maximum possible amount of product

• The amount of reactants left unreacted

Which of the following is NOT a reason for actual yield being less than theoretical yield?

• Pure reactants

• Side reactions

• Reversible reactions

• Incomplete reactions

How does a reversible reaction affect the actual yield?

• It increases the actual yield

• It decreases the actual yield

• It doubles the actual yield

• It has no effect on the actual yield

What is the formula for calculating percentage yield?

• Theoretical yield minus actual yield, multiplied by 100

• Actual yield divided by theoretical yield, multiplied by 100

• Actual yield plus theoretical yield, divided by 100

• Theoretical yield divided by actual yield, multiplied by 100

Why is a high percentage yield economically desirable?

• It requires more raw materials

• It results in more waste

• It decreases the amount of product

• It leads to a more profitable process

In a reaction with a theoretical yield of 300 grams and a percentage yield of 25%, what is the actual yield?

• 25 grams

• 50 grams

• 75 grams

• 100 grams