Calculating Yield and Percentage Yield in Chemical Reactions

The video tutorial covers the concepts of yield and percentage yield in chemical reactions, using an example of copper oxide reacting with hydrochloric acid to calculate percentage yield. It explains why the actual yield may differ from the theoretical yield. The tutorial also introduces atom economy, comparing two methods of producing copper chloride and calculating their atom economies.

What is the percentage yield if 5 grams of product is obtained from a reaction with a theoretical yield of 10 grams?

• 50%

• 100%

• 75%

• 25%

In the example reaction, what is the theoretical mass of copper chloride that should be produced?

• 10 grams

• 5 grams

• 8.47 grams

• 6.5 grams

Which of the following is NOT a reason for not achieving 100% yield in a reaction?

• Impurities in reactants

• Loss of product during separation

• Accurate measurement of products

• Incomplete reaction

What does atom economy measure in a chemical reaction?

• The cost of the reactants

• The speed of the reaction

• The efficiency of converting reactants to useful products

• The amount of waste produced

How is the atom economy calculated?

• By multiplying the mass of reactants by 100

• By dividing the mass of desired products by the total mass of reactants

• By subtracting the mass of waste from the mass of products

• By adding the mass of reactants and products

Which method of producing copper chloride has a higher atom economy?

• Using copper carbonate and hydrochloric acid

• Neither method has a high atom economy

• Using copper oxide and hydrochloric acid

• Both methods have the same atom economy

What is the atom economy percentage for the method using copper oxide and hydrochloric acid?

• 50%

• 76.7%

• 88.2%

• 68.4%