Calculating Theoretical Yield in Chemical Reactions

The video tutorial explains how to calculate the theoretical yield of a chemical reaction, which is the maximum mass of product that can be formed. It provides examples using calcium carbonate and iron oxide to demonstrate the calculation process. The tutorial also covers how to determine the percentage yield by comparing the actual yield to the theoretical yield.

What is the theoretical yield in a chemical reaction?

• The speed of the reaction

• The amount of reactants used

• The maximum possible amount of product formed

• The actual amount of product obtained

In the example of calcium carbonate, what is the molecular mass of calcium carbonate?

• 56 grams per mole

• 100 grams per mole

• 112 grams per mole

• 160 grams per mole

How many moles of calcium oxide are formed from 5 moles of calcium carbonate?

• 10 moles

• 1 mole

• 5 moles

• 2.5 moles

What is the molecular mass of iron oxide used in the example?

• 100 grams per mole

• 112 grams per mole

• 160 grams per mole

• 56 grams per mole

How many moles of iron are produced from 1,000,000 moles of iron oxide?

• 500,000 moles

• 1,000,000 moles

• 2,000,000 moles

• 3,000,000 moles

What is the actual yield of iron in tonnes if the theoretical yield is 112 tonnes and the percentage yield is 75%?

• 150 tonnes

• 84 tonnes

• 112 tonnes

• 56 tonnes

How is the percentage yield calculated?

• Actual yield plus theoretical yield, divided by 2

• Theoretical yield divided by actual yield, multiplied by 100

• Actual yield divided by theoretical yield, multiplied by 100

• Theoretical yield minus actual yield, multiplied by 100