GCSE Chemistry - Percentage Yield #33

The video tutorial explains the concept of yield in chemical reactions, distinguishing between actual and theoretical yield. It provides an example calculation using hydrogen and oxygen to form water. The tutorial discusses common reasons for discrepancies between actual and theoretical yields, such as incomplete reactions, side reactions, and product loss. It also covers how to calculate percentage yield, using the example to demonstrate the calculation process.

What is the term used to describe the amount of product we expect to get based on calculations?

• Practical yield

• Theoretical yield

• Expected yield

• Actual yield

Which of the following is NOT a reason for obtaining less product than expected in a chemical reaction?

• Excess reactants

• Side reactions

• Loss of product

• Incomplete reaction

In a reversible reaction, why might the reaction not go to completion?

• The reaction is irreversible

• The reaction reaches equilibrium

• All reactants are consumed

• The reaction is too fast

What happens during a side reaction?

• Reactants form the expected product

• Reactants form a different product

• Reactants do not react at all

• Reactants are completely consumed

How do you calculate the percentage yield of a reaction?

• Divide theoretical yield by actual yield and multiply by 100

• Subtract actual yield from theoretical yield and multiply by 100

• Add actual yield to theoretical yield and multiply by 100

• Divide actual yield by theoretical yield and multiply by 100