Stoichiometry - Limiting Reagents & Percent Yield

​Stoichiometry -

Limiting Reagents & Percent Yield​

Multiple Choice

What is a limiting reactant?

• the reactant that determines how much product can be made

• the reactant that is in excess

• the product that you can make the most of

• the amount of reactants that react with each other

Multiple Choice

The limiting reactant

• slows the reaction down

• is used up first

• is the reactant that is left over

• controls the speed of the reaction

Multiple Choice

When does a chemical reaction stop?

• When the lab is finished

• When the excess reactant is used up

• When the limiting reactant is used up

• Chemical reactions never stop

Multiple Choice

How many grams of ammonia (NH₃) can be produced from the reaction of 28 g of nitrogen gas and 25 grams of hydrogen gas? 

• 43 g

• 34 moles

• 25 grams

• 34 grams

Multiple Choice

What is the measured amount of a product obtained from a chemical reaction?

• mole ratio

• theoretical yield

• percentage yield

• actual yield

Multiple Choice

If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the

• theoretical yield

• mole ratio

• actual yield

• percentage yield

Multiple Choice

Complete the equation for the percent yield of a chemical reaction: Percent yield=(________)÷(________)×100%

• actual yield; theoretical yield

• theoretical yield; actual yield

Multiple Choice

If the percentage yield for a chemical reaction is 80.0%, the 

• actual yield is 80.0g for every theoretical yield of 100g.

• actual yield is 80 times as much as the theoretical yield.

• theoretical yield is 80 times as much as the actual yield. 

• theoretical yield is 80.0 g for every actual yield of 100g.

Multiple Choice

Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.

• 1.16%

• 116%

• 85%

• 76%