Practice Problem: Limiting Reagent and Percent Yield

Professor Dave explains how to solve a problem involving limiting reagents and percent yield. The tutorial covers converting reactant masses to moles, identifying the limiting reagent using stoichiometric coefficients, calculating the theoretical yield, and determining the percent yield. The video provides a step-by-step approach to understanding these concepts, ensuring clarity and comprehension.

What is the first step in solving a problem involving limiting reagents and percent yield?

• Determine the theoretical yield

• Identify the limiting reagent

• Calculate the percent yield

• Convert masses to moles

Why is it important to convert masses to moles in stoichiometric calculations?

• Moles provide a common unit for comparison

• Masses are easier to work with

• Moles are not affected by temperature

• Masses are always constant

Which of the following is true about the limiting reagent?

• It is always the reactant with the smallest mass

• It is the reactant that produces the least amount of product

• It is the reactant with the largest molar mass

• It is the reactant that is in excess

How can you determine the limiting reagent in a chemical reaction?

• By observing the color change

• By measuring the temperature change

• By calculating the moles of product each reactant can produce

• By comparing the initial masses of reactants

What does the theoretical yield represent in a chemical reaction?

• The actual amount of product obtained

• The amount of reactant used

• The amount of excess reactant

• The maximum possible amount of product

How is percent yield calculated?

• Actual yield divided by theoretical yield, multiplied by 100

• Actual yield plus theoretical yield, divided by 2

• Theoretical yield minus actual yield, divided by 100

• Theoretical yield divided by actual yield, multiplied by 100

If the actual yield is 2.89 grams and the theoretical yield is 3.32 grams, what is the percent yield?

• 87.0%

• 80.0%

• 90.0%

• 95.0%