Multiple Choice
A reaction uses 32.5 g of Zn and produces 28.0 g of ZnCl_2. If the theoretical yield of ZnCl_2 is 40.5 g, what is the percent yield for the reaction?
58
views
3. Chemical Reactions
Percent Yield
Multiple Choice
Which of the following best describes how to determine the actual yield in a chemical reaction?
A
Divide the theoretical yield by the percent yield.
B
Measure the amount of product actually obtained from the experiment.
C
Subtract the mass of reactants from the mass of products.
D
Calculate the amount of product expected based on stoichiometry.
Verified step by step guidance1
Understand that the actual yield is the quantity of product that you actually obtain from performing the experiment in the lab.
Recognize that the theoretical yield is the amount of product predicted by stoichiometric calculations based on the limiting reactant.
Know that the percent yield relates the actual yield to the theoretical yield by the formula: \(\text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100\%\).
To determine the actual yield, you must directly measure the mass or amount of product obtained after the reaction is complete and the product is isolated.
Avoid confusing actual yield with theoretical yield or percent yield calculations; actual yield is an experimental measurement, not a calculated value.
Related Videos
Related Practice
