Percent Yield Calculation Worksheet
This worksheet provides practice problems for calculating percent yield in chemical reactions, suitable for Grade 11 Chemistry students.
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Percent Yield Calculation Worksheet
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Read each question carefully and show all your work for full credit. Use the formula: Percent Yield = (Actual Yield / Theoretical Yield) x 100%.
1. In an experiment, 25.0 g of calcium carbonate (CaCO₃) is heated to produce calcium oxide (CaO) and carbon dioxide (CO₂). If 12.5 g of CaO is actually produced, what is the percent yield of the reaction? (Molar mass of CaCO₃ = 100.09 g/mol, CaO = 56.08 g/mol)
2. When 15.0 g of potassium iodide (KI) reacts with excess lead(II) nitrate (Pb(NO₃)₂), 18.0 g of lead(II) iodide (PbI₂) is collected. Calculate the percent yield for the reaction. (Molar mass of KI = 166.00 g/mol, PbI₂ = 461.01 g/mol)
3. The yield is the maximum amount of product that can be formed from a given amount of reactant.
4. The yield is the amount of product actually obtained from a reaction.
5. A percent yield of 100% means that the yield is equal to the yield.
6. Which of the following factors can lead to a percent yield less than 100%?
Impurities in reactants
Side reactions
Incomplete reactions
All of the above
7. What is the theoretical yield if a reaction starts with 10.0 g of reactant A and has a 75% percent yield, producing 7.5 g of product B?
7.5 g
10.0 g
12.5 g
15.0 g
8. The actual yield is always greater than or equal to the theoretical yield.
True
False
9. A percent yield of 0% means no product was formed.
True
False
10. An experiment is set up in a beaker as shown below. If the reaction is expected to yield 50.0 g of product, but only 40.0 g is isolated, calculate the percent yield.
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