Actual Yield Calculations: Grade 12 Chemistry
This worksheet focuses on understanding and calculating actual yield, theoretical yield, and percent yield in chemical reactions for Grade 12 Chemistry students.
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Standards
Topics
Actual Yield Calculations
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Read each question carefully and provide detailed answers. Show all your work for calculations.
1. The amount of product actually obtained from a reaction is called the .
2. The maximum amount of product that can be formed from a given amount of reactant is the .
3. The ratio of actual yield to theoretical yield, expressed as a percentage, is known as the .
1. Which of the following factors can lead to an actual yield being less than the theoretical yield?
Impurities in reactants
Incomplete reaction
Loss of product during transfer
All of the above
2. A percent yield of 100% indicates that:
The actual yield was greater than the theoretical yield.
The actual yield was equal to the theoretical yield.
No product was formed.
The reaction did not occur.
1. In an experiment, 25.0 g of calcium carbonate (CaCO₃) is heated to produce calcium oxide (CaO) and carbon dioxide (CO₂). If the actual yield of CaO is 12.0 g, and the theoretical yield is 14.0 g, calculate the percent yield for this reaction. (Molar mass of CaCO₃ = 100.09 g/mol, CaO = 56.08 g/mol)
2. Consider the reaction: 2Al(s) + 3Cl₂(g) → 2AlCl₃(s). If you start with 10.0 g of aluminum and an excess of chlorine gas, and you obtain 30.0 g of aluminum chloride in the lab, what is the percent yield of AlCl₃? (Molar mass of Al = 26.98 g/mol, AlCl₃ = 133.34 g/mol)
1. The actual yield can never be greater than the theoretical yield.
True
False
2. A percent yield of 75% means that 25% of the reactants were not converted into product.
True
False
Explain in detail why the actual yield of a chemical reaction is almost always less than the theoretical yield. Discuss at least three distinct reasons.