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What is theoretical yield in a chemical reaction?
What is theoretical yield in a chemical reaction?
- The percentage of reactants converted into products
- The mass of reactants before the reaction
- The mass of product actually obtained from a reaction
- The maximum possible mass of product that could be produced (correct)
Percentage yield is calculated by dividing actual yield by theoretical yield and multiplying by 100.
Percentage yield is calculated by dividing actual yield by theoretical yield and multiplying by 100.
True (A)
What is the actual yield if the process was 82% efficient and the theoretical yield is 100 g?
What is the actual yield if the process was 82% efficient and the theoretical yield is 100 g?
82 g
The formula for calculating percentage yield is __________.
The formula for calculating percentage yield is __________.
Match the following terms with their definitions:
Match the following terms with their definitions:
Flashcards
Theoretical Yield
Theoretical Yield
The maximum amount of product that can be produced in a chemical reaction, calculated from the balanced equation.
Actual Yield
Actual Yield
The actual mass of product obtained from a chemical reaction.
Percentage Yield
Percentage Yield
A measure of how efficiently a reaction converts reactants to products, expressed as a percentage.
Percentage Yield Calculation
Percentage Yield Calculation
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Calculating Theoretical Yield
Calculating Theoretical Yield
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Study Notes
Chemical Reaction Yields
- Chemical reactions don't always produce the exact amount of product predicted by balanced equations.
- Theoretical Yield: The maximum possible mass of product that could be produced.
- Actual Yield: The actual mass of product obtained from a reaction.
- Percentage Yield: A measure of how efficiently a reactant is converted to a product. Calculated as (actual yield / theoretical yield) * 100%.
Example Calculation
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Reaction: HBrO3 + 5HBr → 3Br2 + 3H2O
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Given: 10.0 g of HBrO3 reacted with excess HBr; 26.3 g of Br2 produced.
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i) Moles of Reactant:
- Calculate molar mass of HBrO3 (128.91 g/mol)
- Calculate moles of HBrO3 used (10.0 g / 128.91 g/mol = 0.0776 mol)
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ii) Theoretical Yield:
- Calculate moles of Br2 produced from moles of HBrO3 (0.0776 mol HBrO3 * (3 mol Br2 / 1 mol HBrO3) = 0.233 mol)
- Calculate molar mass of Br2 (159.81 g/mol)
- Calculate theoretical yield (0.233 mol * 159.81 g/mol = 37.2 g)
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iii) Percentage Yield:
- Calculate percentage yield (26.3 g / 37.2 g) * 100% = 70.7%
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Additional Example: If the reaction was 82% efficient, the actual yield would be 30.5g.
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