Actual Yield in Chemical Reactions
Grade 11 Chemistry worksheet focusing on understanding and calculating actual yield, theoretical yield, and percent yield in chemical reactions.
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Actual Yield in Chemical Reactions
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Read each question carefully and provide your answers in the space provided. Show all your work for calculations.
1. The amount of product actually obtained from a chemical reaction is called the .
2. The maximum amount of product that can be formed from given amounts of reactants is the .
3. The ratio of the actual yield to the theoretical yield, multiplied by 100, is known as the .
4. Reactions rarely achieve 100% yield due to factors like incomplete reactions, side reactions, and during purification.
5. Which of the following is NOT a reason for a percent yield less than 100%?
Reactants are impure.
The reaction goes to completion.
Side reactions occur.
Product is lost during transfer.
6. In the reaction 2Na(s) + Cl₂(g) → 2NaCl(s), if 46.0 g of sodium reacts with excess chlorine, and 100.0 g of sodium chloride is collected, what is the theoretical yield of NaCl?
7. For the reaction in question 6, what is the actual yield of NaCl?
8. Calculate the percent yield for the reaction in question 6.
9. The actual yield can never be greater than the theoretical yield.
True
False
10. Explain why chemists are interested in the percent yield of a reaction and what factors they might try to control to maximize it.