3. Chemical Reactions

Percent Yield

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The reduction of iron (III) oxide creates the following reaction:
Fe₂O₃ (s) + 3 H₂ (g) → 2 Fe (s) + 3 H₂O (g)
If the above reaction only went to 75% completion, how many moles of Fe₂O₃ were required to produce 0.850 moles of Fe?
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Which statement best describes the difference between actual yield and theoretical yield in a chemical reaction?
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In a chemical reaction, if the theoretical yield of product is 50 g and the actual yield obtained is 40 g, what is the percent yield of the process?
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Which statement correctly describes the actual yield and the theoretical yield of a chemical reaction?
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Which of the following best describes how to determine the theoretical yield in a chemical reaction?
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Cyanogen (CN)₂ has been observed in the atmosphere of Titan, Saturn’s largest moon, and in the gases of interstellar nebulas. On Earth, it is used as a welding gas and a fumigant. In its reaction with fluorine, carbon tetrafluoride (CF₄) and nitrogen trifluoride (NF₃) gases are produced:
(CN)₂ + 7 F₂ → 2 CF₄ + 2 NF₃
What is the percent yield of the reaction if 45.0 g of CF₄ are isolated from the reaction between 75.0 g each of (CN)₂ and F₂?
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Which of the following best describes what percent yield indicates in a chemical reaction?
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Which of the following factors would reduce the percent yield of a chemical reaction?
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Which of the following statements best explains why a percent yield of 85% for a chemical reaction is considered reasonable?
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If the theoretical yield of Fe in a reaction is 10.0 g and 8.88 g of Fe was actually obtained, what is the percent yield of Fe?
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If the percent yield for the following reaction is 75.0% and 35.0 g of NO2 are consumed in the reaction, how many grams of nitric acid, HNO3(aq), are produced?
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If 42.0 g of HCl are produced from the reaction of 62.0 g of PCl_3, what is the percent yield of HCl? (Assume the reaction is: PCl_3 + 3 H_2O → H_3PO_3 + 3 HCl. Molar masses: PCl_3 = 137.33 g/mol, HCl = 36.46 g/mol.)
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A commercial vinegar sample is analyzed to determine the percent yield of acetic acid produced in a reaction. If the theoretical yield of acetic acid is 5.00 g and the actual yield obtained from the experiment is 4.20 g, what is the percent yield?
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A student reacts 10.0 g of CaCO_3 with excess HCl to produce CaCl_2, CO_2, and H_2O. If the balanced equation is CaCO_3 + 2 HCl → CaCl_2 + CO_2 + H_2O, what is the theoretical yield of CaCl_2 (in grams)? (Molar masses: CaCO_3 = 100.1 g/mol, CaCl_2 = 110.98 g/mol)
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Which of the following is NOT a reason why the actual yield is less than the theoretical yield in a chemical reaction?
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