Chapter 7 7.3: Percentage Yield.

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Presentation transcript:

Chapter 7 7.3: Percentage Yield

Theoretical Yield vs. Actual Yield Theoretical yield: the amount of product predicted by stoichiometry Actual yield: the amount of product obtained by experiment

Theoretical Yield vs. Actual Yield Why do they differ? - Imperfect techniques - Impure reactants - Competing reactions Competing reaction: a reaction that occurs at the same time and involves the same reactants and products. Chemists have a percentage that is used to express the “success” of a reaction. This percentage is called the percentage yield.

Percentage Yield Percentage yield: compares the actual yield with the theoretical yield % yield= AY x 100 TY

Percentage Yield Sample Problem #1 N2(g) +3H2(g)  2NH3(g) When 75.0g of nitrogen reacts with sufficient hydrogen, the theoretical yield of ammonia is 9.10g. If 2.14g of ammonia is obtained by experiment, what is the percentage yield of the reaction? (Ans: 23.5%)

Percentage Yield Sample Problem #2 2P(s) + 3Cl2(g)  2PCl3(l) 7.50g of chlorine is reacted with excess phosphorus. What is the theoretical yield of PCl3 for this reaction? (Ans: 9.71g) b) If 1.25g of PCl3 is produced, what is the percentage yield? (Ans: 12.9%)

Predicting Actual Yield Sample Problem #3 C3H8(g) + 5O2 (g) → 3CO2 (g) + 4H2O (g) 37.0g of oxygen reacts with excess propane (C3H8) . If the percentage yield is 94.0%, how much carbon dioxide is produced? (Ans: 28.8g) Step 1: find theoretical yield Answer: 30.6g Step 2: find actual yield Answer: 28.8g

Inv 7A – due next class…lab quiz **TEST Unit 3 (Ch 5-7) in 3 days** Textbook p 262 #31-33 p 266 #34-37 Inv 7B - Complete prediction - Copy obs table - Read (formal report) Reminders: Inv 7A – due next class…lab quiz **TEST Unit 3 (Ch 5-7) in 3 days**