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Limiting Reactants and % Yield

Limiting Reactants and % Yield. Limiting Factors. Limiting factors are those factors which control the speed or the outcome of a reaction or a situation Have you ever been behind a school bus in the morning? You can only go as fast as the bus in front of you.

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Limiting Reactants and % Yield

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  1. Limiting Reactants and % Yield

  2. Limiting Factors • Limiting factors are those factors which control the speed or the outcome of a reaction or a situation • Have you ever been behind a school bus in the morning? • You can only go as fast as the bus in front of you. • The bus one limiting factor preventing you from getting to school on time.

  3. Limiting Reactants Ingredients for making “S’mores”: 2 graham crackers 1 marshmallow 1 Hershey bar How many “S’mores” can you make with 14 graham crackers, 5 marshmallows, and 6 Hershey bars? 5 “S’mores” How many of each ingredient are left over? 0 marshmallows 4 graham crackers 1 Hershey bar

  4. Limiting Reactant • The limiting reactant is the reactant which controls the rate of reaction or the amount of product that can be made • The limiting reactant is determined using stoichiometric relationships

  5. Excess • The reactant that you have more than you need to perform a chemical reaction is called the excess reactant • It is not completely used up in a chemical reaction.

  6. Here’s an example • You are making ham and cheese sandwiches and you have: • 5 pieces of ham • 5 pieces of cheese • 8 pieces of bread • Which of these ingredients do you have more than enough of (excess reactant)? • Which of these do you not have enough of (limiting reactant?

  7. Yield • Yield is how much product that you produce • In industry, the amount of yield needs to be calculated so that production schedules can be made • You also need to know how much product you are going to be making so that you will have the appropriate size collection container

  8. Real or Not? • Actual yield refers to the amount of product that is actually generated • Theoretical yield refers to the amount of product that you expect to generate

  9. Calculating Yield • In order to calculate the theoretical yield you need to • Write a balanced chemical equation. • Calculate the amount of product produced from each reactant individually. • The reactant that produces the least amount of product is the limiting reactant. • The reactant that you have enough of is the excess reactant.

  10. Percentage Yield You recently bought a new car. The EPA sticker says that you should get 28 mpg in “average driving”. Your actual miles per gallon turns out to be less than 28 mpg. Why?

  11. Theoretical Yield vs. Actual Yield You perform a mass-mass calculation to determine how much chemical should be produced in a reaction. The actual results of the experiment produce less chemical than calculated. Why?

  12. Calculating Percent Yield • Calculate the theoretical yield (mass-mass calculation). • Determine the actual yield. • Calculate the % yield % Yield = Actual yield x 100 Theoretical yield

  13. A Percent Yield Problem A chemist starts with 1.75 g of salicylic acid (C7H6O3) and excess methanol (CH3OH) and reports the production of 1.42 g oil of wintergreen (C8H8O3) in the following reaction: C7H6O3 + CH3OH  C8H8O3 + H2O What is the percent yield for this reaction?

  14. Solving the Problem C7H6O3 + CH3OH  C8H8O3 + H2O 1.75 g ?g 1. 2. 3. 1.75 g x 1 mol = 138 g 0.0127 mol C7H6O3 4. 0. 0127 mol C7H6O3 x 1 molC8H8O3 = 1 molC7H6O3 0.0127 mol C8H8O3 5. 0.0127 mol C8H8O3 x 152 g = 1 mol 1.93 g C8H8O3

  15. % Yield cont. 6. (Actual Yield ÷ Theoretical Yield) x 100 (1.42 g ÷ 1.93 g) x 100 = 73.6 % Yield

  16. Practice Problems • A chemist carried out a reaction that should produce 21.8 g of a product, according to a mass-mass calculation. However, the chemist was able to recover only 13.9 g of the product. What percentage yield did the chemist get? • A calculation indicates that 82.2 g of a product should be obtained from a certain reaction. If a chemist actually gets 30.7 g, what is the percentage yield? • Chromium(III) hydroxide will dissolve in sodium hydroxide according to the following equation: • NaOH + Cr(OH)3 NaCr(OH)4 • If you begin with 66.0 g of Cr(OH)3 and obtain 38.4 g of product, what is your % yield?

  17. Solutions #1. (13.9g / 21.8g) x 100 = 63.8% #2. (30.7g / 82.2g) x 100 = 37.3% #3. NaOH + Cr(OH)3 NaCr(OH)4 66.0g ?g 66.0g Cr(OH)3 x 1mol/103g = 0.641molCr(OH)3 = 0.641mol NaCr(OH)4x 143g / 1mol NaCr(OH)4 = 91.66g NaCr(OH)4 (38.4g / 91.7g) x 100 = 41.9%

  18. Practice Problem Identify the limiting reactant and the theoretical yield of H3PO3 if 225 g of PCl3 is mixed with 125 g of H2O PCl3 + 3H2O  H3PO3 + 3HCl Convert each mass to moles: 225 g PCl3 x 1 mol/137 g = 1.64 mol PCl3 125 g H2O x 1 mol/ 18 g = 6.94 mol H2O 1.64 mol PCl3 requires 4.92 mol H2O PCl3 is the limiting reactant 1.64 mol PCl3 = 1.64 mol H3PO3 1.64 mol H3PO3 x 82 g/1 mol = 134 g H3PO3 ?g 125g 225g

  19. Classwork • P. 314 #1-3 • p. 317 #1-3 • p. 318 #1-3

  20. Homework • P. 319 1-13

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