Percent Yield. Definitions The theoretical yield is the maximum amount of product that could be made from the reactants. The actual yield is the amount.

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Presentation transcript:

Percent Yield

Definitions The theoretical yield is the maximum amount of product that could be made from the reactants. The actual yield is the amount of product that actually forms when the reactions happens. The percent yield is a ratio of the actual yield to the theoretical yield, expressed as a percent.

Equation % yield = actual yield x 100 theoretical yield

A real life problem A baker is following a recipe that is supposed to make 3 dozen cookies. She only gets 33 cookies when she is done. What is the % yield for her recipe?

Cookies % yield = actual yield x 100 theoretical yield

Cookies % yield = actual yield x 100 theoretical yield 33 X 100 = = 92% 36

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 4 steps! 1. Change grams of reactant to moles of reactant. 2. Convert moles of reactant to moles of product. 3. Convert moles of product to grams of product. 4. Calculate the % yield.

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 1. Change grams of reactant to moles of reactant.

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 1. Change grams of reactant to moles of reactant g x 1 mol = mol CaCO g

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 2. Convert moles of reactant to moles of product.

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 2. Convert moles of reactant to moles of product mol CaCO 3 x 1 mol CaO = 1 1 mol CaCO 3 = mol CaO

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 3. Convert moles of product to grams of product.

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 3. Convert moles of product to grams of product mol CaO x g CaO 1 1 mol CaO = g CaO rounded to 13.9 g CaO. This is your theoretical yield!

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 4. Calculate the % yield.

CaCO 3  CaO + CO 2 You have 24.8 g of CaCO 3. Determine the theoretical yield of CaO and then the % yield of this reaction if the actual yield was 12.0 g of CaO was obtained. 4. Calculate the % yield. 12.0g x g = rounded to 86.3%

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 1. Change grams of reactant to moles of reactant. 2. Convert moles of reactant to moles of product. 3. Convert moles of product to grams of product. 4. Calculate the % yield.

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 1. Change grams of reactant to moles of reactant.

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 1. Change grams of reactant to moles of reactant g Fe 2 O 3 x 1 mol Fe 2 O g Fe 2 O 3 = mol Fe 2 O 3

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 2. Convert moles of reactant to moles of product.

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 2. Convert moles of reactant to moles of product mol Fe 2 O 3 x 2 mol Fe 1 1 mol Fe 2 O 3 = mol Fe

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 3. Convert moles of product to grams of product.

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 3. Convert moles of product to grams of product mol Fe x g Fe 1 1 mol Fe = g Fe Rounded to 59.3 g Fe (this is your theoretical yield).

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 4. Calculate the % yield.

Fe 2 O 3 + 3CO  2Fe + 3CO g of Fe 2 O 3 is available in this reaction grams of Fe are made. What is the % yield? 4. Calculate the % yield. 50.0g x 100 = Rounded to 84.3% 59.3g

Last one: CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 1. Change grams of reactant to moles of reactant. 2. Convert moles of reactant to moles of product. 3. Convert moles of product to grams of product. 4. Calculate the % yield.

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 1. Change grams of reactant to moles of reactant.

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 1. Change grams of reactant to moles of reactant g CaCO 3 x 1 mol CaCO g CaCO 3 = mol CaCO 3

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 2. Convert moles of reactant to moles of product.

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 2. Convert moles of reactant to moles of product mol CaCO 3 x 1 mol CaO 1 1 mol CaCO 3 = mol CaO

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 3. Convert moles of product to grams of product.

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 3. Convert moles of product to grams of product mol CaO x g CaO 1 1 mole CaO = g CaO rounded to 13.9 g CaO This is your theoretical yield

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 4. Calculate the % yield.

CaCO 3  CaO + CO 2 What is the percent yield if 13.1 g CaO is actually produced when 24.8g CaCO 3 is available? 4. Calculate the % yield g CaO x 100 = = 94.2% 13.9 g CaO

Practice Complete the % yield practice sheet. If you do not finish, this will become homework, due at the beginning of our next class.