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Actual and Percent Yields

Actual and Percent Yields. So far when we have been talking about reactions we have been talking about 100% of the (limiting) reactant becoming a product.

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Actual and Percent Yields

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  1. Actual and Percent Yields So far when we have been talking about reactions we have been talking about 100% of the (limiting) reactant becoming a product. However in real- life most of the time some of the reactants do not react so our theoretical (if 100% of reactants become product) yield is different from our actual yield. We can express this difference as a percentage to see if a reaction would be viable.

  2. LiOH + KCl KOH + LiCl If I start this reaction with 20g of LiOH, what mass of LiCl should I get? If I actually get 6g of LiCl, what is my percent yield? Step 1: Write a balanced equation Step 2: Calculate the number of moles of reactant 1 mole LiOH = 24g 20g = 20/24 moles = 0.83 moles

  3. Step 3: Use mole ratios to calculate the mass of product 1 mole LiOH : 1 mole LiCl 0.83 moles LiOH : 0.83 moles LiCl 1 mole LiCl = 42.5g 0.83 moles = 42.5 x 0.83 = 35.28g Theoretical Yield From question Step 4: Calculate percent yield using the formula Actual yield % yield = 6 X 100 X 100 Theoretical yield 35.28 From step 3 = 17% yield

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