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Understanding Percent Yield in Chemical Reactions: Theoretical vs. Actual Yield

This resource explains the concepts of theoretical and actual yield in chemical reactions, emphasizing the significance of percent yield in evaluating reaction efficiency. Theoretical yield represents the maximum possible amount of product obtainable based on stoichiometric calculations, while actual yield refers to the quantity of product actually produced. Various factors such as incomplete reactions, unexpected side reactions, losses during separation, and impurities can cause actual yield to be less than theoretical yield. The formula for percent yield is provided, along with practical calculation examples for clarity.

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Understanding Percent Yield in Chemical Reactions: Theoretical vs. Actual Yield

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Presentation Transcript

  1. Percent Yeild

  2. Percent Yields • Theoretical yield: max amount of a product that is formed in a reaction (based on calculations). • Actual yield: amount of product that is actually obtained in a reaction • Usually less than theoretical. Why?

  3. Why? • Theoretical has assumed that all of limiting reagent has completely reacted. • Many reactions do not go to completion • Unexpected competing side reactions limit the formation of products. • Some reactants are lost during the separation process • Impure reactants • Faulty measuring • Poor experimental design or technique

  4. How to calculate? Percent Yield = Actual Yield x 100% Theoretical yield

  5. Practice: HBrO3 + 5HBr  3H2O + 3 Br2 20g of HBrO3 is reacted with excess HBr. • What is the theoretical yield of Br2? • What is the percent yield, if 47.3g is produced?

  6. Practice alone: When 35g of Ba(NO3)2 is reacted with excess Na2SO4, 29.8g of BaSO4 is recovered. Ba(NO3)2 +Na2SO4 BaSO4 + 2NaNO3 • Calculate the theoretical yield of BaSO4 • Calculate the percent yield of BaSO4

  7. Practice • Pg.368 #7, 8, 9

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