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Limiting Reactants and Percent Yield in Chemical Reactions

Learn about the concepts of limiting reactants, excess reactants, and percent yield in chemical reactions. Practice problems included to help grasp the calculations involved. Gain a deeper understanding of how to determine the limiting factor and calculate the theoretical and actual yields.

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Limiting Reactants and Percent Yield in Chemical Reactions

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  1. Limiting ReactantsandPercent Yield

  2. Definitions • The Limiting Reactant is the reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction. • The excess reactant is the substance that is not used up in a reaction.

  3. = 1engine + 4 tires  1 car • If you have two engines and seven tires which is your limiting reactant and which is in excess? 4 tires 2 engines 8 tires 1 engine

  4. = Practice problem#1 • SiO2 + 4HF → SiF4 + 2H2O • If 2.0 moles of HF are exposed to 4.5 moles of SiO2, which is the limiting factor? 2 mol HF 1 mole SiO2 0.5 moles SiO2 4 moles HF

  5. Practice problems • N2H4 + 2H2O2→ N2 + 4 H2O a) Which is the limiting reactant in this reaction when .750moles of N2H4 is mixed with .500 mol of H2O2? • How much of the excess reactant, in moles, is left over?

  6. Practice problems • Pg.368 #’s 20-21

  7. Percent Yield • The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant. (The result of a mass-mass problem) • The actual yield is the measured amount of a product obtained from a reaction.

  8. 38.8g actual yield = = theoretical yield 53.0g When 36.8 g of C6H6 react with excess Cl2, the actual yield of C6H5Cl is 38.8g. What is the percent yield of C6H5Cl? • C6H6 + Cl2→C6H5Cl + HCl • Do a mass-mass problem to determine your theoretical yield. • Divide your actual yield by your theoretical yield and convert to percent. .732 x100 = 73.2%

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