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Chemistry 1 Notes #4b Chapter 12 Part II

Chemistry 1 Notes #4b Chapter 12 Part II. June 7, 2014. Limiting Reactant. The limiting reactant is the reactant that: is completely consumed yields the LEAST amount of product. Calculations dealing with Limiting Reactants.

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Chemistry 1 Notes #4b Chapter 12 Part II

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  1. Chemistry 1 Notes #4bChapter 12 Part II June 7, 2014

  2. Limiting Reactant • Thelimiting reactantis the reactant that: • is completely consumed • yields the LEAST amount of product

  3. Calculations dealing with Limiting Reactants • If amounts are given for more than one reactant, you’ve got a limiting reactant problem! •  Strategy: • calculate the amount of product (in mols) you could produce for each reactant • the lowest yield is thetheoretical yield • the reactant givinglowest yield is thelimiting reactant.

  4. Example Nitrogen dioxide and water react to produce nitric acid and nitrogen monoxide. Given 100.0 g of NO2 and 20.0 g of water, what is the limiting reactant and what is the theoretical yield of nitric acid, in grams? Step #1 Write out a balanced chemical equation 3NO2 + H2O 2HNO3 + NO

  5. Example (cont)… Step #2 Calculate the amount of product that can be made for each reactant 100.0 gNO2 x 1 mol NO2x 2 mol HNO3 =1.449 mol HNO3 46 g NO2 3 mol NO2 20.0 gH2O x 1 mol H2Ox 2 mol HNO3 = 2.222 mol HNO3 18 g H2O 1 mol H2O LIMITING reactant—made the LEAST amount of product

  6. Example (cont)… The last part of the problem asked, “What is the theoretical yield of nitric acid in grams?” Theoretical yield how much product could potentially be made if the reaction were done perfectly.

  7. Example (cont)… 1.449 mol HNO3 x 63g HNO3 1 mol HNO3 =91.29 g HNO3

  8. Percent Yield % yield = actual yield (experimental) X 100% theoretical yield What percent of the perfect amount did you obtain (taking into account human/mechanical error)

  9. Question… If we weighed out our product HNO3 at the end of the last problem, and we obtained 76.45g HNO3, what is our percent yield? Remember: Limiting reactant calculations told us that the theoretical yield = 91.29g HNO3 % yield = actual yield (experimental) X 100% theoretical yield X 100% =83.74% yield 76.45g HNO3 91.29g HNO3

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