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Mastering Stoichiometry for Optimal Yields in Reactions

Explore stoichiometry, limiting reactants, and percent yield calculations with balanced equations. Learn to determine the amount of reactants needed, predict product yields, and find the limiting reagent for optimal results in chemical reactions.

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Mastering Stoichiometry for Optimal Yields in Reactions

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  1. CH 12 Review for TEST!!! Stoichiometry Limiting Reactants Percent Yield

  2. Start with a Balanced Equation! • __NH3 + __NO  __N2 + __H2O

  3. Start with a Balanced Equation! • 4 NH3 + 6 NO  5 N2 + 6 H2O • What does the coefficients mean? • 4___NH3 + 6____NO  5____N2+ 6__H2O • 4 molecules NH3 + 6 molecules NO  5 molecules N2 + 6 molecules H2O • 4 moles NH3 + 6 moles NO  5 moles N2 + 6 moles H2O • 4 volumes NH3 + 6 volumes NO  5 volumes N2 + 6 volumes H2O

  4. Use like a recipe (moles to moles) • 4 NH3 + 6 NO  5 N2 + 6 H2O • If you have 15 moles of NH3, how many moles do you need of NO? 4 moles NH3 = 15 moles NH3 6 moles NO X moles NO X = 22.5 moles of NO

  5. Use like a recipe (grams to grams) • 4 NH3 + 6 NO  5 N2 + 6 H2O • If you have 96 grams of NO, how many grams of NH3 do you need? • 68 g NH3 = Xg NH3 180 g NO 96 g NO X= 36.3 g NH3

  6. Use like a recipe (liters to liters) • 4 NH3 + 6 NO  5 N2 + 6 H2O • How many liters of Nitrogen gas will you make if you start with 13 liters of nitrogen monoxide? 6 (22.4L) NO = 13 L NO 5 (22.4 L) N2 X L N2 X = 10.8 L N2

  7. Find your limiting reactant (reagent) • 4 NH3 + 6 NO  5 N2 + 6 H2O • If you have 102 grams of NH3 and 360 grams of NO, what is your percent yield if you made 140 g of water? • 68 g NH3 = 102 g NH3 180 g NO X g NO X = 270 g NO but you have 360 grams. • You have tons of NO, in fact you have an EXCESS. • Your limiting reagent is NH3

  8. Find how much product you expect (THEORETICAL YIELD) • 4 NH3 + 6 NO  5 N2 + 6 H2O • If you have 102 grams of NH3 and 360 grams of NO, what is your percent yield if you made 140 g of water? • Use your limiting reagent in your calculation…that is what is determining how much product you can make. • 68 g NH3 = 102 g NH3 108 g H2OX g H2O X = 162 g H2O. This is your THEORETICAL YIELD

  9. Percent Yield • 4 NH3 + 6 NO  5 N2 + 6 H2O • If you have 102 grams of NH3 and 360 grams of NO, what is your percent yield if you made 140 g of water? • Actual amount x 100 = % yield theoretical yield • 140 g H2O X 100 = 86% 162 g H2O

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