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Limiting Reactants and Percentage Yield

Limiting Reactants and Percentage Yield. 9.2. Reactants. Excess Reactant – will not be completely ______ up in a ______ that goes to __________ Limiting Reactant – is ________ completely in a ________ that goes to ___________ Sandwich example. Limiting Reactant.

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Limiting Reactants and Percentage Yield

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  1. Limiting Reactants and Percentage Yield 9.2

  2. Reactants • Excess Reactant – will not be completely ______ up in a ______ that goes to __________ • Limiting Reactant – is ________ completely in a ________ that goes to ___________ • Sandwich example

  3. Limiting Reactant • If there are 152.5 grams of CO and 24.50 g of H2, how much CH3OH could be produced? • Need a balanced equation • CO + 2H2 CH3OH • Determine # of moles of product

  4. Limiting Reactant • With 752.4 grams of ZnCO3 and 1921 grams of C6H8O7, which is the limiting reactant? • How much Zn3(C6H5O7)2 is produced? • 3ZnCO3 + 2C6H8O7 Zn3(C6H5O7)2 + 3CO3

  5. Limiting Reactant • Identify the limiting reactant and calculate the theoretical yield of phosphorous acid (H3PO3) if 225 grams of PCl3 is mixed with 123 grams of H2O. • PCl3 + 3H2O  H3PO3 + 3HCl

  6. Yield • Actual Yield – _________ amount of ________ from a reaction. • Doesn’t always _______ amounts that it __________. • Don’t go to _____________ • ________ equilibrium • Not _____ situations

  7. Percent Yield • % Yield – ____ of _____ ____to the ____________ yield multiplied by ____ • % yield = actual yield x 100 theoretical yield

  8. Calculating % Yield • Determine the limiting reactant, the theoretical yield (in grams), if 14.0 g of N2 are mixed with 9.0g H2. • N2 + H2 NH3

  9. Calculating % Yield • Make sure the equation is balanced. • Find limiting reactant first • Then identify actual yield • Then calculate % yield • % yield = Actual/Theoretical x 100

  10. Theoretical Yield • Determine the limiting reactant and the theoretical yield if 16.1 grams of bromine are mixed with 8.42 grams of chlorine. • Br2 + Cl2 2BrCl

  11. Stoichiometry Review • 2N2H4 + (CH3)2N2H2 + 3N2O4  6N2 + 2CO2 + 8H2O • The density of N2H4 is 0.982 g/mL • How many mL of N2H4 is needed to produce 20 grams of N2?

  12. Stoichiometry Review • 2N2H4 + (CH3)2N2H2 + 3N2O4  6N2 + 2CO2 + 8H2O • How many molecules of N2H4 are needed to produce 50 grams of N2?

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