Percent yield and limiting reactants
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Percent Yield and Limiting Reactants. Using Reaction Stoichiometry. Percent Yield. % Yield= Actual Yield / Theoretical Yield x 100 Actual Yield - from a lab (what was actually produced)

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Percent Yield and Limiting Reactants

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Percent yield and limiting reactants

Percent Yield and Limiting Reactants

Using Reaction Stoichiometry


Percent yield

Percent Yield

  • % Yield= Actual Yield / Theoretical Yield x 100

    • Actual Yield- from a lab (what was actually produced)

    • Theoretical Yield- from a reaction stoichiometry problem (mathematical value… what you should have gotten)


Percent yield practice

Percent Yield Practice

PbS + O2PbO + SO2

  • Balance the equation above.

  • What is the theoretical yield of PbO if 200.0g of PbS is reacted?

  • If 170.0g of PbO is obtained in a chemical reaction, what is the percent yield?


More practice

More practice…

  • Upon heating, solid calcium carbonate decomposes to form solid calcium oxide and carbon dioxide gas.

    • Write the complete balanced chemical reaction for the reaction.

    • Determine the percent yield if 235.0g of calcium carbonate is heated and 97.5g of carbon dioxide is collected.


Limiting reactants

Limiting Reactants

  • Limiting Reactant- the reactant (reagent) that produces the fewest moles of product.

    • Reaction can only form the amount of product “allowed” by the limiting reactant.


Limiting reactant steps

Limiting Reactant Steps

  • Balance the Equation

  • Use mole ratios to find the moles of a product formed by each reactant (using the amounts given in the problem)

  • The reactant that makes the smallest number of moles of product is the limiting reactant. The other is the excess reactant.

  • The smallest number of moles produced will be the actual amount of product formed in the reaction.

    To find excess reactant remaining:

  • Subtract the two amounts of product formed (from step #2 above) and use mole ratios convert back to the reactant.


Limiting reactant practice

Limiting Reactant Practice

H2+ O2 → H2O

  • If 12.2 mol H2 and 8.4 mol O2 react…

    • What is the limiting reactant/reagent? The excess reactant?

    • How many moles of water are produced?

    • How many grams of water are produced?

    • How many moles of excess reactant remain?


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