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Percent Yield and Limiting Reactants Using Reaction Stoichiometry.

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Presentation on theme: "Percent Yield and Limiting Reactants Using Reaction Stoichiometry."— Presentation transcript:

1 Percent Yield and Limiting Reactants Using Reaction Stoichiometry

2 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)

3 Percent Yield Practice PbS + O 2  PbO + SO 2  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?

4 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.

5 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.

6 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.

7 Limiting Reactant Practice H 2 + O 2 → H 2 O  If 12.2 mol H 2 and 8.4 mol O 2 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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