Presentation on theme: "Percent Yield and Limiting Reactants"— Presentation transcript:
1Percent Yield and Limiting Reactants Using Reaction Stoichiometry
2Percent 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)
3Percent Yield Practice PbS + O2 PbO + SO2Balance 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?
4More 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.
5Limiting ReactantsLimiting Reactant- the reactant (reagent) that produces the fewest moles of product.Reaction can only form the amount of product “allowed” by the limiting reactant.
6Limiting Reactant Steps Balance the EquationUse 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.
7Limiting Reactant Practice H O2 → H2OIf 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?