1 / 7

# Percent Yield and Limiting Reactants - PowerPoint PPT Presentation

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)

I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.

## PowerPoint Slideshow about 'Percent Yield and Limiting Reactants' - rigg

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.

- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript

### Percent Yield and Limiting Reactants

Using Reaction Stoichiometry

• % 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)

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?

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

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

• 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.

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?