1 / 8

Limiting Reactants and Percent Yield

Limiting Reactants and Percent Yield. Definitions. The Limiting Reactant is the reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction. The excess reactant is the substance that is not used up in a reaction. =.

gsandra
Télécharger la présentation

Limiting Reactants and Percent Yield

An Image/Link below is provided (as is) to download presentation 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. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Limiting ReactantsandPercent Yield

  2. Definitions • The Limiting Reactant is the reactant that limits the amounts of the other reactants that can combine and the amount of product that can form in a chemical reaction. • The excess reactant is the substance that is not used up in a reaction.

  3. = 1engine + 4 tires  1 car • If you have two engines and seven tires which is your limiting reactant and which is in excess? 4 tires 2 engines 8 tires 1 engine

  4. = Practice problem#1 • SiO2 + 4HF → SiF4 + 2H2O • If 2.0 moles of HF are exposed to 4.5 moles of SiO2, which is the limiting factor? 2 mol HF 1 mole SiO2 0.5 moles SiO2 4 moles HF

  5. Practice problems • N2H4 + 2H2O2→ N2 + 4 H2O a) Which is the limiting reactant in this reaction when .750moles of N2H4 is mixed with .500 mol of H2O2? • How much of the excess reactant, in moles, is left over?

  6. Practice problems • Pg.368 #’s 20-21

  7. Percent Yield • The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant. (The result of a mass-mass problem) • The actual yield is the measured amount of a product obtained from a reaction.

  8. 38.8g actual yield = = theoretical yield 53.0g When 36.8 g of C6H6 react with excess Cl2, the actual yield of C6H5Cl is 38.8g. What is the percent yield of C6H5Cl? • C6H6 + Cl2→C6H5Cl + HCl • Do a mass-mass problem to determine your theoretical yield. • Divide your actual yield by your theoretical yield and convert to percent. .732 x100 = 73.2%

More Related