1 / 4

Example : C 6 H 6 + Cl 2 --> C 6 H 5 Cl + HCl

Example : C 6 H 6 + Cl 2 --> C 6 H 5 Cl + HCl When 36.8 g of C 6 H 6 reacts with an excess of Cl 2 , the actual yield of C 6 H 5 Cl is 38.8 g. What is the percent yield of C 6 H 5 Cl ? Can we use the 2 mass amounts in the problem above to solve?

decker
Télécharger la présentation

Example : C 6 H 6 + Cl 2 --> C 6 H 5 Cl + HCl

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. Example: C6H6 + Cl2 --> C6H5Cl + HCl When 36.8 g of C6H6 reacts with an excess of Cl2, the actual yield of C6H5Cl is 38.8 g. What is the percent yield of C6H5Cl? Can we use the 2 mass amounts in the problem above to solve? No, because they are for different compounds. Your mass amounts need to relate to the same compound. So…first we need to use the grams of of C6H6 to determine how much C6H5Cl will theoretically be formed. This will be our theoretical yield. THEN calculate % yield. Try that now…

  2. Which one of these will be used up first? What happens when one reactant is gone?

  3. Example: SiO2+ 4 HF SiF4 + 2 H2O If 2 mol of HF are exposed to 4.5 mol of SiO2, which is the limiting reactant? Try to figure this out, and we will go over it in class!!

More Related