March 28, 2024, 11:02:20 AM
Forum Rules: Read This Before Posting


Topic: Aspirin Equation  (Read 4267 times)

0 Members and 1 Guest are viewing this topic.

Offline IDudeScience

  • Regular Member
  • ***
  • Posts: 17
  • Mole Snacks: +0/-0
Aspirin Equation
« on: March 13, 2010, 06:35:47 PM »
Salicylic Acid + Acetic Anhydride --> Aspirin + acetic acid

Is the mole ratio 1:1 for everything here?

Offline IDudeScience

  • Regular Member
  • ***
  • Posts: 17
  • Mole Snacks: +0/-0
Re: Aspirin Equation
« Reply #1 on: March 15, 2010, 12:36:46 AM »
Anyone know why no matter what you can't expect a 100% yield of aspirin from that equation?

Offline AWK

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7981
  • Mole Snacks: +555/-93
  • Gender: Male
Re: Aspirin Equation
« Reply #2 on: March 15, 2010, 06:04:00 AM »
This is an equilibrium reaction
AWK

Offline IDudeScience

  • Regular Member
  • ***
  • Posts: 17
  • Mole Snacks: +0/-0
Re: Aspirin Equation
« Reply #3 on: March 15, 2010, 09:15:02 PM »
How can you tell?

Offline AWK

  • Retired Staff
  • Sr. Member
  • *
  • Posts: 7981
  • Mole Snacks: +555/-93
  • Gender: Male
Re: Aspirin Equation
« Reply #4 on: March 16, 2010, 02:19:20 AM »
For 100 % yield you should use an excess of acetic anhydride. Moreover some other reactions are possible
AWK

Offline Mitch

  • General Chemist
  • Administrator
  • Sr. Member
  • *
  • Posts: 5298
  • Mole Snacks: +376/-3
  • Gender: Male
  • "I bring you peace." -Mr. Burns
    • Chemistry Blog
Re: Aspirin Equation
« Reply #5 on: March 16, 2010, 06:20:26 AM »
How can you tell?

Most reaction are in equilibrium. Unless you perturb the system by removing something, but then it really wouldn't be equilibrium. ;)
Most Common Suggestions I Make on the Forums.
1. Start by writing a balanced chemical equation.
2. Don't confuse thermodynamic stability with chemical reactivity.
3. Forum Supports LaTex

Sponsored Links