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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: IDudeScience on March 13, 2010, 06:35:47 PM

Title: Aspirin Equation
Post by: IDudeScience on March 13, 2010, 06:35:47 PM

Salicylic Acid + Acetic Anhydride --> Aspirin + acetic acid

Is the mole ratio 1:1 for everything here?

Title: Re: Aspirin Equation
Post by: IDudeScience 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?

Title: Re: Aspirin Equation
Post by: AWK on March 15, 2010, 06:04:00 AM

This is an equilibrium reaction

Title: Re: Aspirin Equation
Post by: IDudeScience on March 15, 2010, 09:15:02 PM

How can you tell?

Title: Re: Aspirin Equation
Post by: AWK 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

Title: Re: Aspirin Equation
Post by: Mitch on March 16, 2010, 06:20:26 AM

Quote from: IDudeScience on March 15, 2010, 09:15:02 PM

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. ;)