Homework Help: Chemistry 2

Posted by Robert on Friday, August 3, 2012 at 12:42pm.

Supposed you stoppered the flasks after your titration to determine the equilibrium constant and kept the solutions for another day so that the equilibrium was re-established. What would happen to the amount of ethanol present? What would be the relationship of the original equilibrium constant you calculated to the new one?

Okay so this is my attempt at the answer, but I'm really not sure if this is right:

Because ethanol is more volatile than water, some of it, after a day, will evaporate, so we'll have less products, so the equilibrium constant will be different from the one we have and so the equilibrium will be towards the right to compensate for the evaporated ethanol, so K < 1.

Is this correct?

Thank you!

Chemistry 2 - DrBob222, Friday, August 3, 2012 at 1:40pm
I'm in the dark as to what you did.
Chemistry 2 - Robert, Friday, August 3, 2012 at 1:46pm
oh this is just a theoretical question. It's about the hydrolysis of ethyl acetate, it gives ethanol and acetic acid as the products
Chemistry 2 - DrBob222, Friday, August 3, 2012 at 2:18pm
It appears to me that if you stoppered the flask there is no question that the ethanol could NOT evaporate.
Chemistry 2 - Robert, Friday, August 3, 2012 at 4:08pm
oh okay, well in that case there's no change? Nothing happens to the ethanol and we get the same K constant that we had previously?
Chemistry 2 - Anonymous, Monday, April 15, 2013 at 7:49pm
Supposed you (stoppered) the flasks

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