Thursday
April 24, 2014

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!

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