Monday
October 20, 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!

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - Two colourless solutions are mixed in a stoppered flask. as the ...
Chemistry - Two flasks containing the same inert gas are at the same temperature...
chemistry - Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) ...
Chemistry - PCl5 --> PCl3 + Cl2 (Kp = 630 at 546 K) A system is prepared by ...
chemistry - For the reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g...
chemistry - The chemical reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) is at ...
chemistry - The chemical reaction N2(g) + 3 H2(g) ↔ 2 NH3(g) is at ...
Chemistry - SO this is my first time doing this... lol i need help on an AP ...
Chemistry - .924moles of A(g) is placed in 1L at 700C where 38.8% dissociated ...
chemistry - Determine the expression for the equilibrium constant for this ...

Search
Members