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Help with question 11.7

Posted: Wed Jan 09, 2019 9:42 pm
by Kenan Kherallah 2C
11.7 The following flasks show the dissociation of a diatomic molecule, X2, over time. (a) Which flask represents the point in time at which the reaction has reached equilibrium?
(b) What percentage of the X2 molecules have decomposed at equilibrium? (c) Assuming that the initial pressure of X2 was 0.10 bar, calculate the value of K for the decomposition.
I really need help with c. I dont get why the mole fraction formula gives you the correct answers? Can someone please explain.


Re: Help with question 11.7

Posted: Wed Jan 09, 2019 11:38 pm
by Jerome Mercado 2J
The fractions of the molecules is equivalent to to partial pressures of each molecule; just multiply those fractions by .10 to convert to partial pressures. Then use the equilibrium expression of partial pressures to get the equilibrium constant. Hope this helps.

Re: Help with question 11.7

Posted: Thu Jan 10, 2019 7:46 pm
by Matthew Tran 1H
Pressure is directly proportional to the number of molecules/particles since all pressure really is is collisions of the particles against the container. So in this problem, there are 11 X2 molecules in the original container, so each molecule contributes a pressure of 0.10/11 bar per molecule. At equilibrium, there are 17 particles (5 X2, and 12 X from the decomposition of 6 X2), so therefore the total pressure is (17/11)*0.10 bar (size of the molecule doesn't matter when calculating pressure). You then could use fraction of X and X2 in the equilibrium container to find the partial pressures and calculate K. Hopefully you can see how you use both mole ratios and pressure ratios to get the answer!