Question 11.11

Moderators: Chem_Mod, Chem_Admin

arif_latif_2G
Posts: 60
Joined: Fri Sep 28, 2018 12:23 am

Question 11.11

Postby arif_latif_2G » Sun Jan 13, 2019 10:34 pm

6th Edition
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.

Can someone help answer part C? The answers for the other parts: (a) Flask 3 represents the point of reaction equilibrium. (b) 54.5%;

Rebecca Altshuler 1D
Posts: 61
Joined: Fri Sep 28, 2018 12:15 am

Re: Question 11.11

Postby Rebecca Altshuler 1D » Sun Jan 13, 2019 11:11 pm

In order to start doing part c, find the percentages for both the products and the reactants (#molecules in question/# total molecules) the multiply these fractions by .10 bar. These should give you the partial pressures needed to solve the problem.

Vanadium Wang 4H
Posts: 60
Joined: Fri Sep 28, 2018 12:19 am

Re: Question 11.11

Postby Vanadium Wang 4H » Mon Jan 14, 2019 12:02 am

I believe this question is actually 11.7. To calculate the value of K you use the equation (Px)2/PX2. Multiply the mole fraction of the reactant and product respectively by the initial pressure of 0.1 bar to get the partial pressures. Solve and you should get 0.17


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 3 guests