6th Edition 11.7 part c

Albert Duong 4C
Posts: 66
Joined: Fri Sep 28, 2018 12:17 am
Been upvoted: 1 time

6th Edition 11.7 part c

Assuming that the initial pressure of X2 was 0.10 bar, calculate the value of K for the decomposition.
Can someone show me how to do this?

Matthew Tran 1H
Posts: 165
Joined: Fri Sep 28, 2018 12:16 am

Re: 6th Edition 11.7 part c

For this question, it is important to know that each particle contributes equally to the pressure; that is, X and X2 each contribute the same amount of pressure even though they are different sizes. There are 11 particles initially, and the pressure is 0.10 bar. Try using this as a ratio to help solve the problem. Good luck!

Posts: 37
Joined: Mon Apr 23, 2018 3:00 am

Re: 6th Edition 11.7 part c

You also want to look at flask #3, when the reaction has reached equilibrium. I used the number of X2 and the number of X over the total number of molecules (17) for the mole fraction when calculating the partial pressures for X2 and X (mole fraction times total pressure) to find K. Hope that helps!

Laurence Tacderas 1K
Posts: 30
Joined: Fri Sep 28, 2018 12:20 am

Re: 6th Edition 11.7 part c

The flask shows the reaction at equilibrium - while the number of X2 molecules and X atoms are different compared to their initial amounts (no X initially), the total number of moles is the same before and after the reaction. By taking the mole fractions (the number of moles X2 or X / the total number of moles) of the reactant/product and multiplying each by the initial partial pressure of X2, you can find their equilibrium partial pressures to calculate Kp.

Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests