11.57 6th Edition

Moderators: Chem_Mod, Chem_Admin

Sarah Bui 2L
Posts: 61
Joined: Fri Sep 28, 2018 12:29 am

11.57 6th Edition

Postby Sarah Bui 2L » Thu Jan 24, 2019 5:36 pm

A reaction mixture consisting of 2.00 mol CO and 3.00 mol H2 is placed in a 10.0-L reaction vessel and heated to 1200. K. At equilibrium, 0.478 mol CH4 was present in the system. Determine the value of Kc for the reaction

In the solutions manual, they used moles in their ICE table, can we just convert them all into M? Is it assumed that the 0.478 mol CH4 is also placed in a 10.0 L reaction vessel?

Douglas Nguyen 2J
Posts: 71
Joined: Fri Sep 28, 2018 12:15 am

Re: 11.57 6th Edition

Postby Douglas Nguyen 2J » Thu Jan 24, 2019 7:56 pm

The CH4 isn't placed in the vessel but rather is produced through the chemical reaction involving CO and H2.

Celine Cheng 1H
Posts: 33
Joined: Fri Sep 28, 2018 12:21 am
Been upvoted: 1 time

Re: 11.57 6th Edition

Postby Celine Cheng 1H » Thu Jan 24, 2019 9:04 pm

I'm p sure you can also convert everything into molarity and calculate it from there (and it makes it easier when calculating Kc imo)! Also, the amount of CH4 they mentioned is the amount present at equilibrium, so it gives you a hint as to where to place it in the ICE table ;)


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 1 guest