Hi all.
I'm attempting to do a problem where I'm given the molarity of both the reactions and products side. However, I'm never given a Kc in this problem. Is there a value that one would use in case the Kc isn't given or does the Kc always need to be explicitly stated? Any help would be greatly appreciated!
What to do if Kc isn't given.
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 34
- Joined: Mon Jan 09, 2023 9:26 am
Re: What to do if Kc isn't given.
Usually, Kc is given when trying solve these equilibrium problems and you should not try to have a place-holding number if Kc is not given. However, if Kc is not given, then the problem is probably asking for you to find Kc using the concentrations given.
-
- Posts: 23858
- Joined: Thu Aug 04, 2011 1:53 pm
- Has upvoted: 1253 times
-
- Posts: 18
- Joined: Mon Jan 09, 2023 9:35 am
Re: What to do if Kc isn't given.
Hi all.
The question I'm answering is:
When 0.70 mol NO2 was placed in a 1.00 L flask and allowed to reach equilibrium, it’s
concentration was found to be 0.28 M, once equilibrium was established. Calculate Kc for
this reaction.
a) 1.9
b) 0.94
c) 0.47
d) 0.14
I've set up an ICE table but it seems a bit of a hassle to solve since there isn't much I can do unless I'm looking at it incorrectly. If it helps, the correct answer ends up being c).
The question I'm answering is:
When 0.70 mol NO2 was placed in a 1.00 L flask and allowed to reach equilibrium, it’s
concentration was found to be 0.28 M, once equilibrium was established. Calculate Kc for
this reaction.
a) 1.9
b) 0.94
c) 0.47
d) 0.14
I've set up an ICE table but it seems a bit of a hassle to solve since there isn't much I can do unless I'm looking at it incorrectly. If it helps, the correct answer ends up being c).
Return to “Equilibrium Constants & Calculating Concentrations”
Who is online
Users browsing this forum: No registered users and 19 guests