Equilibrium Constants

Moderators: Chem_Mod, Chem_Admin

haleyervin7
Posts: 61
Joined: Fri Sep 28, 2018 12:15 am

Equilibrium Constants

Postby haleyervin7 » Thu Jan 17, 2019 12:23 am

How does K differ from Kc? If there is a difference, how would you solve for K when given Kc and vice versa?

mcredi
Posts: 63
Joined: Fri Sep 28, 2018 12:16 am

Re: Equilibrium Constants

Postby mcredi » Thu Jan 17, 2019 9:22 am

Kc and Kp are the equilibrium constants of gaseous mixtures. However, the difference between the two constants is that Kc is defined by molar concentrations, whereas Kp is defined by the partial pressures of the gasses inside a closed system.

annabel 2A
Posts: 67
Joined: Fri Sep 28, 2018 12:18 am

Re: Equilibrium Constants

Postby annabel 2A » Thu Jan 17, 2019 10:05 am

Also, Kp=Kc*RT^[(moles of products)-(moles of reactants)]

Courtney Quan 1C
Posts: 60
Joined: Fri Sep 28, 2018 12:26 am
Been upvoted: 2 times

Re: Equilibrium Constants

Postby Courtney Quan 1C » Thu Jan 17, 2019 12:14 pm

K itself is the equilibrium constant, but Kc specifies usage of concentrations in mols/L rather than Kp, which specifies usage of partial pressures (applicable to gases only).

Madeline Motamedi 4I
Posts: 62
Joined: Fri Sep 28, 2018 12:23 am

Re: Equilibrium Constants

Postby Madeline Motamedi 4I » Thu Jan 17, 2019 3:36 pm

You will notice that Kp only is calculate for reactions where the products and reactants are all gasses. If they aren't, you're most likely going to be dealing with Kc.

Tatum Keichline 2B
Posts: 64
Joined: Fri Sep 28, 2018 12:26 am

Re: Equilibrium Constants

Postby Tatum Keichline 2B » Thu Jan 17, 2019 6:16 pm

Kc is specific to concentration while Kp is for gases and partial pressures. Kc can be used for gaseous mixtures I believe, but it's more likely for Kp to be used.


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests