Equilibrium Constants

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

Equilibrium Constants

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

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

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

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).

Posts: 62
Joined: Fri Sep 28, 2018 12:23 am

Re: Equilibrium Constants

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

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.