Difference Between Kp and Kc

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Jennifer1E
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Joined: Fri Jun 23, 2017 11:39 am

Difference Between Kp and Kc

Postby Jennifer1E » Mon Jul 31, 2017 10:28 pm

What is the essential difference between Kp and Kc?

Kyle Sheu 1C
Posts: 87
Joined: Fri Jun 23, 2017 11:39 am

Re: Difference Between Kp and Kc

Postby Kyle Sheu 1C » Mon Jul 31, 2017 11:45 pm

Kp is an equilibrium involving the partial pressures of the gases involved, whereas Kc (for the same gaseous reaction) is an equilibrium involving the concentrations of the gases.
In the former, we would use partial pressure=(nRT)/V, while in the latter, we would have M=n/V=P/(RT).

When solving for Kp, you would substitute in the values for partial pressure as you would for any other equilibrium question.

Yeyang Zu 2J
Posts: 58
Joined: Fri Sep 29, 2017 7:06 am

Re: Difference Between Kp and Kc

Postby Yeyang Zu 2J » Tue Nov 21, 2017 8:51 am

Kc And Kp. K and K 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

Alex Leve 3F
Posts: 20
Joined: Fri Sep 29, 2017 7:07 am

Re: Difference Between Kp and Kc

Postby Alex Leve 3F » Tue Nov 21, 2017 2:15 pm

If you are confused on knowing when to use which one, you just need to know that you can only use Kp when there is one or more gaseous product or reactant and no aqueous products or reactants.

Essly Mendoza 1J
Posts: 25
Joined: Fri Sep 29, 2017 7:04 am

Re: Difference Between Kp and Kc

Postby Essly Mendoza 1J » Tue Nov 21, 2017 4:58 pm

How are the equilibrium expression K and the equilibrium expression Kc different? Thank you.


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