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Equations

Posted: Fri Jan 11, 2019 5:15 pm
by jane_ni_2d
What is the difference between Kc and Kp?

Re: Equations

Posted: Fri Jan 11, 2019 5:52 pm
by Matthew Tran 1H
Kc is calculated using the equilibrium molar concentrations of products and reactants while Kp is calculated using the equilibrium partial pressures of products and reactants and can only be used for gases. You can relate the two using P=(concentration)RT.

Re: Equations

Posted: Sun Jan 13, 2019 1:02 pm
by Jonathan Zhao 4H
Yes, you could easily convert between partial pressure to concentration by using PV=nRT.

Re: Equations

Posted: Sun Jan 13, 2019 1:33 pm
by anthony_trieu2L
When you are given equilibrium concentrations, you must use Kc to calculate the equilibrium constant. This can apply to both aqueous solutions and gases. In contrast, Kp can only be used to calculate the equilibrium constant of partial pressures. Kp cannot be applied to aqueous solutions since they do not have partial pressures.

Re: Equations

Posted: Sun Jan 13, 2019 3:11 pm
by Cole Doolittle 2K
Kp = Kc x (RT) ^ stoichiometric coefficient

In general, Kp uses partial pressures and Kc uses concentrations

Re: Equations

Posted: Sun Jan 13, 2019 4:13 pm
by Phil Timoteo 1K
Kc uses concentration and Kp uses partial pressure

Re: Equations

Posted: Sun Jan 13, 2019 4:56 pm
by Hilda Sauceda 3C
Kc- concentration and Kp- partial pressure