K

[Alexis Robles 2k]

What is the difference between all the K?

[Vuong_2F]

Kc is the equilibrium constant when it's found using concentrations, while Kp is the equilibrium constant when it's found using partial pressures.

[Maika Ngoie 1B]

Kc is the equilibrium constant when it's found using concentrations, while Kp is the equilibrium constant when it's found using partial pressures.

It's important to note that they are all calculated the same way

[Gabriel Ordonez 2K]

There’s Kc and Kp. Kc concerns the use of the equilibrium constant in reference to concentrations. Kp concerns the use of the equilibrium constant in reference to partial pressures. Solution vs. gas.

[Julie_Reyes1B]

It is interesting to note that in the textbook, K automatically means Kp, and if they want you to use Kc they will specifically say Kc. Dr. Lavelle will usually specify which is helpful.

[Philomena 4F]

Kc and Kp are both measures of equilibrium constants of a reaction based on the molar concentration and partial pressure of molecules respectively. Although they follow the same ratio of P/R, be mindful that Kc uses [] and Kp uses () while both have their coefficients in the reaction represented as exponents.

[Cavalli_1H]

Kc denotes concentrations (aqueous solutions) and Kp denotes partial pressure (gas). when solving for Kc, make sure you do your work using brackets to specify the concentrations, and use parentheses for Kp to specify your partial pressures.

[ShastaB4C]

So would it be incorrect to put brackets around a partial pressure?

[504939134]

Kc is the equilibrium constant used for aqueous solutions, because they have concentration values. Kp is the equilibrium constant for gases, since they have partial pressures.

[DHavo_1E]

So would it be incorrect to put brackets around a partial pressure?

Hi,

I would write them using parentheses because brackets are a notation used for concentration.

[SimranSangha4I]

Kp is used within partial pressures while Kc is the constant within concentrations.