Equations
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 67
- Joined: Fri Sep 28, 2018 12:23 am
-
- Posts: 165
- Joined: Fri Sep 28, 2018 12:16 am
Re: Equations
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.
-
- Posts: 57
- Joined: Fri Sep 28, 2018 12:26 am
Re: Equations
Yes, you could easily convert between partial pressure to concentration by using PV=nRT.
-
- Posts: 60
- Joined: Fri Sep 28, 2018 12:29 am
Re: Equations
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.
-
- Posts: 30
- Joined: Fri Sep 28, 2018 12:20 am
Re: Equations
Kp = Kc x (RT) ^ stoichiometric coefficient
In general, Kp uses partial pressures and Kc uses concentrations
In general, Kp uses partial pressures and Kc uses concentrations
-
- Posts: 101
- Joined: Fri Apr 06, 2018 11:05 am
-
- Posts: 76
- Joined: Fri Sep 28, 2018 12:24 am
Return to “Equilibrium Constants & Calculating Concentrations”
Who is online
Users browsing this forum: No registered users and 19 guests