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### Equations

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

### Re: Equations

Posted: Fri Jan 11, 2019 5:52 pm
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
Yes, you could easily convert between partial pressure to concentration by using PV=nRT.

### Re: Equations

Posted: Sun Jan 13, 2019 1:33 pm
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
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
Kc uses concentration and Kp uses partial pressure

### Re: Equations

Posted: Sun Jan 13, 2019 4:56 pm
Kc- concentration and Kp- partial pressure