## Kc to Kp Conversion

Posts: 60
Joined: Sat Jul 22, 2017 3:00 am
Been upvoted: 1 time

### Kc to Kp Conversion

Will we need to know how to convert values of Kc to values of Kp, and vice versa? If so, how do we do this? Do you need to use the Ideal Gas Law (PV=nRT)? There were a few problems like this on a worksheet my TA gave me, so I just wanted to clarify.

Salman Azfar 1K
Posts: 50
Joined: Thu Jul 13, 2017 3:00 am

### Re: Kc to Kp Conversion

I am not sure as to whether or not we will need to know how to do this, but basically you need to use the ideal gas law. If given pressure to get Kc, you need to put pressure into the ideal gas law and calculate the unknown values (most likely moles). Then use those moles to get concentrations and calculate Kc. There are more specific ways to describe this, but that is the basic way.

Sammy Thatipelli 1B
Posts: 63
Joined: Thu Jul 27, 2017 3:01 am
Been upvoted: 1 time

### Re: Kc to Kp Conversion

On one of the chemical equilibrium models, there are questions that Dr. Lavelle wrote that ask you to convert concentrations to pressures and vice versa. Yes, you would use the equation PV=nrt, and know that concentration is equal to P/rt. I would definitely study this because it was one the module post assessments

Julia Meno 1D
Posts: 28
Joined: Fri Sep 29, 2017 7:04 am

### Re: Kc to Kp Conversion

When we say concentration = P/(RT), is "concentration" the molar concentration (Kc)?

Shannon Wasley 2J
Posts: 71
Joined: Fri Sep 29, 2017 7:06 am
Been upvoted: 1 time

### Re: Kc to Kp Conversion

The concentration would be in reference to the specific molar concentration of the compound whose partial pressure is being used in the equation.

nanditasundarapandian1D
Posts: 21
Joined: Sat Jul 22, 2017 3:01 am

### Re: Kc to Kp Conversion

also concentration is n/v in the PV = nRT equation. That's why we are able to get a correlation between them.