ICE Chart with Gas Pressures

[Isabel_Eslabon_2G]

Hello.

So when we are given Kp and pressures of compounds in bar, do we just use those pressures in the ICE chart instead of molarity amounts? Adding onto that, do we need to convert to atm?

[Gwendolyn Hill 2F]

Hi!
So for the sake of this class, Lavelle said that we are using 1 bar = 1 atm, so you can just kind of "say" they are equal. And yes! That is how you would do the ICE chart. Use whatever version of the compounds you are given unless stated otherwise!

[Keshav Patel 14B 2B]

Yup exactly you want to use bar and you want to use pressures not molarity. Pressure equilibrium is different from concentration of molarity.

[Kat Stahl 2K]

Yea! you just use the pressure values instead of molarity values! We use bar and atm and lavelle told us they are basically interchangeable.

[Rose_Malki_3G]

Yes we use them in the ice chart like we would with concentrations. You do not need to convert the units.

[Joshua Chung 2D]

Yep; they are completely interchangeable in this coursel; just remember to keep the units of measurement consistent throughout the problem.

[Charlotte Adams 1A]

Yes, you do the same ICE table and procedure as you would if given concentration and I remember Dr. lavelle saying 1 bar= 1atm

[Kristina Krivenko 3I]

Hi! Yes, you're correct! If we're given Kp and partial pressures, we can use ICE table just like we would if we were given Kc and molar concentrations.

And since 1 atm = 1.01325 bar, Dr. Lavelle mentioned in his lecture that, in this course, we can approximate that 1 atm = 1 bar to simplify our approximations.

[Christine Ma 3L]

The above posters already talked about how you can just use pressures instead of concentration in the ICE chart. But for the unit question, you don't need to convert to atm. Unless the question requires it or it makes calculations easier, you can leave your answer in bar.