Partial Pressures for Different Temperatures
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 32
- Joined: Sun Jan 21, 2018 3:00 am
Partial Pressures for Different Temperatures
For 5G.9 it asks whether the partial pressures will be the same in both containers when the second container has a higher molarity. I have the answer key and it says the partial pressures will be different, but I don't understand why. If each container is held at the same temperature, wouldn't the partial pressures stay the same? Or does it change because the molarity changes, and if so, why?
-
- Posts: 96
- Joined: Fri Sep 28, 2018 12:16 am
- Been upvoted: 2 times
Re: Partial Pressures for Different Temperatures
In the second container, since the concentration of O2 is greater the partial pressure is greater. Pressure and concentration are directly proportional as shown by P=(conc.)RT, so if concentration is greater, then pressure is also greater (given that T is the same).
Re: Partial Pressures for Different Temperatures
Molarity and Partial Pressure are directly related.
We can tell from PV=nRT when the equation is written
- (n/V) = P/(RT) or
- concentration = P/(RT)
that when the pressure increases the concentration will also increase.
We can tell from PV=nRT when the equation is written
- (n/V) = P/(RT) or
- concentration = P/(RT)
that when the pressure increases the concentration will also increase.
Return to “Equilibrium Constants & Calculating Concentrations”
Who is online
Users browsing this forum: No registered users and 24 guests