11.73 Concept Question

Moderators: Chem_Mod, Chem_Admin

Emily Duggan 1F
Posts: 42
Joined: Fri Sep 29, 2017 7:07 am

11.73 Concept Question

Postby Emily Duggan 1F » Sun Dec 03, 2017 6:04 pm

I know that an increase in pressure means a decrease in volume due to PV=nRT, but how does this apply to the direction of the reaction?

Tanaisha Italia 1B
Posts: 55
Joined: Fri Sep 29, 2017 7:04 am

Re: 11.73 Concept Question

Postby Tanaisha Italia 1B » Sun Dec 03, 2017 6:10 pm

I think that a decrease in volume would inadvertently increase the concentration, since there are the same number of moles in a smaller volume of solvent. Thus, if the pressure on the left side increased, the reaction would move towards the right because reactions move in terms of higher to lower concentration.

Sara Varadharajulu
Posts: 60
Joined: Thu Jul 13, 2017 3:00 am
Been upvoted: 1 time

Re: 11.73 Concept Question

Postby Sara Varadharajulu » Sun Dec 03, 2017 6:15 pm

when you decrease the volume and that results in an increase in pressure, the reaction will go toward the side with less mols (bc that has lower pressure in terms of concentration).
when you increase the pressure in terms of inert gas, nothing happens.

Kyra LeRoy 1E
Posts: 52
Joined: Sat Jul 22, 2017 3:00 am

Re: 11.73 Concept Question

Postby Kyra LeRoy 1E » Sun Dec 03, 2017 6:18 pm

If there are more moles of reactant, then an increase in pressure and decrease in volume makes the equation shift to the right.
If there are more moles of product, increased pressure and decreased volume will mean a shift to the right.

However, make sure you note that if pressure is increased because of inserting an inert gas, nothing will happen to equilibrium because moles & volume of everything stay the same, and therefore concentration stays the same.

Return to “Applying Le Chatelier's Principle to Changes in Chemical & Physical Conditions”

Who is online

Users browsing this forum: No registered users and 1 guest