Pressure  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Posts: 104
Joined: Fri Sep 28, 2018 12:19 am


Postby inlovewithchemistry » Mon Jan 14, 2019 10:30 pm

Can someone explain the significance of pressure when discussing equilibrium constants? For example, how would adding an inert gas to a system at equilibrium change anything?

Shally Li 2C
Posts: 30
Joined: Fri Sep 28, 2018 12:22 am

Re: Pressure  [ENDORSED]

Postby Shally Li 2C » Mon Jan 14, 2019 10:40 pm

Adding an inert gas has no effect on the equilibrium concentration so it does not change the constant.

Posts: 72
Joined: Fri Sep 28, 2018 12:29 am

Re: Pressure

Postby Kate_Santoso_4F » Mon Jan 14, 2019 10:46 pm

If the pressure of a reaction vessel is increased by adding an inert gas, then moles of reactant, product, and volume are constant. Therefore, there is no change in the reactant and product concentration and no effect on the reaction. Remember that an inert gas does not undergo chemical reactions under a set of given conditions. Therefore, if the moles of reactant, product, and volume remain constant then the composition of the reaction is the same and the K remains constant.

Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 0 guests