Equilibrium Constant vs Reaction Quotient  [ENDORSED]

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Ronica_Patel_3G
Posts: 10
Joined: Sat Jul 09, 2016 3:00 am

Equilibrium Constant vs Reaction Quotient

Postby Ronica_Patel_3G » Wed Nov 09, 2016 2:02 pm

Since you calculate the reaction quotient Q and the equilibrium constant K using the same method, how will you be able to compare the two values to determine the direction it will go? Wouldn't they be the same value?

Sangita_Sub_3H
Posts: 23
Joined: Sat Jul 09, 2016 3:00 am

Re: Equilibrium Constant vs Reaction Quotient  [ENDORSED]

Postby Sangita_Sub_3H » Wed Nov 09, 2016 2:04 pm

Hi! Although Q and K are calculated the same way, the same numbers are not used. For Q, the numbers that are used for the calculation are not at equilibrium; rather, they are measured values at a specific point in time. However, when measuring K, the values used are at equilibrium, which is why Q and K are comparable.

Hope this helps!

nick_pantoja_3G
Posts: 25
Joined: Sat Jul 09, 2016 3:00 am

Re: Equilibrium Constant vs Reaction Quotient

Postby nick_pantoja_3G » Fri Nov 11, 2016 2:46 pm

And with those Q and K values, you will be able to compare and see which side is favored.

Marisa_Woo_2G
Posts: 24
Joined: Wed Sep 21, 2016 2:56 pm

Re: Equilibrium Constant vs Reaction Quotient

Postby Marisa_Woo_2G » Mon Nov 14, 2016 10:24 am

Just to clarify, the values used to calculate K and Q should be concentrations? Would this refer to molar concentrations like moles/liter and molarity for aqueous solutions? And then partial pressure for concentrations of gas?

Julia Nakamura 2D
Posts: 33
Joined: Wed Sep 21, 2016 2:57 pm

Re: Equilibrium Constant vs Reaction Quotient

Postby Julia Nakamura 2D » Mon Nov 14, 2016 11:21 am

Yes. So when calculating Q and K, either pressures (for gases) or concentrations in moles/L (molarity for aqueous solutions) are used. Q and K do not have units, but the values used to solve for Q and K will have units.


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