Why is K only affected by temperature? (1 Viewer)

[Lucas_]

If you changed pressure/volume, wouldn't equilibrium lie to either side and hence different amounts of product and reactant are made, changing the value of K (as K = [P]/[R])

Likewise, if you change concentration of either P or R wouldn't that directly change K?

The syllabus dot point is:
4.2.3 -"identify that temperature is theonly factor that changes the value
of the equilibrium constant (K) for
a given equation

PS: I'm sure this has probably been asked many times before, so sorry!

 

[lvella10]

A change in temperature is the only thing that will affect K.
The effect of K when a change in temperature is made can be worked out using Le Chatelier’s principal.
Adding heat will shift the equilibrium to the left (due to Le Chatelier’s Principle) and will result in a larger denominator and hence the value of K will become smaller (decrease).

 

[lvella10]

This theory can obviously be reversed depending on whether the reaction is exothermic or endothermic

 

[barbernator]

A change in temperature is the only thing that will affect K.
The effect of K when a change in temperature is made can be worked out using Le Chatelier’s principal.
Adding heat will shift the equilibrium to the left (due to Le Chatelier’s Principle) and will result in a larger denominator and hence the value of K will become smaller (decrease).

i think he is more asking why pressure does not change the value rather then why temperature does.

 

[Lucas_]

i think he is more asking why pressure does not change the value rather then why temperature does.

Yeah Barber's right; I know the theory but I want to know why

 

[Aykay]

It's because the volume and concentration are considered in the calculation of the equilibrium constant. Because temperature isn't considered, it will affect the value of the constant.

 

[lvella10]

My bad, misread it