Change in K

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Olivia Young 1A
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Joined: Fri Sep 28, 2018 12:24 am

Change in K

Postby Olivia Young 1A » Mon Jan 14, 2019 10:56 pm

In lecture, why was a change in temperature described as a change in K, while a change in concentration and a change in pressure is described as no changes in K?

Ashley Kim
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Re: Change in K

Postby Ashley Kim » Tue Jan 15, 2019 12:23 am

If you increase the temperature of a reaction, you drive the equilibrium backwards (in the endothermic direction), and therefore increase the concentration of reactants and decrease the concentration of products. The two are inherently connected!

This does not apply to either pressure or concentration.

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Joined: Fri Sep 28, 2018 12:23 am

Re: Change in K

Postby Brandon_Tran_2E » Tue Jan 15, 2019 12:53 am

Temperature changes K because temperature (average kinetic energy) of the molecules are increased/decreased which means the rate of collisions of the molecules are affected which ultimately affects the K equilibrium constant because the rates of both forward and reverse reactions are now changed because of temperature. Pressure change (if it's not due to inert gases) ultimately affects the concentrations of the reaction as well and does not affect K constant because reaction will eventually achieve equilibrium again.

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