How does the effect of concentration and pressure affect #K_p#?

1 Answer
Al E.
Nov 11, 2017

#K_p# is the equilibrium constant for gaseous mixtures.

For instance

#N_2(g)+3H_2(g)rightleftharpoons2NH_3(g)#

If I increase the partial pressure or concentration of various gases, the reaction will shift to the right or left based on Le Chatlier's principle to consume or produce a gas that is in excess or lacking relative to the concentration at equilibrium.

Since volume and pressure are generally inversely related. I could also decrease the volume of the container this reaction is occurring in and it will shift to the side with the least moles of gas (e.g. the right).

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