Question

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

Answer 1

`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).