If you consider this equilibrium reaction:

2A(s) + B(g) <--> 2C(g) with some value of K, equilibrium constant

Why won't changing the pressure not change the equilibrium constant?

only thing that changes the equilibrium constant is TEMPERATURE!!!!!

I've seen the part you mentioned about temperature too. However, I've also read that increasing the pressure will favor the side with less moles of gas, and vice versa for decreasing the pressure. Why wouldn't this shift in equilibrium change the equilibrium constant?

because increasing one cause decreasing another one in your "K" equation then K will be constant

You can shift the equilibrium by changing the pressure meaning that your equilibrium will lie more towards one mole of gas than two, but the Keq/equilibrium constant will never change unless temp is changed.