I am really confused about how reducing partial pressure of a gas by a certain percentage would impact the behavior of an equilibrium system.
e.g $\ce{POCl3_{(g)} <=> POCl_{(g)} + Cl2_{(g)}}$ is at equilibrium. How would this system behave if the partial pressure of $\ce{Cl2}$ is reduced by 75%?
I understand the partial pressure is related to moles but having a hard time applying it here. My guess is that the reactant would be consumed to produce more of the $\ce{Cl2}$ since its pressure and thus moles are decreasing. However, my instructor said the system would react by consuming $\ce{POCl}$, the reason for which was not explained too well.
If I could get an explanation, it would be much appreciated.