The following system is at equilibrium:X(s)+3Y(g)⇌Z(g)X(s)+3Y( g)⇌Z(g)Classify each of the following actions by whether it causes a leftward shift, a rightward shift, or no shift in the direction of the net reaction.

Explanation:

The principle applied here is Le Chatelier's principle which states that for a reaction at equilibrium, a change in the temperature, pressure , concentration will shift the position to the right or to the left by way of favoring the forward or the backward reaction so as to annul or neutralize the equilibrium state.

The equilibrium constant expression for the reaction ; Keq = [Z]/[Y]^3

solid and liquid have a value of 1, as such if we add more of X to the reactants side or remove more of X, it will have no effect on the position of the equilibrium.

Also, an increase in volume will result in a decrease in pressure which will shift the equilibrium position to the left there by favoring the forward reaction i.e product formation.

Also, a decrease in volume will result to an increase in pressure which will shift the equilibrium position to the right thereby favoring the backward reaction i.e reactant formation

idk i’m struggling too