In this problem, we want to determine in which direction and equilibrium reaction will shift in order to reestablish equilibrium. If we know that Q is less than K, we think about a generic equilibrium reaction of reacting a reverse oblique producing brought a B. We assume that this reaction is balanced with one mole of each A and B in that both A and B or either gases or equally species and solutions so that we can express both of them in terms of their concentrations. And we can write out the expression for the reactant reaction quotient. Q. Be equal to the concentration of product. Be divided by the concentration of reacting. A. This ratio is also equal to the equilibrium. Constant expression K Where again we have the concentration of product be invited by the concentration of reactive A at a given temperature, the value for the equilibrium constant K is constant. So that means for a given Were you given concentration of product beef, whatever, whatever the concentration of of reacting a is when we divide the concentration of B I. A. It has to always equal this constant value at equilibrium, and so in order for you to be less than cave which is the case in this problem, then that means that in order to decrease this ratio that either we decreased the concentration of product, be where we increased the concentration of reacting a and so in order to reestablish equilibrium, meaning in order for Q to to change the concentrations of being A respectively to maintain this ratio again so that when we divide them we get this equilibrium expression this that same constant for K that the system will respond to the disturbance in a way to counter act that. So if we decrease the concentration of B, which would lead to a decrease in Q, then we need to increase the concentration of B in order to get that came ratio back for equilibrium. In order to increase the concentration of product be, we have to four more product in favor the right side of this equilibrium reaction. Likewise, an increase in reacting a would be another way to decrease que so the system would respond by decreasing the concentration of react in a we decrease the concentration of reacting A. It must mean that were forming more product, be since the forward of the former direction of this reaction would lead to a decrease in the concentration of a so Either way you look at it when Q is less than K. In order to reestablish equilibrium, reaction will shift to the right to produce more product so that when you take the concentration of the products invited by the concentration of the reactant, you take that ratio, you can re establish that constant value for the equilibrium.