If the reaction quotient (Q) is smaller than the equilibrium constant (K), it indicates that the concentrations of the reactants are lower compared to the concentrations at equilibrium. In this scenario, the reaction will tend to shift in the forward direction in order to reach equilibrium. The following explains the reasons behind this:

Understanding the Reaction Quotient (Q) and Equilibrium Constant (K)
The reaction quotient (Q) is a measure of the relative concentrations of the reactants and products at any given point during a chemical reaction. It is calculated by substituting the concentrations of the reactants and products into the equilibrium expression, using the coefficients from the balanced chemical equation. Q helps determine if the reaction is at equilibrium or not.

The equilibrium constant (K) is the value of the reaction quotient (Q) when the system is at equilibrium. It is a constant at a given temperature and provides information about the relative concentrations of reactants and products at equilibrium. The value of K indicates the extent of the reaction, with larger values indicating a higher concentration of products compared to reactants at equilibrium.

If Q < />
When the reaction quotient (Q) is smaller than the equilibrium constant (K), it means that the system is not at equilibrium. In this case, the concentrations of the reactants are lower than what they would be at equilibrium. To reach equilibrium, the system must shift in the direction that will increase the concentrations of the products and decrease the concentrations of the reactants.

Le Chatelier's Principle
Le Chatelier's Principle states that if a system at equilibrium is subjected to a change, it will respond in a way that tends to counteract that change and restore equilibrium. In this case, the change is the lower concentration of reactants compared to equilibrium. To counteract this change, the system will shift in the forward direction to produce more products.

Continuous Increase in Reaction Quotient
As the system shifts in the forward direction, the concentrations of the reactants decrease further, while the concentrations of the products increase. This causes the value of the reaction quotient (Q) to increase continuously. The system will continue to shift in the forward direction until the concentrations of the reactants increase and the concentrations of the products decrease, reaching a point where Q is equal to K.

Conclusion
In summary, when the reaction quotient (Q) is smaller than the equilibrium constant (K), the system will shift in the forward direction to reach equilibrium. This shift will continue until the concentrations of the reactants increase and the concentrations of the products decrease, resulting in Q being equal to K.