Assertion: The reaction quotient, Q has the same form as the equilibrium constant Keq and is evaluated using any given concentrations of the species involved in the reaction, and not necessarily equilibrium concentrations.

Reason: If the numerical value of Q is not the same as the value of equilibrium constant, a reaction will occur.

Explanation:

Reaction Quotient (Q):
The reaction quotient, Q, is a mathematical expression that relates the concentrations (or partial pressures) of the reactants and products at any given point during a reaction. It has the same form as the equilibrium constant, Keq, but is evaluated using any given concentrations, not necessarily equilibrium concentrations.

Equilibrium Constant (Keq):
The equilibrium constant, Keq, is a constant value that expresses the ratio of the concentrations (or partial pressures) of the products to the concentrations (or partial pressures) of the reactants at equilibrium. It is determined at a specific temperature and remains constant as long as the temperature is not changed.

Relationship between Q and Keq:
The relationship between Q and Keq can be understood by comparing their mathematical expressions. Both Q and Keq are calculated using the concentrations (or partial pressures) of the reactants and products, raised to the power of their stoichiometric coefficients in the balanced chemical equation.

If the numerical value of Q is equal to the value of Keq, it means that the system is at equilibrium. This implies that the reaction has reached a state where the rates of the forward and reverse reactions are equal, and there is no net change in the concentrations of the reactants and products.

If the numerical value of Q is not equal to the value of Keq, it indicates that the system is not at equilibrium. This suggests that the reaction has not yet reached its equilibrium state, and there is a tendency for the reaction to proceed in the direction that will minimize the difference between Q and Keq.

Conclusion:
In conclusion, the assertion is correct. The reaction quotient, Q, has the same form as the equilibrium constant, Keq, and is evaluated using any given concentrations of the species involved in the reaction, not necessarily equilibrium concentrations. The reason is also valid because if the numerical value of Q is not the same as the value of Keq, a reaction will occur to establish equilibrium.