At a given temperature, the reaction quotient $Q$ for a reaction is found to be LESS than the equilibrium constant $K$. Which way will the reaction proceed?

1. $Q$ has the SAME functional form as $K$ but uses CURRENT (non-equilibrium) concentrations. 2. NCERT §6.6.2 gives the rule: if $Q < K$, products are under-represented; the reaction proceeds FORWARD to increase product concentration until $Q$ rises to $K$. 3. If $Q > K$, the reaction proceeds in REVERSE (option B is the wrong case). If $Q = K$, the system is already at equilibrium (option C is the wrong case). 4. The reaction never just "stops" (option D) — it is dynamic; only the NET rate becomes zero at equilibrium. _Source: NCERT Class 11 Chemistry, Ch 6, §6.6.2 (Predicting the Direction of the Reaction, $Q$ vs $K$), p. 15._