If the rate of reaction for 2A + B → products is k[A]2[B] and A is present in large excess then order of reaction is

Explanation

When a reactant is present in large excess, its concentration remains practically constant throughout the reaction. In this case, the reactant in large excess is A. Let's analyze the impact on the rate of the reaction:Initially, the rate depends on the concentrations of both A and B, as indicated by the rate law: k[A]^2[B].However, as A's concentration remains almost constant due to its excess, its change in concentration won't significantly affect the reaction rate.Therefore, the rate becomes essentially independent of [A] and primarily depends on the concentration of B: rate ≈ k[B].This effectively reduces the order of the reaction with respect to A.