Final answer:
The order of the reaction where doubling the concentration of A has no effect on the reaction rate is zero-order. so, option a is the correct answer.
Step-by-step explanation:
If doubling the concentration of reactant A has no effect on the reaction rate for the reaction A → products, this suggests that the order of the reaction with respect to A is zero. Therefore, the reaction is zero-order with respect to A, meaning the rate of the reaction is independent of the concentration of A. The rate law for a zeroth-order reaction is given by the equation rate = k, where the rate is constant and does not depend on the concentration of the reactant.
The reaction in question is a second-order reaction. The rate law for the reaction is rate = k [A] [B], and the overall reaction order is 2.
The reaction in question is a second-order reaction. This can be determined by observing that doubling the concentration of either reactant, A or B, will double the reaction rate. Therefore, the rate law for the reaction is:
rate = k [A] [B]
Where k is the rate constant. This reaction is first order with respect to A and first order with respect to B, resulting in an overall reaction order of 2 (or second order). The rate law and the order of a reaction must be determined experimentally.