Rate of constant (k)=10−3M−1sec−1 ∵1−n=−1 [unit of k=M1−nsec−1] n=2⇒2nd order reaction rate =k[A]2 (A) If concentration of A is 4 times then reaction will become 16 times. (B) Order of reaction is 2. (C) Half-life of the reaction is independent of the concentration of the reactant for 1st order, not for 2nd order reaction. (D) Decomposition of N2O5 is example of 1st order reaction (E) Graph of ℓ
[R]0
[R]t
vs t is straight line for 1st order not for 2nd order reaction. So statement (A) & (B) are correct.