Question is in the description

Question

Reaction: A+B-> C+D rate = K[A]^2[B]^2

initial rate is 0.0970 M/s

what will the initial rate be if [A] is halved and [B] is tripled

Answer 1

This reaction is 2nd order in A and 2nd order in B

If only A was halved, the rate would be (0.5)² = 0.25 or 1/4 the initial rate

If only B was tripled, the rate would be (3)² = 9 or 9x the initial rate

Therefore, when both A is halved, and B is tripled, the rate will be 0.25 x 9 = 2.25 x the initial rate

Rate = 2.25 x 0.0970 M/s = 0.218 M/s