🤓 Based on our data, we think this question is relevant for Professor Lewis' class at USF.

The reaction A + B yields C + D rate = k[A][B] ^{2 }has an intial rate of 0.0220 M/s.

a) What will the initial rate be if [A] is halved and [B] is tripled? Answer must be in M/s.

b) What will the intial rate be if [A] is tripled and [B] is halved? Answer must be in M/s.

a) $Rate = k[A][B]^2$

Original initial rate: $0.0220 \ M/s = k[1][1]^2$

New initial rate: $Rate = [Â½] [3]^3 = 9/2$ times the original

Rate Law