The reaction' A+B--> C+D rate=k[A][B]2

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1

The reaction’
A+B–> C+D rate=k[A][B]2

Has an initial rate of 0.0770 M/S

  1. what will the initial rate be if [A] is halved and [B] is tripled?
  2. what will the initial rate be if [A] is tripled and [B] is halved?

Answer:

Use everything like a coefficient basically:
x will be the coefficient for rate, so solve for x
x = (1/2)(3^2)
x = 4.5 Thus 4.5 times .0770 is .3465
Now for part 2:
x = 3 (1/2)^2
x = .75
.75 times .0770 = .0.05575