The reaction A + B 2C + D was studied starting with the following initial concentrations [A]0 = 0.50 M and [B]0 = 2.00x10-4 M. The progress of the reaction was followed by determining the concentration of any of the reagents.

t, s [B]. M

0.00 2.00x10^-4

5.00 1.00x10^-4

12.07 0.50x10^-4

22.07 0.25x10^-4

In another experiment, the initial concentrations were [B]0 = 0.50 M and [A]0 = 1.00x10-4 M and the results were:

t, s [A]. M

0.00 1.00x10^-4

5.00 0.50x10^-4

15.00 0.25x10^-4

35.00 0.125x10^-4

Assuming a rate law of the type r = [A]^ [B]^, determine the order with respect to A and B. (Hint: a) Notice that these are not half-life times but times. b) Record the time between times and the changes in concentration and transform the data.)