For the  hypothetical reaction 2A +B --> C  + D, the following rate data was collected.     Exp #  [A] [B] Rate (M/s) 1 0.300 0.100   2.300 x 10 -4 M/s 2 0.200 0.100   1.533 x 10-4 M/s 3 0.300 0.150   5.175 x 10-4 M/s Determine the rate law and calculate the value of k  (3 sig figs) For the reaction in the question above, if  [A] = 0.250 and [B] = 0.175, what will the rate of the reaction be?

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