An experiment carries out the reaction a → products at three different initial concentrations of a and the initial reaction rate were measured, as indicated in the table. [a](m) initial rate (m/s) 0.15 0.010 0.30 0.040 0.45 0.090 based on this data, what is the rate law for the reaction? view available hint(s) an experiment carries out the reaction at three different initial concentrations of and the initial reaction rate were measured, as indicated in the table. initial rate 0.15 0.010 0.30 0.040 0.45 0.090 based on this data, what is the rate law for the reaction? rate = k[a]2 rate = k[a]3 rate = k[a] rate = k

First lets tabulate the data
                 [a]                              rate  (m/s)
              0.15                             0.010
              0.30                             0.040
              0.45                             0.090            
x - order of reaction with respect to a
since a is the only reactant, the order with respect to a is the order of the reaction 
rate equation;
Rate = k [a]ˣ
where k - rate constant 
substituting rate values and [a]
0.010  = k[0.15 ]ˣ1)
0.040  = k [0.30]ˣ2)
divide 2 by 1
4 = 2ˣ
x = 2
therefore order with respect to a is 2
this is therefore a second order reaction 
Rate = k [a]²