Question

Consider the following data showing the initial rate of action (A rightarrow products) at several different concentrations Write a rate law for the reaction. Rate = k[A] Rate = k[A]^2 Rate = k Rate = k[A]^3 Estimate the value of the rate constant, k. Express your answer using two significant figures. k = s^-1

Answer 1

A)

we see that when concentration of A, doubles, initial rate also doubles

So it is 1st order reaction

rate = k [A]

put any values:
0.008 = k*0.15
k = 0.053 s-1
Answer: 0.053 s-1