Chapter 14.2, Problem 1CP

Answer questions 14.2.1 through 14.2.4 using the table of initial rate data for the reaction:

$\text{A +2B }\underset{}{\to }\text{2C + D}$

Experiment	[A] (M)	Initial [B] (M)	Rate (M/s)
1	0.12	0.010	$2.2\times {10}^{-3}$
2	0.36	0.010	$6.6\times {10}^{-3}$
3	0.12	0.020	$2.2\times {10}^{-3}$

What is the rate law for the reaction?

$\begin{array}{l}\text{a)}\hfill \\ \text{rate = }k\left[\text{A}\right]{\left[\text{B}\right]}^{\text{2}}\hfill \\ \text{b)}\hfill \\ \text{rate = }k{\left[\text{A}\right]}^{\text{2}}\left[\text{B}\right]\hfill \\ \text{c)}\hfill \\ \text{rate = }k{\left[\text{A}\right]}^{\text{3}}\hfill \\ \text{d)}\hfill \\ \text{rate = }k{\left[\text{A}\right]}^{\text{2}}\hfill \\ \text{e)}\hfill \\ \text{rate = }k\left[\text{A}\right]\hfill \end{array}$