Limited access

Upgrade to access all content for this subject

Analyze the following reaction and data:

$$A + B \longrightarrow C$$

[A] [B] Initial Rate (M/s)
0.200 0.100 $4.0 \times 10^{-3}$
0.200 0.200 $4.0 \times 10^{-3}$
0.400 0.100 $1.6 \times 10^{-2}$

$\ $
Which of the following is the rate law given the data provided?

A

$\text{rate} = k [A][B]$

B

$\text{rate} = k [A]^2[B]$

C

$\text{rate}= k [B]^2$

D

$\text{rate}= k [A]^2$

Select an assignment template