Question

For the reaction given below, the following mechanism has been given:

Reaction - $2NO+B{r}_2\to 2NOBr$

Mechanism:

$NO+B{r}_2\stackrel{fast}{\to }NOB{r}_2$

$NOB{r}_2+NO\stackrel{slow}{\to }2NOBr$

Hence, the rate law is :

• A. $k\left[NO{]}^2\right[B{r}_2]$
• B. $k\left[NO\right]\left[B{r}_2\right]$
• C. $k\left[NOB{r}_2\right]\left[NO\right]$
• D. $k\left[NO\right][B{r}_2{]}^2$

Answer 1

The correct option is B $k\left[NO\right]\left[B{r}_2\right]$