question_answer

For the reaction, \[2NO+B{{r}_{2}}\to 2NOBr\], the following mechanism has been given             

a. \[NO+B{{r}_{2}}\overset{fast}{leftrightarrows}NOB{{r}_{2}}\]

b. \[NOB{{r}_{2}}+NO\overset{slow}{leftrightarrows}2NOBr\]

Hence rate law is

A) \[r=k{{[NO]}^{2}}[B{{r}_{2}}]\] 

B) \[r=k[NO][B{{r}_{2}}]\]

C) \[r=k[NOB{{r}_{2}}][NO]\]          

D) \[r=k[NO]{{[B{{r}_{2}}]}^{2}}\]