Ask Questions, Get Answers

Want to ask us a question? Click here
Browse Questions
0 votes

Consider proposed mechanism for reaction between nitrogen monoxide and hydrogen gas.Step (i):$2NO\rightarrow N_2O_2$,Step 2:$N_2O_2+H_2\rightarrow N_2O+H_2O$,Step 3:$N_2O+H_2\rightarrow N_2+H_2O$.If step 2 rate determining step,then rate law for reaction and all the intermediate of reaction will be

Options Rate law Intermediates
(a) $R=K[NO][H_2]$ $N_2O_2$
(b) $R=[NO]^2[H_2]$ $N_2O_2,N_2O$
(c) $R=K[NO][H_2]$ $N_2O_2,N_2O$
(d) $R=K[NO]^2[H_2]$ $N_2O_2$


Can you answer this question?

1 Answer

0 votes
$2NO\rightarrow N_2O_2$
$N_2O_2+H_2\rightarrow N_2O+H_2O$
$N_2O+H_2\rightarrow N_2+H_2O$
$2NO+2H_2\rightarrow N_2+2H_2O$
Through step 2 two molecules of $NO$ and one molecule of $H_2$ have reacted,so if step 2 is R.D.S then rate law would be
An intermediate is a substance that is produced in one elementary step and consumed in later steps.So intermediates are $N_2O_2$ and $N_2O$
Hence (b) is the correct answer.
answered Dec 18, 2013 by sreemathi.v

Related questions

Ask Question
student study plans
JEE MAIN, CBSE, NEET Mobile and Tablet App
The ultimate mobile app to help you crack your examinations
Get the Android App