| In the reversible reaction, |
| \[2N{{O}_{2}}{{N}_{2}}{{O}_{4}}\] |
| the rate of disappearance of \[N{{O}_{2}}\] is equal to |
A) \[\frac{2{{k}_{1}}}{{{k}_{2}}}\,{{[N{{O}_{2}}]}^{2}}\]
B) \[2{{k}_{1}}\,{{[N{{O}_{2}}]}^{2}}-2{{k}_{2}}\,[{{N}_{2}}{{O}_{4}}]\]
C) \[2{{k}_{1}}{{[N{{O}_{2}}]}^{2}}-{{k}_{2}}[{{N}_{2}}{{O}_{4}}]\]
D) \[(2{{k}_{1}}-{{k}_{2}})\,[N{{O}_{2}}]\]
Correct Answer: B
Solution :
| \[2N{{O}_{2}}\underset{{{k}_{2}}}{\overset{{{k}_{1}}}{\mathop{\rightleftharpoons }}}\,{{N}_{2}}{{O}_{4}}\] |
| Rate \[=\frac{1}{2}\frac{d[N{{O}_{2}}]}{2dt}\] |
| \[={{k}_{1}}{{[N{{O}_{2}}]}^{2-}}-{{k}_{2}}[{{N}_{2}}{{O}_{4}}]\] |
| \[\therefore \] Rate of disappearance of |
| \[N{{O}_{2}}=-\frac{d[N{{O}_{2}}]}{dt}\] |
| \[=2{{k}_{1}}{{[N{{O}_{2}}]}^{2}}-2{{k}_{2}}[{{N}_{2}}{{O}_{4}}]\] |
You need to login to perform this action.
You will be redirected in
3 sec
