Medium
$2 \ NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2 \ NOCl_{(g)}$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
$Run$ $[NO]_{0}$ $[Cl_{2}]_{0}$ $r_{0}$ $1$ $0.10$ $0.10$ $0.18$ $2$ $0.10$ $0.20$ $0.35$ $3$ $0.20$ $0.20$ $1.40$
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
This reaction was studied at $-10^{\circ} C$ and the following data was obtained:
| $Run$ | $[NO]_{0}$ | $[Cl_{2}]_{0}$ | $r_{0}$ |
| $1$ | $0.10$ | $0.10$ | $0.18$ |
| $2$ | $0.10$ | $0.20$ | $0.35$ |
| $3$ | $0.20$ | $0.20$ | $1.40$ |
$[NO]_{0}$ and $[Cl_{2}]_{0}$ are the initial concentrations and $r_{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
- A$1$
- B$2$
- C$3$
- D$4$
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Difficult
View SolutionFor the reaction:
$2NO_{2(g)} + O_{3(g)} \to N_2O_{5(g)} + O_{2(g)}$
The rate law is $R = K[NO_2]^1 [O_3]^1$.
Which of these possible reaction mechanisms is consistent with the rate law?
Mechanism $I$:
$NO_{2(g)} + O_{3(g)} \to NO_{3(g)} + O_{2(g)}$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_{5(g)}$ (fast)
Mechanism $II$:
$O_{3(g)} \rightleftharpoons O_{2(g)} + [O]$ (fast)
$NO_{2(g)} + [O] \to NO_3$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_5$ (fast)
$2NO_{2(g)} + O_{3(g)} \to N_2O_{5(g)} + O_{2(g)}$
The rate law is $R = K[NO_2]^1 [O_3]^1$.
Which of these possible reaction mechanisms is consistent with the rate law?
Mechanism $I$:
$NO_{2(g)} + O_{3(g)} \to NO_{3(g)} + O_{2(g)}$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_{5(g)}$ (fast)
Mechanism $II$:
$O_{3(g)} \rightleftharpoons O_{2(g)} + [O]$ (fast)
$NO_{2(g)} + [O] \to NO_3$ (slow)
$NO_{3(g)} + NO_{2(g)} \to N_2O_5$ (fast)
Difficult
View SolutionFor the non-stoichiometric reaction $2A + B \rightarrow C + D,$ the following kinetic data were obtained in three separate experiments,all at $298 \, K.$
Initial Concentration $(A)$ Initial Concentration $(B)$ Initial rate of formation of $C$ $(mol \, L^{-1} \, s^{-1})$ $0.1 \, M$ $0.1 \, M$ $1.2 \times 10^{-3}$ $0.1 \, M$ $0.2 \, M$ $1.2 \times 10^{-3}$ $0.2 \, M$ $0.1 \, M$ $2.4 \times 10^{-3}$
The rate law for the formation of $C$ is:
| Initial Concentration $(A)$ | Initial Concentration $(B)$ | Initial rate of formation of $C$ $(mol \, L^{-1} \, s^{-1})$ |
| $0.1 \, M$ | $0.1 \, M$ | $1.2 \times 10^{-3}$ |
| $0.1 \, M$ | $0.2 \, M$ | $1.2 \times 10^{-3}$ |
| $0.2 \, M$ | $0.1 \, M$ | $2.4 \times 10^{-3}$ |
The rate law for the formation of $C$ is:
DifficultJEE MAIN 2014
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