The mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is
$(i)\,\,N{O_2}\,\xrightarrow{{slow}}\,NO + O$
$(ii)\,\,{F_2} + O + NO\,\xrightarrow{{fast}}\,N{O_2}F + F$
$(iii)\,\,F + N{O_2}\,\xrightarrow{{fast}}\,N{O_2}F$
Select the correct one
The mechanism of the reaction $2NO_2 + F_2 \to 2NO_2F$ is
$(i)\,\,N{O_2}\,\xrightarrow{{slow}}\,NO + O$
$(ii)\,\,{F_2} + O + NO\,\xrightarrow{{fast}}\,N{O_2}F + F$
$(iii)\,\,F + N{O_2}\,\xrightarrow{{fast}}\,N{O_2}F$
Select the correct one
- A
the reaction is of $3^{rd}$ order
- B
the molecularity of the reaction is sum of molecularities of all steps
- C
reaction is zero order w.r.t. $F_2$
- D
half life of reaction depends upon initial conc. of $NO_2$
Similar Questions
Match the rate expressions in $LIST-I$ for the decomposition of $X$ with the corresponding profiles provided in $LIST-II$. $X _5$ and $k$ constants having appropriate units.
Match the rate expressions in $LIST-I$ for the decomposition of $X$ with the corresponding profiles provided in $LIST-II$. $X _5$ and $k$ constants having appropriate units.
- [IIT 2022]
What is molecularity of a relation ? Explain its types by examples.
What is molecularity of a relation ? Explain its types by examples.
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
Experiment No.
$\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$
Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$
$1$
$0.2$
$0.1$
$0.1$
$6.0 \times 10^{-5}$
$2$
$0.2$
$0.2$
$0.1$
$6.0 \times 10^{-5}$
$3$
$0.2$
$0.1$
$0.2$
$1.2 \times 10^{-4}$
$4$
$0.3$
$0.1$
$0.1$
$9.0 \times 10^{-5}$
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
| Experiment No. | $\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$ | Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$ |
| $1$ | $0.2$ | $0.1$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $2$ | $0.2$ | $0.2$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $3$ | $0.2$ | $0.1$ | $0.2$ | $1.2 \times 10^{-4}$ |
| $4$ | $0.3$ | $0.1$ | $0.1$ | $9.0 \times 10^{-5}$ |
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
- [IIT 2019]
In hydrogenation reaction at ${27\,^o}C$, it is observed that hydrogen gas pressure falls from $2\,atm$ to $1.2\,atm$ in $50\,\min$. Calculate the rate of disappearance of hydrogen
In hydrogenation reaction at ${27\,^o}C$, it is observed that hydrogen gas pressure falls from $2\,atm$ to $1.2\,atm$ in $50\,\min$. Calculate the rate of disappearance of hydrogen
If the rate of the reaction is equal to the rate constant, the order of the reaction is
If the rate of the reaction is equal to the rate constant, the order of the reaction is
- [AIPMT 2003]