For the reaction $2NO_2 + F_2 \to 2NO_2F$ , following mechanism has been provided
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + F\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as
For the reaction $2NO_2 + F_2 \to 2NO_2F$ , following mechanism has been provided
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + F\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as
- A
$r = K [NO_2]^2[F_2]$
- B
$r = K [NO_2]$
- C
$r = K [NO_2][F_2]$
- D
$r = K [F_2]$
Similar Questions
The incorrect order indicated against the rate of reaction is Rate Order
$A+B\xrightarrow{K}C$
Rate Order
The incorrect order indicated against the rate of reaction is Rate Order
$A+B\xrightarrow{K}C$
Rate Order
Select the incorrect option :
Select the incorrect option :
For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is
For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is
- [AIEEE 2002]
The rate constant for a second order reaction is $8 \times {10^{ - 5}}\,{M^{ - 1}}\,mi{n^{ - 1}}$. How long will it take a $ 1\,M $ solution to be reduced to $0.5\, M$
The rate constant for a second order reaction is $8 \times {10^{ - 5}}\,{M^{ - 1}}\,mi{n^{ - 1}}$. How long will it take a $ 1\,M $ solution to be reduced to $0.5\, M$
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]