During the kinetic study of the reaction, $2A + B \rightarrow C + D,$ following results were obtained
Run
$[A]/mol\,L^{-1}$
$[B]/mol\,L^{-1}$
Initial rate of formation of $D/mol\,L^{-1}\,min^{-1}$
$I.$
$0.1$
$0.1$
$6.0 \times 10^{-3}$
$II.$
$0.3$
$0.2$
$7.2 \times 10^{-2}$
$III.$
$0.3$
$0.4$
$2.88 \times 10^{-1}$
$IV.$
$0.4$
$0.1$
$2.40 \times 10^{-2}$
Based on the above data which one of the following is correct?
During the kinetic study of the reaction, $2A + B \rightarrow C + D,$ following results were obtained
| Run | $[A]/mol\,L^{-1}$ | $[B]/mol\,L^{-1}$ | Initial rate of formation of $D/mol\,L^{-1}\,min^{-1}$ |
| $I.$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II.$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III.$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV.$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Based on the above data which one of the following is correct?
- [AIPMT 2010]
- A
Rate $= k[A]^2[B]$
- B
Rate $= k[A][B]$
- C
Rate $= k[A]^2[B]^2$
- D
Rate $= k[A][B]^2$
Similar Questions
The possible mechanism for the reaction
$2NO + Br \to 2NOBr$ is
$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)
$NOBr_2 + NO \to 2NOBr$ (Slow)
The rate law expression is
The possible mechanism for the reaction
$2NO + Br \to 2NOBr$ is
$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)
$NOBr_2 + NO \to 2NOBr$ (Slow)
The rate law expression is
The data for the reaction $A + B \to C$ is
Exp
$[A]_0$
$[B]_0$
initial rate
$1$
$0.012$
$0.035$
$0.10$
$2$
$0.024$
$0.035$
$0.80$
$3$
$0.012$
$0.070$
$0.10$
$4$
$0.024$
$0.070$
$0.80$
The data for the reaction $A + B \to C$ is
| Exp | $[A]_0$ | $[B]_0$ | initial rate |
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.035$ | $0.80$ |
| $3$ | $0.012$ | $0.070$ | $0.10$ |
| $4$ | $0.024$ | $0.070$ | $0.80$ |
The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
$2 NO +2 H _{2} \rightarrow N _{2}+2 H _{2} O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.
Reaction serial number
Initial pressure of $H _{2}$ / $kPa$
Initial Pressure of $NO /$ $kPa$
Initial rate $\left(\frac{- dp }{ dt }\right) /( kPa / s )$
$1$
$65.6$
$40.0$
$0.135$
$2$
$65.6$
$20.1$
$0.033$
$3$
$38.6$
$65.6$
$0.214$
$4$
$19.2$
$65.6$
$0.106$
The order of the reaction with respect to $NO$ is $...........$
$2 NO +2 H _{2} \rightarrow N _{2}+2 H _{2} O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.
| Reaction serial number | Initial pressure of $H _{2}$ / $kPa$ | Initial Pressure of $NO /$ $kPa$ | Initial rate $\left(\frac{- dp }{ dt }\right) /( kPa / s )$ |
| $1$ | $65.6$ | $40.0$ | $0.135$ |
| $2$ | $65.6$ | $20.1$ | $0.033$ |
| $3$ | $38.6$ | $65.6$ | $0.214$ |
| $4$ | $19.2$ | $65.6$ | $0.106$ |
The order of the reaction with respect to $NO$ is $...........$
- [JEE MAIN 2022]
If $50\%$ of a reaction occurs in $100$ seconds and $75\%$ of the reaction occurs in $200$ seconds, the order of this reaction is
If $50\%$ of a reaction occurs in $100$ seconds and $75\%$ of the reaction occurs in $200$ seconds, the order of this reaction is
- [JEE MAIN 2018]