For reaction a $A \to x\;P$, when $[A] = 2.2\,m\,M$, the rate was found to be $2.4\;m\,M\;{s^{ - 1}}$. On reducing concentration of $A$ to half, the rate changes to $0.6\;m\,M\;{s^{ - 1}}$. The order of reaction with respect to $A$ is
For reaction a $A \to x\;P$, when $[A] = 2.2\,m\,M$, the rate was found to be $2.4\;m\,M\;{s^{ - 1}}$. On reducing concentration of $A$ to half, the rate changes to $0.6\;m\,M\;{s^{ - 1}}$. The order of reaction with respect to $A$ is
- [AIIMS 2005]
- A
$1.5$
- B
$2$
- C
$2.5$
- D
$3$
Similar Questions
Catalyst decomposition of hydrogen peroxide is a ........ order reaction
Catalyst decomposition of hydrogen peroxide is a ........ order reaction
The three experimental data for determine the differential rate of reaction $Cl _{2( g )} + 2NO _{( g )} \rightarrow 2 NOCl_{( g )}$ at $310\, K$ temperature.
$(a)$ Derive differential rate of reaction.
$(b)$ Calculate order of reaction.
$(c)$ Calculate value of rate constant.
The three experimental data for determine the differential rate of reaction $Cl _{2( g )} + 2NO _{( g )} \rightarrow 2 NOCl_{( g )}$ at $310\, K$ temperature.
$(a)$ Derive differential rate of reaction.
$(b)$ Calculate order of reaction.
$(c)$ Calculate value of rate constant.
The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$ :
$NO(g) + Br_2 (g) \rightleftharpoons NOBr_2 (g)$
$NOBr_2(g)+ NO(g) \longrightarrow 2NOBr(g)$
If the second step is the rate determining step, the order of the reaction with respect to $NO(g)$ is
The following mechanism has been proposed for the reaction of $NO$ with $Br_2$ to form $NOBr$ :
$NO(g) + Br_2 (g) \rightleftharpoons NOBr_2 (g)$
$NOBr_2(g)+ NO(g) \longrightarrow 2NOBr(g)$
If the second step is the rate determining step, the order of the reaction with respect to $NO(g)$ is
- [AIEEE 2006]
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
Experiment
$[ A ] / mol\, ^{-1}$
$[ B ] / mol\, ^{-1}$
Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$
$I$
$0.1$
$0.1$
$2.0 \times 10^{-2}$
$II$
-
$0.2$
$4.0 \times 10^{-2}$
$III$
$0.4$
$0.4$
-
$IV$
-
$0.2$
$2.0 \times 10^{-2}$
The reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
| Experiment | $[ A ] / mol\, ^{-1}$ | $[ B ] / mol\, ^{-1}$ | Initial rate $/$ $mol$ $L^{-1}$ $min$ $^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | - | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | - |
| $IV$ | - | $0.2$ | $2.0 \times 10^{-2}$ |