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]
- A
$I$ $\rightarrow P ;$ II $\rightarrow Q ; III \rightarrow S ; IV \rightarrow T$
- B
$I$ $\rightarrow R; II \rightarrow S; III \rightarrow S; IV \rightarrow T$
- C
$I$ $\rightarrow P; II \rightarrow Q; III \rightarrow Q ; IV \rightarrow R$
- D
$I$ $\rightarrow R ; II \rightarrow S ; III \rightarrow Q ; IV \rightarrow R$
Similar Questions
The alkaline hydrolysis of ethyl acetate is represented by the equation$C{H_3}COO{C_2}{H_5} + NaOH \to C{H_3}COONa + {C_2}{H_5}OH$ Experimentally it is found that for this reaction$\frac{{dx}}{{dt}} = k[C{H_3}COO{C_2}{H_5}]\,[NaOH]$ Then the reaction is
The alkaline hydrolysis of ethyl acetate is represented by the equation$C{H_3}COO{C_2}{H_5} + NaOH \to C{H_3}COONa + {C_2}{H_5}OH$ Experimentally it is found that for this reaction$\frac{{dx}}{{dt}} = k[C{H_3}COO{C_2}{H_5}]\,[NaOH]$ Then the reaction is
For the elementary reaction $M \rightarrow N$, the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :
For the elementary reaction $M \rightarrow N$, the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :
- [IIT 2014]
For the non - stoichimetre 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
$(A)$
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 :
For the non - stoichimetre 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 $(A)$ |
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 :
- [JEE MAIN 2014]
For $n^{th}$ order reaction where $(n < 1)$
For $n^{th}$ order reaction where $(n < 1)$
Which of the following is correct ?
Which of the following is correct ?