For the reaction $A \to B$, the rate increases by a factor of $2.25 $ when the concentration of $A$ is increased by $ 1.5$. What is the order of the reaction
For the reaction $A \to B$, the rate increases by a factor of $2.25 $ when the concentration of $A$ is increased by $ 1.5$. What is the order of the reaction
- A
$3$
- B
$0$
- C
$2$
- D
$1$
Similar Questions
$A_2 + 2\,B \to 2\,AB$
$[A_2]$
$[B]$
${-d\,[A_2]/dt}$
$0.1$
$0.2$
$1 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$
$0.2$
$2 \times {10^{ - 2}}\,M{s^{ - 1}}$
$0.2$
$0.4$
$8 \times {10^{ - 2}}\,M{s^{ - 1}}$
Order of reaction w.r.t. $A_2$ and $B$ are respectively
$A_2 + 2\,B \to 2\,AB$
| $[A_2]$ | $[B]$ | ${-d\,[A_2]/dt}$ |
| $0.1$ | $0.2$ | $1 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
| $0.2$ | $0.2$ | $2 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
| $0.2$ | $0.4$ | $8 \times {10^{ - 2}}\,M{s^{ - 1}}$ |
Order of reaction w.r.t. $A_2$ and $B$ are respectively
The mechanism of the reaction $A + 2B \to D$ is
$2B\xrightarrow{k}{B_2}$ [Slow]
${B_2} + A \to D$ [Fast]
The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively
The mechanism of the reaction $A + 2B \to D$ is
$2B\xrightarrow{k}{B_2}$ [Slow]
${B_2} + A \to D$ [Fast]
The rate law expression, order with respect to $A$, order with respect to $'B'$ and overall order are respectively
Order of a reaction is decided by
Order of a reaction is decided by
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
Experiment
$[ A ] / molL ^{-1}$
$[ B ] / molL ^{-1}$
Initial $rate/molL$ $^{-1}$ $\min ^{-1}$
$I$
$0.1$
$0.1$
$6.00 \times 10^{-3}$
$II$
$0.1$
$0.2$
$2.40 \times 10^{-2}$
$III$
$0.2$
$0.1$
$1.20 \times 10^{-2}$
$IV$
$X$
$0.2$
$7.20 \times 10^{-2}$
$V$
$0.3$
$Y$
$2.88 \times 10^{-1}$
$X$ and $Y$ in the given table are respectively :
The results given in the below table were obtained during kinetic studies of the following reaction:
$2 A + B \longrightarrow C + D$
| Experiment | $[ A ] / molL ^{-1}$ | $[ B ] / molL ^{-1}$ | Initial $rate/molL$ $^{-1}$ $\min ^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.00 \times 10^{-3}$ |
| $II$ | $0.1$ | $0.2$ | $2.40 \times 10^{-2}$ |
| $III$ | $0.2$ | $0.1$ | $1.20 \times 10^{-2}$ |
| $IV$ | $X$ | $0.2$ | $7.20 \times 10^{-2}$ |
| $V$ | $0.3$ | $Y$ | $2.88 \times 10^{-1}$ |
$X$ and $Y$ in the given table are respectively :
- [JEE MAIN 2020]