The one which is unimolecular reaction is
The one which is unimolecular reaction is
- A
$2HI \to {H_2} + {I_2}$
- B
${N_2}{O_5} \to {N_2}{O_4} + \frac{1}{2}{O_2}$
- C
${H_2} + C{l_2} \to 2HCl$
- D
$PC{l_3} + C{l_2} \to PC{l_5}$
Similar Questions
For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways
$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ; $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$
So the correct relation between $K$ and $K_1$ is
For a reaction, $AB_5 \to AB + 4B$ The rate can be expressed in following ways
$\frac{{ - d[A{B_5}]}}{{dt}} = K[A{B_5}]$ ; $\frac{{d[B]}}{{dt}} = {K_1}[A{B_5}]$
So the correct relation between $K$ and $K_1$ is
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]
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]
In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at
In a reaction $2A + B \to {A_2}B$, the reactant $ A $ will disappear at
Rate constant for a reaction ${H_2} + {I_2} \to 2HI$ is $49$, then rate constant for reaction $2HI \to {H_2} + {I_2}$ is
Rate constant for a reaction ${H_2} + {I_2} \to 2HI$ is $49$, then rate constant for reaction $2HI \to {H_2} + {I_2}$ is