For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?
For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?
- A
$(i)$ can't be defined, $(ii)\,\, 1$
- B
$(i)\,\, 2, (ii)\,\, 2$
- C
$(i)\,\, 1, (ii)\,\, 1$
- D
$(i)\,\, 1, (ii)\,\, 2$
Similar Questions
The rate of the reaction $CC{l_3}CHO + NO \to CHC{l_3} + NO + CO$ is given by Rate $ = K\,[CC{l_3}CHO]\,[NO]$. If concentration is expressed in moles/litre, the units of K are
The rate of the reaction $CC{l_3}CHO + NO \to CHC{l_3} + NO + CO$ is given by Rate $ = K\,[CC{l_3}CHO]\,[NO]$. If concentration is expressed in moles/litre, the units of K are
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
Experiment No.
$\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$
$\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$
Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$
$1$
$0.2$
$0.1$
$0.1$
$6.0 \times 10^{-5}$
$2$
$0.2$
$0.2$
$0.1$
$6.0 \times 10^{-5}$
$3$
$0.2$
$0.1$
$0.2$
$1.2 \times 10^{-4}$
$4$
$0.3$
$0.1$
$0.1$
$9.0 \times 10^{-5}$
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
Consider the kinetic data given in the following table for the reaction $A + B + C \rightarrow$ Product.
| Experiment No. | $\begin{array}{c}{[ A ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ B ]} \\ \left( mol dm ^{-3}\right)\end{array}$ | $\begin{array}{c}{[ C]} \\ \left( mol dm ^{-3}\right)\end{array}$ | Rate of reaction $\left( mol dm ^{-3} s ^{-1}\right)$ |
| $1$ | $0.2$ | $0.1$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $2$ | $0.2$ | $0.2$ | $0.1$ | $6.0 \times 10^{-5}$ |
| $3$ | $0.2$ | $0.1$ | $0.2$ | $1.2 \times 10^{-4}$ |
| $4$ | $0.3$ | $0.1$ | $0.1$ | $9.0 \times 10^{-5}$ |
The rate of the reaction for $[ A ]=0.15 mol dm ^{-3},[ B ]=0.25 mol dm ^{-3}$ and $[ C ]=0.15 mol dm ^{-3}$ is found to be $Y \times 10^{-5} mol dm d ^{-3} s ^{-1}$. The value of $Y$ i. . . . . . .
- [IIT 2019]
Why molecularity is applicable only for elementary reactions and order is applicable for elementary as well as complex reactions ?
Why molecularity is applicable only for elementary reactions and order is applicable for elementary as well as complex reactions ?
Time required for completion of ionic reactions in comparison to molecular reactions is
Time required for completion of ionic reactions in comparison to molecular reactions is
The following results were obtained during kinetic studies of the reaction $2A+B$ $\to$ products
Experiment
$[A]$
(in $mol\, L^{-1})$
$[B]$
(in $mol\, L^{-1})$
Initial rate of reaction
(in $mol\, L^{-1}\,min^{-1})$
$I$
$0.10$
$0.20$
$6.93 \times {10^{ - 3}}$
$II$
$0.10$
$0.25$
$6.93 \times {10^{ - 3}}$
$III$
$0.20$
$0.30$
$1.386 \times {10^{ - 2}}$
The time(in minutes) required to consume half of $A$ is
The following results were obtained during kinetic studies of the reaction $2A+B$ $\to$ products
| Experiment |
$[A]$ (in $mol\, L^{-1})$ |
$[B]$ (in $mol\, L^{-1})$ |
Initial rate of reaction (in $mol\, L^{-1}\,min^{-1})$ |
| $I$ | $0.10$ | $0.20$ | $6.93 \times {10^{ - 3}}$ |
| $II$ | $0.10$ | $0.25$ | $6.93 \times {10^{ - 3}}$ |
| $III$ | $0.20$ | $0.30$ | $1.386 \times {10^{ - 2}}$ |
The time(in minutes) required to consume half of $A$ is
- [JEE MAIN 2019]