The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
The three experimental data for determine the differential rate of reaction $2 NO _{( g )}+ Cl _{2( g )} \rightarrow 2 NOCl_{( g )}$ at definate temperature. are given below.
$(a)$ Calculate order of reaction.
$(b)$ Calculate value of rate constant.
$(a)$ Rate $=-\frac{d\left[\mathrm{Cl}_{2}\right]}{d t}=k[\mathrm{NO}]^{\frac{1}{2}}\left[\mathrm{Cl}_{2}\right]^{1}$ Order of reaction $=\frac{1}{2}+1=\frac{3}{2}=1.5$
$(b)$ $k=0.175\left(\mathrm{~mol} \mathrm{~L}^{-1}\right)^{-\frac{1}{2}} \mathrm{~s}^{-1}$
Similar Questions
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 $/$ $mol$ $L^{-1}$ $min$ $^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | - | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | - |
| $IV$ | - | $0.2$ | $2.0 \times 10^{-2}$ |
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$
$2 NO +2 H _{2} \rightarrow N _{2}+2 H _{2} O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.
Reaction serial number
Initial pressure of $H _{2}$ / $kPa$
Initial Pressure of $NO /$ $kPa$
Initial rate $\left(\frac{- dp }{ dt }\right) /( kPa / s )$
$1$
$65.6$
$40.0$
$0.135$
$2$
$65.6$
$20.1$
$0.033$
$3$
$38.6$
$65.6$
$0.214$
$4$
$19.2$
$65.6$
$0.106$
The order of the reaction with respect to $NO$ is $...........$
$2 NO +2 H _{2} \rightarrow N _{2}+2 H _{2} O$
The above reaction has been studied at $800^{\circ} C$. The related data are given in the table below.
| Reaction serial number | Initial pressure of $H _{2}$ / $kPa$ | Initial Pressure of $NO /$ $kPa$ | Initial rate $\left(\frac{- dp }{ dt }\right) /( kPa / s )$ |
| $1$ | $65.6$ | $40.0$ | $0.135$ |
| $2$ | $65.6$ | $20.1$ | $0.033$ |
| $3$ | $38.6$ | $65.6$ | $0.214$ |
| $4$ | $19.2$ | $65.6$ | $0.106$ |
The order of the reaction with respect to $NO$ is $...........$
- [JEE MAIN 2022]
For the reaction $2HI$ $\rightleftharpoons$ ${H_2} + {I_2}$, the rate of the reaction is proportional to ${[HI]^2}$. This means that the reaction is
For the reaction $2HI$ $\rightleftharpoons$ ${H_2} + {I_2}$, the rate of the reaction is proportional to ${[HI]^2}$. This means that the reaction is
During Kinetic study of reaction $2 A+B \rightarrow C+D$, the following results were obtained :
$A[M]$
$B[M]$
initial rate of
formation of $D$
$i$
$0.1$
$0.1$
$6.0 \times 10^{-3}$
$ii$
$0.3$
$0.2$
$7.2 \times 10^{-2}$
$ii$
$0.3$
$0.4$
$2.88 \times 10^{-1}$
$iv$
$0.4$
$0.1$
$2.40 \times 10^{-2}$
Based on above data, overall order of the reaction is $\qquad$
During Kinetic study of reaction $2 A+B \rightarrow C+D$, the following results were obtained :
| $A[M]$ | $B[M]$ |
initial rate of formation of $D$ |
|
| $i$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $ii$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $ii$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $iv$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Based on above data, overall order of the reaction is $\qquad$
- [JEE MAIN 2024]