Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
Consider the reaction, $2A + B \rightarrow$ products. When concentration of $B$ alone was doubled, the half-life did not change. When the concentration of $A$ alone was doubled, the rate increased by two times. The unit of rate constant for this reaction is
- [AIEEE 2007]
- A
$s^{-1}$
- B
$L\, mol^{-1} \,s^{-1}$
- C
no unit
- D
$mol\, L^{-1}\, s^{-1}$
Similar Questions
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Differential form of the rate equation is
$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$
Which statement about the above equation is wrong?
Determine the order of reaction on the basis of following data for the reaction $A + B \to C$
Exp.
$[A]$
$[B]$
Rate of reaction
$1$
$0.1$
$0.1$
$2 \times {10^{ - 3}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$
$2$
$0.4$
$0.1$
$0.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$
$3$
$0.1$
$0.2$
$1.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$
Determine the order of reaction on the basis of following data for the reaction $A + B \to C$
| Exp. | $[A]$ | $[B]$ | Rate of reaction |
| $1$ | $0.1$ | $0.1$ | $2 \times {10^{ - 3}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$ |
| $2$ | $0.4$ | $0.1$ | $0.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$ |
| $3$ | $0.1$ | $0.2$ | $1.4 \times {10^{ - 2}}\,mol\,{L^{ - 1}}\,{\sec ^{ - 1}}$ |
The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step$-1$ : ${\text{A + E }} \rightleftharpoons AE$ (fast)
Step$-2$ :${\text{AE + A }} \to {A_2} + E$ (slow)
Step$-3$ :${{\text{A}}_2}{\text{ + B }} \to {\text{D}}$ (fast)
what rate law best agrees with this mechanism
The hypothetical reaction : $2A + B \to C + D$ is catalyzed by $E$ as indicated in the possible mechanism below -
Step$-1$ : ${\text{A + E }} \rightleftharpoons AE$ (fast)
Step$-2$ :${\text{AE + A }} \to {A_2} + E$ (slow)
Step$-3$ :${{\text{A}}_2}{\text{ + B }} \to {\text{D}}$ (fast)
what rate law best agrees with this mechanism
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.
Which one of the following statements for the order of a reaction is incorrect?
Which one of the following statements for the order of a reaction is incorrect?
- [AIPMT 2011]