Which of the following is correct ?
Which of the following is correct ?
- A
molecularity of a reaction can be fractional
- B
Zero order reaction never stops
- C
A first order reaction must be homogeneous
- D
The rate constant of a reaction becomes equal to the pre-exponential factor when the absolute temperature is infinity.
Similar Questions
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
Which of the following is the fastest reaction
Which of the following is the fastest reaction
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor
The experimental data for the reaction $2A + {B_2} \to 2AB$ isThe rate equation for the above data is
Exp.
$[A]_0$
$[B]_0$
Rate (mole $s^{-1}$)
$(1)$
$0.50$
$0.50$
$1.6 \times {10^{ - 4}}$
$(2)$
$0.50$
$1.00$
$3.2 \times {10^{ - 4}}$
$(3)$
$1.00$
$1.00$
$3.2 \times {10^4}$
The experimental data for the reaction $2A + {B_2} \to 2AB$ isThe rate equation for the above data is
|
Exp. |
$[A]_0$ |
$[B]_0$ |
Rate (mole $s^{-1}$) |
|
$(1)$ |
$0.50$ |
$0.50$ |
$1.6 \times {10^{ - 4}}$ |
|
$(2)$ |
$0.50$ |
$1.00$ |
$3.2 \times {10^{ - 4}}$ |
|
$(3)$ |
$1.00$ |
$1.00$ |
$3.2 \times {10^4}$ |
- [AIPMT 1997]
Following is the rate constant of reaction what is the overall order of reaction ?
$(a)$ $2.418 \times 10^{-5}\,hr ^{-1}$
$(b)$ $7.1 \times 10^{-4} \,atm \,s ^{-1}$
Following is the rate constant of reaction what is the overall order of reaction ?
$(a)$ $2.418 \times 10^{-5}\,hr ^{-1}$
$(b)$ $7.1 \times 10^{-4} \,atm \,s ^{-1}$