Why can’t molecularity of any reaction be equal to zero ?
Why can’t molecularity of any reaction be equal to zero ?
Molecularity is the number of molecules taking part in an elementary step. For this we require at least a single molecule leading to the value of minimum molecularity of one.
Similar Questions
The reaction $2 NO + Br _2 \rightarrow 2 NOBr$
takes places through the mechanism given below :
$NO + Br _2 \Leftrightarrow NOBr _2 \text { (fast) }$
$NOBr _2+ NO \rightarrow 2 NOBr \text { (slow) }$
The overall order of the reaction is $.....$.
The reaction $2 NO + Br _2 \rightarrow 2 NOBr$
takes places through the mechanism given below :
$NO + Br _2 \Leftrightarrow NOBr _2 \text { (fast) }$
$NOBr _2+ NO \rightarrow 2 NOBr \text { (slow) }$
The overall order of the reaction is $.....$.
- [JEE MAIN 2023]
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
$(i)$ doubled
$(ii)$ reduced to half $?$
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
$(i)$ doubled
$(ii)$ reduced to half $?$
The order of the reaction occurring by following mechanism should be
$(i)$ ${A_2} \to A + A$ (fast)
$(ii)$ $A + {B_2} \to AB + B$ (slow)
$(iii)$ $A + B \to $ (fast)
The order of the reaction occurring by following mechanism should be
$(i)$ ${A_2} \to A + A$ (fast)
$(ii)$ $A + {B_2} \to AB + B$ (slow)
$(iii)$ $A + B \to $ (fast)
For the following reaction scheme (homogeneous), the rate constant has units
$A+B\xrightarrow{K}C$:
For the following reaction scheme (homogeneous), the rate constant has units
$A+B\xrightarrow{K}C$:
Reaction $2A + B \to$ product, rate law is $\frac{{ - d[A]}}{{dt}}\, = \,K[A].$ At a time when $t\, = \,\frac{{{t_{1/2}}}}{{\ln\,2}},$ concentration of the reactant is
Reaction $2A + B \to$ product, rate law is $\frac{{ - d[A]}}{{dt}}\, = \,K[A].$ At a time when $t\, = \,\frac{{{t_{1/2}}}}{{\ln\,2}},$ concentration of the reactant is