Which of the following statements regarding the molecularity of a reaction is wrong
Which of the following statements regarding the molecularity of a reaction is wrong
- A
It is the number of molecules of the reactants taking part in a single step chemical reaction
- B
It is calculated from the reaction mechanism
- C
It may be either a whole number or fractional
- D
It depends on the rate determining step in the reaction
Similar Questions
The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below
${O_3}(g)\, + \,C{l^ * }(g)\, \to \,{O_2}(g) + Cl{O^ * }(g)$ ..... $(i)$ $[{K_i} = 5.2 \times {10^9}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$
$Cl{O^ * }(g) + {O^ * }(g)\, \to \,{O_2}(g) + \,C{l^ * }(g)$ ..... $(ii)$ $[{K_{ii}} = 2.6 \times {10^{10}}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$
The closest rate constant for the overall reaction
${O_3}(g){\mkern 1mu} + {\mkern 1mu} {O^*}(g){\mkern 1mu} \to {\mkern 1mu} 2{O_2}(g)$ is ........... $L\,\,mo{l^{ - 1}}\,{s^{ - 1}}$
The reaction of ozone with oxygen atoms in the presence of chlorine atoms can occur by a two step process shown below
${O_3}(g)\, + \,C{l^ * }(g)\, \to \,{O_2}(g) + Cl{O^ * }(g)$ ..... $(i)$ $[{K_i} = 5.2 \times {10^9}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$
$Cl{O^ * }(g) + {O^ * }(g)\, \to \,{O_2}(g) + \,C{l^ * }(g)$ ..... $(ii)$ $[{K_{ii}} = 2.6 \times {10^{10}}\,\,L\,mo{l^{ - 1}}\,{s^{ - 1}}]$
The closest rate constant for the overall reaction
${O_3}(g){\mkern 1mu} + {\mkern 1mu} {O^*}(g){\mkern 1mu} \to {\mkern 1mu} 2{O_2}(g)$ is ........... $L\,\,mo{l^{ - 1}}\,{s^{ - 1}}$
- [JEE MAIN 2016]
An example of a pseudo -unimolecular reaction is
An example of a pseudo -unimolecular reaction is
The rate constant for a second order reaction is $8 \times {10^{ - 5}}\,{M^{ - 1}}\,mi{n^{ - 1}}$. How long will it take a $ 1\,M $ solution to be reduced to $0.5\, M$
The rate constant for a second order reaction is $8 \times {10^{ - 5}}\,{M^{ - 1}}\,mi{n^{ - 1}}$. How long will it take a $ 1\,M $ solution to be reduced to $0.5\, M$
The half life for second order reaction is $30\, minutes$. If the initial concentration is $0.1\, M$ then the value of rate constant will be ............ $M^{-1}\, min^{-1}$
The half life for second order reaction is $30\, minutes$. If the initial concentration is $0.1\, M$ then the value of rate constant will be ............ $M^{-1}\, min^{-1}$
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 $=k\left[ C _{2} H _{5} Cl \right]$