For a reaction $A+ B\to $  Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.

In the reaction $A + B \to $ Products, if $B$ is taken in excess, then it is an example of

The possible mechanism for the reaction

$2NO + Br \to 2NOBr$ is

$NO + Br_2 \rightleftharpoons NOBr_2$ (Fast)

$NOBr_2 + NO \to 2NOBr$ (Slow)

The rate law expression is

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  ........... $L\,\,mo{l^{ - 1}}\,{s^{ - 1}}$

For reaction a $A \to x\;P$, when $[A] = 2.2\,m\,M$, the rate was found to be $2.4\;m\,M\;{s^{ - 1}}$. On reducing concentration of $A$ to half, the rate changes to $0.6\;m\,M\;{s^{ - 1}}$. The order of reaction with respect to $A$ is

For a given reaction ${t_{1/2}} = \frac{1}{{Ka}}.$. The order of the reaction is