An elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?

The reaction of formation of phosgene from $CO$ and $Cl_2$ is $CO + Cl_2 \to COCl_2.$ The proposed mechanism is

$(i)$  $C{l_2}\,\underset{{{k_2}}}{\overset{{{k_1}}}{\longleftrightarrow}}\,2Cl$

$(ii)$  $Cl + CO\,\underset{{{k_4}}}{\overset{{{k_3}}}{\longleftrightarrow}}\,COCl$

$(iii)$  $COCl\, + \,C{l_2}\,\,\xrightarrow{{{k_5}}}\,COC{l_2}\, + \,Cl$ (slow)

Find the correct expression of rate law

From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$

What is the order of reaction $r\, = \,k{[A]^{\frac{3}{2}}}\,{[B]^2}$ ?

The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :

 $\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$

The order of reaction is -

For the following parallel chain reaction. What will be that value of overall half-life of $A$ in minutes ?

Given that  $\left[ {\frac{{{{\left[ B \right]}_t}}}{{{{[C]}_t}}} = \frac{{16}}{9}} \right]$

$A\,\xrightarrow{{{K_1}\, = \,2\, \times \,{{10}^{^{ - 3}\,}}{S^{ - 1}}}}4B$

$A\to C$