The mechanism of the reaction,

$2NO(g) + 2{H_2}(g) \to {N_2}(g) + 2{H_2}O(g)$ is :

Step $1$ : $2NO(g) + {H_2}(g)\xrightarrow{{slow}}{N_2} + {H_2}{O_2}$

Step : $2$ ${H_2}{O_2} + {H_2}\xrightarrow{{fast}}2{H_2}O$

Then the correct statement is

If the rate expression for a chemical reaction is given by Rate $ = k{[A]^m}{[B]^n}$

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

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

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

$A\to C$

For the reaction $A + 2B \to C,$ rate is given by $R$ $ = [A]{[B]^2}$ then the order of the reaction is

Which of the following rate laws has an overall order of $0.5$  for reaction involving substances $x$, $y$ and $z$

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