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 -

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

For a reaction $\mathrm{A} \xrightarrow{\mathrm{K}_4} \mathrm{~B} \xrightarrow{\mathrm{K}_2} \mathrm{C}$

If the rate of formation of $B$ is set to be zero then the concentration of $B$ is given by :

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

Inversion of sucrose is

For the reaction $2NO_2 + F_2 \to 2NO_2F$ , following mechanism has been provided

$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$

$N{O_2} + F\xrightarrow{{fast}}N{O_2}F$

Thus rate expression of the above reaction can be written as