Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$

Which statement about the above equation is wrong?

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

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

$(i)$ $3 NO ( g ) \rightarrow N _{2} O$ $(g)$ Rate $=k[ NO ]^{2}$

For a given reaction $t_{1/2} = \frac{1}{k.a}$ the order of reaction will be

For the reaction $2NO_2 + F_2 \to  2NO_2F$, following mechanism has been provided :
$N{O_2} + {F_2}\xrightarrow{{slow}}N{O_2}F + F$
$N{O_2} + {F_2}\xrightarrow{{fast}}N{O_2}F$
Thus rate expression of the above reaction can be written as

Which one of the following statements for the order of a reaction is incorrect?