The unit of rate constant for a zero order reaction is

How can you determine the rate law of the following reaction ?

$2NO\,(g) + O_2\,(g)\to 2NO_{2} \,(g)$

For the following reaction scheme (homogeneous), the rate constant has units

$A+B\xrightarrow{K}C$:

For a certain reaction : $(A)(g)  \to  B(g)$ Half life for different initial pressures of $A$  is given below

 $\begin{array}{|l|l|l|} \hline {P_{{A_0}}}(atm) & 0.1 & 0.025 \\ \hline {t_{1/2}}(\sec\,\,) & 100 & 50 \\ \hline \end{array}$

The correct statement about order of reaction is

Write about elementary and complex reactions.

The given data are for the reaction :

$2NO(g) + Cl_2(g) \to 2NOCl(g)$ at $298\, K$

$[Cl_2]$                $[NO]$                       Rate $(mol\, L^{-1} \sec^{-1})$

$I$    $0.05\, M$       $0.05\,M$                           $1 \times 10^{-3}$

$II$   $0.15\, M$      $0.05\,M$                           $3 \times 10^{-3}$

$III$  $0.05\, M$      $0.15\,M$                           $9 \times 10^{-3}$

The rate law for the reaction is