The half-lives of two samples are $0.1 \ s$ and $0.4 \ s$. Their respective concentrations are $200$ and $50$. What is the order of the reaction?

Which of the following statements is $NOT$ true for a reaction having rate law $r=k[H_2][I_2]$?

For the reaction $aA + bB \to$ product,the rate of reaction is given by $Rate = k[A]^3 [B]^0$. If the concentration of $A$ is doubled and the concentration of $B$ is halved,the rate of reaction will be: (in $\times$)

Write about elementary and complex reactions.

The given data are for the reaction:
$2NO_{(g)} + Cl_{2(g)} \to 2NOCl_{(g)}$ at $298 \ K$

Experiment	$[Cl_2] \ (M)$	$[NO] \ (M)$	Rate $(mol \ L^{-1} \sec^{-1})$
$I$	$0.05$	$0.05$	$1 \times 10^{-3}$
$II$	$0.15$	$0.05$	$3 \times 10^{-3}$
$III$	$0.05$	$0.15$	$9 \times 10^{-3}$

The rate law for the reaction is:

The following graph shows how $T_{1/2}$ (half-life) of a reactant $R$ changes with the initial reactant concentration $a_0$. The order of the reaction will be: