For a reaction $A \rightarrow 2 B + C$ the half-lives are $100 \ s$ and $50 \ s$ when the concentration of reactant $A$ is $0.5 \ mol \ L^{-1}$ and $1.0 \ mol \ L^{-1}$ respectively. The order of the reaction is (Nearest Integer).

The rate constant for the reaction $2N_2O_5 \rightarrow 4NO_2 + O_2$ is $3.0 \times 10^{-5} \text{ s}^{-1}$. If the rate of reaction is $2.4 \times 10^{-5} \text{ mol L}^{-1} \text{ s}^{-1}$, then the concentration of $N_2O_5$ in $\text{mol L}^{-1}$ is:

The mechanism for the reaction is given below:
$2P + Q \to S + T$
$P + Q \to R + S$ (slow)
$P + R \to T$ (fast)
The rate law expression for the reaction is:

For a reaction $2NO_{(g)} + Cl_{2(g)} \rightleftharpoons 2NOCl_{(g)}$,when the concentration of $Cl_2$ is doubled,the rate of reaction becomes two times the original. When the concentration of $NO$ is doubled,the rate becomes four times. What is the order of the reaction?

What is the order of reaction $A + B \to C$?

Observation	$[A] \ (mol \ L^{-1})$	$[B] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ sec^{-1})$
$1$	$0.1$	$0.1$	$2 \times 10^{-3}$
$2$	$0.4$	$0.1$	$3.2 \times 10^{-3}$
$3$	$0.1$	$0.2$	$8 \times 10^{-3}$

Match List-$I$ with List-$II$:

List-$I$ (Order of Reaction)	List-$II$ (Unit of rate constant)
$A$. Zero order	$I$. $mol^{-1} L s^{-1}$
$B$. First order	$II$. $mol^{-2} L^{2} s^{-1}$
$C$. Second order	$III$. $s^{-1}$
$D$. Third order	$IV$. $mol L^{-1} s^{-1}$