For a certain reaction $A_{(g)} \to B_{(g)}$,the half-life for different initial pressures of $A$ is given below:

$P_{A_0} \text{ (atm)}$	$0.1$	$0.025$
$t_{1/2} \text{ (sec)}$	$100$	$50$

The correct statement about the order of reaction is:

Consider the following reaction: $A \longrightarrow \text{Products}$. This reaction is completed in $100 \ min$. The rate constant of this reaction at $t_1 = 10 \ min$ is $10^{-2} \ min^{-1}$. What is the rate constant (in $min^{-1}$) at $t_2 = 20 \ min$?

Fill in the blanks:
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$

For the reaction,$CH_3Br_{(aq)} + OH_{(aq)}^{-} \rightarrow CH_3OH_{(aq)} + Br_{(aq)}^{-}$,the rate law is $\text{rate} = k[CH_3Br][OH^{-}]$. What is the change in the rate of reaction if the concentration of both reactants is doubled?

For a reaction of order $(n - 1)$,what is the relationship between the half-life period $(t_{1/2})$ and the initial concentration of the reactant $([R]_0)$?

For a reaction $A + B \to$ product,it was found that the rate of reaction increases four times if the concentration of $A$ is doubled,but the rate of reaction remains unaffected if the concentration of $B$ is doubled. Hence,the rate law for the reaction is