$A$ chemical reaction proceeds through the following steps:
Step-$I$: $2A \rightleftharpoons X$ (fast)
Step-$II$: $X + B \rightarrow Y$ (slow)
Step-$III$: $Y + B \rightarrow \text{Product}$ (fast)
The rate law for the overall reaction is:

For a reaction $A \longrightarrow P$,a plot between $[A]_0$ $Vs$ $\frac{1}{t_{1/2}}$ is a straight line having a positive slope. When the initial concentration is $1 \times 10^{-2} \ M$,its half-life period is found to be $20 \ min$. When the concentration of $A$ is $2 \times 10^{-2} \ M$,then the half-life will be (in $min$)?

For the reaction $2A + B \rightarrow A_2B$,if the concentration of reactant $A$ is doubled and the concentration of reactant $B$ is halved,the rate of the reaction will:

$1 \ L$ of $2 \ M$ $CH_3COOH$ is mixed with $1 \ L$ of $3 \ M$ $C_2H_5OH$ to form an ester. The rate of the reaction with respect to the initial rate when each solution is diluted with an equal volume of water will be (in times).

The rate of reaction between $A$ and $B$ increases by a factor of $100$ when the concentration of $A$ is increased $10$ folds. The order of reaction with respect to $A$ is

Which among the following statements is $NOT$ true about rate constant?