For the reaction $A + B \rightleftharpoons AB$,if the concentrations of both $A$ and $B$ are doubled,the rate of the reaction will become .......

The reaction of hydrogen and iodine monochloride is given as
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
This reaction is of first order with respect to $H_{2(g)}$ and $ICl_{(g)}$. Which of the following mechanisms is consistent with the given information?
Mechanism $A$:
$H_{2(g)} + 2ICl_{(g)} \to 2HCl_{(g)} + I_{2(g)}$
Mechanism $B$:
$H_{2(g)} + ICl_{(g)} \to HCl_{(g)} + HI_{(g)}$ (Slow)
$HI_{(g)} + ICl_{(g)} \to HCl_{(g)} + I_{2(g)}$ (Fast)

If $a$ is the initial concentration and $n$ is the order of the reaction and the half-life period is $T$,then:

If the concentration of reactant $A$ is increased by $10$ times,the rate of reaction increases $100$ times. What is the order of reaction if the rate law is $r = k[A]^x$?

Which one of the following is a second order reaction?

The half-life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $P_0$ as follows:

$P_0 \text{ (mmHg)}$	$250$	$300$
$t_{1/2} \text{ (minutes)}$	$135$	$112.5$

The order of reaction is -