For the reaction $A + B \to C$,it is found that doubling the concentration of $A$ increases the rate by $4$ times,and doubling the concentration of $B$ doubles the reaction rate. What is the overall order of the reaction?

$A$ reaction is first order with respect to $A$ and second order with respect to $B$. How many times the rate of reaction is affected on increasing the concentration of $B$ three times?

The value of the rate constant of a pseudo first order reaction:

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)

The rate of the reaction $CCl_3CHO + NO \to CHCl_3 + NO + CO$ is given by $Rate = K [CCl_3CHO] [NO]$. If concentration is expressed in $mol \ L^{-1}$,the units of $K$ are:

The rate law for the reaction,$NO_{2(g)} + CO_{(g)} \rightarrow NO_{(g)} + CO_{2(g)}$ is given as $R = k[NO_2]^2$. What is the order of reaction with respect to $CO$?