For a reaction,$K = 4.5 \times 10^{-4} \ L \ mol^{-1} \ s^{-1}$. What is the order of the reaction?

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

For a gaseous reaction,the rate is given by $Rate = k [A] [B]$. If the volume of the container is reduced to $1/4$ of its initial volume,the rate of the reaction will become how many times the initial rate?

The data for the reaction $A + B \to C$ is given below. The rate law corresponding to the above data is:

$Exp.$	$[A]_0$	$[B]_0$	Initial rate
$(1)$	$0.012$	$0.035$	$0.10$
$(2)$	$0.024$	$0.070$	$0.80$
$(3)$	$0.024$	$0.035$	$0.10$
$(4)$	$0.012$	$0.070$	$0.80$

For the reaction $2A + 2B \rightarrow 2C + D$,the rate law is expressed as $\text{rate} = k[A]^2[B]$. Calculate the rate constant if the rate of reaction is $0.24 \ mol \ dm^{-3} \ s^{-1}$ where $[A] = 0.5 \ M$ and $[B] = 0.2 \ M$.

For a fourth-order reaction,what is the unit of $K$?