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 will be the unit of rate constant for the reaction having Rate $= K[A]^{\frac{1}{2}} \cdot [B]^{\frac{3}{2}}$ ?

The rate of a certain reaction depends on concentration according to the equation $\frac{-dc}{dt} = \frac{K_1 C}{1 + K_2 C}$. What is the order of the reaction when the concentration $(C)$ is very high?

The experimental data for the reaction $2A + B_2 \longrightarrow 2AB$ is given below:

Exp.	$[A] \ (mol \ L^{-1})$	$[B_2] \ (mol \ L^{-1})$	Rate $(mol \ L^{-1} \ S^{-1})$
$1$	$0.50$	$0.50$	$1.6 \times 10^{-4}$
$2$	$0.50$	$1.00$	$3.2 \times 10^{-4}$
$3$	$1.00$	$1.00$	$3.2 \times 10^{-4}$

Determine the rate law for the reaction.

For the reaction $X + Y \rightarrow Z$,the rate law is $r = K[X][Y]$. If the concentration of $Y$ is increased significantly,what will be the order of the reaction?

What is the molecularity of a reaction? Explain its types with examples.