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?

For the reaction $A + B \rightarrow \text{product}$,the rate of reaction is $3.6 \times 10^{-2} \ mol \ dm^{-3} \ sec^{-1}$. When $[A] = 0.2 \ mol \ dm^{-3}$ and $[B] = 0.1 \ mol \ dm^{-3}$,calculate the rate constant of the reaction if the reaction is first order in $A$ and second order in $B$.

What is the unit of the rate constant for a $4^{th}$ order reaction?

Inversion of cane sugar is an example of $-$

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 -

For a reaction $A + B \rightarrow \text{Product}$,the rate of reaction doubles when the concentration of $A$ is doubled. The rate becomes four times when the concentrations of both $A$ and $B$ are doubled. What is the order of the reaction with respect to $A$ and $B$ respectively?