The reaction $2N_2O_5 \rightleftharpoons 4NO_2 + O_2$ follows first order kinetics. Hence,the molecularity of the reaction is

For a reaction $A + B \longrightarrow P$,the following data are provided. The rate constant for this reaction in standard units is:

Entry	$[A]$ in $M$	$[B]$ in $M$	Initial rate $(M/s)$
$1$	$0.02$	$0.02$	$2 \times 10^{-2}$
$2$	$0.02$	$0.04$	$4 \times 10^{-2}$
$3$	$0.04$	$0.04$	$8 \times 10^{-2}$

The decomposition of dimethyl ether leads to the formation of $CH_4$,$H_2$ and $CO$ and the reaction rate is given by
Rate $= k [CH_3OCH_3]^{3/2}$
The rate of reaction is followed by increase in pressure in a closed vessel,so the rate can also be expressed in terms of the partial pressure of dimethyl ether,i.e.
Rate $= k (p_{CH_3OCH_3})^{3/2}$
If the pressure is measured in $bar$ and time in $minutes$,then what are the units of rate and rate constants?

State whether the following sentences are true $(T)$ or false $(F)$:
$(a)$ There is more than one reactant in a pseudo first order reaction.
$(b)$ In a pseudo first order reaction,the concentration of both reactants is the same.
$(c)$ In a pseudo first order reaction,the concentration of one reactant is very high.

The rate constant for the reaction,$2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-4} \ s^{-1}$. If the reaction starts with $1.0 \ mol \ L^{-1}$ of $N_2O_5$,calculate the rate of formation of $NO_2$ at the moment when the concentration of $O_2$ is $0.1 \ mol \ L^{-1}$.

The rate law for the reaction $A + 2B \rightarrow C + 2D$ is given by: