Write differential rate expression of following reaction and give its order of reaction :

$2 N _{2} O _{5} \rightarrow 4 NO _{2}( g )+ O _{2}$

$C _{4} H _{9} Cl + OH ^{-} \rightarrow C _{4} H _{9} OH + Cl ^{-}$

For a certain reaction the expression for half life is $t \propto \frac{1}{{{a^{n - 1}}}}$ then the order of reaction is

For conversion of compound $A \rightarrow B$, the rate constant of the reaction was found to be $4.6 \times 10^{-5}\,L\, mol ^{-1}\, s ^{-1}$. The order of the reaction is $..........$ 

For a reaction whose rate expression is : Rate $ = k{[A]^{1/2}}{[B]^{3/2}}$, the order would be

Consider the following single step reaction in gas phase at constant temperature.

$2 \mathrm{~A}_{(\mathrm{g})}+\mathrm{B}_{(\mathrm{g})} \rightarrow \mathrm{C}_{(\mathrm{g})}$

The initial rate of the reaction is recorded as $r_1$ when the reaction starts with $1.5 \mathrm{~atm}$ pressure of $\mathrm{A}$ and $0.7 \mathrm{~atm}$ pressure of B. After some time, the rate $r_2$ is recorded when the pressure of $C$ becomes $0.5 \mathrm{~atm}$. The ratio $r_1: r_2$ is $\qquad$ $\times 10^{-1}$.

(Nearest integer)

For the reaction $2P + Q \to  R$. If the rate of appearance of $R$ is $0.5\, mol/L-hour$ then the rate of disappearance of $P$ and $Q$ are