From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.

$(iv)$ $C _{2} H _{5} Cl ( g ) \rightarrow C _{2} H _{4}( g )+ HCl ( g ) \quad$ Rate $=k\left[ C _{2} H _{5} Cl \right]$

For the reaction, $2N_2O_5 \to 4NO_2 + O_2$ rate and rate constant are $1.02 \times 10^{-4}\, mol\,L^{-1}\,s^{-1}$ and $3.4 \times10^{-5}\,s^{-1}$ respectively. The concentration of $N_2O_5$ in $mol\,L^{-1}$ will be

Differential form of the rate equation is

$\frac{{dx}}{{dt}} = k\left[ P \right]{\left[ Q \right]^{0.5}}{\left[ R \right]^{0.5}}$

Which statement about the above equation is wrong?

If $R = K{[NO]^2}[{O_2}],$ rate constant may be increased by

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)

$2 NO ( g )+ Cl _{2}( g ) \rightleftharpoons 2 NOCl ( s )$

This reaction was studied at $-10^{\circ} C$ and the following data was obtained

$[ NO ]_{0}$ and $\left[ Cl _{2}\right]_{0}$ are the initial concentrations and $r _{0}$ is the initial reaction rate.

The overall order of the reaction is ..........

(Round off to the Nearest Integer).