Exercise 1

Thermal decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ occurs as per the equation below: 

$2 {\mathrm{N}}_2{\mathrm{O}}_5\to 4{\mathrm{NO}}_2+{\mathrm{O}}_2$.

The correct statement is:

For a $1^{\text{st }}$ order chemical reaction:

For an elementary reaction of reversible nature, net rate is: $\left(\frac{\mathrm{dx}}{\mathrm{dt}}\right)={\mathrm{k}}_1{\left[\mathrm{A}\right]}^2{\left[\mathrm{B}\right]}^1-{\mathrm{k}}_2\left[\mathrm{C}\right]$, hence, given reaction is:

The rate constant of a chemical reaction at a very high temperature will approach:

It takes $1 \mathrm{h}$ for a first-order reaction to go to $50\%$ completion. The total time required for the same reaction to reach $87.5\%$ completion will be:

Consider the following reversible first-order reaction of $\mathrm{X}$ at an initial concentration ${\left[\mathrm{X}\right]}_0$. The values of the rate constants are ${\mathrm{k}}_{\mathrm{f}}=2{\mathrm{s}}^{-1}$ and ${\mathrm{k}}_{\mathrm{b}}=1{\mathrm{s}}^{-1}$.

A plot of concentration of $\mathrm{X}$ and $\mathrm{Y}$ as function of time is:

A reaction has an activation energy of $209 \mathrm{kJ} {\mathrm{mol}}^{-1}$. The rate increases $10$-fold when the temperature is increased from $27°\mathrm{C}$ to $\mathrm{X}°\mathrm{C}$. The temperature $\mathrm{X}$ is closest to:

[Gas constant, $\mathrm{R}=8.314 \mathrm{J} {\mathrm{mol}}^{-1} {\mathrm{K}}^{-1}$]

For an elementary reaction, the net rate is $\left(\frac{\mathrm{dx}}{\mathrm{dt}}\right)=\mathrm{k}{\left[\mathrm{A}\right]}^2-{\mathrm{k}}^{\text{'}}\left[\mathrm{C}\right]{\left[\mathrm{B}\right]}^2$. Thus, select the correct statement: