The thermal decomposition of ${\mathrm{N}}_2{\mathrm{O}}_5$ occurs in the following steps.

Step- $\mathrm{I}$ ${\mathrm{N}}_2{\mathrm{O}}_5\stackrel{ \mathrm{slow} }{⟶}{\mathrm{NO}}_2+{\mathrm{NO}}_3$

Step- $\mathrm{II}$ ${\mathrm{N}}_2{\mathrm{O}}_5+{\mathrm{NO}}_3\stackrel{ \mathrm{fast} }{⟶}3{\mathrm{NO}}_2+{\mathrm{O}}_2$

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

Suggest the rate expression.

The reaction $2\mathrm{NO}+{\mathrm{Br}}_2⟶2\mathrm{NOBr}$, obeys the following mechanism.

(i) $\mathrm{NO}+{\mathrm{Br}}_2\stackrel{\mathrm{Fast}}{=}{\mathrm{NOBr}}_2$
(ii) ${\mathrm{NOBr}}_2+\mathrm{NO}\stackrel{\mathrm{Slow}}{⟶}2\mathrm{NOBr}$

Suggest the rate expression.

Given the following steps in the mechanism for a chemical reaction:

$\mathrm{A}+\mathrm{B}⟶\mathrm{C}$           (fast)

$\mathrm{B}+\mathrm{C}⟶\mathrm{D}+\mathrm{E}$   (Slow)

$\mathrm{D}+\mathrm{F}⟶\mathrm{A}+\mathrm{E}$    (fast)

At any time $\left[\mathrm{C}\right]$ is directly proportional to $\left[\mathrm{A}\right].$
(a) What is the stoichiometric equation for the reaction?
(b) Which species, if any, are catalysts in this reaction ?
(c) Which species, if any, are intermediates in this reaction?
(d) Write the rate law for the rate-determining step.
(e) Write the rate law for this reaction.
(f) What is overall order of the reaction ?

Rate of formation of product at $20$ seconds is:

In the following reaction, $\begin{array}{c}\mathrm{xA}⟶\mathrm{yB}\\ \log \left[-\frac{\mathrm{d}\left[\mathrm{A}\right]}{\mathrm{dt}}\right]=\log \left[\frac{\mathrm{d}\left[\mathrm{B}\right]}{\mathrm{dt}}\right]+0.3\end{array}$ where, negative sign indicates rate of disappearance of the reactant. Thus, $\mathrm{x}: \mathrm{y}$ is

Rate of formation of ${\mathrm{SO}}_3$ in the following reaction:

$2{\mathrm{SO}}_2+{\mathrm{O}}_2\to 2{\mathrm{SO}}_3$, is $100 \mathrm{g} {\min }^{-1}.$ Hence, the rate of disappearance of ${\mathrm{O}}_2$ is:

$\mathrm{aA}+\mathrm{bB}⟶$ Product, $\mathrm{dx}/\mathrm{dt}=\mathrm{k}\left[\mathrm{A}{]}^{\mathrm{a}}\right[\mathrm{B}{]}^{\mathrm{b}}.$ If concentration of $\mathrm{A}$ is doubled, rate is four times. If concentration of $\mathrm{B}$ is made four times, rate is doubled. What is relation between rate of disappearance of $\mathrm{A}$ and that of $\mathrm{B}?$