Jake R.

Calculate the volume, in liters, occupied by each of the following

a. 2.00 $mol H_{2}$ at 300.0 $K$ and 1.25 $\mathrm{atm}$
b. 0.425 $\mathrm{mol} NH_{3}$ at $37^{\circ} C$ and 0.724 $\mathrm{atm}$
c. 4.00 $\mathrm{g} O_{2}$ at $57^{\circ} C$ and 0.888 $\mathrm{atm}$

Consider the following mechanism for the reaction of hydrogen and iodine monochloride:
$\begin{array}{ll}{\text {Step } 1 .} & {\mathrm{H}_{2}(g)+\mathrm{ICl}(g) \longrightarrow \mathrm{HI}(g)+\mathrm{HCl}(g)} \\ {S t e p 2} & {\mathrm{HI}(g)+\mathrm{ICl}(g) \longrightarrow \mathrm{I}_{2}(g)+\mathrm{HCl}(g)}\end{array}$
(a) Write the equation for the overall reaction.
(b) Identify any reaction intermediates.
(c) What is the molecularity of each elementary step?

The following mechanism has been proposed for the reaction of nitric oxide and chlorine:
$\begin{array}{ll}{\text {Step } 1 .} & {\mathrm{NO}(g)+\mathrm{Cl}_{2}(g) \longrightarrow \mathrm{NOCl}_{2}(g)} \\ {\text { Step } 2 .} & {\mathrm{NOCl}_{2}(g)+\mathrm{NO}(g) \longrightarrow 2 \mathrm{NOCl}(g)}\end{array}$
(a) What is the overall reaction?
(b) Identify any reaction intermediates.
(c) What is the molecularity of each elementary step?

Give the molecularity and the rate law for each of the following elementary reactions:
(a) $\mathrm{O}_{3}(g)+\mathrm{Cl}(g) \longrightarrow \mathrm{O}_{2}(g)+\mathrm{ClO}(g)$
(b) $\mathrm{NO}_{2}(g) \longrightarrow \mathrm{NO}(g)+\mathrm{O}(g)$
(c) $\mathrm{ClO}(g)+\mathrm{O}(g) \longrightarrow \mathrm{Cl}(g)+\mathrm{O}_{2}(g)$
(d) $\mathrm{Cl}(g)+\mathrm{Cl}(g)+\mathrm{N}_{2}(g) \longrightarrow \mathrm{Cl}_{2}(g)+\mathrm{N}_{2}(g)$

Identify the molecularity and write the rate law for each of the following elementary reactions:
(a) $\mathrm{I}_{2}(g) \longrightarrow 2 \mathrm{I}(g)$
(b) $2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \longrightarrow 2 \mathrm{NOBr}(g)$
(c) $\mathrm{N}_{2} \mathrm{O}_{5}(g) \longrightarrow \mathrm{NO}_{2}(g)+\mathrm{NO}_{3}(g)$

The thermal decomposition of nitryl chloride, $\mathrm{NO}_{2} \mathrm{Cl},$ is believed to occur by the following mechanism:
$$\mathrm{NO}_{2} \mathrm{Cl}(g) \stackrel{k_{1}}{\longrightarrow} \mathrm{NO}_{2}(g)+\mathrm{Cl}(g)$$
$$\mathrm{Cl}(g)+\mathrm{NO}_{2} \mathrm{Cl}(g) \stackrel{k_{2}}{\longrightarrow} \mathrm{NO}_{2}(g)+\mathrm{Cl}_{2}(g)$$
(a) What is the overall reaction?
(b) What is the molecularity of each of the elementary steps?
(c) What rate law is predicted by this mechanism if the first step is rate-determining?