Chapter 16

Automobile Engine The following reaction takes place in an automobile's engine and exhaust system. $$\quad \mathrm{NO}_{2}(\mathrm{g})+\mathrm{CO}(\mathrm{g}) \rightarrow \mathrm{NO}(\mathrm{g})+\mathrm{CO}_{2}(\mathrm{g})$$ The reaction's rate law at a particular temperature is Rate \(=0.50 \mathrm{L} /(\mathrm{mol} \cdot \mathrm{s})\left[\mathrm{NO}_{2}\right]^{2}\) . What is the reaction's initial, instantaneous rate when \(\left[\mathrm{NO}_{2}\right]=0.0048 \mathrm{mol} / \mathrm{L} ?\)

The concentrations in a chemical reaction are expressed in moles per liter and time is expressed in seconds. If the overall rate law is third-order, what are the units for the rate and the rate constant?

Visualize the reaction energy diagram for a one-step, endothermic chemical reaction. Compare the heights of the activation energies for the forward and reverse reactions.

Apply the method of initial rates to determine the order of a chemical reaction with respect to Reactant \(\mathrm{X}\) . Create a set of hypothetical experimental data that would lead you to conclude that the reaction is second order in X.

Apply collision theory to explain two reasons why increasing the temperature of a reaction by 10 K often doubles the reaction rate

Hydrocarbons Heating cyclopropane \(\left(\mathrm{C}_{3} \mathrm{H}_{6}\right)\) converts it to propene \(\left(\mathrm{CH}_{2}=\mathrm{CHCH}_{3}\right) .\) The rate law is first order in cyclopropane. If the rate constant at a particular temperature is \(6.22 \times 10^{-4} \mathrm{s}^{1}\) and the concentration of cyclopropane is held at \(0.0300 \mathrm{mol} / \mathrm{L},\) what mass of propene is produced in 10.0 \(\mathrm{min}\) in a volume of 2.50 \(\mathrm{L}\) ?

For the following categories of elements, state the possible number(s) of electrons in their outermost orbitals in the ground state? (Chapter 5\()\) \begin{equation} \begin{array}{l}{\text { a. p-block elements }} \\ {\text { b. nitrogen-group elements }} \\ {\text { c. d-block elements }} \\ {\text { d. noble-gas elements }} \\ {\text { e. s-block elements }}\end{array} \end{equation}

Classify each of the following elements as a metal, nonmetal, or metalloid. (Chapter 6\()\) \begin{equation} \begin{array}{l}{\text { a. molybdenum }} \\ {\text { b. bromine }} \\\ {\text { c. arsenic }} \\ {\text { d. neon }} \\ {\text { e. cerium }}\end{array} \end{equation}

Balance the following equations. (Chapter 9) \begin{equation} \begin{array}{l}{\text { a. } \mathrm{Sn}(\mathrm{s})+\mathrm{NaOH}(\mathrm{aq}) \rightarrow \mathrm{Na}_{2} \mathrm{SnO}_{2}+\mathrm{H}_{2}} \\ {\text { b. } \mathrm{C}_{8} \mathrm{H}_{18}(1)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1)} \\ {\text { c. } \mathrm{Al}(\mathrm{s})+\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})}\end{array} \end{equation}

What mass of iron(III) chloride is needed to prepare 1.00 L of a 0.255\(M\) solution? (Chapter 14)

What information must you know to calculate the boiling point elevation of a solution of hexane in benzene? (Chapter 14)

\(\Delta H\) for a reaction is negative. Compare the energy of the products and the reactants. Is the reaction endother- mic or exothermic? (Chapter 15\()\)

The rate law is rate \(=k[\) phenolphthalein]. If the rate constant for the reaction is \(1.0 \times 10^{-2} \mathrm{s}^{-1}\) , what is the instantaneous rate of reaction when the concentra- tion of phenolphthalein is 0.0025\(M ?\)