Problem 1
A general formula for gasoline is \(\mathrm{C}_{7} \mathrm{H}_{13}\). Calculate the air to gasoline mass ratio required for stoichiometric combustion.
Problem 3
Suppose propene \(\left(\mathrm{CH}_{2}=\mathrm{CH}-\mathrm{CH}_{3}\right)\) is the hydrocarbon that reacts with the hydroxyl radical - OH. Write the set of chemical reactions which ultimately produce an aldehyde. What is this final aldehyde?
Problem 5
The atmospheric ratio of PAN - PAN + inorganic nitrate varies from less than \(0.1\) to \(0.9 .\) High values of the ratio are associated with 'photochemically aged' air masses, situations where precipitation has recently occurred, and situations where unusually high night-time nitrogen oxide concentrations are found (Roberts, J. M., The atmospheric chemistry of organic nitrates. Atmospheric Environment, 24A(2) (1990), 243-287. What do these observations tell us about factors affecting the relative rates of formation and removal of nitrogen oxide compounds?
Problem 6
Nitrogen oxide is formed at night by dissociation of dinitrogen pentoxide. For the first order reaction $$ \mathrm{N}_{2} \mathrm{O}_{5} \rightarrow \mathrm{NO}_{2}+\mathrm{NO}_{3} $$ the rate constant is \(3.14 \times 10^{-2} \mathrm{~s}^{-1}\) at \(25^{\circ} \mathrm{C}\), and \(1.42 \times 10^{-3} \mathrm{~s}^{-1}\) at \(55^{\circ} \mathrm{C}\). Calculate the half life of this molecule at the two temperatures. For a concentration of \(\mathrm{N}_{2} \mathrm{O}_{5}\) of \(3.6 \mathrm{ppbv}\), calculate the length of time it could take for the concentration to be reduced to \(1.0 \mathrm{ppbv}\) at a constant temperature of \(25^{\circ} \mathrm{C}\). Calculate the Arrhenius parameters, \(A\) and \(E_{2}\). for the reaction.
