Chapter 20: Problem 52
What are primary and secondary pollutants?
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Chapter 20: Problem 52
What are primary and secondary pollutants?
These are the key concepts you need to understand to accurately answer the question.
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As stated in the chapter, carbon monoxide has a much higher affinity for hemoglobin than oxygen does. (a) Write the equilibrium constant expression \(\left(K_{\mathrm{c}}\right)\) for the following process: $$ \mathrm{CO}(g)+\mathrm{HbO}_{2}(a q) \rightleftharpoons \mathrm{O}_{2}(g)+\mathrm{HbCO}(a q) $$ where \(\mathrm{HbO}_{2}\) and \(\mathrm{HbCO}\) are oxygenated hemoglobin and carboxyhemoglobin, respectively. (b) The composition of a breath of air inhaled by a person smoking a cigarette is \(1.9 \times 10^{-6} \mathrm{~mol} / \mathrm{L} \mathrm{CO}\) and \(8.6 \times 10^{-3} \mathrm{~mol} / \mathrm{L} \mathrm{O}_{2} .\) Calculate the ratio of \([\mathrm{HbCO}]\) to \(\left[\mathrm{HbO}_{2}\right]\), given that \(K_{\mathrm{c}}\) is 212 at \(37^{\circ} \mathrm{C}\).
Suggest ways to minimize the formation of photochemical smog.
The molar heat capacity of a diatomic molecule is \(29.1 \mathrm{~J} / \mathrm{K} \cdot \mathrm{mol} .\) Assuming the atmosphere contains only nitrogen gas and there is no heat loss, calculate the total heat intake (in kilojoules) if the atmosphere warms up by \(3^{\circ} \mathrm{C}\) during the next \(50 \mathrm{yr}\). Given that there are \(1.8 \times 10^{20}\) moles of diatomic molecules present, how many kilograms of ice (at the North and South Poles) will this quantity of heat melt at \(0^{\circ} \mathrm{C} ?\) (The molar heat of fusion of ice is \(6.01 \mathrm{~kJ} / \mathrm{mol} .)\)
Although the hydroxyl radical (OH) is present only in a trace amount in the troposphere, it plays a central role in its chemistry because it is a strong oxidizing agent and can react with many pollutants as well as some CFC substitutes (see Section 20.3 ). The hydroxyl radical is formed by the following reactions: $$ \begin{array}{r} \mathrm{O}_{3} \stackrel{\lambda<320 \mathrm{nm}}{\longrightarrow} \mathrm{O}^{*}+\mathrm{O}_{2} \\ \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{OH} \end{array} $$ where \(\mathrm{O}^{*}\) denotes an electronically excited atom. (a) Explain why the concentration of \(\mathrm{OH}\) is so small even though the concentrations of \(\mathrm{O}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}\) are quite large in the troposphere. (b) What property makes OH a strong oxidizing agent? (c) The reaction between \(\mathrm{OH}\) and \(\mathrm{NO}_{2}\) contributes to acid rain. Write an equation for this process. (d) The hydroxyl radical can oxidize \(\mathrm{SO}_{2}\) to \(\mathrm{H}_{2} \mathrm{SO}_{4} .\) The first step is the formation of a neutral \(\mathrm{HSO}_{3}\) species, followed by its reaction with \(\mathrm{O}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) to form \(\mathrm{H}_{2} \mathrm{SO}_{4}\) and the hydroperoxyl radical \(\left(\mathrm{HO}_{2}\right)\). Write equations for these processes.
Describe the removal of \(\mathrm{SO}_{2}\) by \(\mathrm{CaO}\) (to form \(\mathrm{CaSO}_{3}\) ) in terms of a Lewis acid-base reaction.
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