Problem 34
Almost equal masses of \(\mathrm{SO}_{2}\) and \(\mathrm{NO}_{x}\) are produced by human activities in the United States. a. How does their production compare based on a mole basis? Assume that all the \(\mathrm{NO}_{x}\) is produced as \(\mathrm{NO}_{2}\). b. Suggest reasons why the U.S. percentage of global emissions is greater for \(\mathrm{NO}_{x}\) than for \(\mathrm{SO}_{2}\).
Problem 35
Reactive nitrogen compounds affect the biosphere both directly and indirectly through other chemicals they help form. a. Name a direct effect of reactive nitrogen compounds that is a benefit. b. Name two direct effects of reactive nitrogen compounds that are harmful to human health. c. Ozone formation is a harmful indirect effect. Explain the connection between reactive nitrogen compounds and the formation of ozone.
Problem 38
Here are examples of what an individual might do to reduce acid rain. For each, explain the connection to producing acid rain. a. Hang your laundry to dry it. b. Walk, bike, or take public transportation to work. c. Avoid running dishwashers and washing machines with small loads. d. Add additional insulation on hot water heaters and pipes. e. Buy locally grown produce and locally produced food.
Problem 42
In the United States over the past few decades, emissions of ammonia have dramatically increased, although less so in the east than in the west. a. Show with a chemical equation that ammonia dissolves in rain to form a basic solution. b. Write the neutralization reaction for rain that contains both ammonia and nitric acid. c. Ammonium sulfate also is found in rain. Write a chemical equation that demonstrates how it could have formed.
Problem 44
The mass of \(\mathrm{CO}_{2}\) emitted during combustion reactions is much greater than the mass of \(\mathrm{NO}_{x}\) or \(\mathrm{SO}_{2}\), but there is less concern about the contributions of \(\mathrm{CO}_{2}\) to acid rain than from the other two oxides. Suggest two reasons for this apparent inconsistency.
Problem 45
The average \(\mathrm{pH}\) of precipitation in New Hampshire and Vermont is low, even though these states have relatively fewer cars and virtually no industry that emits large quantities of air pollutants. How do you account for this low \(\mathrm{pH}\) ?
Problem 47
The chemistry of NO in the atmosphere is complicated. NO can destroy ozone, as seen in Chapter 2. But remember from Chapter 1 that NO can react with \(\mathrm{O}_{2}\) to form \(\mathrm{NO}_{2}\). In turn, \(\mathrm{NO}_{2}\) can react in sunlight to produce ozone. Summarize these reactions, noting in which region of the atmosphere they each occur.
Problem 48
a. Efforts to control air pollution by limiting the emission of particulates and dust can sometimes contribute to an increase in the acidity of rain. Offer a possible explanation for this observation. Hint: These particulates may contain basic compounds of calcium, magnesium, sodium, and potassium. b. In Chapter 2 , stratospheric ice crystals in the Antarctic were involved in the cycle leading to the destruction of ozone. Is this effect related to the observations in part a? Explain.
Problem 49
Discuss the validity of the statement, "Photochemical smog is a local issue, acid rain is a regional one, and the enhanced greenhouse effect is a global one." Describe the chemistry behind each issue. Do you agree that the magnitudes of the problems are really so different in scope?
Problem 56
One way to compare the acid-neutralizing capacity of different substances is to calculate the mass of the substance required to neutralize \(1 \mathrm{~mol}\) of hydrogen ion, \(\mathrm{H}^{+}\). a. Write a balanced equation for the reaction of \(\mathrm{NaHCO}_{3}\) with \(\mathrm{H}^{+}\). Use it to calculate the acidneutralizing capacity for \(\mathrm{NaHCO}_{3}\). b. If \(\mathrm{NaHCO}_{3}\) costs \(\$ 9.50 / \mathrm{kg}\), determine the cost to neutralize one mole of \(\mathrm{H}^{+}\).
