Tag Archives: ozone

EPA’s New Ozone Rule: Part 20

Had the EPA succeeded in lowering the primary standard to 70 ppb and introducing a secondary standard of 13 ppm-hours, how much would that have cost industry? Would the benefits of a stricter standard justify that cost?

Here I must confess that I am at a considerable disadvantage. I do not know how to estimate industry costs, although I can report on other people’s claims. If I had all the time I needed, I would interview as many businesspeople I could on how tighter ozone restrictions imposed in 1998 affected them. In particular, I would want to know what new equipment they needed to buy to comply with the new standards. Did the new standards affect their decisions to buy equipment they were going to buy anyway and in what manner? How much more did they feel obliged to spend because of the new standards? Alas, time is short, I’m not getting paid to do this, I have no training in estimating costs, and I feel the need to move on to new topics. But these are still very important questions.

What I really would like is to compare three versions of one state’s State Implementation Plan (SIP). The first version would be designed to comply with the 0.084 ppm standard, the second with the 0.075 ppm standard, and the third to comply with the 0.070 ppm standard. Where are they the same? Where are they different? What are businesses expected to do differently to comply with the stricter standards? What kind of equipment are they expected to acquire under the three standards?

Do the benefits of a stricter standard justify the costs? Critics didn’t think so, such as the organization Americans for Tax Reform quoting a report by Oklahoma Senator James Inhofe:

EPA itself estimated that its ozone standard would cost $90 billion a year, while other studies have projected that the rule could cost upwards of a trillion dollars and destroy 7.4 million jobs.1

A couple of comments on this. The $90 billion a year figure and the trillion dollar figure are not contradictory. If the rule would cost us $90 billion a year for a dozen years, that will cost us more than a trillion dollars. Both figures are the upper limits of ranges, so that $90 billion a year and $1 trillion overall may be worst-case scenarios. According to a chart produced by the EPA which I will present in a later post, going to a 0.070 ppm standard would cost between $19 and $25 billion 2006 dollars by 20202. It is important to note that nobody can know for sure just how much the rule will cost either in money or in jobs. What experts do is estimate a range wide enough so that they think they will be right 95% of the time (95% confidence interval). That is to say, if an expert made an estimate of a range in twenty circumstances, in 19 times the true numbers will fall somewhere within those ranges.

Also, it should be pointed out that lowering ozone limits brings economic benefits in terms of lower medical costs and increased worker productivity (mainly because employees are out sick less). This is brought home by another EPA chart which estimates that if we had gone to a 0.070 ppm standard in 2011, we could have saved 170,000 sick days from work and eliminated 6,600 visits to the hospital and emergency rooms2. That all needs to be subtracted from the economic cost.

And what is the meaning of the destruction of 7.4 million jobs? Does that mean 7.4 million layoffs or 7.4 million people not hired who otherwise would be, or is it a combination of both? How does one determine how many jobs will be lost? (Note that Senator Inhofe is claiming two-digit accuracy: 7.4 million jobs, not 7.3 million or 7.5 million, so he is claiming more accuracy than a mere rough estimate. That kind of accuracy comes from a calculation and not just from a guess.) Do we need to balance that figure against jobs that might be created by the new rule, for example if companies that produce antipollution equipment saw an upsurge in business?

I am not an economist, but I think that the cost to business needs to be put into two categories. There are purchases that companies must make to comply with the new rule. The money doesn’t disappear; it merely goes somewhere else. If businesses buy American pollution control equipment, that is not a loss to the U.S. economy. Then there is the loss of productivity or efficiency that can come with compliance. That really could mean destroyed wealth, although it may be justified by the health and other benefits of the new rule.

Also, it is important to distinguish between capital expenditures, money spent on equipment, and operating expenses, money spent on operating that equipment. Money spent on equipment is a one-time investment, whereas money spent on operating that equipment is an ongoing commitment.

The EPA produced two very important documents that do a thorough cost-benefit analysis: Final Ozone NAAQS Regulatory Impact Analysis, March 2008, and its updated addendum, Regulatory Impact Analysis Final National Ambient Air Quality Standard for Ozone, July 2011. We will discuss these two documents in the next post.

Footnotes

  1. Website of Americans for Tax Reform, EPA Regulation of the Day: Ozone Rule. To view, click here.
  2. See my post in this blog EPA’s New Ozone Rule: Part 22.

EPA’s New Ozone Rule: Part 4

This post is based on information provided by two websites:

  • Washington University in St. Louis, Missouri. Chemistry 152: How Does Ozone Form? Unfortunately, the link to this website has been broken and the website is no longer available. (A shame, as it was really well done.)
  • NASA Earth Observatory, Chemistry in the Sunlight: The Chemistry of Ozone Formation To view, click here

See also Geoffrey Tyndal, Peroxy Radicals: Big Players on Ozone Production, website hosted by the project Stratopheric Processes And Their Role in Climate (SPARC) (University of Toronto). To view, click here.

Special thanks to Dr. Tyndal who graciously answered my questions regarding ozone formation. He explained to me how the VOC molecule whose peroxy radical had surrendered a oxygen atom to nitric oxide could continue to form more ozone, allowing concentrations to grow.

See also the website Environmental Science Published for Everybody Round the Earth (ESPERE), Lower Atmosphere: Oxidation in the Atmosphere. To view, click here.

If I am misunderstanding or misinterpreting the information, readers are urged to correct me. First, I want to describe the chemicals that we will be discussing here:

Nitrogen oxides consist of some combination of nitrogen and oxygen. We will be discussing two here. The first is nitric oxide, whose molecule consists of one nitrogen atom bonded to one oxygen atom:

NO

Nitrogen dioxide is a gas whose molecules consist of one nitrogen atom bonded to two oxygen atoms:

NO2

Volatile organic compounds (VOCs) are organic compounds (compounds containing carbon) that can exist as a gas or vapor in the atmosphere. Examples include natural gas, drinking alcohol, gasoline, fresh paint, nail polish remover, cooking aromas, women’s perfume.

Radicals are fragments of molecules that have one or more unpaired electrons. This makes them highly reactive: they are desperate to attach themselves to any molecule that will take them. They can have a positive, negative, or neutral charge. We will mention three types of radicals in this post, all of them neutral:

  • hydroxyl radicals consists of a hydrogen atom bonded to an oxygen atom, the chemical formula being (the mid dot [·] after the formula denotes electric neutrality):

    OH·

  • Peroxyl radicals consists of two oxygen atoms. Normally, O2 is ordinary oxygen gas, but it can act as a radical, as we shall see.
  • Hydroperoxyl radicals consists of a hydrogen and two oxygen atoms bonded together:

    HO2

  • In my last post, I wrote about the formation of stratospheric ozone that it is primarily produced by ultraviolet radiation from the sun. The ozone there does an excellent job in absorbing the radiation, so that very little ultraviolet radiation (of the type that forms ozone) reaches the ground. Ground-level ozone, by contrast, forms as the result of the chemical reactions of atmospheric nitrogen oxides. These nitrogen oxides are mostly formed by the burning of fuel in the presence of nitrogen and oxygen, the two most prevalent gases of Earth’s atmosphere. The high temperature of combustion fuses the nitrogen and oxygen into one molecule. This is why the exhaust of cars and coal-burning electric plants can be laden with nitrogen oxides. Lightning and chemical processes in the soil are also sources.

    There are many forms of nitrogen oxides; the two that are relevant here are nitric oxide (NO) and nitrogen dioxide (NO2). Only nitrogen dioxide directly produces ozone. A nitrogen dioxide molecule struck by a photon of sunlight (represented here as hv) will break down into nitric oxide and a free oxygen atom:

    NO2 + hv → NO + O    (1)

    The free oxygen atom is highly reactive and will quickly combine with a nearby oxygen molecule to form ozone.

    O2 + O → O3    (2)

    If that was all there was to it, the ozone problem would be much more manageable. Ozone is not a stable molecule: it reacts with surrounding chemicals to break down into ordinary oxygen. For example, ozone recombines with nitric oxide to reform nitrogen dioxide and ordinary oxygen:

    O3 + NO → NO2 + O2    (3)

    The amount of ozone would be much lower than it actually is, because it would be destroyed soon after being formed. There is a complicating factor, however.

    Volatile organic compounds (VOCs) can convert nitric oxide back into nitrogen dioxide with the help of the hydroxyl radical, a substance that composes a tiny proportion of the atmosphere (parts per trillion!) but can have a significant impact nonetheless. Suppose we represent a VOC molecule with the single chemical symbol R. Now VOC molecules usually have several hydrogen atoms. What we will do is exclude a single hydrogen atom from what is represented by R, such that the entire molecule is represented by the symbol:

    R-H

    where H represents the single hydrogen atom.

    When the VOC molecule contacts a molecule of ordinary oxygen and a hydroxyl radical (OH·), the single hydrogen atom is replaced with a peroxy radical (O2·). A water molecule is also formed. The reaction is:

    R-H + HO· + O2 → RO2· + H2O    (4)

    When the VOC molecule with the peroxy radical attached encounters a molecule of nitric oxide (NO), the peroxy radical gives up one atom of oxygen to the nitric oxide, converting it into nitrogen dioxide:

    RO2· + NO → RO· + NO2    (5)

    The nitrogen dioxide is then free to form more ozone.

    But it doesn’t stop there. If the VOC molecule with the extra oxygen atom has another hydrogen atom (and it usually does), it can react with an oxygen molecule to form a carbonyl compound (a compound where an oxygen and a carbon atom share a double bond) plus a hydroperoxyl radical (HO2·). I represent the VOC molecule in the following equation as RCHO· to emphasize the presence of a carbon atom, a hydrogen atom, and an oxygen atom radical, and I represent the carbonyl compound as RC=O:

    RCHO· + O2 → HO2· + RC=O    (6)

    The hydroperoxyl radical can then react with nitric oxide to form the hydroxyl radical plus nitrogen dioxide, both of which can participate in further reactions to form more ozone:

    HO2· + NO → HO· + NO2    (7)

    This description is an oversimplification. There are other chemical pathways for ozone to form. Also, small amounts of ozone can drift down from the stratosphere. But this gives a good idea how much of ground-level ozone is created. The main point is that ozone creation is a cycle. Nitrogen dioxide reacts with ordinary oxygen to form nitric oxide and ozone. Nitric oxide is converted back to nitrogen dioxide by the peroxy radical in VOC molecules. It is then free to convert more oxygen to ozone, and on the cycle goes. The presence of VOCs in the atmosphere, therefore, maintains a level of ozone in that vicinity.

    Why is this information important to our question of ozone regulation? We need to sit down with industry and discuss what needs to be done to reduce ozone concentrations at ground level. Industry emits very little ozone; it does emit ozone precursors and these need to be controlled. By knowing how much these precursors need to be reduced, we can work with industry to set up best practices while minimizing the burden, trying to keep both necessary capital expenditures and additional operational costs as low as possible.

    Finally, it appears that a small amount of ground-level ozone (below 15 ppb, perhaps?) is actually beneficial, because it generates the hydroxyl radical. The hydroxyl radical has been called the detergent of the atmosphere, because it is very good at eliminating many atmospheric pollutants. The hydroxyl radical constantly needs to be replenished, because its atmospheric lifespan is only a few seconds. See the article written by Phillip Ball entitled Fast-Acting Atmospheric Detergent (starting with the fifth paragraph) in the journal Nature, November 3, 2000, which you can view by clicking here.

EPA’s New Ozone Rule: Part 3

To understand atmospheric ozone, it is important to know how it is formed. In a previous post, I pointed out how ground-level ozone affects humans differently than the higher-up stratospheric ozone (thus the quip, “Good on high, bad nearby”1.) The way they are formed is different as well. Stratospheric ozone is formed when solar ultraviolet radiation strikes ordinary oxygen molecules (O2) and disassociates them into single atoms of oxygen. The ultraviolet energy is absorbed by the oxygen and does not reach the ground. These single atoms are extremely reactive and combine with nearby oxygen molecules to form triatomic oxygen or ozone (O3)2.

The ultraviolet radiation that forms ozone also destroys it when the radiation strikes an ozone molecule and breaks it up into an ordinary oxygen molecule and a free atom of oxygen. Thus ozone in the stratosphere is constantly being created and destroyed so that it does not accumulate past a certain amount3. In my next post, I’ll discuss how ground-level ozone is formed.


Footnotes:

  1. For example, see the Almanac of Policy Issues. To view, click here.
  2. NASA Earth Observatory, Chemistry in the Sunlight: The Chemistry of Ozone Formation To view, click here. You can see an excellent YouTube video of the process by clicking here.
  3. NASA Earth Observatory, Chemistry in the Sunlight: The Chemistry of Ozone Formation To view, click here.

Topic: The EPA’s New Ozone Rule Part I

Welcome to the very first topic of this blog, The EPA’s New Ozone Rule. It’s a rather long topic, consisting of 24 posts. If you arrived at this post via a link, you can navigate between posts using the arrows that appear above each post heading. Click on the right arrow (→) to go to the next post. Click on the left arrow (←) to go to the previous post.

On September 2, 2011, the White House released a statement that President Obama had requested the Director of the Environmental Protection Agency (EPA) Lisa Jackson to withdraw a recent EPA proposal to tighten standards for ground-level ozone1.  This proposal would lower the maximum allowable concentration of ground-level ozone from the current standard set in 1997 of 0.08 parts per million (ppm)2 3 to somewhere in a range between 0.060 and 0.070 ppm4.

This change in policy evoked cheers from political conservative and business circles and outrage from the environmental community. Jack Gerard, president of the American Petroleum Institute, was quoted by the newspaper USA Today as saying, “The president’s decision is good news for the economy and Americans looking for work. EPA’s proposal would have prevented the very job creation that President Obama has identified as his top priority.”5 The same article quotes Michael Steel, spokesperson for Speaker of the House John Boehner as saying, “We’re glad that the White House responded to the speaker’s letter and recognized the job-killing impact of this particular regulation.”6 On the other hand, environmentalists were furious. Gene Karpinski, president of the League of Conservation Voters, was quoted by the USA Today article as saying, “The Obama administration is caving to big polluters at the expense of protecting the air we breathe. This is a huge win for corporate polluters and huge loss for public health.”7  Conservatives and business interests, then, see the new rule as an undue burden on business. Environmental groups regard the rule as vital in protecting the public health. Who is correct?

It is possible that both sides have valid points and that the truth lies somewhere between them. I suspect that the rule would place a heavy burden on business, but not as heavy as its opponents make it out to be. Similarly, the rule would probably contribute to public health, although not as critically as its proponents think it will. Perhaps it would be wise to delay implementing the rule, but not to postpone it indefinitely.

I hope in my next postings to analyze the proposed rule, spell out exactly what claims are being made for it, and examine closely the claims of its opponents.


Footnotes:

  1. Statement by the President on the Ozone National Ambient Air Qualities Standards. White House website. To view, click here.
  2. National Ambient Air Quality Standards. EPA website. To view, click here.
  3. The 1997 standard is widely quoted as being 0.084 ppm rather than 0.08 ppm. This is because the EPA only demands an accuracy of 0.01 ppm. Therefore, any reading of ozone concentration between 0.075 ppm and 0.084 ppm would be rounded to 0.08 ppm and be considered in compliance. However, a reading of 0.085 ppm would be rounded to 0.09 ppm and would not be considered in compliance. Practically speaking then, 0.084 is the highest reading possible that remains in compliance. See EPA’s March 2008 National Ambient Air Quality Standards for Ground-Level Ozone: General Overview, p. 3. To view, click here. By the way, this is an excellent review of the case against ground-level ozone.
  4. Federal Register Vol. 75 No. 11, p. 2938 Tuesday, January 19, 2010. Docket no. EPA-HQ-OAR-2005-0172. To view, click here.
  5. USA Today, “Obama decides against tougher ozone standards” September 2, 2011, paragraph 14. To view, click here.
  6. Ibid. Paragraph 7
  7. Ibid. Paragraph 26