Lecture 15 AOSC/CHEM 637 Atmospheric Chemistry R. Dickerson Ammonia, NH3, and Nitrous Oxide, N2O And The Nitrogen Cycle -orReading: Finlayson-Pitts Ch 14; Seinfeld and Pandis Chapters 2, 7 & 10. [Cicerone, 1989; Mosier and Kroeze, 1998; Dentener and Crutzen, 1994; Galloway, et al., 2004; Mosier, et al., 1998; NRC, 2003] Copyright © 2010 R. R. Dickerson 1 What color was dinosaur poop? Copyright © 2010 R. R. Dickerson 2 Life requires Nitrogen • • • • • • • Proteins, chains of amino acids, are central to life. Only lightning and a few organisms can fix N. Plants use nitrates to make amino acids. Amino acids decompose to CO2, H2O, and NH3. Ammonia is toxic. Ammonia moderately soluble. Urea, costs 4 ATP molecules, but is highly soluble. Copyright © 2010 R. R. Dickerson 3 Ammonia is toxic to most animals; 100 ppm begins to cause adverse effects and 5000 ppm is rapidly fatal. Fish can easily expel ammonia because it is moderately soluble and lost to the water passing through their gills. But ammonia with a Henry’s Law coefficient of 60 M atm-1 is not soluble enough for us. You would have to drink at least 1000 L of water per day to get rid of 100 g of ammonia. To solve this problem, your body expends 4 ATP molecules (~15% of the total available energy of an amino acid) to make each molecule of urea. The solubility of urea exceeds 1000 g/L, so you can get rid of your excess ammonia that way. Because urea lies uphill thermodynamically it is easily converted back to ammonia and carbon dioxide. In soils ammonia/ammonium can be nitrified and used by plants. Copyright © 2010 R. R. Dickerson 4 Mammals excrete urea: (NH2)2CO Copyright © 2010 R. R. Dickerson 5 • SOURCES: Direct emissions from industrial processes and cars with catalytic converters are minor. The main sources are fertilized soils and hydrolysis of urea in animal waste. • Urease enzymes in manure quickly hydrolyze urea to ammonia and carbon dioxide. • (NH2)2CO + H2O → 2NH3 + CO2 Copyright © 2010 R. R. Dickerson 6 The Nitrogen Cycle NO Copyright © 2010 R. R. Dickerson 7 The Nitrogen Cascade Atmospheric stratosphere ozone depletion greenhouse gases ozone particulate matter troposphere “new” nitrogen Energy Production & combustion of fossil fuels Food Production NOx NOy, NHx, Norg Terrestrial NHx & creation of synthetic fertilizers Vegetated biogeochemical cycling ecosystem productivity soils NOx NH3, Norg Populated Agricultural crops grasslands forests landscape people animals soils soils N2O NOy, NHx, Norg NOy , NHx Norg Aquatic Surface Water & Wetlands acidification eutrophication N2O Groundwater Coastal Bays & Estuaries Oceans denitrification potential Copyright © 2010 R. R. Dickerson 9 Copyright © 2010 R. R. Dickerson 10 Atmospheric Ammonia, NH3 I. Fundamental Properties Importance • Only gaseous base in the atmosphere. • Major role in biogeochemical cycles of N. • Produces particles & cloud condensation nuclei. • Haze/Visibility • Radiative balance; direct & indirect cooling • Stability wrt vertical mixing. • Precipitation and hydrological cycle. • Potential source of NO and N2O. Copyright © 2010 R. R. Dickerson 11 US Ammonia Emissions 2000 Industruial processes Fuel Combustion Transportation Agricurtral crops Agricurtral livestock Copyright © 2010 R. R. Dickerson 12 Fundamental Properties, continued Thermodynamically unstable wrt oxidation. NH3 + 1.25O2 → NO + 1.5H2O H°rxn = −53.93 kcal mole-1 G°rxn = −57.34 kcal mole-1 But the kinetics are slow: NH3 + OH· → NH2 + H2O k = 1.6 x 10-13 cm3 s-1 (units: (molec cm-3)-1 s-1) Atmospheric lifetime for [OH] = 106 cm-3 τNH3 = (k[OH])-1 ≈ 6x106 s = 72 d. Compare to τH2O ≈ 10 d. Copyright © 2010 R. R. Dickerson 13 Fundamental Properties, continued Gas-phase reactions: NH3 + OH· → NH2· + H2O NH2· + O3 → NH, NHO, NO NH2· + NO2 → N2 or N2O (+ H2O) Potential source of atmospheric NO and N2O in low-SO2 environments. Last reaction involved in combustion “deNOx” operations. Copyright © 2010 R. R. Dickerson 14 Fundamental Properties, continued Aqueous phase chemistry: NH3(g) + H2O ↔ NH3·H2O(aq) ↔ NH4 + + OH− Henry’s Law Coef. = 62 M atm-1 Would not be rained out without atmospheric acids. Weak base: Kb = 1.8x10-5 Copyright © 2010 R. R. Dickerson 15 Formation of Aerosols Nucleation – the transformation from the gaseous to condensed phase; the generation of new particles. H2SO4/H2O system does not nucleate easily. NH3/H2SO4/H2O system does (e.g., Coffman & Hegg, 1995). Copyright © 2010 R. R. Dickerson 16 Formation of aerosols, continued: NH3(g) + H2SO4(l) → NH4HSO4(s, l) (ammonium bisulfate) NH3(g) + NH4HSO4(l) → (NH4)2SO4(s, l) (ammonium sulfate) Ammonium sulfates are stable solids, or, at most atmospheric RH, liquids. Deliquescence – to become liquid through the uptake of water at a specific RH (∽ 40% RH for NH4HSO4). Efflorescence – the become crystalline through loss of water; literally to flower. We can calculate the partitioning in the NH4/SO4/NO3/H2O system with a thermodynamic model; see below. Copyright © 2010 R. R. Dickerson 17 Formation of aerosols, continued NH3(g) + HNO3(g) ↔ NH4NO3(s) G°rxn = −22.17 kcal mole-1 [NH4NO3] Keq = ------------------ = exp (−G/RT) [NH3][HNO3] Keq = 1.4x1016 at 25°C; = 1.2x1019 at 0°C Solid ammonium nitrate (NH4NO3) is unstable except at high [NH3] and [HNO3] or at low temperatures. We see more NH4NO3 in the winter in East. Copyright © 2010 R. R. Dickerson 18 Ammonium Nitrate Equilibrium in Air = f(T) NH3(g) + HNO3(g) ↔ NH4NO3(s) – ln(K) = 118.87 – 24084 – 6.025ln(T) (ppb)2 1/Keq 298K = [NH3][HNO3] (ppb)2 = 41.7 ppb2 (√41.7 ≈ 6.5 ppb each) 1/Keq 273K = 4.3x10-2 ppb2 Water in the system shifts equilibrium to the right. Copyright © 2010 R. R. Dickerson 19 Aqueous ammonium concentration as a function of pH for 1 ppb gas-phase NHCopyright Seinfeld © 2010 R. R. and Pandis (1998). 3. From Dickerson 20 ⇗ Copyright © 2010 R. R. Dickerson Cloud 21 Radiative impact on stability: Aerosols reduce heating of the Earth’s surface, and can increase heating aloft. The atmosphere becomes more stable wrt vertical motions and mixing – inversions are intensified, Copyright © 2010 R. R. 22 convection (and rain) inhibited (e.g., Park et al., JGR., 2001). Dickerson Additional Fundamental Properties • Radiative effects of aerosols can accelerate photochemical smog formation. • Condensed–phase chemistry tends to inhibit smog production. • Too many ccn may decrease the average cloud droplet size and inhibit precipitation. • Dry deposition of NH3 and HNO3 are fast; deposition of particles is slow. Copyright © 2010 R. R. Dickerson 23 Nitrogen Deposition Past and Present mg N/m2/yr 5000 2000 1000 750 500 250 100 50 25 5 1993 1860 Galloway et al., 2003 Copyright © 2010 R. R. Dickerson 24 II. Local Observations Copyright © 2010 R. R. Dickerson 25 Fort Meade, MD Annual mean visibility across the United states (Data acquiredCopyright from the IMPROVE network) © 2010 R. R. Dickerson 26 Fort Meade, MD Copyright © 2010 R. R. Dickerson 27 Inorganic compounds ~50% (by mass) Carbonaceous material ~40% (by mass) Summer: Sulfate dominates. Winter: Nitrate/carbonaceous particles play bigger roles. Copyright © 2010 R. R. Dickerson 28 Copyright © 2010 R. R. of NO , NO -, and NH + at FME. 29 • Seasonal variation of 24-hr average concentration 4 y 3 Dickerson ISORROPIA Thermodynamic Model (Nenes, 1998; Chen 2002) Inputs: Temperature, RH, T-SO42-, T-NO3-, and T-NH4+ Output: HNO3, NO3-, NH3, NH4+, HSO4-, H2O, etc. Copyright © 2010 R. R. Dickerson 30 ISORROPIA Thermodynamic Model (Nenes, 1998; Chen, 2002) Inputs: Temperature, RH, T-SO42-, T-NO3-, and T-NH4+ Output: HNO3, NO3-, NH3, NH4+, HSO4-, H2O, etc. Copyright © 2010 R. R. Dickerson 31 (DataCopyright acquired 1999) © 2010inR.July R. Dickerson 32 (Water amount estimated by ISORROPIA) Copyright © 2010 R. R. Dickerson 33 Interferometer for NH3 Detection Schematic diagram detector based on heating of NH3 with a CO2 laser Copyright 2010 R. R. 34 tuned to 9.22 μm and a HeNe laser©interferometer (Owens et al., 1999). Dickerson Linearity over five orders of magnitude. Copyright © 2010 R. R. Dickerson 35 Response time (base e) of laser interferometer ∽ 1 s. Copyright © 2010 R. R. Dickerson 36 Copyright © 2010 R. R. Dickerson 37 *Emissions from vehicles important in urban areas. Copyright ©can 2010 be R. R. Dickerson 38 Summary: • Ammonia plays a major role in the chemistry of the atmosphere. • Major sources – agricultural. • Major sinks – wet and dry deposition. • Positive feedback with pollution – thermal inversions & radiative scattering. • Multiphase chemistry • Inhibits photochemical smog formation. • Major role in new particle formation. • Major component of aerosol mass. • Thermodynamic models can work. • Rapid, reliable measurements will put us over the top. Copyright © 2010 R. R. Dickerson 39 Nitrous Oxide, N2O SOURCES: Bacterial nitrification in soils and waters. Emissions from fertilized soils and animal feeding operations now dominate the global budget. Combustion was thought to be a major source (e.g., Hao et al. J. G. R. 1987), but work by Muzio and Kramlich (G. R. L., 1988) showed that SO2 and NO in the grab sampling cans can produce artifact N2O. Biomass burning, atmospheric ammonia oxidation, and industrial processes are minor sources. Copyright © 2010 R. R. Dickerson 40 Global averages of the concentrations of the major, well-mixed, long-lived greenhouse gases. http://www.esrl.noaa.gov/gmd/aggi/ Copyright © 2010 R. R. Dickerson 41 Copyright © 2010 R. R. Dickerson 42 CHEMISTRY: In the troposphere there is none! In the stratosphere nitrous oxide is broken down to molecular nitrogen or odd nitrogen, 90% through photolysis and about 10% through attack by electronically excited oxygen atoms. N2O + hυ → N2 + O N2O + O(1D) → 2 NO → N2 + O2 (1) (2a) (2b) Rxn 2a is the principal source of odd nitrogen and thus ozone destruction in the stratosphere. SINKS: Nitrous oxide in the stratosphere is converted to nitric oxide that eventually oxidizes to nitric acid. This nitric acid diffuses down to the troposphere where it can be rained out. Copyright © 2010 R. R. Dickerson 43 Atmospheric Nitrous Oxide Budget Stratosphere N2O + O(1D) → 2 NO HNO3 Troposphere N2O 1600 TgN HNO3 Oceans 3 Soils 6.6 Mankind (ag) 8.1 Earth’s surface Copyright © 2010 R. R. Dickerson 44 BUDGET: In pretty good shape because N2O is long lived, and can be accurately measured. Note in general the longer the lifetime of a species, the better the global budget. Atmospheric burden is given by [N2O] times the number of moles of air in troposphere times the molecular weight of N. The mean mixing is about 320 ppb, and relatively constant (σ/[N2O] = 0.5%) over the entire globe. 320x10-9 * 1.8x1020 * 28 = 1.6x1015 g = 1600 TgN Estimated source strength = 9-17 Tg(N) / yr Lifetime = 1600/17 to 1600/9 = 100 to 180 yr The mixing ratio (concentration) is growing at a rate of about 0.2% (1.4 ppb) per year, and N2O is a greenhouse gas with a global warming potential 300 times that of CO2. Copyright © 2010 R. R. Dickerson 45 An Unbalanced BUDGET: When fertilizer is applied to soils, about 0.5% of the N is quickly released as N2O and then the emission rate drops to a low level found in most soils. This number has been used to estimate that agriculture (crops plus animals) accounts for about 3 Tg N yr-1 The current N2O destruction rate is 11.9 Tg N yr-1. The rate of increase in the global atmospheric N2O burden is3.9 Tg N yr-1, thus the total emission rate has to be equal to the sum of these two or about 15.8 Tg N yr-1. Natural sources add up to about 10.2 Tg N yr-1 thus anthropogenic sources have to total 15.8 minus 10.2, or 5.6 Tg N yr-1. This is about 4% of the total N fixed by man each year of 127 Tg N yr-1. Crutzen et al. (2007) have used these facts to conclude that long-term N recycling in soils and waters leads to a total leakage of 4% of the originally applied N. If correct, this implies that N-rich biofuels have a greater warming impact than fossil fuels. Copyright © 2010 R. R. Dickerson 46 Mammals excrete urea: (NH2)2CO Copyright © 2010 R. R. Dickerson 47 What color was dinosaur poop? Many birds, snakes, and lizards, under great pressure to minimize their water use, burn a few additional ATP molecules to excrete uric acid rather than urea. Copyright © 2010 R. R. Dickerson 48 Uric Acid C5N4H4O3 An insoluble semi-solid that requires no water as a carrier. Copyright © 2010 R. R. Dickerson 49 Nest made of guano. Copyright © 2010 R. R. Dickerson 50