CHAPTER

2

INDUSTRIAL PROCESSES

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INDUSTRIAL PROCESSES

2. INDUSTRIAL PROCESSES
2.1

Overview
Greenhouse gas emissions are produced from a variety of industrial activities which are
not related to energy. The main emission sources are industrial production processes
which chemically or physically transform materials. During these processes, manydifferent greenhouse gases, including CO2, CH4, N2O, and PFCs, can be released.
Cement production is a notable example of an industrial process that releases a significant
amount of CO2. Different halocarbons (and SF6) are also consumed in industrial
processes or used as alternatives to ozone depleting substances (ODS) in various
applications. Table 2-1 gives an overview of potential industrial emission sources of
GHGs and ozone and aerosol precursors (NOx, NMVOCs, CO and SO2).
In some instances industrial process emissions are produced in combination with fuelcombustion emissions and it may be difficult to decide whether a particular emission
should be reported within the energy or industrial processes sector. Where the main
purpose of the fuel combustion is to use the heat released, the resulting emissions areincluded as energy emissions, not industrial process emissions. There are, however, somechemical processes or stages of processes, which oxidise carbon as a feedstock and areexothermic. The reduction of iron in a blast furnace through the combustion of coke isan example. Invariably the heat released is used within the processes or for other energy
needs of the producer. However, in this case, since the primary purpose of cokeoxidisation is to produce pig iron, the emissions are considered to be industrial.
In some cases not all fuel feedstock delivered to petrochemical plants is used for
manufacture of other products. Some feedstock may in fact be used for energy purposesin the sense that it is combusted for the heat released. This may be included as energy inthe national energy balance, but not necessarily. The separation of the feedstock andenergy uses and the identification of any fuel by-products from the processes is anotoriously difficult area of energy statistics.
Where a country has difficulty in distinguishing whether an emission is energy- or
industrial-based, compilers of industrial-process emissions statistics should liaise closelywith their energy counterparts and compare their basic data for fuel use in the industrial
processes to avoid double counting.
All emissions, including evaporative emissions, which occur in energy transformation
activities are discussed in the Energy Chapter. Emissions from petrochemical processes
are, however, covered in this chapter. Emissions of NMVOCs from use of solvents are
discussed in the chapter “Solvents and other product use” even if they originate from anindustrial process.
CO2 from use of biological carbon as feedstock and fermentation processes should not
be reported under “Industrial Processes” or any other sector of the IPCC Guidelines ifthey originate from sources of carbon that are from a closed cycle.
Non-combustion industrial processes resulting in N2O emissions are recognised asimportant anthropogenic contributors to global N2O emissions. It is estimated that thissource category represents 10 to 50 per cent of anthropogenic N2O emissions and 3 to20 per cent of all global emissions of N2O (IPCC, 1992). The main sources of industrial
anthropogenic N2O emissions are adipic acid and nitric acid production.

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Hydrofluorocarbons (HFCs), perfluorocarbons (PFCs) and sulphur hexafluoride (SF6) areused as alternatives to ozone depleting substances being phased out under the Montreal
Protocol. Current and expected applications of these compounds include refrigeration
and air-conditioning, fire extinguishing, aerosols, solvents, and foam production. Thesechemicals are either emitted instantaneously or slowly being leaked out over time. Manyof these compounds have high global warming potentials (GWPs) and long atmospheric
lifetimes. Consumption of HFCs, and to some extent PFCs and SF6, is expected to growsubstantially in the next decades due to their importance as substitutes for ozone
depleting substances.
HFCs, PFCs and SF6 are also emitted from industrial processes, such as production ofaluminium, magnesium and halocarbons (e.g., HCFC-22). In some countries PFC
emissions from industrial processes could be an important contributor to national GHG
emissions, due to high GWPs.
Much of the information on the greenhouse gases contained within this chapter is basedon four key documents: ”Anthropogenic Emissions of CO2, CH4 and N2O in Norway”,(Rypdal, 1993), “Greenhouse gas emissions in Norway”, Norwegian Pollution Control
Authority (1994), “Workbook for Industrial Emissions and Solvent Use”, National
Greenhouse Gas Inventory Committee, Australia (Workbook, Australia, 1995), and theprevious version of the Industrial Processes Chapter in the IPCC Guidelines for National
Greenhouse Gas Inventories (IPCC, 1995). In addition, several experts, within and outsideof the Industrial Processes Expert Group, have contributed to this chapter.

2.2

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INDUSTRIAL PROCESSESTABLE 2-1
POTENTIAL EMISSIONS FROM INDUSTRIAL PROCESSES.
Process

Greenhouse Gases
CO2

CH4

N2O

PFC

Ozone and Aerosol Precursors
SF6

HFC

NOx

NMVOC

CO

SO2

Mineral Products
Cement productionx

xLime productionx

x

Limestone use

xSoda Ash prod. and usexAsphalt roofing
Road paving
Other

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

Chemical industry
Ammoniax

Nitric acidxx

Adipic acid

x

x

Urea

x

Carbidesxx

Caprolactamxx

Petrochemicals

x

x

x

x

x

Metal Production
Iron, steel and ferroalloysxx

Aluminiumxx

Magnesiumx

Other metals

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

x

Other
Pulp and paper
Food and drink productionx

Production of halocarbons

x

x

x

Use of halocarbons and SF6

x

x

x

x

x

x

Other sources

x

x

x

x

x

The table does not necessarily cover all potential GHGs or industrial sources. A cross in the table does not imply that the emission estimations
methodology is available in this report or that the emission of a given source and gas is significant.

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2.2

General Methodology
2.2.1 Overview
The general methodology employed to estimate emissions associated with each industrial
process involves the product of activity level data, e.g., amount of material produced or
consumed, and an associated emission factor per unit of consumption/production
according to the following method:
TOTALij = Aj x EFij
where:TOTALij= process emission (tonnes) of gas i fromindustrial sector jAj= amount of activity or production of processmaterial in industrial sector j (tonnes/yr)EFij= emission factor associated with gas i per unit ofactivity in industrial sector j (tonne/tonne)

This general method represents the fundamental relationship to evaluate industrial
process emissions. It should be noted, however, that a number of mathematical steps
may be involved in reducing more complex mathematical formulae to the simplified formof the formula above. In cases where mathematical transformations are involved,
justifications are presented.
Often process emissions from a certain industrial sector are caused by emissions from a
few plants in each country. Therefore, measurement data are often available. Emission
estimates should be based on such data if they exist instead of a more generalised
methodology. Even if measurements are not available, calculations should preferably bebased on plant-specific data.

2.2.2

Approaches to Avoid Double Counting of
CO2

The IPCC Methodology for national GHG inventories requires an intentional double
reporting of NMVOCs, methane and carbon monoxide, firstly in their individual
inventories, and as CO2 equivalent in the national CO2 inventory. Whether an explicit
addition to the CO2 inventory is required depends on how the national CO2 inventory
has been calculated. Guidance on this point is contained under “Double Counting of
Emissions” (See Overview) contained in each volume of the IPCC Guidelines.

2.4

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2.3

Cement Production
2.3.1 Overview
Carbon dioxide emitted during the cement production process represents the mostimportant source of non-energy industrial process of global carbon dioxide emissions.
Cement production accounts for about 2.4 per cent of total global industrial and energy
CO2 emissions (Marland et al., 1989). Carbon dioxide is produced during the productionof clinker and intermediate product from which cement is made. High temperatures incement kilns chemically change raw materials into cement clinker (greyish-black pellets
about the size of 12 mm-diameter marbles). Specifically, calcium carbonate (CaCO3)
from limestone, chalk or other calcium-rich materials is heated, forming lime (calciumoxide or CaO) and carbon dioxide in a process called calcination or calcining:
CaCO3 + Heat → CaO + CO2
This lime combines with silica-containing materials, provided to the kiln as clays or shales,
to form dicalcium or tricalcium silicates, two of the four major compounds in cementclinker (Griffin, 1987). The clinker is then removed from the kiln, cooled, and pulverised
into an extremely fine grey powder. During this operation a small amount of gypsum isadded to regulate the setting time of the cement. The finished product is called"Portland" cement1.
It should be noted that when poured concrete is curing, some CO2 is reabsorbed by theconcrete from the atmosphere. This CO2 reabsorption is, however, believed to be onlya small fraction of the CO2 emission resulting from cement production and is therefore
usually ignored in emission calculations.
Most of the cement currently produced in the world is of Portland cement type, whichcontains 60 per cent to 67 per cent lime by weight. Other speciality cements are lower
in lime, but are typically used in small quantities. Research is underway on cement
formulations that have similar structural properties to Portland cement, but require lesslime (Tresouthick and Mishulovich, 1990). Carbon dioxide emissions from cement
production are essentially directly proportional to lime content, so production of
cements lower in lime yield less CO2.
Because CO2 is emitted during clinker production (rather than cement production itself),
emission estimates should be based on the lime content and production of clinker.
Estimating emissions based on the lime content and production of finished cement ignoresthe consideration that some domestic cement may be made from imported clinker, orthat some finished cement may use additional lime that is not accounted for in the cement
calculations. Clinker statistics, however, may not be readily available in some countries.
If this is the case, cement statistics can be used. The differences between the lime
content and production of clinker and cement, in most countries, are not significant enoughto affect the emission estimates.

1 In some countries, e.g., Japan, an effort has been made to substitute blast furnace slag

for lime. If this non-Portland type forms a significant quantity of cement production, it
can reduce the average emission factor.

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2.3.2 Emission Estimation Methodology for CO2
Estimation of CO2 emissions from cement production is accomplished by applying anemission factor, in tonnes of CO2 released per tonne of clinker produced, to the annual
clinker output.2 The emission factor (EF) is the product of the fraction of lime used in
the cement clinker and a constant reflecting the mass of CO2 released per unit lime.
EFclinker = Fraction CaO x (44.01 g/mole CO2 / 56.08 g/mole CaO)
or
EFclinker = Fraction CaO x 0.785

There are two methods for calculating this emission factor. The first is to assume anaverage CaO fraction in clinker. Since clinker is mixed with gypsum, which contains nolime per unit, to make cement, clinker has a higher lime percentage than finished cement.
The average clinker lime percentage has been estimated to be 64.6 per cent.3 This
number when multiplied by the molecular weight ratio of CO2/CaO (0.785) gives aclinker emission factor of 0.5071 tonnes of CO2/tonne of clinker produced.
EFclinker = 0.646 x 0.785 = 0.5071

A second method is to assemble country or regional data on clinker production by typeand clinker CaO content by type, then calculate a weighted average for cement lime
content in the country. In most countries, the difference in the results of these two
methods is likely to be small; any error in the lime content assumption is likely to besmaller than the uncertainty in clinker and cement production figures (Griffin, 1987).
If information on clinker production is not readily available, an emission factor in tonnesof CO2 released per tonne of cement produced can be applied to annual cement
production instead. This approach has been followed by Marland et al. (1989), who took
the average CaO content of cement to be 63.5 per cent, yielding an emission factor of
0.4985 CO2/cement (0.136 tonne CO2 as C/tonne cement).
EFcement = 0.635 x 0.785 = 0.4985

Additional research indicates that "masonry cement", as opposed to "Portland cement",
requires additional lime, over and above the lime used in its clinker. The following
formula can be used to account for this activity:

2 Note that the estimation of CO

2 from energy use during cement production is
explained in the energy chapter; these emissions should be reported under Energy: Fuel
Combustion activities.

3 Gregg Marland, ORNL, personal communication.

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a x (All Cement Production) x ((1-1/(1+b)) x c) x 0.785=
tonnes CO2 from CaO added to masonry cement
where:a=fraction of all cement produced that is masonry cement (e.g., 0.10.2)b=fraction of weight added to masonry cement by non-plasticiser
additives such as lime, slag, and shale (e.g., 0.03, 0.05)c=fraction of weight of non-plasticiser additives that is lime (e.g., 0.60.8)

a x (All Cement Production) = masonry cement production((1-1/(1+b)) x c) = fraction of lime in masonry cement
not attributable to clinker((1-1/(1+b)) x c) x 0.785 = an emission factor of CO2 frommasonry cement additives

The recommended method for estimating CO2 emissions from cement production is tomultiply the most reliable figures available for tonnes of clinker produced by an emission
factor of 0.5071 tonne CO2/tonne clinker. Alternatively, cement production can be
multiplied by an emission factor of 0.4985 tonne CO2/tonne cement.
International cement production data are available from the United Nations (1988) andfrom the U.S. Bureau of Mines (1988). In some countries, national data may be available
from appropriate government ministries. There is substantial overlap between the U.S.
Bureau of Mines and the UN data sets, but the former is more complete. Publishedinformation is also available from the European Cement Association (CEMBUREAU,
1990).

2.3.3 Emissions Estimation Methodology for SO2
EMEP/CORINAIR has classified cement production as both an industrial combustion andan industrial process (SNAP codes 30311 and 40612, respectively). However, nodescription of emission factors for the non-combustion emissions are presented. A
default methodology is, therefore, presented below.
SO2 emissions will originate from sulphur in the fuel and in the clay raw material. Most
(about 70-95 per cent) of the SO2 generated in the process will be absorbed in the
produced alkaline clinker (U.S. EPA 1995). The fuel emissions are counted as energy
emissions while the SO2 from the clay should be counted as non-combustion emissions.
A non-combustion emission factor of 0.3 kg SO2/tonne cement has been calculated frommeasurements in Norwegian plants (Rypdal 1995). This factor may vary from plant toplant as the sulphur content of raw materials and degree of absorption will vary. If noinformation on sulphur content and degree of absorption is available and there are nomeasurement data, a factor of 0.3 kg SO2/tonne cement is suggested.

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2.4

Lime Production
2.4.1 Overview
Calcined limestone (or quicklime) is formed by heating limestone to decompose thecarbonates. This is usually done at high temperatures in a rotary kiln and the process
releases carbon dioxide. Depending on the product requirements (e.g., metallurgy, pulp
and paper, construction materials, effluent treatment, water softening, pH control andsoil stabilisation), primarily high calcium limestone (calcite) is processed in this mannerfrom the quarried limestone to produce quicklime in accordance with the following
reaction:
CaCO3 (limestone) + heat → CaO (quicklime) + CO2

Hydrated (slaked) lime is also produced, with additional hydration operations, at somefacilities. Dolomitic limestone or magnesite may also be processed at high temperature
to obtain dolomitic lime (and release CO2) in accordance with the following reaction:
CaCO3.Mg CO3 (dolomite) + heat → CaO.MgO (dolomitic lime) + 2CO2

The production of lime involves a series of steps comparable to those used in the
production of Portland cement clinker. These include quarrying the raw materials,
crushing and sizing, calcining (i.e., high temperature heat processing ~ 1100° C) the raw
materials to produce lime, hydrating the lime to calcium hydroxide followed bymiscellaneous transfer, storage and handling operations.

2.4.2

Emissions
CO2

Estimation

Methodology

for

The mass of CO2 produced per unit of lime manufactured may be estimated from themolecular weights and the lime content of products. On the basis of the calcination
reaction, one mole of carbon dioxide is formed for each mole of quicklime produced
from burning calcium carbonate. This was used to derive an emission factor based on theamount of quicklime produced (ORTECH, 1991), assuming complete dissociation of the
carbonate rock and no reabsorption of CO2 by lime in the kiln. In instances where
dolomitic limestone is calcined, the emission factor was derived based on the lime:
magnesia product (ORTECH, 1991). The emission factors are tabulated in Table 2-2.
For high calcium lime, CO2 emissions are estimated according to:
EF = 44.01 g/mole CO2 /56.08 g/mole CaO= 785 kg CO2 /tonne high calcium lime

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For dolomitic lime, CO2 emissions are estimated according to:
EF = 2 x 44 .01 g/mole CO2 /96.39 g/mole CaO • MgO= 913 kg CO2 /tonne dolomitic lime
The coefficient 2 relates to the stoichiometric ratio of CO2 to CaO.MgO in the
calcination process.
Both formulas assume pure lime, but in some cases the purity may range from 85 to 95
per cent (Workbook, Australia, 1995). In these cases, the formulas should be adjusted
according to the lime purity.

TABLE 2-2
SUMMARY OF EMISSION FACTORS
Process

Component

Lime Kiln-Calcite Feed

CO2

0.79 tonnes CO2/tonnes
quicklime produced

ORTECH, 1991

Lime
Feed

CO2

0.91 tonnes CO2/tonnes
dolomitic lime

ORTECH, 1991

Kiln-Dolomite

Emission Factor

Reference

The consumption of lime may in cases result in the removal of CO2 from theatmosphere. The use of hydrated lime (for water softening) for example, results in CO2
reacting with lime to form calcium carbonate. Lime is also used as a CO2 absorbent foratmospheric control in the storage of fruit. At this time, data is not available to reliably
estimate the extent of atmospheric CO2 removal from the use of lime.

2.4.3 Emissions Estimation Methodology for SO2
Details for deriving emissions for this sector are not yet available. SO2 should beconsidered. The non-combustion emissions will depend on the sulphur content andmineralogical form (pyrite or gypsum) of the stone feed, the quality of the lime produced
and the type of kiln (U.S. EPA 1995). In this process, SO2 emissions from combustion willusually exceed the non-combustion emissions (U.S. EPA 1995). Until more information
becomes available, it is recommended that only emissions from fuel combustion (Energy
Chapter) are considered.

2.5

Limestone and Dolomite Use
2.5.1 Overview
Limestone (CaCO3) and dolomite (CaCO3.MgCO3) are basic raw materials having
commercial applications in a number of industries including metallurgy (e.g., iron andsteel), glass manufacture, agriculture, construction and environmental pollution control.
In industrial applications involving the heating of limestone or dolomite at hightemperatures, CO2 is generated.

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CO2 from liming of soils should be reported in the Land-use Change and Forestry
Chapter. Limestone and dolomite used in cement and lime production should bereported under that industry sector. Under this section are inventoried all other uses oflimestone and dolomite which produce CO2 emissions.

2.5.2 Emissions Estimation Methodology for CO2
The mass of CO2 emitted from the use of limestone and dolomite may be estimated froma consideration of consumption, purity of the raw materials and the stoichiometry of thechemical processes.
Emission factor, EFls, for limestone use:
EFls = f x [44.01 g/mole CO2] / [(100.09 g/mole CaCO3)]= (440 x f ) kg CO2 / tonne limestonewhere:
f is the fractional purity of limestone in CaCO3 per tonne of total raw material
weight (if unknown, the default factor for f is equal to 1).
Emission factor, EFls, for dolomite use:
Efd = f x [2 x 44.01 g/mole CO2] / [(184.41 g/mole CaCO3MgCO3)]= (477 x f) kg CO2 / tonne dolomite

The total CO2 emission from limestone and dolomite use in Gg/yr calculated as:
TotalId = {(Als x EFls) + (Ad x EFd) }/106= {(440 x f x Als) + (477 x f x Ad)}/106

where:
Totalld is the process emission of CO2 from limestone and dolomite use (Gg/yr)
Als is the consumption of limestone (tonnes/yr). Consumption is assumed to equalmaterial mined (or dredged) plus material imported minus material exported. The
consumption entering this calculation excludes limestone used for producing cement
and lime, agriculture and processes where CO2 is not generated.
Ad is the consumption of dolomite (tonnes/yr). Consumption is assumed to equalmaterial mined plus material imported minus material exported. The consumption
entering this calculation excludes limestone used for producing lime and magnesium,and processes where CO2 is not generated.

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2.6

Soda Ash Production and Use
2.6.1 Overview
Soda ash (sodium carbonate, Na2CO3) is a white crystalline solid that is used as a raw
material in a large number of industries including glass manufacture, soap and detergents,
pulp and paper production and water treatment. Carbon dioxide is emitted from the useof soda ash, and may be emitted during production, depending on the industrial processused to manufacture soda ash.
Emissions of CO2 from the production of soda ash vary substantially with the
manufacturing process. Four different processes may be used commercially to produce
soda ash.
Three of these processes, monohydrate, sesquicarbonate and direct
carbonation, are referred to as natural processes. The fourth, the Solvay process, isclassified as a synthetic process.
About 25 per cent of the world production is produced from natural sodium carbonatebearing deposits referred to as natural processes. During the production process, trona(the principal ore from which natural soda ash is made) is calcined in a rotary kiln andchemically transformed into a crude soda ash. Carbon dioxide and water are generated
as by-products of this process. Carbon dioxide emissions can be estimated based on thefollowing chemical reaction:
Na2CO3 x NaHCO3 x 2H2O→ 3Na2CO3 + 5H2O + CO2
Trona

Soda Ash

According to this reaction, it takes 10.27 tonnes of trona to produce 1 tonne of carbon
dioxide. Hence, for natural soda ash production, emissions of carbon dioxide can becalculated by the following formula:
EF = 0.097 tonne CO2 / tonne of Trona

About 75 per cent of the world production is synthetic ash made from sodium chloride.
In the Solvay process, sodium chloride brine, limestone, coke and ammonia are the raw
materials in a series of reactions leading to the production of soda ash. Ammonia,
however, is recycled and only a small amount is lost. The series of reactions involved in
the Solvay process may be presented as follows:
CaCO3 + heat → CaO + CO2
CaO + H2O → Ca(OH)2
NaCl + H2O + NH3 + CO2 → NaHCO3 + NH4Cl
2NaHCO3 + heat → Na2CO3 + CO2 + H2O
Ca(OH)2 + 2NH4Cl → CaCl2 + 2NH3 + 2H2O

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CaCO3 + 2NaCl → Na2CO3 + CaCl2

From the series of reactions presented above, CO2 is generated in two pyrolysis
processes. The CO2 generated is captured, compressed and directed to Solvay
precipitating towers for consumption in a mixture of brine (aqueous NaCl) and ammonia.
Although CO2 is generated as a by-product, the carbon dioxide is recovered and recycled
for use in the carbonation stage and in theory the process is neutral, i.e., generation of
CO2 equals uptake.
In practice, however, CO2 is emitted to the atmosphere during the production of soda
ash because more CO2 is produced than is stoichiometrically required. The excess CO2
is produced by calcining limestone with metallurgical grade coke (approximately 7 percent of limestone weight). In order to avoid double counting, CO2 emissions associatedwith the use of coke in soda ash production should be accounted for separately and thoseemissions associated with the non-energy use of coke subtracted from the totals in the
combustion section.
Carbon dioxide emissions are associated with the use of soda ash. Some of the major
uses include glass manufacture, chemicals, soaps, detergents and flue gas desulphurisation.
For each of these uses, it is assumed that for each mole of soda ash use, one mole of
CO2 is emitted (U.S. EPA, 1994b).

2.6.2 Emission Estimation Methodology for CO2
Soda Ash Production
From stoichiometric considerations, the industrial process emission of CO2 associatedwith the Solvay process is zero. The excess CO2 emitted from soda ash production
originates from coke oxidation (see the Energy Chapter for appropriate emission rate forcoke combustion and use appropriate national statistics on coke use in soda ash
production). For processes utilising trona, emissions can be calculated by the following
formula:EF = 0.097 tonne CO2 / tonne of Trona

During the production of soda ash in the Solvay process, calcium chloride is produced. In
cases where calcium chloride is discharged to the sea, calcium chloride dissolves to form
calcium and chloride ions. Calcium ions in turn take part in a number of chemical
reactions, including the sequestering of carbonate ions to form calcium carbonate which
represents a sink for CO2. Available experimental data from Australia indicate thatapproximately 0.23 tonnes of CO2 is sequestered from the ocean for each tonne of soda
ash produced (Workbook, Australia, 1995).

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Soda Ash Use
For each mole of soda ash use, one mole of CO2 is emitted, so that the mass of CO2
emitted from the use of soda ash may be estimated from a consideration of consumption
data and the stoichiometry of the chemical process as follows:
EF = 44.01 g/mole CO2 /105.99 g/moleNa2CO3= 415 kg CO2/tonne Na2CO3

2.7

Production
andMineral Products

Use

of

Miscellaneous

2.7.1 Asphalt Roofing Production
This is the production of saturated felt, roofing and siding shingles and roll roofing andsidings. Most of these products are used in roofing and other building applications.
Emissions from these processes can be estimated from the national total mass of
products. The emission factors in Table 2-3 given in the EMEP/CORINAIR Guidebook(SNAP 40610) are default factors.

TABLE 2-3
EMISSION FACTORS FOR ASPHALT ROOFING PRODUCTION (KG/TONNE PRODUCT)
Emission Factor(Saturation with Spray)

Emission Factor(Saturation without Spray)

0.13 - 0.16

0.046 - 0.049

NAV

0.0095NMVOC
CONAV = Not Available

Asphalt blowing (SNAP 60310) is the process of polymerising and stabilising asphalt toimprove its weathering characteristics. Air blown asphalts are used in the production ofasphalt roofing products. The blowing may take place in a refinery, an asphalt processing
plant or an asphalt roofing plant. This activity leads to emissions of NMVOC. The
emission factors in the EMEP/CORINAIR Guidebook range from 0.1 to 30 kg totalorganic compounds/tonne asphalt blown depending on the degree of control and it may
be assumed that all the mass of asphalt used for non-paving use will be blown.

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2.7.2 Road Paving with Asphalt
Asphalt road surfaces are composed of compacted aggregate and asphalt binder. Gases
are emitted from the asphalt plant, the road surfacing operations and from thesubsequent road surface. The emissions of NMVOC depend on the type of asphalt (slow,
medium or rapid cure) and the amount of diluent. Emission factors given in Table 2-4 use
the default assumptions given in the EMEP/CORINAIR Guidebook (SNAP 40611). The
amount of diluent used is usually lower in warm countries than in the colder, and hence
lower emission factors may be expected in warm countries.

TABLE 2-4
EMISSION FACTORS FOR ROAD PAVING WITH ASPHALT ( KG/TONNE ASPHALT)
SO2

NOx

CO

NMVOC

Asphalt Plant

0.12

0.084

0.035

0.023

Road Surface

NAV

NAV

NAV

320

If the tonnes of asphalt paved is not known but rather the area paved, a conversion factorof 100 kg asphalt/m2 road surface may be used.

2.7.3 Production of Other Mineral Products
There may be several other mineral production processes emitting pollutants. These areprobably not significant on a global scale, but may be significant on a national or local
scale. There is generally little information about emissions from these processes.
One emission source is the production of concrete pumice stone. As for cement
production, SO2 emissions will originate from the fuel use and sulphur in clay. About 45
per cent of the SO2 generated in the process will be sequestered in the product. An
emission factor of about 0.5kg SO2/tonne product has been calculated frommeasurements in Norwegian plants (Rypdal 1995), and used where plant-specific data are
not available.
NMVOCs may be emitted from manufacture of glass. An emission factor of 4.5 kg/tonne
product has been derived from CASPER (1995).

2.8

Ammonia Production
2.8.1 Overview
In most instances, anhydrous ammonia is produced by catalytic steam reforming of naturalgas (mostly CH4) or other fossil fuels. As can be seen in the following reactions withmethane as a feedstock, carbon dioxide is produced.
C + H2O → CO + H2
CH4 + H2O → CO + 3H2
N2 + 3H2 → 2NH3

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In general, the processes that affect CO2 emissions in the production of ammonia are:• carbon monoxide shift at two temperatures using iron oxide, copper oxide and/or
chromium oxide catalyst for conversion to carbon dioxide;• carbon dioxide absorption by a scrubber solution of hot potassium carbonate,monoethanolamine (MEA), Sulfinol (alkanol amine and tetrahydrothiophene dioxide)or others;• methanation of residual CO2 to methane with nickel catalysts to purify the synthesisgas.
Natural gas is used as the feedstock in most plants, while other fuels (e.g., heavy oils) may
be used with the partial oxidation process. In addition, plants may use by-producthydrogen, rather than natural gas, to produce ammonia (thereby eliminating the releaseof CO2 from the synthesis process) (CFI, 1992). The production of ammonia represents
a significant non-energy industrial source of CO2 emissions.

2.8.2 Process Description
The primary release of CO2 at plants using the natural gas catalytic steam reforming
process occurs during regeneration of the CO2 scrubbing solution with lesser emissions
resulting from condensate stripping.
Carbon Dioxide Regenerator
After absorption of CO2 from the process gas, the saturated scrubbing solutions (e.g.,potassium carbonate, MEA, etc.) are regenerated (i.e., for re-use) with steam stripping
and/or boiling to release CO2 from the bicarbonates according to the following reactions:
Heat
Heat

2KHCO3 → K2CO3 + H2O + CO2(C2H5ONH2) 2 + H2CO3 → 2C2H5ONH2 + H2O + CO2

The stripping gas, containing CO2 and other impurities, may be directed to a urea plant(where operational), to a liquid carbonic acid plant, or vented to the atmosphere(Environment Canada, 1987).
Condensate Stripper
Cooling the synthesis gas after low temperature shift conversion forms a condensate
containing small quantities of CO2 and other process impurities. The condensate is
stripped by steam, whereby the components may be vented to the atmosphere, but
normally recycled to the process together with the process stream (U.S. EPA, 1985).

2.8.3 Emission Estimation Methodology for CO2
Emissions of CO2 will depend on the amount and composition of gas (or oil) used in theprocess. It is assumed that all carbon will be emitted to air. It is recommended thatinventory contributions are compiled using point source methods due to the rather
limited number of plants. Where greatest accuracy is desired, this will require directcontact with producers. Alternatively, total sector emissions may be determined on anarea source basis using available emission factors and methods noted below.

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The most accurate method of estimation will be:
Emission (kt) = Consumption of gas (kt) x carbon content x 44/12

If the gas consumption is not available, an alternative is to calculate the emissions fromthe ammonia production:
Emission (kt) = Production of ammonia x Emission factor

In both cases, in order to avoid double counting, the quantities of oil or gas used must be
subtracted from the quantity reported under energy and non-energy use in the Energy
Chapter.
The CO2 from ammonia production may be used for producing urea or dry ice. This
carbon will only be stored for a short time. Therefore, no account should consequently
be taken for intermediate binding of CO2 in downstream manufacturing processes andproducts.
Emission Factor Information
If the emissions are calculated from the gas or oil consumption, the standard emission
factors suggested in the energy chapter will be relevant. The carbon content of natural
gas may vary, and it is recommended that this is determined for each plant.
Some emission factors related to the production of ammonia are shown in Table 2-5.

TABLE 2-5
AMMONIA PRODUCTION EMISSION FACTORSCountry

Emission Factor a,b
Tonne CO2/tonne NH3 produced

Reference

Canadac

1.6

Jaques, 1992
Industrial Chemicals, 1980

Norway1.5

Norsk Hydro, 1996

a Reductions should be applied to account for any ammonia that is produced from by-product hydrogen.
b Figure for Norway excludes gas used as a fuel. It is not clear if this is included in the Canadian figure. The figures
are dependent on the carbon content in the feedstock.
c Assumes 812 m3 gas/tonnes NH3 and 0.525 kg carbon/m3 gas.

2.8.4

Emission
Estimation
Methodology
Ozone Precursors and SO2

for

The production of ammonia is described in Section 2.8.1. However, emission methods
have not yet been developed for the EMEP/CORINAIR Guidebook (SNAP 40403).
SO2, NOx, CO and NMVOC may be emitted in addition to CO2. Default emission
factors for uncontrolled emissions in Table 2-6 are taken from U.S. EPA 1995.

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INDUSTRIAL PROCESSESTABLE 2-6
EMISSION FACTORS FOR AMMONIA PRODUCTION(KG/TONNE PRODUCT)
SO2

TOC a

CO

Desulphurisation

0.03

3.6

6.9

Carbon dioxide regenerator

NE

0.5

1.0

Condensate steam stripper

NE

0.6

NE

Total

0.03

4.7

7.9

a Total organic compounds
NE = negligible

There will usually be few ammonia plants in a country, and it is recommended thatemissions from plant specific data be estimated.

2.9

Nitric acid Production
2.9.1 Overview
The production of nitric acid (HNO3) generates nitrous oxide (N2O) as a by-product of
the high temperature catalytic oxidation of ammonia (NH3).
Nitric acid is used as a raw material mainly in the manufacture of nitrogenous-based
fertiliser. Nitric acid may also be used in the production of adipic acid and explosives(e.g., dynamite), for metal etching and in the processing of ferrous metals.
Nitric acid production involves three distinct chemical reactions:
4NH3 + 5O2 → 4NO + 6H2O
2NO + O2 → 2NO2
3NO2 + H2O → 2HNO3 + NO

Nitrous oxide generation during the production of nitric acid is not well documented.
Nitrogen oxidation steps under overall reducing conditions are considered to be potential
sources of N2O. Nitric oxide (NO), an intermediate in the production of nitric acid, isalso documented to readily decompose to N2O and nitrogen dioxide (NO2) at highpressures for a temperature range of 30 to 50°C (Cotton and Wilkinson, 1988).

2 . 9 . 2 E m i s s i o n D a t a o f N 2O
Table 2-7 gives examples of emissions factors from nitric acid production plants, based on
measurements. Emission rates depend upon technology and operating conditions.

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INDUSTRIAL PROCESSESTABLE 2-7
EMISSION FACTORS FOR N2O FROM NITRIC ACID PRODUCTION
Emission Factor
kg N2O/tonne nitric acid

Reference

USA

2-9 a

Reimer et al., 1992

Norway: - modern, integrated plants<2

Norsk Hydro, 1996

- atmospheric pressure plants

4-5“- medium pressure plants

6-7.5

”

2.2-5.7

Japan Environment
Agency, 1995

Japan

a. Emission factors up to 19 kg N2O/tonne nitric acid have been reported for plants not equipped with nonselective catalytic reduction technology (NSCR) (Choe et al., 1993; Olivier, 1996; Oonk, 1996).

2 . 9 . 3 E m i s s i o n E s t i m a t i o n M e t h o d o l o g y f o r N 2O
There are usually only very few plants in each country producing nitric acid, so measured
data on N2O emissions are often available. These data also take into account the effectof any abatement technology installed at the specific plants. Emissions vary significantly
from one plant to another, and if measured data are available, emission estimates should
be based upon such data. Every effort should therefore be made to obtain measurement
data.
However, if such data are not available, emissions should be calculated from production
data of nitric acid within a country, and specific emission figures based on the actualtechnology, for which Table 2-7 can be consulted. When no measured data exist, specificemission factors at the upper end of the appropriate range should be chosen.
N2O-emissions = Production level x Specific Emission Factor

2.9.4 Emission Estimation Methodology for NOX
Nitric acid is produced from the catalytic oxidation of ammonia. The process is describedin Section 2.9.1 and in the EMEP/CORINAIR Guidebook (under SNAP 40402). In
addition to the GHGs described in Section 2.9.1, there may be non-combustion emissionsof NOx.
Emissions are estimated from the amount of nitric acid produced. Factors range from
0. 1- 1.0 NOx/tonnes acid produced for the direct strong acid production process to 1020 kg/tonnes acid produced for the low pressure process. 12.0 kg NOx/tonnes nitric acidshould be used where the process and technology details are not known.
There will usually be few nitric acid plants in a country, and it is recommended thatemissions are calculated from plant specific data.

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2.10 Adipic Acid Production
2.10.1 Overview
Adipic acid is used in the manufacture of a large number of products including synthetic
fibres, coatings, plastics, urethane foams, elastomers and synthetic lubricants. The
production of Nylon 6.6 accounts for the bulk of adipic acid use.
Adipic acid is a dicarboxylic acid manufactured by a two-stage process. The first stage ofmanufacturing involves the oxidation of cyclohexane or cyclohexanone to form acyclohexanone/cyclohexanol mixture. The mixture is then oxidised by nitric acid in thepresence of a catalyst to form adipic acid. N2O is generated as a by-product of the nitricacid oxidation stage:(CH2)5CO+(Cyclohexanone)(CH2)5CHOH(Cyclohexanol)

+

wHNO3

→
HOOC(CH2)4COOH (Adipic Acid) + xN2O + yH2O

Adipic acid production also results in the emissions of NMVOC, CO and NOx. Process
emissions from the production of adipic acid vary substantially with the level of emission
control employed.

2.10.2Emission
N 2O

Estimation

Methodology

for

Adipic acid production unavoidably produces N2O as a by-product with an associatedemission factor (for unabated emissions) of 300g N2O/kg adipic acid produced (Thiemens
and Trogler, 1991). Japanese emissions (measured at 264 g N2O/kg adipic acid) areconsistent with this value (Japan Environment Agency, 1995).
N2O emissions (kg) = Adipic Acid Production(tonnes)
x 300 kg N2O/ tonne Adipic Acid

Often, the abatement of N2O results from the treatment of the off-gases4 in a reductive
furnace. A number of adipic acid producers treat the off-gases with the aim of reducing
NOx emissions, but the treatment also destroys N2O (Reimer et al., 1992).
There is a range of abatement efficiencies attainable with currently available technologies.
Any reduction in N2O emissions due to the installation of abatement systems should beassessed on a plant-specific basis where possible.

4 “Off-gases” are gases that are released from the process.

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2.10.3Emission
Estimation
Ozone Precursors

Methodology

forThe production of adipic acid is described in Section 2.10.1 and (under SNAP 40521) inthe EMEP/CORINAIR Guidebook.
The EMEP/CORINAIR Guidebook indicates that there may be emissions of CO2, NO andNO2 in addition to N2O, but does not propose emission factors at present.
Furthermore, European reported emission data indicate that pollutants other than N2O
are not significant (CORINAIR-90). U.S. EPA emission factors are given in Table 2-8(U.S. EPA 1995).

TABLE 2-8
EMISSION FACTORS FOR ADIPIC ACID PRODUCTION ( KG/TONNE PRODUCT)
NOX

CO

VOC

8.1

34.4

43.3

2.11 Carbide Production
2.11.1CO2 and
CH4
Production

fromSiliconCarbideIn the production of silicon carbide, CO2 is released as a by-product from a reaction
between quartz and carbon. Petrol coke is used as a carbon source. Silicon carbide isextremely hard and is widely used as an abrasive. The formula describing the reaction is
given below but in practice it does not proceed in the stoichiometric proportions
indicated.
O2

SiO2 + 3C → SiC + 2CO → 2CO2Some carbon, about 35 per cent, is sequestered in the product.
Generally, the emissions from silicon carbide production can be calculated from a massbalance approach as:
CO2 emissions (tonnes) = A x C (100-S) x 3.67 x 10-4

where:

2.20

A= consumption of coke in tonnesC= per cent carbon content in cokeS

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