Chapter 1: Hydrogen Generation Flashcards

1
Q

Examples of oil spills

A
  • Exxon Valdez (Alaska, 1989)
  • BP (Gulf of Mexico, 2010)
  • Mauritius oil spill (2020)
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2
Q

Combustion engine by-products:

A
  • CO (carbon monoxide)
  • NOx (Urban Smog)
  • Unburned hydrocarbons (urban ozone)
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3
Q

1 Gallon of gas is equivalent to…

A

20 lbs CO2

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4
Q

‘Hydrogen Economy’

A

Potentially the future of energy in a system where hydrogen is used as the primary energy carrier and used for a wide range of applications.

It has the potential to significantly reduce greenhouse gas emissions.

There are many technical, infrastructural, and economic challenges to overcome.

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5
Q

Advantages of the ‘Hydrogen Economy’

A
  • Elimination of pollution caused by fossil fuel
  • Elimination of greenhouse gases
  • Elimination of economic dependence
  • Distributed and localized production
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6
Q

Where does the hydrogen come from?

A
  • Reforming of hydrocarbons
  • Reforming of biomass
  • Pyrolysis
  • Electrolysis of water

Hydrogen must be derived from renewable sources

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7
Q

Current uses of Hydrogen

A
  • NH3, HCl, CO(NH2)2, and other commodities
  • Fertilizers
  • ‘Bosch-Meiser’
    2NH3 + CO2 <=> H2N-COONH4
    H2N-COONH4 <=> (NH2)2CO + H2O
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8
Q

Ways to create electricity

A
  • Nuclear power
  • Hydroelectric dams
  • Wind turbines
  • Wave and tidal power
  • Geothermal power
  • Solar cells
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9
Q

Safety aspect of hydrogen as a fuel

A
  • Colourless and odourless
  • Low ignition energy
  • High flame temperature
  • Invisible flame in daylight conditions
  • Negative Joule Thompson Coefficient, (i.e. a leak may self ignite
  • Small molecular size (2.016 g/mol vs.vs.~107.0 g/mol for gasoline
  • Wide range of lower explosive limit to upper explosive limit (4.0 75.0 volume%)

However, hydrogen is less flammable than gasoline and other fossil fuels

Liquid hydrogen: spilling –> Burns, explosions

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10
Q

Safety factors to be considered for hydrogen as a fuel

A
  • Catastrophic rupture of the tank
  • Mixture of fuel cells reactant in the cells
  • Leaks due to punctures, faulty controls, stress cracks, etc.
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11
Q

How to prevent accidents involving hydrogen:

A
  • Testing tanks and equipment (leak prevention)
  • Installing more valves
  • Designing equipment for shocks, vibrations and wide T ranges
  • Inserting H 2 , O 2 , and leak detectors
  • Keeping fuel cells supply lines physically separated from other equipment
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12
Q

Methods for producing hydrogen:
Steam Reforming (most common)

A

(1) CH4 + H2O ==> CO + 3H2 (+ 206.4 kJ/mol)
Catalyst : Ni , highly endothermic, T = 700 - 1100

(2) CO + H2O ==> CO2 + H2 (-41, kJ/mol)
Catalyst: Fe, Cr Oxides, mildly exothermic, water gas-shift reaction

Heat needed in (1) is provided by
(3) CH4 + 2O2 ==> CO2 + 2H2O (-880 Kj/mol)

Combining (1) and (2)
(4) CH4 + 2H2O (+165 kJ/mol) ==> CO2 + H2
Efficiency: 65% - 75%

CO (traces) and CO2 are removed using adsorption processes “pressure swing adsorption”

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13
Q

Disadvantage of steam reforming to produce hydrogen

A

Costs: still 2-3 times higher than producing gasoline from
crude oil Improving

Steam (methane) reforming not to be confused with catalytic reforming of naphta (octane gasoline and H2 as a by product)

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14
Q

Methane Cracking

A

CH4 + 74.9 KJ/mol ==> C + 2H
(Excess of steam is effective in preventing coke formation)

2CO ==> C + CO2 + 172.4 KJ/mol
Carbon Contamination

Current natural gas steam reforming is not aimed at fuel cell use of
H2 produced, so CO is not eliminated

Commonly in SMR: CO: 0.3-3%
CO: in the range of 10-50 ppm

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15
Q

Partial Oxidation Reforming
(6) reactions

A
  • CH4 + 1/2 O2 ==> CO = 2H2 (-35.7 kJ/mol)
    Exothermic , partial oxidation
  • CH4 + O2 ==> CO2 + 2H2 (-319.1KJ/mol)
    Exothermic, partial oxidation
  • CH4 ==> C + 2H2 (+75 KJ/mol)
    Endothermic, Thermal decomposition

CH4 + 2O2 ==> CO2 + 2H2O (liq) (-880 KJ/mol)
Exothermic, Methane Combustion

CO + 1/2 O2 ==> CO2 (-283.4 KJ/mol)
Exothermic, CO combustion

H2 + 1/2 O2 ==> H2O (liq) (-286 KJ/mol)
Exothermic, H2 combustion

Complete combustion: CO2 , H2O; no H2 , CO, O2 or fuel
Incomplete combustion: H2 , CO (in the presence of a catalyst)

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16
Q

Example of combustion: Conservation of mass

A

The number of moles of H, C, and O must be equal on both sides of the equation.

Stochiometry

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17
Q

Autothermal Reforming

A

It is a combination of:
- Steam reforming reaction
- Partial oxidation reaction
- The water gas-shift reaction

(1) in the same chemical reactor
(2) The heat required by the (endothermic) SR and WGS reaction is exactly provided by the (exothermic) POX reaction
(3) Steam (for SR) as a reactant
(4) Substoichiometric amount of O2 for (POX)

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18
Q

Autothermal Reforming: Reaction

A

CxHy + zH2O (l) + (x-0.5z)O2 <===> xCO2 + (z+0.5y)H2

z/x = steam to carbon ratio

It should be chosen such that the reaction is energy neutral
(neither exothermic nor endothermic)

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19
Q

Coal Gasification : Reaction

A

C + aO2 + bH2O <===> cCO2 + dCO + eH2 + “other species”

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20
Q

Coal Gasification: Devolatilisation

A

From carbon to complex gaseous mixture and porous solid char residue

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21
Q

Coal Gasification: gaseous mixture

A

Combination of partial oxidation, SR, and WGS reactions

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22
Q

Coal Gasification: Char Particles

A

Gasified to CO through partial oxidation of C

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23
Q

Absorption force and Adsorption force:

A

Weakest: Hydrogen/Helium, Oxygen

Strongest: Water

24
Q

CO cleanup

A

Reformative stream: CO = 0.2% (2000 ppm)
Fuel cell catalyst tolerance: CO = 1-10 ppm

Goal: Reduce CO yield to extremely low level

Physical separation: Pressure swing adsorption, Palladium membrane separation

Chemical reaction: Selective methanation of CO
Selective oxidation of CO

25
Selective Methanation
- Manage heat of reaction - Designing a catalyst that maintains its activity after prolonged exposure to high T (1) CO + 3H2 <==> CH4 + H2O Catalyst: Co, Fe, Ru; highly exothermic; Δ H= 206.1KJ/mol Reduce CO and H2 yield (2) CO2 + 4H2 <===> CH4 + 2H2O ΔH= 165.2KJ/mol CO is not reduced; it consumes even more H2 Need a catalyst that to promote (1) while suppressing (2)
26
Selective Oxidation of CO
A catalyst selectively promotes a reaction that removes CO over another that consumes H2 CO + 0.5 O2 <==> CO2 H2 + 0.5 O2 <==> H2O The change in Δ G (Gibbs free energy) for the CO reaction is increasingly more negative at lower T CO reaction is favourite at lower T (ie a higher of CO adsorbs onto the catalytic surface) Series of consecutive selective oxidation catalyst beds that operate at increasingly lower T
27
Shale Gas
Shale gas is methane (natural gas) which is trapped in impermeable shale rock deep underground The gas cannot flow through the shale, so simply drilling a well, as you would for conventional natural gas, is not enough The shale rock must be cracked to free the gas, so large quantities of water, sand, and a range of chemicals are pumped in under high pressure (fracking = hydraulic fracturing) Tens or hundreds as many wells are needed to produce as much gas as in a conventional gas field
28
How 'Fracking' works
stage 1: Drill down to shale level stage 2: Water sand and chemicals pumped to a pressure of approx 1500 lb/inch^2, forcing the rock apart releasing the gas in the pores stage 3: Liquid pumped out of well, sand keeps the rock separated allowing gas to seep out of the broken shale layer to be piped to the surface.
29
Pros of Fracking
- Energy security - Job creation - Lower emission than liquefied natural gas - Natural gas is cleaner than coal and oil (clean oil is very expensive) - Horizontal drilling - Cheaper (???)
30
Cons of Fracking
* Environmental pollution (aquifer, soil, water, air, chemicals): Barnett shale: heavy metals release, Se, Sr, As . * Use of huge quantity of water (but compared to what?) * Earthquakes * Impact on habitat, landscape? (Assessment and Impact studies are still very limited, REGULATIONS????)
31
Methane Clathrate
Methane trapped in the crystal structure of water ( (CH4) 5.75(H2O) ) Present in seabeds and permafrost 1m^3 of methan clathrate = 168 m^3 CH4 Reservoir (sediments) = 2- 10 times conventional natural gas Estimates = 1 × 10^15 and 5 × 10^15 m³ (500 2500 Gt C) Widely distributed, but low total volume and low concentration at the sites, so is it economically viable?
32
Pressure swing adsorption
Physical separation process that removes CO2, CO but also other species except H2 H2 = 99,99% Beds composed by zeolites, silica, and carbons Adsorption based on molecular weight at high P
33
Palladium membrane separation
Palladium membrane hydrogen purifiers operate via pressure driven diffusion across palladium membranes H2 molecules in contact with the Pd membrane surface dissociates into monatomic hydrogen and passes through the membrane On the side of the Pd membrane, the monatomic hydrogen is recombined into molecular hydrogen Only hydrogen can diffuse through the palladium membrane Pd is very expensive (less expensive than Pt)
34
What is Biomass
Biomass is a biological derived from living or recently living organisms Biomass is composed of a mixture of organic molecules containing hydrogen usually including atoms of oxygen, nitrogen and also small quantities of other species, such as alkali, alkaline earth and heavy metals
35
What is Bio energy
Energy produced from biomass including woody biomass, agricultural biomass, and other biological materials
36
Biomass : Plants
For plants, The carbon is absorbed from the atmosphere as CO2 by plant life, using energy from the sun Microbial degradation: CO2, CH4 Burning: CO2 "Carbon Cycle"
37
Fossil Fuels
Coal,oil, gas It derives too from biological materials (i e CO2 adsorbed millions of years ago fossil fuels => burning => CO2 + energy (and heat) Difference of timescale from biomass
38
Biomass vs Fossil Fuels
Biomass: While it is growing C is taken out from atmosphere and returns to it when it is burned (in relatively shorter times) - sustainable Fossil: Oil, gas, coal: produced from C sequestered millions of years ago. CO2 generated released quickly. - not sustainable
39
Biomass: from which materials? ( the 5 materials)
Huge resources of residues, by products and waste are potentially become available, in quantity, at relatively low, or even negative costs where there is currently a requirement to pay for disposal. 1. Virgin wood: from forestry, arboricultural and from wood processing activities 2. Energy crops high yield crops grown specifically for energy applications 3.Agricultural residues residues from agriculture harvesting or processing 4.Food waste from food and drink manufacture, preparation and processing, and post consumer waste 5.Industrial waste and by products from manufacturing and industrial processes
40
Why to use biomass? (benefits)
- Renewable - Widely available - Significant reduction in net carbon emissions when compared with fossil fuels - Sustainable It is a “carbon lean, so it produces a fraction of carbon emissions of fossil fuels Sourced locally Local business opportunity and support rural economy If not used they would generally rot. This will generate CO2 in any case, and may also produce methane (CH4 ), a greenhouse gas 21 times more potent that CO2
41
Pre processing processes: (Physical Pre processing)
Pre processing may be required to change the physical form or to reduce the moisture content. Physical pre processing consists of: Cutting to uniform length Chipping Grinding or shredding Reducing moisture content
42
Virgin wood:
-Suitable for a range of energy applications - It can be burned for heat and/or power at a range of scales - Virgin wood is untreated and clean - It may range in moisture content from oven dry to 60% or higher as freshly harvested, green wood
43
Energy Crops
Energy crops are grown specifically for use as fuel and offer high output per hectare with low inputs. Short rotation energy crops Grasses and non woody energy crops (miscanthus, oilseed rape,......) Agricultural energy crops (sugar, starch, and oil crops) Aquatics (hydroponics)
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Agricultural residues:
Dry: Straw Corn Stover Poultry Litter Wet: Grass silage Animal slurry and farmyard manure
45
Food waste :
Dry & Wet About a third of all food grown for human consumption in the UK is thrown away
46
Industrial waste & co-products
“Woody” Materials and “Non Woody” Materials Combustion: Basic process of oxidation Gasification: It is a partial oxidation process whereby a carbon source such as coal, natural gas or biomass, is broken down into CO, H2 CO2 and possibly hydrocarbon such as CH4 Pyrolysis: It is the precursor to gasification, and takes place as part of both gasification and combustion. It consists of thermal decomposition in the absence of O2 . Ex.: charcoal burning.
47
Gasification
Gasification is a thermochemical process in which biomass at high heat is turned directly from a solid into a gaseous fuel called syngas (a mixture of CO, H 2 and some CH4)
48
Pyrolysis
Pyrolysis is the thermal degradation of organic components in biomass in the absence of O 2 . Major products are oil, gas, and char.
49
ways of producing H2 from biomass
1. Thermochemical 2. Biological
50
Carnol Process
This is a high T two step process involving: (i) thermal conversion of CH4 ( CH4 ==> C + 2H2) (ii) Methanol Synthesis ( CO2 + 3H2 ==> CH3OH + H2O ) (iii) Overall (2CO2 + 3CH4 ==> 2CH3OH + 2H2O + 3C) Near zero CO2 emission results from removal of CO 2 from the coal burning plant and emission of equivalent amount of CO2 when methanol is burnt as a fuel
51
Hynol Process
This process produces H2 and CH3OH from biomass with reduced CO2 emissions. Phase 1: (1a) C + CH2 ==> CH4 (1b) C + 2H2O ==> CO + H2 (1c) CO2 + H2 ==> CO + H2O Phase 2: (2a) CH4 + H2O ==> CO2 + 3H2 (2b) CO2 + H2 ==> CO + H2O Phase 3: (3a) CO + 2H2 ==> CH3 + OH (3b) CO2 + 3H2 ==> CH3Oh + H2O
52
Technical issues:
*Since H2 content in Biomass is low, the yield of H2 is low (ca 6% vs 25% of CH4) *Energy content of biomass is also low due to 40% O2 content *Low energy content of biomass is an inherent limitation of the process since over half of H2 from biomass comes from splitting of water in steam reforming *The production of H2 from biomass is not presently economically competitive with natural gas SR without the advantage of high value co products, very low cost biomass and potential environmental incentives
53
Aerobic digestion
Aerobic digestion is a process in which bacteria use O2 to convert organic material into CO2. Products include nutrient rich fertilizers (N, P derivatives) and composts
54
Anaerobic digestion
Anaerobic Digestion is the decomposition of biomass by bacteria in the absence of O2. Biogas, or CH4 is the primary product produced.
55
Fermentation
Fermentation is a biological process in which enzymes produced by microorganisms cause chemical reactions to occur. Products include EtOH, commercial levels of therapeutic and research enzymes, antibiotics, and specialty chemicals.
56
Forms of crude oil
- Diesel - Jet fuel - Kerosene - Gasoline
57
Diesel + Pros and Cons
Pros: Low CO, CO2 , HC emission Cons: NOx , sulfur, particulate matter (PM) General: -Heavier than gasoline (C 14 H 30 ) vs (C 9 H 20 -Easier to refine compared to gasoline -Cheaper -Higher energy density (147K BTU vs 132K)