CО2 sequestration in mining residues – probing heat effects associated to carbonation

/ Literature review
Description du projet de thèse / Description of the project
Méthodologie du projet proposé / Methodology
Résultats préliminaires / First results
Conclusion
Échéancier envisagé / Education plan

continue to rise, the enhanced greenhouse effect may permanently change the climate system in the world.
According to the IPCC association, an increase in the global average surface temperature more than 20C contains potential significant damage to the ecosystems upon which we depend directly.

(http://www.smh.com.au/federal-politics/political-news/australian-coal-mining-threatens-co2-target-20130122-2d5ck.html)

zeolites)
Membranes (fibers, microporous)
Bioligical (algae, cyanobacteria)

(IPCC Special Report on Carbon Dioxide Capture and Storage, p. 4)

Storage: 

Geological
Ocean
Mineral

Carbon dioxide sequestration by mineral carbonation. Literature Review (W.J.J. Huijgen & R.N.J. Comans)

with CO2 either in the gaseous or aqueous phase

Indirect carbonation
Involves the extraction of reactive components (Mg2+, Ca2+) from the minerals, using acids or other solvents, followed by the rection of the extracted components with CO2 either in the gaseous or aqueous phase

A review of mineral carbonation technologies to sequester CO2 (A. Sanna et al.) Carbon Mineralization: From Natural Analogues to Engineered Systems (Ian M. Power et al.),
Carbon Sequestration via Mineral Carbonation: Overview and Assessment (H. Herzog)

W. Seifritz, CO2 disposal by means of silicates (1990)
H. Dunsmore, A geological perspective on global warming and
the possibility of carbon dioxide removal as calcium carbonate mineral (1992)
K. Lackner et al., Carbon dioxide disposal in carbonate minerals (1995)
O'Connor et al., Carbon dioxide sequestration by direct mineral carbonation with carbonic acid (2000)

L. Harrison et al.)
Passive offsetting of CO2 emissions at the Mount Keith Nickel Mine, Western Australia: A basis for geoengineering carbon neutral mines (Siobhan A. Wilson et al.)
Exploring The Mechanism That Control Olivine Carbonation Reactivity During Aqueous Mineral Carbonation (Michael J. McKelvy et al.)

The Netherlands
Finland
Japan

China
U.S. and Canada
Switzerland
Australia

Active carbonation concept

Power plant –
source of CO2

Mineral carbonation plant

Sources of feedstock:

Waste cement/concrete

Industrial wastes

Storage

MgCO3

Mining tailings

CO2 (A. Sanna et al.)
CO2-depleted warm air venting from chrysotile milling waste (Thetford Mines, Canada): Evidence for in-situ carbon capture from the atmosphere (J. Pronost et al.)

1) Long term stability
2) Raw materials are abundant
3) Potential to be economically viable

Low speed of the process
No control under ambient conditions

Passivation under Environmental Conditions (Assima, G. et al.)
Fixation of CO2 by chrysotile in low-pressure dry and moist carbonation: Ex-situ and in-situ characterizations
(Larachi, F. et al.)
Carbon sequestration kinetic and storage capacity of ultramafic mining waste (Pronost, J. et al.)
Multivariate study of the dynamics of CO2 reaction with brucite-rich ultramafic mine tailings (Entezari Zarandi, A. et al.)

G. Assima:
1) The presence of the T difference in a reactor between bed with NiMR and recirculating gas
2) Water content accelerates the process and leads to the bigger CO2 capture
3) More alkaline carbonates are formed at elevated temperatures
J. Pronost:
Hot-spots in the waste heap surface – the sign of the exothermic behavior of the reaction
Carbonation potential of ultramafic material depends on the brucite content
A. Entezari Zarandi:
The rapid CO2 uptake in the early minutes of reaction caused a sharp drop in pH
The highest carbonation reactivity is attained with 3% brucite doping of an already carbonated NiMR
Carbonation proceeds through formation of a porous flaky carbonate phase topping mainly the high-pH brucite surfaces

IR thermography

What’s new?

Science

Industry

The way to get back some energy and use it for an industrial needs

CO2 sequestration.

(A review of mineral carbonation technologies to sequester CO2, www.rsc.org/csr)

Serpentine group(Lizardite)~80-90%
Brucite ~ 0-12%
Olivine group (Forsterite) ~ 5%
Rest ~ 3%

Group of minerals based on Magnesium carbonate is an environmentally stable and non-toxic.

H2O sat. (rain) =0...50%

Spring/Autumn
T = 0...+150C
H2O sat.(rain) = 50...100%

(https://nuclear-news.net/information/wastes/)

+ 2H2Ol +(-64kJ/mol CO2)

Mg2SiO4s + 2CO2g = 2MgCO3s + SiO2s +(-90 kJ/mol CO2)

Mg(OH)2s + CO2g = MgCO3s + H2Ol +(-81 kJ/mol CO2)

Lizardite

Brucite

Forsterite

Mg(OH)2s+CO2g+2H2Ol = Mg(HCO3)OH · 2H2Os +(-86 kJ/mol CO2)

-1,95 MJ/kg of CO2

2Mg3Si2O5(OH)4s+3CO2g+6H2Ol =3(Mg(HCO3)OH · 2H2O)s+ Mg3Si4O10(OH)2s+
(-72,4kJ/mol CO2)

Mg2SiO4s+2CO2g+6H2Ol =2(Mg(HCO3)OH·2H2O)s +SiO2s +(-91 kJ/mol CO2)

-1,64 MJ/kg of CO2

-2,07 MJ/kg of CO2

external heat stimulation

Energy source is required to produce a thermal contrast between the feature of interest and the background

(Infrared Thermography for NDT: Potentials and Applications, X. P. V. Maldague, slide 19)

(Infrared Thermography, C. Ibarra-Castanedo and X. P. V. Maldague, p. 180)

(Infrared Thermography, C. Ibarra-Castanedo and X. P. V. Maldague, p. 178)

on T0C.

(http://www.flir.com/legacy/view/?id=51542)

(http://fiveboroughhomeinspection.com/inspection-service/infrared-camera-inspection-service/)

Indigo Phoenix Thermal Camera

50% water saturation :

Chemistry of the laboratory process

9 g of ore will react with 1,02 l of CO2

· 2H2Os

Laboratory conditions: ω(CO2) = 20%, T=298K,
50% saturation
V CO2 = 1,06 litres
n (CO2) = 0,047 mol
ΔrH = -85836 J/mol of CO2 ΔT = 13,46K
Q = -ΔrH·n = 4061,88 J
Q = Cp·ΔT
Ambient conditions(mine site):ω(CO2) = 400ppm, T=298K,
50% saturation
V CO2 = 0,00212 litres
n (CO2) = 9,46·10-5 mol
ΔrH = -85836 J/mol of CO2 ΔT = 0,027K
Q = -ΔrH·n = 8,12 J
Q = Cp·ΔT

V total = 5,3 l

2H2Ol= Mg(HCO3)OH · 2H2Os

Laboratory conditions: ω(CO2) = 10%, T = 298K, 50% saturation
V CO2 = 0,2 litres
n (CO2) = 0,009 mol
ΔrH = -94714 J/mol of CO2 ΔT = 2,54K
Q = -ΔrH·n = 766,39 J
Q = Cp·ΔT

V total = 2 l

CO2
 Duration = 15 h
0.56% of CO2 left

35g Mg(OH)2 (11%)+SiO2

sat.
9.83% of CO2
Duration = 9 h

33 min: T = 22.25 C, ΔT=1.65 C

35 g of the ore

expériences
GCH-6000: Communication scientifiques orale et écrite I
GIF-7006: Vision en inspection industrielle

Carbonation

By MSc student
Aksenova Diana
Department of Chemical Engineering

Supervisor: Prof. Faical Larachi
Co-Supervisors: Prof. Xavier Maldague and Prof. Georges Beaudoin

feedstock:

Waste cement/concrete

Industrial wastes

Storage

MgCO3

Mining tailings

Exploring The Mechanism That Control Olivine Carbonation Reactivity During Aqueous Mineral Carbonation (Michael J. McKelvy et al.)

OR

injections

 

Ex-situ

In-situ

HCO3–(aq)
HCO3–(aq) → H+(aq) + CO32–(aq)
Mg (OH)2(s) + H+(aq) → Mg2+(aq) + H2O(l)+ OH–(aq)
Mg2+(aq) + HCO3–(aq) + OH–(aq) + 2H2O(l) → Mg (HCO3) (OH)·2H2O (s)

Mg2+ – series of the reactions

converted
into thermal energy in 4 kW and above,
there is an energy consumption - 25%

Mg(HCO3)OH · 2H2Os

:

Chemistry of the laboratory process

Mg3Si2O5(OH)4s+ 3CO2g + 7H2Ol =3(Mg(HCO3)OH · 2H2O)s + 2SiO2
Lizardite/chrysotile Nesquehonite
0,145 mol (40 g – 80%) 0,0234 mol

Mg2SiO4s + 2CO2g + 6H2Ol =2(Mg(HCO3)OH · 2H2O)s + SiO2
Forsterite Nesquehonite
0,0286 mol (4 g – 8%) 0,0156 mol

Mg(OH)2s + CO2g + 2H2Ol = Mg(HCO3)OH · 2H2Os
Brucite Nesquehonite
0,103 mol (6g – 12%) 0,0078 mol

9 g of ore
will react with
1,02 l of CO2

+ 2H2Ol Mg(HCO3)OH · 2H2Os

V CO2 = 0,2 litres
n (CO2) = 0,009 mol
ΔrH = -94714 J/mol of CO2 ΔT = 2,54K
Q = -ΔrH·n = 766,39 J
Q = Cp·ΔT

V total = 2 l

 

ΔT = 0,86 K

Laboratory conditions: ω(CO2) = 10%, T = 298K, 50% saturation