CO2-water–basalt interaction. Low temperature experiments and implications for CO2 sequestration into basalts

Gysi, Alexander P.; Stefánsson, Andri

doi:10.1016/j.gca.2011.12.012

Cited by 127 publications

(78 citation statements)

References 56 publications

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“…It is therefore of advantage to inject at relatively high partial pressure of CO 2 ; it saves water and pore space. This predicted reaction path simulation has been confirmed by experiments in the laboratory [32,33].…”

Section: Mineral Carbon Storage Within Basaltic Rocks Review Of Expesupporting

confidence: 67%

“…The Mg-Fe-Ca carbonates at intermedia pH and Ca-carbonates to be most important at the highest pH. This is what is seen in a natural analogue in West Greenland where CO 2 rich fluids invaded basaltic rocks at low temperature [31] and basalt water CO 2 experiments in the laboratory [32,33]. The carbonates in the altered rocks in West-Greenland are with decreasing partial pressure of CO 2 ; Fe and Mg rich carbonates; at intermediate CO 2 pressure Mg-Ca carbonates dominate and at the lowest partial pressure, Ca carbonates are most common.…”

Section: Mineral Carbon Storage Within Basaltic Rocks Review Of Expementioning

confidence: 64%

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Rapid solubility and mineral storage of CO2 in basalt

et al. 2014

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The long-term security of geologic carbon storage is critical to its success and public acceptance. Much of the security risk associated with geological carbon storage stems from its buoyancy. Gaseous and supercritical CO 2 are less dense than formation waters, providing a driving force for it to escape back to the surface. This buoyancy can be eliminated by the dissolution of CO 2 into water prior to, or during its injection into the subsurface. The dissolution makes it possible to inject into fractured rocks and further enhance mineral storage of CO 2 especially if injected into silicate rocks rich in divalent metal cations such as basalts and ultra-mafic rocks. We have demonstrated the dissolution of CO 2 into water during its injection into basalt leading to its geologic solubility storage in less than five minutes and potential geologic mineral storage within few years after injection [1][2][3]. The storage potential of CO 2 within basaltic rocks is enormous. All the carbon released from burning of all fossil fuel on Earth, 5000 GtC, can theoretically be stored in basaltic rocks [4].

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Section: Mineral Carbon Storage Within Basaltic Rocks Review Of Expesupporting

confidence: 67%

Section: Mineral Carbon Storage Within Basaltic Rocks Review Of Expementioning

confidence: 64%

Rapid solubility and mineral storage of CO2 in basalt

et al. 2014

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“…Seifritz, 1990;Lackner et al, 1995;Xu et al, 2005;Marini, 2007;Flaathen et al, 2011). Carbon storage via carbonate mineral precipitation appears to be particularly favoured in basaltic and ultramafic rocks due to their high reactivity and the prevalence of divalent cations such as Ca 2+ and Mg 2+ (McGrail et al, 2006;Alfredsson et al, 2008;Oelkers et al, 2008;Matter et al, 2009Matter et al, , 2011Schaef et al, 2010Schaef et al, , 2011Gislason et al, 2010;Gysi and Stefansson, 2012;Aradóttir et al, 2012;Oskierski et al, 2013;Gislason and Oelkers, 2014). Whereas anhydrous calcium carbonates such as calcite and aragonite precipitate readily at ambient temperatures (e.g.…”

Section: Introductionmentioning

confidence: 99%

The experimental determination of hydromagnesite precipitation rates at 22.5–75ºC

Berninger

Jordan²,

Schott

et al. 2014

Mineral. mag.

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Natural hydromagnesite (Mg 5 (CO 3 ) 4 (OH) 2 ·4H 2 O) dissolution and precipitation experiments were performed in closed-system reactors as a function of temperature from 22.5 to 75ºC and at 8.6 < pH < 10.7. The equilibrium constants for the reaction Mg 5 (CO 3 ) 4 (OH) 2 ·4H 2 O + 6H + = 5Mg 2+ + 4HCO 3 À + 6H 2 O were determined by bracketing the final fluid compositions obtained from the dissolution and precipitation experiments. The resulting constants were found to be 10 33.7Ô0.9 , 10 30.5Ô0.5 and 10 26.5Ô0.5at 22.5, 50 and 75ºC, respectively. Whereas dissolution rates were too fast to be determined from the experiments, precipitation rates were slower and quantified. The resulting BET surface areanormalized hydromagnesite precipitation rates increase by a factor of~2 with pH decreasing from 10.7 to 8.6. Measured rates are approximately two orders of magnitude faster than corresponding forsterite dissolution rates, suggesting that the overall rates of the low-temperature carbonation of olivine are controlled by the relatively sluggish dissolution of the magnesium silicate mineral.

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“…In granitic caves, speleothems are fairly common (Vidal Romaní et al, 2010) and although many different speleothemforming minerals have been identified (for example evansite, bolivarite, struvite, pigotite, taranakite, allophane, hematite, goethite, halite, gypsum, anhydrite, plumbo-aragonite and even calcite), the most common authigenic mineral of speleothems in granitic caves is opal-A, an amorphous hydrated polymorph of silica (Vidal Romaní et al, 2013). Although calcite has not been reported as a major speleothem forming mineral from granitic caves before, many studies (e.g., Woo et al, 2008;Baskar et al, 2009;Gysi & Stefánsson 2012a, 2012bHövelmann et al, 2012;Oskierski, 2013;Schwarzenbach et al, 2013;Van Noort et al, 2013) mention the existence of calcite in caves developed in plutonic or volcanic magmatic rocks such as granodiorites, peridotites, serpentinites and basalts. In lava caves hosted in mafic volcanic rocks, speleothems are frequently formed by precipitation of opal-A and calcite as well as other minerals like oxides and sulfides (Woo et al, 2008;Baskar et al 2009;White, 2010).…”

Section: Samplesmentioning

confidence: 99%