CLVI.—The influence of colloids and fine suspensions on the solubility of gases in water. Part II. Solubility of carbon dioxide and of hydrogen

Findlay, Alexander; Shen, Bucchok

doi:10.1039/ct9120101459

Cited by 27 publications

(8 citation statements)

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“… (a,b). Comparison of the experimental CO 2 solubility in various aqueous salt solutions at 298.15 K and 0.1 MPa based on different concentration scales: (a) percent of salt by weight; (b) ionic strength. Solid lines represent the calculated values from the PSUCO2 model.…”

Section: Discussionmentioning

confidence: 99%

“… (a–d). Comparison of the model calculations against the experimental CO 2 solubility , , in aqueous KCl solutions. (a) 0.1 MPa, 288–313 K, 0–4.75 mol kg −1 KCl; (b) 0.4–9.1 MPa, 314–433 K, and 2 mol kg −1 KCl; (c) 0.6–9.4 MPa, 313–433 K, and 4 mol kg −1 KCl; (d) Comparison of the experimental CO 2 solubility between Pérez‐Salado Kamps and Kiepe et al at the same P‐T‐x conditions, the modeling results are in excellent agreement with the experimental results reported by Pérez‐Salado Kamps …”

Section: Discussionmentioning

confidence: 99%

“…In Table , the modeling results of CO 2 solubility in the aqueous phase from various models (PSUCO2, SP2010, DS2006, and OLI) were compared to the experimental data , in terms of average absolute deviation (AAD %), which is defined as below

AAD true(% true) = \frac{100}{N_{normalp}} {true \sum}_{i = 1}^{N} false| \frac{m_{{CO}_{2}, i}^{calc} - m_{{CO}_{2}, i}^{exp}}{m_{{CO}_{2}, i}^{exp}} false| %

where

m_{{CO}_{2}, i}^{calc}

represents the calculated CO 2 solubility values from the CO 2 solubility models (PSUCO2, SP2010, DS2006, and OLI);

m_{{CO}_{2}, i}^{exp}

denotes the experimental CO 2 solubility taken from literature and obtained in this study; and N means the total number of experimental data in each work. Table demonstrates that the PSUCO2 model predicts the CO 2 solubility in aqueous CaCl 2 , Na 2 SO 4 , MgCl 2 , and KCl solutions with a high degree of accuracy over a wide P‐T‐x range [288–433 K, 1–71 MPa, and ionic strength up to 20.7 mol kg −1 for CaCl 2 (aq), 7.2 mol kg −1 for Na 2 SO 4 (aq), 15 mol kg −1 for MgCl 2 (aq), and 4.8 mol kg −1 for KCl(aq)].…”

Section: Modelingmentioning

confidence: 99%

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Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions

2015

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The phase equilibria of CO2 and aqueous electrolyte solutions are important to various chemical‐, petroleum‐, and environmental‐related technical applications. CO2 solubility in aqueous CaCl2, MgCl2, Na2SO4, and KCl solutions at a pressure of 15 MPa, the temperatures from 323 to 423 K, and the ionic strength from 1 to 6 mol kg−1 were measured. Based on the measured experimental CO2 solubility, the previous developed fugacity‐activity thermodynamic model for the CO2‐NaCl‐H2O system was extended to account for the effects of different salt species on CO2 solubility in aqueous solutions at temperatures up to 523 K, pressures up to 150 MPa, and salt concentrations up to saturation. Comparisons of different models against literature data reveal a clear improvement of the proposed PSUCO2 model in predicting CO2 solubility in aqueous salt solutions. © 2015 American Institute of Chemical Engineers AIChE J, 61: 2286–2297, 2015

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Section: Discussionmentioning

confidence: 99%

Section: Discussionmentioning

confidence: 99%

AAD true(% true) = \frac{100}{N_{normalp}} {true \sum}_{i = 1}^{N} false| \frac{m_{{CO}_{2}, i}^{calc} - m_{{CO}_{2}, i}^{exp}}{m_{{CO}_{2}, i}^{exp}} false| %

where

m_{{CO}_{2}, i}^{calc}

represents the calculated CO 2 solubility values from the CO 2 solubility models (PSUCO2, SP2010, DS2006, and OLI);

m_{{CO}_{2}, i}^{exp}

Section: Modelingmentioning

confidence: 99%

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Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions

2015

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“…Findlay and Shan (29) investigated the effect of colloids and fine suspensions on the solubility of CO 2 in water. The results were in harmony with…”

Section: ~-mentioning

confidence: 99%

An Investigation of the Equilibria Existing in Gas-Water Systems Forming Electrolytes

Morgan¹,

Maass²

1931

Can. J. Res.

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The data and theoretical treatment contained in this paper are the continuation of a series of researches instituted to investigate the equilibria existing in certain gaseous-aqueous systems. In this work the vapor pressures and electrolytic conductivities of aqueous solutions of sulphur dioxide, carbon dioxide, and ammonia have been measured with greater precision than ever before over a temperature range from 0 to 25 °C. and over a concentration range where their respective vapor pressures do not exceed one atmosphere. From the data thus derived, equilibria relations have been calculated and certain changes have been made in the mode of theoretical procedure involved in this type of calculation.With regard to the equilibria existing in the three systems, the conclusions drawn may be summarized as follows: Practically all of the ammonia exists in the combined form and practically all the carbon dioxide exists as free carbon dioxide in the aqueous solutions in the temperature range investigated. The amounts of free and combined sulphur dioxide are of the same order of magnitude and the relative amount of combined and free sulphur dioxide can be calculated approximately, the latter increasing markedly with rising temperature. The true dissociation constant can therefore be found for ammonium hydroxide, can be estimated for sulphurous acid, but cannot be calculated for carbonic acid from the available data.

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“…It is reported that pure CO 2 clathrate hydrate decomposed to metastable super-cooled water below the water freezing temperature 17 . Although CO 2 solubility in trehalose aqueous solution was not found in the literature, it is reported that CO 2 solubility both in sucrose aqueous solution 18 and in glucose aqueous solution 19 were lower than that in pure water and decreased with an increase in concentration of sucrose and glucose in solution. CO 2 solubility in the sucrose solution with sucrose mass fraction of 0.12 18 and in the glucose solution with glucose mass fraction of 0.12 19 are approximate 10% and 20% lower than that in pure water, respectively.…”

Section: Resultsmentioning

confidence: 86%

Preservation of carbon dioxide clathrate hydrate in the presence of trehalose under freezer conditions

Nagashima

Takeya

Uchida

et al. 2016

Sci Rep

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To investigate the preservation of CO2 clathrate hydrate in the presence of sugar for the novel frozen dessert, mass fractions of CO2 clathrate hydrate in CO2 clathrate hydrate samples coexisting with trehalose were intermittently measured. The samples were prepared from trehalose aqueous solution with trehalose mass fractions of 0.05 and 0.10 at 3.0 MPa and 276.2 K. The samples having particle sizes of 1.0 mm and 5.6–8.0 mm were stored at 243.2 K and 253.2 K for three weeks under atmospheric pressure. The mass fractions of CO2 clathrate hydrate in the samples were 0.87–0.97 before the preservation, and CO2 clathrate hydrate still remained 0.56–0.76 in the mass fractions for 5.6–8.0 mm samples and 0.37–0.55 for 1.0 mm samples after the preservation. The preservation in the trehalose system was better than in the sucrose system and comparable to that in the pure CO2 clathrate hydrate system. This comparison indicates that trehalose is a more suitable sugar for the novel frozen carbonated dessert using CO2 clathrate hydrate than sucrose in terms of CO2 concentration in the dessert. It is inferred that existence of aqueous solution in the samples is a significant factor of the preservation of CO2 clathrate hydrate in the presence of sugar.

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CLVI.—The influence of colloids and fine suspensions on the solubility of gases in water. Part II. Solubility of carbon dioxide and of hydrogen

Cited by 27 publications

References 0 publications

Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions

Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions

An Investigation of the Equilibria Existing in Gas-Water Systems Forming Electrolytes

Preservation of carbon dioxide clathrate hydrate in the presence of trehalose under freezer conditions

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CLVI.—The influence of colloids and fine suspensions on the solubility of gases in water. Part II. Solubility of carbon dioxide and of hydrogen

Cited by 27 publications

References 0 publications

Experimental studies and modeling of CO2 solubility in high temperature aqueous CaCl2, MgCl2, Na2SO4, and KCl solutions

Experimental studies and modeling of CO2 solubility in high temperature aqueous CaCl2, MgCl2, Na2SO4, and KCl solutions

An Investigation of the Equilibria Existing in Gas-Water Systems Forming Electrolytes

Preservation of carbon dioxide clathrate hydrate in the presence of trehalose under freezer conditions

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Product

Resources

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Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions

Experimental studies and modeling of CO₂ solubility in high temperature aqueous CaCl₂, MgCl₂, Na₂SO₄, and KCl solutions