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Gas blending is the process of mixing gases for a specific purpose where the composition of the resulting mixture is defined, and therefore, controlled. A wide range of applications include scientific and industrial processes, food production and storage and breathing gases.
Carbon dioxide liquid/vapor equilibrium thermodynamic data: Temp. °C P vap Vapor pressure kPa H liq Heat content liquid J/g H vap Heat content vapor J/g Δ vap H o Heat of vapor-ization J/g ρ vap Density of vapor g/cm 3 ρ liq Density of liquid g/cm 3 S liq Entropy liquid J/mol-°C S vap Entropy vapor J/mol-°C −56.6: 518.3: 1.179: −56.0 ...
This makes carbon dioxide preferable for fumigation in situations where a hermetic seal cannot be maintained. Air-tight storage of grains (sometimes called hermetic storage) relies on the respiration of grain, insects, and fungi that can modify the enclosed atmosphere sufficiently to control insect pests.
Supercritical carbon dioxide (s CO 2 ) is a fluid state of carbon dioxide where it is held at or above its critical temperature and critical pressure . Carbon dioxide usually behaves as a gas in air at standard temperature and pressure (STP), or as a solid called dry ice when cooled and/or pressurised sufficiently.
Carbon dioxide is a by-product of food metabolism and in high amounts has toxic effects including: dyspnea, acidosis and altered consciousness. [8] Arterial blood carbon dioxide tension. P a CO 2 – Partial pressure of carbon dioxide at sea level in arterial blood is between 35 mmHg and 45 mmHg. [9] Venous blood carbon dioxide tension
A saturation dome uses the projection of a P–v–T diagram (pressure, specific volume, and temperature) onto the P–v plane. The points that create the left-hand side of the dome represent the saturated liquid states, while the points on the right-hand side represent the saturated vapor states (commonly referred to as the “dry” region).
Liquid carbon dioxide is the liquid state of carbon dioxide (CO 2 ), which cannot occur under atmospheric pressure. It can only exist at a pressure above 5.1 atm (5.2 bar; 75 psi), under 31.1 °C (88.0 °F) (temperature of critical point ) and above −56.6 °C (−69.9 °F) (temperature of triple point ). [ 1 ]
The concentration at saturation depends on the partial pressure of the gas in the supply and of the solubility of the gas in that solvent, under those conditions. If the external partial pressure of the gas (in the lungs) is then reduced, more gas will diffuse out than in. A condition known as supersaturation may develop.