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Introduction
Published in Armen S. Casparian, Gergely Sirokman, Ann O. Omollo, Rapid Review of Chemistry for the Life Sciences and Engineering, 2021
Armen S. Casparian, Gergely Sirokman, Ann O. Omollo
Dalton’s Law states: The total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of all the gases in the mixture. Each partial pressure is the pressure that the gas would exert if the other gases were not present.
Wastewater Stripping
Published in Gaetano Joseph Celenza, Specialized Treatment Systems, 2020
The partial pressure of individual components in an ideal mixture is expressed by Raoult’s Law, stating that at equilibrium the partial pressure (p) of a component in solution is equal to the product of its vapor pressure (P*) and its mole fraction (x) in solution. According to Dalton’s Law the partial pressure of a component in an ideal gas is equal to its mole fraction in the gas times the total pressure. pi=xi·P*inanidealsolutionpi=yi·πin anidealgas
Basic Chemical Hazards to Human Health and Safety — I
Published in Jack Daugherty, Assessment of Chemical Exposures, 2020
The ability of hemoglobin to carry oxygen is directly proportional to the partial pressure of oxygen in the air we breathe. Our bodies have adapted to work efficiently when the volume percent of oxygen in the atmosphere is about twenty-one percent. Dalton’s law of partial pressures states that in any mixture of gases, the total pressure is the sum of the partial pressures of the component gases. The partial pressure of any component gas in the mixture is proportional to the percentage of its molecules in the total mixture, or, in other words, the volume fraction of the gas component. In the case of oxygen in air at sea level: PO2=Pair×%O2=760mmHg×0.21=160mmHg
Oxygen depletion in enclosed spaces
Published in Journal of Marine Engineering & Technology, 2020
As opposed to the methodology used in other studies, our research aims to continuously monitor the oxygen depletion process in a model. This data allows us to determine the rate of oxygen depletion. Dalton’s Law of Partial Pressures states that for a mixture of gases in any container, the total pressure exerted is the sum of the partial pressures that each gas would exert if it were alone in that container. The standard atmosphere is a unit of pressure equal to 101.325 kPa. The partial pressures of each of the air components (in kPa) are equal to the percentage of that component. With the exception of oxygen and water vapour, all constituents of air are inert or unreactive gases; therefore oxygen and water vapour are the only gases which can be consumed in the rusting process. In a closed containment experiment if all the oxygen is used up by corrosion, the pressure in the container is 80.425 kPa which is equal to the atmospheric pressure minus the partial pressure of oxygen (20.9 kPa). Table 1 shows the relationship between the Oxygen level, the absolute pressure within the container and the level of danger within the space.
Energetic, exergetic and entropic study in a simple and hybrid solar distiller
Published in International Journal of Ambient Energy, 2020
Hiba Akrout, Khaoula Hidouri, Ali Benhmidene, Bechir Chaouachi
The specific heat of the air is considered constant, and the enthalpy of the water vapour depends on the temperature. The total pressure of the mixture according to Dalton’s law is the sum of the pressures of the components: