states that the sum of the partial pressures of each gas in a mixture is equal to the total pressure of the mixture.
Dalton's law of partial pressure. The total pressure exerted by a mixture of gases is the sum of the pressures that each gas would exert if it were alone. For example, if dry oxygen gas at 713 torr is saturated with water vapor at 25 torr, the pressure of the wet gas is 738 torr.
Vapor pressure created in a container by a mixture of gases is equal to sum of individual vapor pressures of the gases contained in mixture.
the total pressure exerted by a mixture of gases is equal to the sum of the pressures that would be exerted by each of the gases if it alone were present and occupied the total volume.
(chemistry and physics) law stating that the pressure exerted by a mixture of gases equals the sum of the partial pressures of the gases in the mixture; the pressure of a gas in a mixture equals the pressure it would exert if it occupied the same volume alone at the same temperature
the total pressure exerted by a mixture of gases equals the sum of the pressures that would be exerted if each of the individual gases present were to occupy the same volume by itself
This states that the total pressure of a gas mixture is equal to the sum of the partial pressures of that gas. ie, in air at 1 ATA the PO2 (oxygen) is .21. The PN2 (nitrogen) is .79. The sum of those two gases equals 1.00 or 1 ATA.
States that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the constituent gases. The partial pressure is the pressure each gas would exert if it alone occupied the volume of the mixture. ( 010)
If several types of gas are put into the same container, the total pressure exerted is the sum of the partial pressures that each type of gas would exert if it alone occupied the container.
for " perfect gases," a mixture of gases will have a pressure equal to the sum of the pressures of the individual gases, assuming no chemical reaction has taken place between the gases. Named for John Dalton (1766 - 1844), a British chemist who formulated the concept.
the total pressure exerted by a mixture of gases is equal to the sum of the pressures of each of the different gases making up the mixture. Each gas acting as if it were alone were present and occupied the total volume.
The total pressure of a mixture of gases is the sum of the pressures each component would have if it alone occupied the volume of the mixture at its temperature. Dalton's law is strictly valid only for hypothetical ideal gases but is a good approximation for atmospheric gases at normal terrestrial temperatures and pressures.
States that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the gases. Formulated by John Dalton, an English physicist.
In chemistry and physics, Dalton's law (also called Dalton's law of partial pressures) states that the total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture.
