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Dalton’s law The total pressure

FIGURE 4.19 A representation of the experiment that Dalton performed on a gas mixture. According to Dalton s law, the total pressure, P, of a mixture of gases is the sum of the partial pressures PA and PB of gases A and B. Each partial pressure is the pressure that one of the gases would exert if it were the sole gas in the container (at the same temperature). [Pg.277]

A—I bis experiment requires the ideal gas equation. The mass of the solid is needed (to convert to moles) this eliminates answer choice D. The volume, temperature, and pressure must also be measured during the experiment, eliminating choices B, C, and E. The measured pressure is the total pressure. Eventually the total pressure must be converted to the partial pressure of the gas using Dalton s law. The total pressure is the sum of the pressure of the gas plus the vapor pressure of water. The vapor pressure of water can be looked up in a table when the calculations are performed (only the temperature is needed to find the vapor pressure in a table). Answer A is correct. [Pg.117]

The total pressure of the gaseous mixture is the sum of the partial pressures of all the components (Dalton s law). The total pressure is 55 torr (21 + 34). [Pg.228]

Dalton s law The total pressure of a mixture of gases is equal to the sum of the partial pressures of each constituent gas. Partial pressure is the pressure each gas would exert if it occupied the volume of the mixture alone. [Pg.69]

Dalton s law The total pressure exerted by a mixture of ideal gases is the sum of tihe partial pressures of each of the gases in the mixture. [Pg.1000]

According to Dalton s law the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert at the same temperature in the same vapour space ... [Pg.78]

Plan Because each gas behaves independently, we can use the ideal-gas equation to calculate the pressure each would exert if the other were not present. Per Dalton s law, the total pressure is the sum of these two partial pressures. [Pg.416]

According to Dalton s law, the total pressure of the wet gas is the sum of the two partial pressures. The total pressure can be made equal to the prevailing pressure of the atmosphere (barometric pressure) by adjusting the position of the bottle thus we can write... [Pg.217]

According to Dalton s law, the partial pressure of a gas (Pgas) is equal to its fractional concentration (% total gas) multiplied by the total pressure (Ptot) of all gases in a mixture ... [Pg.259]

The extreme mole fractions, 0 and 1, at either end of the graph relate to pure petrol (x = 0) and pure benzene (x = 1) respectively. The mole fractions between these values represent mixtures of the two. The solid, bold line represents the total mole fraction while the dashed lines represent the vapour pressures of the two constituent vapours. It is clear that the sum of the two dashed lines equals the bold line, and represents another way of saying Dalton s law the total vapour pressure above a mixture of liquids is the sum of the individual vapour pressures. [Pg.226]

From Dalton s law, the total vapour pressure is simply the sum of the individual vapour pressures ... [Pg.227]

Dalton s Law of Portial Pressures. This law may be stated In a mixture of gases, each gas exerts a partial pressure equal to the pressure it would exert if it alone were present in the volume occupied by the mixture. In other words, the total pressure of a mixture of gases is equal to the sum of the partial pressures of its components. For example, consider two vessels of equal voltuues containing methane and ethane respectively, each at a pressure of one atmosphere. If the etiiane were forced into the methane tank at constant temperature, the pressure of the combined gases would be two atmospheres. According to Dalton s Law the partial pressures of the methane and ethane in the mixture would each be one atmosphere. [Pg.21]

In an ideal gas mixture the partial pressure is a useful measure of concentration. By Dalton s law, the partial pressure of is related to the total pressure by... [Pg.21]

If a sealed vessel contains a liquid X (such as ethanol or water) and a gas Y (such as nitrogen), it is usually safe to assume that the gas Y is saturated with the vapour of X. As expected from Dalton s law, the total gas pressure above the liquid is the sum of the gas and vapour pressures. This is illustrated by the following example. [Pg.167]

When kc and K g values are reported in units (SI) of kmoL/[(s m") (kPa)], one must be careful in converting them to a mole-fracdion basis to multiply by the total pressure actually employed in the original experiments and not by the total pressure or the system to Be designed. This conversion is valid for systems in which Dalton s law of partial pressures p = ypr) is valid. [Pg.602]

Dalton S Law of Partial Pressures. The total pressure (P) of a gaseous mixture equals the sum of the partial pressures of its components. By definition, the partial pressure of any component gas is the hypothetical pressure it would exert by occupying the entire volume (V) of the mixture at the same temperature (T). That is,... [Pg.339]

Dalton s Law of partial pressures considers a mixture of two or more gases, and states that the total pressure of the mixture is equal to the sum of the individual pressures, if each gas separately occupied the space. [Pg.5]

If we assume that Dalton s law of partial pressure holds in the vapor phase, it is easy to show that >2 is related to the total pressure, p, by the equation... [Pg.406]

FIGURE 8.35 The vapor pressures of the two components of an ideal binary mixture obey Raoult s law. The total vapor pressure is the sum of the two partial vapor pressures (Dalton s law). The insets below the graph represent the mole fraction of A. [Pg.459]

This is Dalton s law of partial pressures. To obtain a total pressure, simply add the contributions from all gases present Ptotal Pi + P2 + P3 +------------ Pi... [Pg.314]

This is Dalton s Law of partial pressures. The total pressure of the gang is equal to the sum of their individual efforts. Here, A could be the isopropyl alcohol and B the isobutyl, (it doesn t matter) but PTotal must be the atmospheric pressure, Patm. So a special version of Dalton s Law of partial pressures for use in fractional distillation will be... [Pg.294]

Well, at 99.6°C, quinoline contributes 10 torr to the total vapor pressure, and water must make up the difference (750 torr) in order to satisfy Dalton s Law of partial pressures to make PTotal 760 torr at boiling. Using the relationships for the composition of the vapor over a liquid, we can calculate the quinoline/water ratio coming over. [Pg.309]

By Dalton s law of partial pressures, P = T,PA, that is the total pressure is equal to the summation of the partial pressures. Since in an ideal gas or vapour the partial pressure is proportional to the mole fraction of the constituent, then ... [Pg.546]

The most abundant gases present in the ocean and atmosphere are listed in Table 6.1. In the atmosphere, each gas exerts a pressure, called a partial pressure. Because of their relatively low concentrations, most atmospheric gases exhibit near ideal behavior such that their partial pressures are independent of each other. In this case, the total atmospheric pressure (Aj) is the sum of the partial pressures of the component gases. This is termed Dalton s Law of Partial Pressures. For air ... [Pg.148]

As mentioned above, gases in solution are often measured in partial pressures. Recall that Dalton s Law of Partial Pressures states that the total pressure is the sum of the pressures partially exerted by all of the component, noninteracting gases. For one gaseous component in equilibrium with the same component dissolved in a liquid, the partial pressure of that gas in solution is the pressure that gas would exert in the atmosphere. It is symbolized by either p or P followed by the specific gas (eg, either or pO ). For example, typical blood P02 levels range between 75 and 100 torr (or, 10.0 to 13.3 kPa since the pascal (Pa) is an SI unit). [Pg.163]

Dalton s Laws of Partial Pressure states that in a mixture of gases each gas exerts a pressure independent of the other gases. The total pressure is the sum of the partial pressures... [Pg.107]


See other pages where Dalton’s law The total pressure is mentioned: [Pg.469]    [Pg.469]    [Pg.72]    [Pg.485]    [Pg.363]    [Pg.603]    [Pg.271]    [Pg.192]    [Pg.82]    [Pg.121]    [Pg.107]   


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