Partial Pressures and Mole Fractions

Let s consider a container which has different gases in it. According to the Dalton s law of partial pressures, the partial pressures of the gases present in a gaseous mixture can be added to get the net total pressure of the mixture. But, what is partial pressure Partial pressure is the pressure exerted by a particular gas in a mixture of ises. Now that you know what partial pressure is, take a look at the boxed information which summarizes the whole idea of Dalton s law of partial pressures. 

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Concentration, Moles, Partial Pressure, and Mole Fraction. 7-5... 

The amount of gas introduced into a diving tank can be determined by weighing the tank before and after charging the tank with gas. A diving shop placed 80.0 g of O2 and 20.0 g of He in a 5.00-L tank at 298 K. Determine the total pressure of the mixture, and find the partial pressures and mole fractions of the two... 

C05-0025. Find the partial pressures and mole fractions of a gas mixture that contains 1.00 g each of H2 and N2, if the total pressure of this mixture is 2.30 atm. 

Hence, if no experimental value for AuHi is available (i.e., from measurements of Ka( ) at different temperatures), it can be obtained from experimental (or estimated) AvapH, and Hfe values. Finally, we should note that Eq. 6-8 applies in a strict sense only if we express the amount of the compound in the gas and liquid phase as partial pressure and mole fraction, respectively. However, if we assume that the molar volume of the liquid, Vi, is not significantly affected by temperature changes, we may also apply Eq. 6-8 to describe the temperature dependence of K,n ( ) (Eq. 6-5) with a constant term that is given by constant + In Ve Furthermore, if we express the amount of the compound in the gas phase in molar concentrations (Eq. 6-6), then we have to add the term RTm to Aa< // where rav (in K) is the average temperature of the temperature range considered (see Section 3.4) ... 

In a gaseous mixture containing equal masses of CH4 and C02, the partial pressure of CH4 is 365 Torr. What is the partial pressure and mole fraction of C02 in this mixture ... 

Suppose 15.2 g of NO2 is placed in a 10.0-L flask at high temperature and the flask is cooled to 25°C. The total pressure is measured to be 0.500 atm. What partial pressures and mole fractions of NO2 and N2O4 are present ... 

In a diy atmosphere, the partial pressure and mole fraction are equal. Mole fractions for the major atmospheric gases are presented in Table 3.6, and the temperature dependence of PhjO at equilibrium with seawater, Pn o saturation equilibrium, water... 

The component concentration, moreover, can be converted to partial pressure (and mole fraction) via the equation of state for the total liquid phase, utilizing the compressibility factor, as is subsequently shown. 

Define Dalton s law of partial pressures and mole fraction. Does mole fraction have units ... 

Calculating Partial Pressures and Mole Fractions of a Gas in a Mixture... 

Calculating partial pressures and mole fractions of a gas in a mixture Given the masses of gases in a mixture, calculate the partial pressures and mole fractions. (EXAMPLE 5.10)... 

Commercial membranes today are asymmetric membranes. This means that the active membrane surface is only a very thin layer on top of a porous substrate. Components which permeate the membrane must travel out of the porous membrane substrate before entering the bulk permeate stream. Therefore, the effective partial pressure and mole fraction on the permeate side of the active membrane surface are only a function of the material passing through the membrane, not a function of the bulk permeate stream. 

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