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Gases equilibrium with water

The column (or line entry) headed a gives the volume of gas (in milliliters) measured at standard conditions (0°C and 760 mm or 101.325 kN dissolved in 1 mL of water at the temperature stated (in degrees Celsius) and when the pressure of the gas without that of the water vapor is 760 mm. The line entry A indicates the same quantity except that the gas itself is at the uniform pressure of 760 mm when in equilibrium with water. [Pg.362]

Each gas establishes its own dynamic equilibrium with water. The concentration depends on the partial pressure of the gas in the atmosphere and on the value of its Henry s law constant at 25 °C. Recall from Chapter 5 that the partial pressure of any gas in a mixture is given by the mole fraction (X multiplied by total pressure. [Pg.853]

The hypochlorous acid oxidizes the cell walls and kills bacteria. Solid calcium hypochlorite, Ca(OCl)2, and liquid solutions of sodium hypochlorite, NaOCl, can be used to generate hypochlorous acid in place of chlorine gas, for example, in chlorinating swimming pools. The hypochlorite ion generated from Ca(OCl)2 and NaOCl forms an equilibrium with water represented by the equation ... [Pg.275]

I. R. McHafie studied the cone, of water in the gas phase with air in equilibrium with water. F. Garelli and E. Monath observed no appreciable lowering of the f.p. of stannous chloride by the dissolution of nitrogen. [Pg.76]

A, Volume of gas in milliliters (mL). The line entry A indicates the same quantity as a except that the gas itself is at the uniform pressure of 760 mm when in equilibrium with water. [Pg.461]

This tells us that the solubility of a gas dissolved from a gaseous mixture (air in this problem) is directly proportional to the partial pressure of the gas. The proportionality constant, k, is called Henry s law constant. (Note Some authors define the Henry s law constant as the reciprocal of the % USC(J here.) To evaluate k from the data, note that when pure oxygen is in equilibrium with water at a total pressure of 760 torr,... [Pg.230]

Normal contract specfication for gas to be transmitted through a high-pressure pipeline is a water content of 7 lb of water per million standard cubic feet of natural gas. This is approximately the water content of natural gas in equilibrium with water at the freezing point (32°F) when the gas is under a pressure of 1000 psia. [Pg.921]

At the same time, there is no crude physical controversy in this approach. The largest pores are those which are obtained at given Pc by capillary condensation. Gas filled pores, that is, pores with larger radii than those corresponding to Eq. (3) do not exist, and water-filled pores do not conduct gas. Equilibrium with the gas outside the membrane is established. [Pg.465]

The case kpem 1 corresponds to the situation when the overall water transport is limited by interfacial vaporization exchange. For kpem 1. bulk water permeation in the PEM is the limiting process. For a given type of membrane, a critical thickness IpEM can be defined, which marks the transition between these two regimes, as will be shown below. As noted in Monroe et al. (2008), the condition kpem 1 does not imply that absorbed water at the surface of the PEM attains equilibrium with water vapor in the gas. [Pg.375]

The critical temperature of the second layering transition is always lower than the critical temperature of the first one, and it was found between 0.48 T and 0.59 Tc. Similar behavior was found by density functional calculations for a strongly associative LJ fluid in pores [201-203]. Even near strongly hydrophilic surfaces, there are only two noticeable density oscillations of liquid water when it is in equilibrium with a saturated vapor. Water properties (e.g., orientational ordering) in the third and subsequent layers are close to the bulk ones [205-208]. Therefore, the third and subsequent layering transitions of water should not be expected. When the water-surface interaction weakens, the critical temperature of the second layering transition drops down by about 50°, and the triple point, where 2D gas coexists with water monolayer and with water bilayer, may be seen (lower right panel in Fig. 21). [Pg.42]

I In section 3.8, the heat of subUmation for ice at 0°C was calculated as 51076 J/mol. At 0°C, the partial pressure of saturated water vapour in equilibrium with water and ice is 611.3 Pa. From this information, calculate the partial pressure of saturated water vapour in equilibrium with ice at —6°C The water vapour is assumed to be an ideal gas. [Pg.168]

BrCl exists in equilibrium with bromine and chlorine in both gas and liquid phases. Table 5 lists various physical properties of BrCl. Due to the polarity of BrCl, it shows greater solubility than bromine in polar solvents. In water, it has a solubility of 8.5 gms per 100 gms of water at 20 C (that is, 2.5 times the solubility of bromine 11 times that of chlorine). Bromine chloride s solubility in water is increased greatly by adding chloride ions to form the complex chlorobromate ion, BrCl 2. [Pg.477]

It is possible to inject glycol in a gas line and have it absorb the water vapor in co-current flow. Such a process is not as efficient as countercurrent flow, since the best that can occur is that the gas reaches near equilibrium with the rich glycol as opposed to reaching near equilibrium with... [Pg.200]

Curve A represents the equilibrium condition for tvater entering at 90°F, the gas entering saturated with water vapor at 90°F and isothermal tow er operation. [Pg.359]

Table 21.22 Saturated solubilities of atmospheric gases in sea-water at various temperatures Concentrations of oxygen, nitrogen and carbon dioxide in equilibrium with 1 atm (lOI 325 N m ) of designated gas... Table 21.22 Saturated solubilities of atmospheric gases in sea-water at various temperatures Concentrations of oxygen, nitrogen and carbon dioxide in equilibrium with 1 atm (lOI 325 N m ) of designated gas...
The vapor pressure of water, which is 24 mm Hg at 25°C, becomes 92 mm Hg at 50°C and 1 atm (760 mm Hg) at 100°C. The data for water are plotted at the top of Figure 9.2. As you can see, the graph of vapor pressure versus temperature is not a straight line, as it would be if pressure were plotted versus temperature for an ideal gas. Instead, the slope increases steadily as temperature rises, reflecting the fact that more molecules vaporize at higher temperatures. At 100°C, the concentration of H20 molecules in the vapor in equilibrium with liquid is 25 times as great as at 25°C. [Pg.229]

The preceeding discussion was confined mostly to the carbon deposition curves as a function of temperature, pressure, and initial composition. Also of interest, especially for methane synthesis, is the composition and heating value of the equilibrium gas mixture. It is desirable to produce a gas with a high heating value which implies a high concentration of CH4 and low concentrations of the other species. Of particular interest are the concentrations of H2 and CO since these are generally the valuable raw materials. Also, by custom it is desirable to maintain a CO concentration of less than 0.1%. The calculated heating values are reported as is customary in the gas industry on the basis of one cubic foot at 30 in. Hg and 15.6°C (60°F) when saturated with water vapor (II). Furthermore, calculations are made and reported for a C02- and H20-free gas since these components may be removed from the mixture after the final chemical reaction. Concentrations of CH4, CO, and H2 are also reported on a C02 and H20-free basis. [Pg.49]

Thus, if the mixture of carbon dioxide and oxygen is shaken up with water, both gases will begin to pass into solution, and their partial pressures in the gas mixture will change. When the amount of each in solution stands in a definite ratio to its partial pressure, there will be equilibrium, but the amounts dissolved will not be the same as if each gas had been separately brought in contact with the same quantities of liquid under a pressure equal to its initial partial pressure in the mixture. [Pg.277]

In a packed column, operating at approximately atmospheric pressure and 295 K, a 10% ammonia-air mixture is scrubbed with water and the concentration of ammonia is reduced to 0.1%. If the whole of the resistance to mass transfer may be regarded as lying within a thin laminar film on the gas side of the gas-liquid interface, derive from first principles an expression for the rate of absorption at any position in the column. At some intermediate point where the ammonia concentration in the gas phase has been reduced to 5%. the partial pressure of ammonia in equilibrium with the aqueous solution is 660 N/nr and the transfer rate is ]0 3 kmol/m2s. What is the thickness of the hypothetical gas film if the diffusivity of ammonia in air is 0.24 cm2/s ... [Pg.853]

Whenever we see the symbol it means that the species on both sides of the symbol are in dynamic equilibrium with each other. Although products (water molecules in the gas phase) are being formed from reactants (water molecules in the liquid phase), the products are changing back into reactants at a matching rate. With this picture in mind, we can now define the vapor pressure of a liquid (or a... [Pg.431]


See other pages where Gases equilibrium with water is mentioned: [Pg.386]    [Pg.180]    [Pg.386]    [Pg.84]    [Pg.134]    [Pg.88]    [Pg.290]    [Pg.82]    [Pg.420]    [Pg.199]    [Pg.13]    [Pg.190]    [Pg.396]    [Pg.263]    [Pg.221]    [Pg.1374]    [Pg.339]    [Pg.522]    [Pg.246]    [Pg.600]    [Pg.1360]    [Pg.246]    [Pg.319]    [Pg.196]    [Pg.199]    [Pg.550]    [Pg.188]    [Pg.746]   


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