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** Compression of gases non-ideal **

** Equation of State non-ideal gases **

** Model of non-ideal lattice gas **

Abstract. A phase equilibriums in intermetallic compounds hydrides in the area of disordered a-, (3-phase in the framework of the model of non-ideal lattice gas are description. LaNi5 hydride was chosen as the subject for the model verification. Position of the critical point of the P—w.-transition in the LaNi5-hydrogen system was definite. [Pg.187]

The results of the calculations show that with increasing pressure the equilibrium yield of ammonia is increasing and that the non-ideality of the gas mixtures has in this case a positive effect on the equilibrium conversion. [Pg.57]

It is to emphasize that, the method of estimating Henry s law constants, and the gas partial pressure or concentration units must be specified. Corrections should be made for the possible non-ideality of the gas phase or the non-applicability of Henry s law, particularly, for cases of high pressure and elevated temperature measurements. [Pg.61]

The lattice-gas model allows to use it for studying the effect of the lateral interactions between the adspecies on the surface process rate or, in other words, to consider the non-ideality of the reaction system in the surface process kinetics. In the lattice-gas model the interaction of adspecies / and j in sites / and g at the distance r is set by the energy parameter sjg(r). In the homogeneous lattice systems such distances can be conveniently determined with the use of the numbers of the (c.s.) where site g is located relative to site /. In this case in the parameter y(r) the index r runs a discrete series of values from 1 to R, where R is the interaction radius 1

This can be illustrated by showing the net work involved in various adiabatic paths by which one mole of helium gas (4.00 g) is brought from an initial state in whichp = 1.000 atm, V= 24.62 1 [T= 300.0 K], to a final state in whichp = 1.200 atm, V= 30.7791 [T= 450.0 K]. Ideal-gas behaviour is assumed (actual experimental measurements on a slightly non-ideal real gas would be slightly different). Infomiation shown in brackets could be measured or calculated, but is not essential to the experimental verification of the first law. [Pg.329]

For precise measurements, diere is a slight correction for the effect of the slightly different pressure on the chemical potentials of the solid or of the components of the solution. More important, corrections must be made for the non-ideality of the pure gas and of the gaseous mixture. With these corrections, equation (A2.1.60) can be verified within experimental error. [Pg.359]

For an ideal monoatomic gas, the Gibbs energy at constant temperature and pressure varies with the logarithm of the molecular density. The additional terms in in equation (2.9.25) give the contribution to G due to the non-ideality of the hard-sphere system with respect to an ideal gas. [Pg.83]

Adsorption manometry allows an easy outgassing in a separate unit and lends itself to multiple sample operation, ie to numerous experiments, but requests a satisfactory knowledge about the non-ideality of the gas used. [Pg.728]

H (MPa) (Eq. (13)) and HA (MPa m3 mor1) (Eq. (14)) are often referred to as Henry s constant , but they are in fact definitions which can be used for any composition of the phases. They reduce to Henry s law for an ideal gas phase (low pressure) and for infinitely dilute solution, and are Henry s constant as they are the limit when C qL (or xA) goes to zero. When both phases behave ideally, H depends on temperature only for a dilute dissolving gas, H depends also on pressure when the gas phase deviates from a perfect gas finally, for a non-ideal solution (gas or liquid), H depends on the composition. This clearly shows that H is not a classical thermodynamic constant and it should be called Henry s coefficient . [Pg.1523]

Many process components do not conform to the ideal gas laws for pressure, volume and temperature relationships. Therefore, when ideal concepts are applied by calculation, erroneous results are obtained—some not serious when the deviation from ideal is not significant, but some can be quite serious. Therefore, when data are available to confirm the ideality or non-ideality of a system, then the choice of approach is much more straightforward and can proceed with a high degree of confidence. [Pg.4]

** Compression of gases non-ideal **

** Equation of State non-ideal gases **

** Model of non-ideal lattice gas **

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