Definition of phase , component and degrees of freedom . Ideal and non - ideal solutions , Principal of fractional distillation of liquid-liquid mixtures, azeotrop

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ruchi yadav · Answer

Liquid water is stable over a range of temperatures and pressures - that is, within certain well-defined limits, we can arbitrarily choose a pressure and temperature, and the system will still be in the liquid water field on the phase diagram for water. On the other hand , the equilibrium (i.e., mechanically, thermally and chemically balanced) coexistence of pure liquid water AND pure ice is rather restricted: at an arbitrarily chosen pressure, there is only one temperature at which liquid and solid H2O can coexist in equilibrium. When only one phase is stable, there is a greater degree of freedom in choosing P and T; when two phases are stable, the system has *less freedom*. We say that the number of degrees of freedom has been reduced by one when there is an additional phase in an assemblage. Examining this relationship further, we find that ice/water coexistence at any given pressure is expanded from a unique single temperature at the given pressure to a RANGE of temperatures by adding a second component (such as NaCl) to the system. That is, the degrees of freedom can be increased by increasing the number of components. In general, the number of degrees of freedom in a system of phases is equal to the number of system components + 2 minus the number of phases: F = C + 2 - p the greater the number of components C, the greater the number of degrees of freedom; the greater the number of coexisting phases, p, the fewer the number of degrees of freedom Thank You Ruchi Askiitians Faculty

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Definition of phase , component and degrees of freedom . Ideal and non - ideal solutions , Principal of fractional distillation of liquid-liquid mixtures, azeotrop

Definition of phase , component and degrees of freedom . Ideal and non - ideal solutions , Principal of fractional distillation of liquid-liquid mixtures, azeotrop

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