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where n is the number of phases, N is the number of chemical species, and F is called the degrees of freedom of the system The intensive state of a system at equilibrium is established when its temperature, pressure, and the compositions of all phases are fixed These are therefore phase-rule variables, but they are not all independent The phase rule gives the number of variables from this set which must be arbitrarily specified to fix all remaining phase-rule variables A phase is a homogeneous region of matter A gas or a mixture of gases, a liquid or a liquid solution, and a crystalline solid are examples of phases A phase need not be continuous; examples of discontinuous phases are a gas dispersed as bubbles in a liquid, a liquid dispersed as droplets in another liquid with which it is immiscible, and solid crystals dispersed in either a gas or liquid In each case a dispersed phase is distributed throughout a continuous phase An abrupt change in properties always occurs at the boundary between phases Various phases can coexist, but they must be in equilibrium for the phase rule to apply An example of a three-phase system at equilibrium is a saturated aqueous salt solution at its boiling point with excess salt crystals present The three phases (n= 3) are crystalline salt, the saturated aqueous solution, and vapor generated at the boiling point The two chemical species ( N = 2) are water and salt For this system, F = 1 The phase-rule variables are intensive properties, which are independent of the extent of the system and of the individual phases Thus the phase rule gives the same information for a large system as for a small one and for different relative amounts of the phases present Moreover, only the compositions of the individual phases are phase-rule variables Overall or total compositions are not phase-rule variables when more than one phase is present The minimum number of degrees of freedom for any system is zero When F = 0 , the system is invariant; Eq (27) becomes n = 2 N This value of n is the maximum number of phases which can coexist at equilibrium for a system containing N chemical species When N = 1, this number is 3, characteristic of a triple point (Sec 31) For example, the triple point of water, where liquid, vapor, and the common form of ice exist together in equilibrium, occurs at 27316 K (OOl C) and 00061 bar Any change from these conditions causes at least one phase to disappear.

When a .NET application begins, the framework calls a method named Main somewhere in your code. You indicate which form s Main routine is used through the Startup form field. It includes a list of all forms; just choose the one you want. But wait, you haven t added a Main method to any of your forms No problem. Visual Basic will write a simple Main routine on your behalf that will display the indicated form. This ad hoc Main routine, added at compile time, performs just the minimum processing needed to display the form. If you want to add a custom Main routine to your form, or to some other non-Form class in your application, that s no problem. If you uncheck the Enable application framework field on that same properties form, the Startup form list changes to

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4~osiah Willard Gibbs (1839-1903), American mathematical physicist he justification of the phase rule for nonreacting systems is given in Sec 102, and the phase rule for reacting systems is considered in Sec 138

5 Keep adding and removing selections until you re happy with the result Choose Copy | Edit from the main menu 6 Now you need to create a new home for this image: Choose File | New from the main menu In the New Image dialog box, make sure that the width and height of the new image are at least as big as the selection you just made, and then click OK You should see a new, empty window appear onscreen This is where you re going to paste your selection

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