The phase rule is expressed as

This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. See Answer See Answer See Answer done loading Question:(a) Zero (b) one (c) two (d) three ) 4. For two component system, the phase rule can be expressed as (a) F-4-P (b) F=3-P (c) F=2-P (d) F=1-P 5. One mole ideal gas, initially at 100°C, is expanded isothermally and reversibly from P1 =100kPa to P2 = 50kPa, the internal energy change AU (a) 200 (b) 100 (c) 50 (d) 0 4. F 6. 5. (a) Zero (b) one (c) two (d) three ) 4. For two component system, the phase rule can be expressed as (a) F-4-P (b) F=3-P (c) F=2-P (d) F=1-P 5. One mole ideal gas, initially at 100°C, is expanded isothermally and reversibly from P1 =100kPa to P2 = 50kPa, the internal energy change AU (a) 200 (b) 100 (c) 50 (d) 0 4. F 6. 5. Previous question Next question

Consider the binary system (Figure 2) that describes the 5) and 2Si 2O 8). The melt can range in 5 to pure CaAl 2Si 2O 8, but the solids show no compositional substitution. All phases therefore have the composition of CaSiTiO 5, CaAl 2Si 2O 8, or a P + F = C + 1. In this form it is called the condensed phase rule, for any 5 at the left to pure CaAl 2Si 2O 8 at the right). The phase fields (separated by the A presents a liquid whose composition is 70 percent CaAl 2Si 2O 8 and 30 percent CaSiTiO 5. The B consists of liquid C (43 percent CaSiTiO 5 and 57 percent CaAl 2Si 2O 8) and solid anorthite D. A sample at point E at a lower temperature consists of the solids titanite ( F) and anorthite ( G). Liquid CaAl 2Si 2O 8 cools to produce solid anorthite at 1,550 °C, whereas liquid CaSiTiO 5 cools to produce solid titanite at 1,390 °C. If the batch were a mixture of the two components, the 5, all atoms could add to titanite nuclei to form crystals of titanite. If, however, the melt contained 30 percent CaAl 2Si 2O 8, the rate of formation of titanite nuclei would be decreased, as 30 percent of the melt could not contribute to their formation. In order to increase the rate of formation of titanite nuclei and promote crystallization, the temperature of the melt must be decreased below the freezing point of pure CaSiTiO 5. When cooled, liquid A does not begin crystallization until temperature H is reached. Pure anorthite crystals 2Si 2O 8 from the melt causes the melt composition to...

Phase rule is a theoretical quantitative approach for predicting the effect of change in temperature, pressure, and concentration on a heterogeneous system in equilibrium. This relationship was given by American physicist Gibb’s Phase Rule. It deals with the stability of phases present in the material at equilibrium conditions. According to Gibb’s phase rule, if the heterogeneous equilibrium system is not affected by gravity, electric or magnetic forces, or surface action, but gets influenced by temperature, pressure, and concentration, then the number of degree of freedom (F) of the system is given by F = C – P + 2 where, F = degree of freedom, P = phase, and C = component Thus, Gibb’s phase rule relates the degree of freedom (F), number of components (C), and number of phases of the system (P). Each of these terms has a special significance in the description of the heterogeneous system in equilibrium. Phase A phase is any homogenous part of a system that has the same physical and chemical properties that are separated from other parts by distinct boundary. Phases may either be pure compounds or mixtures such as solid or aqueous solutions, and a system can have one or more phases. For example, a system that contains liquid water, water vapor, and • A system containing two immiscible liquids has two-phase. • Two completely miscible liquids are one-phase systems. • Gaseous mixtures constitute one phase system. • Number of phases for a pure compound (solid, liquid, or gas) ...

\( \newcommand\) No headers \( \newcommand \) We encountered the Gibbs phase rule and phase diagrams in Chapter 8 in connection with single-substance systems. The present chapter derives the full version of the Gibbs phase rule for multicomponent systems. It then discusses phase diagrams for some representative types of multicomponent systems, and shows how they are related to the phase rule and to equilibrium concepts developed in Chapters 11 and 12.