Phase equilibrium studies in some systems with a supercritical or near-critical component.
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Phase equilibrium studies in some systems with a supercritical or near-critical component. by Kassim Mohammed Kassim

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Published by University of Birmingham in Birmingham .
Written in English


Book details:

Edition Notes

Thesis (Ph.D.)- University of Birmingham, Dept of Chemical Engineering, 1977.

ID Numbers
Open LibraryOL20009630M

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The phase condition required for a given reacting system is studied at subcritical and supercritical conditions. The four cardinal points of phase equilibrium engineering are: the chemical plant or process, the laboratory, the modeling of phase equilibria and the simulator. The phase equilibrium is a thermodynamic condition which is required in several processes and products. The definition of this condition is indispensable to provide a food product in the desired specifications. Processes involving heat and mass transfer or even physical changes of state need the knowledge of phase equilibrium. The system consists of 2 phases in equilibrium, a dense liquid and a low density gas. Phase Diagram for Carbon Dioxide This diagram indicates the supercritical fluid region of CO 2. As the critical temperature is approached ( K), the density of the gas at equilibrium becomes denser, and that of the liquid becomes lower. Figure gives the (liquid + liquid) phase equilibrium diagram for the (x 1 n-C 6 H 14 + x 2 CH 3 OH) system. Two liquid phases L 1 and L 2 can exist in equilibrium in this system. Figure a is a graph of temperature against mole fraction with the pressure held constant, with the line giving the compositions of the phases in equilibrium. A horizontal tie-line in the two-phase region.

  The phase equilibrium studies between the solute and the supercritical fluids must be understood precisely for feasible process design, and further research is likely to continue in this area,. Subsequently, research studies will be required to understand the kinetics, mass transfer mechanism along with knowledge about process design and. Phase equilibrium is the study of the equilibrium which exists between or within different states of matter namely solid, liquid and gas. Equilibrium is defined as a stage when chemical potential of any component present in the system stays steady with time. Phase is a region where the intermolecular interaction is spatially uniform or in [ ]. The phase equilibrium of the ternary system carbon dioxide + water + acetic acid and the quaternary systems carbon dioxide + water + acetic acid + (sodium chloride or sodium acetate) was investigated experimentally for temperatures between and K at pressures up to 16 MPa. The measurements were performed with an apparatus realizing the. checking the phase equilibrium when the solid solubility data is measured [24,25]. T h ek now ldg fp a sb v i ru t u n drthSCFc ois a lf v p-m en tof aySCF p rc s.D h very limited data on the phase behavior of solid solutes in supercritical CO 2, which is particularly true for multicompo-nent systems. The reasons for lack of phase behavior data.

A supercritical fluid (SCF) is any substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not can effuse through solids like a gas, and dissolve materials like a liquid. In addition, close to the critical point, small changes in pressure or temperature result in large changes in density, allowing many properties of a supercritical. The phase rule is a general principle governing systems in thermodynamic F is the number of degrees of freedom, C is the number of components and P is the number of phases, then = − + It was derived by Josiah Willard Gibbs in his landmark paper titled On the Equilibrium of Heterogeneous Substances, published in parts between and conditions of the system at equilibrium.) The phase rule applies to dynamic and reversible processes where a system is heterogeneous and in equilibrium and where the only external variables are temperature, pressure and concentration. For one-component systems the maximum number of variables to be considered is two – pressure and temperature. This new book provides, for the first time, a thorough survey of the techniques and equipment for both high- and low-pressure phase equilibrium measurement and addresses the equally challenging task of accurately modeling or predicting the equilibria. The book is unique because it combines in depth and authoritative coverage of both experimental and theoretical procedures in a single volume.