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Supercritical Fluid

Supercritical Fluid. as a liquid is heated in a sealed container, more vapor collects causing the pressure inside the container to rise and the density of the vapor to increase and the density of the liquid to decrease

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Supercritical Fluid

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  1. Supercritical Fluid • as a liquid is heated in a sealed container, more vapor collects causing the pressure inside the container to rise • and the density of the vapor to increase • and the density of the liquid to decrease • at some temperature, the meniscus between the liquid and vapor disappears and the states commingle to form a supercritical fluid • supercritical fluid have properties of both gas and liquid states Tro, Chemistry: A Molecular Approach

  2. http://www.youtube.com/watch?v=yBRdBrnIlTQ Tro, Chemistry: A Molecular Approach

  3. Tro, Chemistry: A Molecular Approach

  4. Tro, Chemistry: A Molecular Approach

  5. The Critical Point • the temperature required to produce a supercritical fluid is called the critical temperature • the pressure at the critical temperature is called the critical pressure • at the critical temperature or higher temperatures, the gas cannot be condensed to a liquid, no matter how high the pressure gets Tro, Chemistry: A Molecular Approach

  6. deposition Sublimation and Deposition • molecules in the solid have thermal energy that allows them to vibrate • surface molecules with sufficient energy may break free from the surface and become a gas – this process is called sublimation • the capturing of vapor molecules into a solid is called deposition • the solid and vapor phases exist in dynamic equilibrium in a closed container • at temperatures below the melting point • therefore,molecular solids have a vapor pressure sublimation solid gas Tro, Chemistry: A Molecular Approach

  7. Sublimation Tro, Chemistry: A Molecular Approach

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  9. Melting = Fusion • as a solid is heated, its temperature rises and the molecules vibrate more vigorously • once the temperature reaches the melting point, the molecules have sufficient energy to overcome some of the attractions that hold them in position and the solid melts (or fuses) • the opposite of melting is freezing Tro, Chemistry: A Molecular Approach

  10. Heating Curve of Water

  11. Phase Diagrams • describe the different states and state changes that occur at various temperature - pressure conditions • areas represent states • lines represent state changes • liquid/gas line is vapor pressure curve • both states exist simultaneously • critical point is the furthest point on the vapor pressure curve • triple point is the temperature/pressure condition where all three states exist simultaneously • for most substances, freezing point increases as pressure increases Tro, Chemistry: A Molecular Approach

  12. Fusion Curve critical point melting freezing 1 atm Sublimation Curve vaporization triple point condensation Vapor Pressure Curve sublimation deposition Phase Diagrams Liquid Solid Pressure normal boiling pt. normal melting pt. Gas Temperature

  13. Tro, Chemistry: A Molecular Approach

  14. critical point 374.1°C 217.7 atm Water Ice Pressure normal melting pt. 0°C normal boiling pt. 100°C 1 atm triple point 0.01°C 0.006 atm Steam Temperature Phase Diagram of Water

  15. Water – An Extraordinary Substance • water is a liquid at room temperature • most molecular substances with small molar masses are gases at room temperature • due to H-bonding between molecules • water is an excellent solvent – dissolving many ionic and polar molecular substances • because of its large dipole moment • even many small nonpolar molecules have solubility in water • e.g., O2, CO2 • water has a very high specific heat for a molecular substance • moderating effect on coastal climates • water expands when it freezes • at a pressure of 1 atm • about 9% • making ice less dense than liquid water Tro, Chemistry: A Molecular Approach

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