3/30/2013. Vapor Pressure and Changes of State Phase Diagrams. Chapter 10 Sections 8, 9
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1 Vapor Pressure and Changes of State Chapter 10 Sections 8, 9 Vapor Pressure In a closed container, liquid evaporates. The vapor starts to condensate. Condensation and evaporation happens simultaneously. Eventually the rates of condensation and evaporation are equal. The pressure of the gas above the liquid is the vapor pressure. Vapor Pressure Liquid with high vapor pressures are volatile. The stronger the intermolecular force the higher the vapor pressure. Which would evaporate the quickest? Water, or Diethyl ether In general larger molecules have a lower vapor pressure. The more electrons, the polarizable it is, the greater the dispersion forces Vapor Pressure increases significantly with temperature. At higher temps more molecules have the minimum amount of energy to escape the intermolecular forces. 1
2 Vapor Pressure ln P vap = H vap R 1 T + C y = m x + b Look at the relationship between P vap and T H vap enthalpy of vaporization the energy to vaporize 1 mole of liquid at 1 atm. Water has a larger slope than diethyl ether. Water has a lower vapor pressure because it takes more energy for the molecules to escape the hydrogen bonds. Changes of State Heating Curve: a plot of temperature verses time for a process where energy is added at a constant rate. Changes of State Heating Curve: a plot of temperature verses time for a process where energy is added at a constant rate. Boiling Point No temperature change Energy increases the random motion of the molecules and thus the temperature Melting point No temperature change Energy is absorbed to overcome intermolecular forces, changing from liquid to gas. H vap enthalpy of vaporization Energy is absorbed to break the lattice, changing from solid to liquid. H fus enthalpy of fusion 2
3 Melting and boiling point are determined by vapor pressure. The point at which the vapor pressure of the solid is equal to the vapor pressure of the liquid is the melting point. Solid will release vapor but the liquid will absorb the vapor in order to reduce vapor pressure and keep its equilibrium. Solid will be converted to liquid through the gas phase. Solid will decrease and liquid will increase and eventually reach equilibrium with the gas Liquid requires a higher vapor pressure. Any gas released from the liquid will be converted to solid so that the solid can reach equilibrium with the gas. Liquid will decrease and solid will increase and eventually reach equilibrium with the gas 3
4 Liquid and solid have the same vapor pressure so they can coexist with the gas. Melting and freezing occur at the same time. Boiling Point Normal boiling point of a liquid is the temperature at which the vapor pressure of the liquid is exactly 1 atmosphere Boiling P = 1 atm When the temp rises enough that the vapor pressure of the liquid is equal to the pressure above the liquid then boiling occurs. Evaporation occurs on the surface In a closed container, liquid evaporates. The vapor starts to condensate. Condensation and evaporation happens simultaneously. Eventually the rates of condensation and evaporation are equal. The pressure of the gas above the liquid is the vapor pressure. Represents phases as a function of temperature and pressure in a closed system normal = temp at 1 atm melting point, boiling point and sublimation point must be defined at a specific temp and pressure 4
5 Sublimation is when the substance goes from solid to the liquid state. Deposition occurs when a substance goes from a vapor state to a solid state. It is the reverse process of Sublimation. Melting occurs when a substance goes from a solid to a liquid state. Fusion is when a substance goes from a liquid to a solid state, the reverse of melting. Vaporization (or evaporation) is when a substance goes from a liquid to a gaseous state. Condensation occurs when a substance goes from a gaseous to a liquid state, the reverse of vaporization. Critical Point the point in temperature and pressure on a phase diagram where the liquid and gaseous phases of a substance merge together into a single phase. Beyond the temperature of the critical point, the merged single phase is known as a supercritical fluid. Triple Point occurs when both the temperature and pressure of the three phases of the substance coexist in equilibrium. LIQUID SOLID GAS 5
6 What is occurring during each experiment if the pressure is constant and temperature is changed? Critical point at high T & P liquid and gas phase are virtually indistinguishable. (D) Critical pressure the minimum pressure to produce liquefaction of a substance at critical temp. Critical temp. the temp at which vapor cannont be liquefied no matter what pressure is applied. Carbon Dioxide Solid CO 2 is more dense than liquid CO 2 CO 2 sublimes at common T & P Water Solid H 2 O is less dense than liquid H 2 O 6
7 Applications of for H 2 O In skating at the blade puts additional pressure on the ice the solid/liquid line is crossed. Water acts as a lubricate so that skating is smooth motion As pressure is increased the volume should be decreased. Solid H 2 O has a lower density than liquid H 2 O. The same mass of H 2 O has a larger volume as a solid than a liquid. So to decrease the volume the H 2 O changes from solid to liquid. There is some debate as to whether the pressure or friction is melting the ice. 7
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