{"id":1635,"date":"2020-06-26T16:36:34","date_gmt":"2020-06-26T20:36:34","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chbe220\/?post_type=part&p=1635"},"modified":"2020-08-10T16:02:09","modified_gmt":"2020-08-10T20:02:09","slug":"phase-equilibrium","status":"publish","type":"part","link":"https:\/\/pressbooks.bccampus.ca\/chbe220\/part\/phase-equilibrium\/","title":{"raw":"Phase Equilibrium","rendered":"Phase Equilibrium"},"content":{"raw":"

Introduction<\/h2>\r\nPhase equilibrium can be used to control the concentration of components. It is also a concept widely used in various types of separation processes. In this chapter, we will learn to collect information from existing diagrams, including variations of phase diagrams for pure components and diagrams summarizing vapour-liquid equilibrium conditions for multicomponent systems. We can use the information to find the phase(s) of components in our processing equipment and the mole fractions of components in each phase.\r\n
\r\n

Learning Objectives<\/p>\r\n\r\n<\/header>\r\n

\r\n\r\nBy the end of this chapter, you should be able to:\r\n\r\nInterpret<\/strong>\u00a0phase diagrams for relevant thermodynamic information (e.g. composition, temperature, pressure\u2026)\r\nApply <\/strong>the definition of intensive and extensive properties to process variables\r\nDescribe <\/strong>the relationship between variables of state for gases\r\nDescribe<\/strong> gas behaviour using the ideal gas law and compressibility factor for equations of state\r\nEstimate<\/strong> the vapour pressure of pure compounds at a given temperature using Antoine's equation\r\nApply<\/strong> properties of ideal mixtures to describe vapour-liquid separations\r\nRead<\/strong> Txy and Pxy diagrams for binary mixtures\r\nFind<\/strong> bubbles points and dew points on the diagrams\r\nCalculate<\/strong> the mole fraction of substances in the vapour and liquid phases\r\n\r\n<\/div>\r\n<\/div>\r\n \r\n\r\nAs you're going through this chapter, here are some important terms for you to take note of:\r\n
    \r\n \t
  • physical properties<\/li>\r\n \t
  • pressure<\/li>\r\n \t
  • manometer<\/li>\r\n \t
  • gauge pressure<\/li>\r\n \t
  • absolute pressure<\/li>\r\n \t
  • temperature<\/li>\r\n \t
  • heat transfer<\/li>\r\n \t
  • absolute temperature<\/li>\r\n \t
  • extensive variables<\/li>\r\n \t
  • intensive variables<\/li>\r\n \t
  • phase transitions<\/li>\r\n \t
  • intermolecular forces<\/li>\r\n \t
  • critical point<\/li>\r\n \t
  • triple point<\/li>\r\n \t
  • phase diagram<\/li>\r\n \t
  • supercritical fluid<\/li>\r\n \t
  • reduced temperature\/pressure<\/li>\r\n \t
  • thermodynamic system<\/li>\r\n \t
  • surroundings\/environment<\/li>\r\n \t
  • boundary<\/li>\r\n \t
  • Gibb's Phase Rule<\/li>\r\n \t
  • degrees of freedom<\/li>\r\n \t
  • compressible\/incompressible<\/li>\r\n \t
  • ideal gas law<\/li>\r\n \t
  • molar volume<\/li>\r\n \t
  • Dalton's law<\/li>\r\n \t
  • Amgat's law<\/li>\r\n \t
  • partial pressure<\/li>\r\n \t
  • mole fraction<\/li>\r\n \t
  • vapour temperature<\/li>\r\n \t
  • vapour pressure<\/li>\r\n \t
  • Antoine equation<\/li>\r\n \t
  • vapour-liquid equilibrium<\/li>\r\n \t
  • Raoult's law<\/li>\r\n \t
  • Henry's law<\/li>\r\n \t
  • volatile<\/li>\r\n \t
  • solubility<\/li>\r\n \t
  • Txy\/Pxy diagram<\/li>\r\n \t
  • ideal mixture<\/li>\r\n \t
  • binary mixture<\/li>\r\n \t
  • bubble point<\/li>\r\n \t
  • dew point<\/li>\r\n \t
  • saturated liquid<\/li>\r\n \t
  • saturated vapour<\/li>\r\n<\/ul>","rendered":"

    Introduction<\/h2>\n

    Phase equilibrium can be used to control the concentration of components. It is also a concept widely used in various types of separation processes. In this chapter, we will learn to collect information from existing diagrams, including variations of phase diagrams for pure components and diagrams summarizing vapour-liquid equilibrium conditions for multicomponent systems. We can use the information to find the phase(s) of components in our processing equipment and the mole fractions of components in each phase.<\/p>\n

    \n
    \n

    Learning Objectives<\/p>\n<\/header>\n

    \n

    By the end of this chapter, you should be able to:<\/p>\n

    Interpret<\/strong>\u00a0phase diagrams for relevant thermodynamic information (e.g. composition, temperature, pressure\u2026)
    \nApply <\/strong>the definition of intensive and extensive properties to process variables
    \nDescribe <\/strong>the relationship between variables of state for gases
    \nDescribe<\/strong> gas behaviour using the ideal gas law and compressibility factor for equations of state
    \nEstimate<\/strong> the vapour pressure of pure compounds at a given temperature using Antoine’s equation
    \nApply<\/strong> properties of ideal mixtures to describe vapour-liquid separations
    \nRead<\/strong> Txy and Pxy diagrams for binary mixtures
    \nFind<\/strong> bubbles points and dew points on the diagrams
    \nCalculate<\/strong> the mole fraction of substances in the vapour and liquid phases<\/p>\n<\/div>\n<\/div>\n

     <\/p>\n

    As you’re going through this chapter, here are some important terms for you to take note of:<\/p>\n

      \n
    • physical properties<\/li>\n
    • pressure<\/li>\n
    • manometer<\/li>\n
    • gauge pressure<\/li>\n
    • absolute pressure<\/li>\n
    • temperature<\/li>\n
    • heat transfer<\/li>\n
    • absolute temperature<\/li>\n
    • extensive variables<\/li>\n
    • intensive variables<\/li>\n
    • phase transitions<\/li>\n
    • intermolecular forces<\/li>\n
    • critical point<\/li>\n
    • triple point<\/li>\n
    • phase diagram<\/li>\n
    • supercritical fluid<\/li>\n
    • reduced temperature\/pressure<\/li>\n
    • thermodynamic system<\/li>\n
    • surroundings\/environment<\/li>\n
    • boundary<\/li>\n
    • Gibb’s Phase Rule<\/li>\n
    • degrees of freedom<\/li>\n
    • compressible\/incompressible<\/li>\n
    • ideal gas law<\/li>\n
    • molar volume<\/li>\n
    • Dalton’s law<\/li>\n
    • Amgat’s law<\/li>\n
    • partial pressure<\/li>\n
    • mole fraction<\/li>\n
    • vapour temperature<\/li>\n
    • vapour pressure<\/li>\n
    • Antoine equation<\/li>\n
    • vapour-liquid equilibrium<\/li>\n
    • Raoult’s law<\/li>\n
    • Henry’s law<\/li>\n
    • volatile<\/li>\n
    • solubility<\/li>\n
    • Txy\/Pxy diagram<\/li>\n
    • ideal mixture<\/li>\n
    • binary mixture<\/li>\n
    • bubble point<\/li>\n
    • dew point<\/li>\n
    • saturated liquid<\/li>\n
    • saturated vapour<\/li>\n<\/ul>\n","protected":false},"parent":0,"menu_order":2,"template":"","meta":{"pb_part_invisible":false,"pb_part_invisible_string":""},"contributor":[],"license":[],"class_list":["post-1635","part","type-part","status-publish","hentry"],"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/pressbooks\/v2\/parts\/1635","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/pressbooks\/v2\/parts"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/wp\/v2\/types\/part"}],"version-history":[{"count":4,"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/pressbooks\/v2\/parts\/1635\/revisions"}],"predecessor-version":[{"id":2505,"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/pressbooks\/v2\/parts\/1635\/revisions\/2505"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/wp\/v2\/media?parent=1635"}],"wp:term":[{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/wp\/v2\/contributor?post=1635"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chbe220\/wp-json\/wp\/v2\/license?post=1635"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}