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Heat of Vaporization

  1. Mar 22, 2005 #1
    How would you calculate the heat of vaporization of titanium (IV) chloride using the following data:

    Ti (s) + 2Cl2 (g)-----TiCl4 (l) Standard Molar Enthalpy of formation= -804.2 KJ/mole

    Ti (s) + 2Cl2 (g)-----TiCl4 (g) Standard Molar Enthalpy of formation= -763.2 KJ/mole



    Is it something as simple as subtracting or adding the two numbers?
     
  2. jcsd
  3. Mar 22, 2005 #2
    What would be your reaction for the heat ot vaporization? How would that relate to the two equations you have written?
     
  4. Mar 23, 2005 #3

    DH

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    this is very easy problem!
    Heat of vaporization of Titanium 4 cloride: heat required to vaporized Tian...
    --> from liquid to gas
    -------------
    Solve: you reverse the first equation:
    TiCl4 (l) --->Ti (s) + 2Cl2 (g) Standard Molar Enthalpy of formation= +804.2 KJ/mole
    Then you combine with the second

    Ti (s) + 2Cl2 (g)-----TiCl4 (g) Standard Molar Enthalpy of formation= -763.2 KJ/mole
    You have:
    Ti (s) + 2Cl2 (g) + TiCl4 (l)-----TiCl4 (g) + Ti (s) + 2Cl2 (g)
    so, TiCl4(l) --> TiCl4(g) Enthalpy = -763.2 + 804.2 = 41 KJ/mole

    -------------------
    This may be the correct answer!
    But this problem is not like that!
     
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