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Total Pressure of the System

  1. Apr 1, 2016 #1
    1. The problem statement, all variables and given/known data
    Introduced into a 1.70 −L flask is 0.120 mol of PCl5(g); the flask is held at a temperature of 227∘C until equilibrium is established.
    PCl5(g)⇌PCl3(g)+Cl2(g)

    What is the total pressure of the gases in the flask at this point? [Hint: Use data from Appendix D in the textbook and appropriate relationships from this chapter.]

    2. Relevant equations
    From the data tables I got ΔG for the following to be:
    Cl2 = 0
    PCl3 = -267.8
    PCl5 = -305
    From this I know ΔG to be 37.2.

    ΔG=-RTln(K) (1)
    PV=nRT (2)

    3. The attempt at a solution
    Using equation (1) I found K and then found the moles of each substance at equilibrium. I added these together and put them into equation (2) to get P. This isn't working for me. Is there a better way to do it?
     
  2. jcsd
  3. Apr 1, 2016 #2
    Show us more of the details, please.
     
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