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What is the equilibrium partial pressure of PCl5?

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Date Posted: 7/2/2008 1:39:17 AM  Status: Live
What is the equilibrium partial pressure of PCl5?
Course Textbook Chapter Problem
General Chemistry N/A N/A N/A
Question Details:
Phosphorous trichloride and phosphorus pentachloride equilibrate in the presense of molecular chlorine according to the reaction

 
Keq=2.01 at 500K. A 1.000L reaction vessel is charged with .300mol of PCl5 and allowed to equilibrate at this temperature.

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Sage
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Date Posted: 7/2/2008 2:19:38 AM  Status: Live
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Response:
the reaction is
 PCl3(g) + Cl2(g)--->PCl5(g)

initial concentration of PCl5= 0.3mol/1L = 0.300M
                      [PCl3]                 [Cl2]                    [PCl5] 
initial:                  0                       0                       0.300 
change:               -x                          -x                    +x
final:                      -x                        -x                 (0.3+x)
the  equilibrium constant is related to the concentrations as
Kc=[PCl5] / [PCl3]  [Cl2] = (0.3+x) /x2= 2.01
solving for x,
we get, x=0.708M
equilibrium concentration of [PCl5] = 1.008mol/L
we know that, PV=nRT
                    p = 1.008mol/L*(0.08206atm.L/mol.K)*500K = 41.36atm
Pyrorei's Comment:
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