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posted by  qman on 9/9/2008 6:40:41 PM  |  status: Live  

gen chem prob

Course Textbook Chapter Problem
General Chemistry N/A N/A N/A
Question Details:
A quanity of 2.40 moles of pure SO2Cl2 gas was placed in an 8.00 L sealed flask. At 500 K, after equilibirum is established, there are 1.60 moles of the product gas SO2 present. Calculate Kc for the reaction.       SO2Cl2 (g)  SO2 (g) + Cl2 (g)

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Sage
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posted by Jesley on 9/9/2008 9:33:01 PM  |  status: Live
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qman's comment:
"thanks, very helpful"
Response Details:
initial concentration of SO2Cl2  = 2.40mol/8.00L
                                                   = 0.300M
the concentration of SO2 at equilibrium = 1.60mol/8.00L
                                                           = 0.200M
for the reaction  the ICE table is
                             SO2Cl2 (g)  SO2 (g) + Cl2 (g)
initial:                     0.300M                0              0
change:                 -0.200M           0.200M         0.200M
equilibrium :           0.100M             0.200M        0.200M
 
the equilibrium constant (Kc) is related to the concentration as
Kc = [SO2 ][Cl2]/[SO2Cl2]
Kc =(0.200M*0.200M)/(0.100M)
            Kc =0.4
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