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I need help with this question:

Sulfur dioxide reacts with chlorine at 227 oC:

SO2(g) +Cl2(g) ↔ SO2Cl2(g)

Kp for this reaction is 5.1 x 10-2 atm-1. Initially, 1.00 g each of SO2 and Cl2 are placed in a 1.00 L reaction vessel. After 15 minutes, the concentration of SO2Cl2 is 45.5 μg/mL. You will determine if the system has reached equilibrium. First, what is Kc (in L/mol)? (A μg is 10-6 g.)

Next determine all initial concentrations. What is the initial sulfur dioxide concentration (in mol/L or M)?


Determine all concentrations after 15 minutes. What is the chlorine concentration?


What is Q after 15 minutes?
This is the one I can't get. I got 1.49, but that's not right?

Then there's this question which is also an extension:
Calculate the mass (in g) of SO2Cl2 expected at equilibrium.

I got .558 but that's not right either.


  • Chem -

    Show your work for (Cl2)
    Show your work for Q after 15 min.
    Show your work for SO2Cl2 at equil. I obtained about 0.0585 g for SO2Cl2.

  • Chem -

    thanks! i had already gotten the first couple of answers, which is why i didn't show what i did.

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