# Chem

posted by
**Anonymous**
.

Hi!

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.)

2.093=answer

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

A=.0156

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

A=.0136

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.

Help?