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A 2.00-mole quantity of SO2Cl2 was placed in a 2.4L container. Initially, there are no products in the container. At equilibrium, it was determined that 49.0% of the SO2Cl2 had dissociated. What is the value of the equilibrium constant under these conditions?

(A) 0.3923203

(B) 0.196

(C) 1.96

(D) 1.8831137

(E) 0.9415686

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Related questions

1)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 ofSO2 and Cl2 are placed in a 1.00 L reaction vessel. After 15minutes, the concentration of SO2Cl2 is 45.5 µg/mL. You willdetermine if the system has reached equilibrium.

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

c)Determine all concentrations after 15 minutes. What is thechlorine concentration?

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