PLEASE ANSWER ALL PARTS. Sulfur dioxide reacts with chlorine at 227 oC: SO2(g) +

Question

PLEASE ANSWER ALL PARTS. 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 ?g/mL. You will determine if the system has reached equilibrium. First, what is Kc (in L/mol)? (A ?g 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? Calculate the mass (in g) of SO2Cl2 expected at equilibrium.

Explanation / Answer

To convert Kp to Kc you will have to use the universal gas equation: pV = nRT And if you work it out you will find. Kc=RT*Kp (T = 500 K) a) The molar mass of SO2 is 64 g/mol. So 1 g = 1g/64 g/mol = 1,56E-002 mol. The volume is 1.00 L. [SO2] = 1,56E-002 M 1 g of Cl2: [Cl2] = 1,41E-002 M [SO2Cl2] = 0 M

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