7. Sulfur oxchloride decomposes to sulfur dioxide and chlorine gases SO2Cl2(g) <

Question

7. Sulfur oxchloride decomposes to sulfur dioxide and chlorine gases SO2Cl2(g) <= > SO 2 (g) + CL 2 (g) at equilibrium at given T , the partial pressures are 1.88 atm , 0.84 atm and 0.27 atm respectively A. calculate K for these conditions B. If some chlorine gas condenses and its parts pressure is reduced to 0.68 atm what will be the value of Q ? C. Considering the Q in which direction will the reaction proceed? 7. Sulfur oxchloride decomposes to sulfur dioxide and chlorine gases SO2Cl2(g) <= > SO 2 (g) + CL 2 (g) at equilibrium at given T , the partial pressures are 1.88 atm , 0.84 atm and 0.27 atm respectively A. calculate K for these conditions B. If some chlorine gas condenses and its parts pressure is reduced to 0.68 atm what will be the value of Q ? C. Considering the Q in which direction will the reaction proceed? 7. Sulfur oxchloride decomposes to sulfur dioxide and chlorine gases SO2Cl2(g) <= > SO 2 (g) + CL 2 (g) at equilibrium at given T , the partial pressures are 1.88 atm , 0.84 atm and 0.27 atm respectively A. calculate K for these conditions B. If some chlorine gas condenses and its parts pressure is reduced to 0.68 atm what will be the value of Q ? C. Considering the Q in which direction will the reaction proceed?

Explanation / Answer

SO2Cl2(g) <= > SO 2 (g) + CL 2 (g)

KP = PSO 2 (g) PCL 2 (g) / PSO2Cl2(g)    P = PARTIAL PRESSURE

KP = .1206

B. Q = PSO 2 (g) PCL 2 (g) / PSO2Cl2(g)    PCL 2 (g) = .68

Q = .303

C. Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

since K < Q, the reaction will proceed in the reverse direction, converting products into reactants

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