The amount of carbon dioxide in a gaseous mixture of CO2 and CO can be determined by passing the gas into an aqueous solution that contains an excess of Ba(OH)2. The CO2 reacts. yielding a precipitate of BaCO3, but the CO does not react. This method was used to analyze the equilibrium composition of the gas obtained when 1.77 g of CO2 reacted 2.0 g of graphite in a 1.000L container at 1100K. The analysis yielded 3.41 g of BaCO3. Use these data to calculate Kp (Equilibrium constant of gas) at 1100K for the reaction:
CO2 (g) + C (s) ---- 2 CO (g)

Question

The amount of carbon dioxide in a gaseous mixture of CO2 and CO can be determined by passing the gas into an aqueous solution that contains an excess of Ba(OH)2. The CO2 reacts. yielding a precipitate of BaCO3, but the CO does not react. This method was used to analyze the equilibrium composition of the gas obtained when 1.77 g of CO2 reacted 2.0 g of graphite in a 1.000L container at 1100K. The analysis yielded 3.41 g of BaCO3. Use these data to calculate Kp (Equilibrium constant of gas) at 1100K for the reaction:
                   CO2 (g) + C (s) ----> 2 CO (g)

anonymous · Answer

I am trying to figure this one out myself, I know that you find the molarity for CO2 and C with the information given.....and then possibly do a chart and solve for x-missing information, but I am not sure what the 3.41 g of BaCO3 is used for.