1. The problem statement, all variables and given/known data A sample of CO2(g) is contained in a 5.00 L flask at 350 K and 3.00 atm pressure. When 30.66 g of BaO(s) was added to the flask, this reaction took place: BaO(s) + CO2(g) => BaCO3(s) Calculate the pressure in the the vessel after the reaction was complete. assume that the temperature is constant and the volume of the solid product is neglegible. 2. Relevant equations PV=nRT 3. The attempt at a solution First, I tried to find the number of moles of CO2 nCO2= PV/RT nCO2= (3.00atm*5.00L)/ 0.0821*350K nCO2= 0.522 mol CO2 Then, should I find the number of moles of the BaO??? nBaO= 30.66g/153.3g/mol of BaO =0.20 mol Now, I stuck, what can I do with all variables that I found? Please help.