# Gaseous pressure calculation

1. Oct 27, 2008

### lucky_star

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.

Last edited: Oct 27, 2008
2. Oct 27, 2008

### Staff: Mentor

Looking at the reaction equation - how much CO2 reacted with 0.20 mol of BaO? How much CO2 was left?

3. Oct 27, 2008

### lucky_star

Wow, I got the answer. Thank you so much!

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