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lucky_star
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Homework Statement
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.
Homework Equations
PV=nRT
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.
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