(adsbygoogle = window.adsbygoogle || []).push({}); 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 CO_{2}

n_{CO2}= PV/RT

n_{CO2}= (3.00atm*5.00L)/ 0.0821*350K

n_{CO2}= 0.522 mol CO_{2}

Then, should I find the number of moles of the BaO???

n_{BaO}= 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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# Gaseous pressure calculation

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