CaCO3(s)=CaO(s)+CO2(g) Volume of CO2?

Question

CaCO3(s)=CaO(s)+CO2(g)
If 4.74 g of calcium carbonate is heated what volume of CO2(g) would be produced when collected at 26C and .997 atm?
Please show me how you got this.TY

Answer 1

You have to find how many moles is 4.74g of CaCO3. The CO2 produced will be the same amount of moles. Then you find how much those moles weigh in the case of CO2 (multiply by the molecular weight), and then you must find the volume of this quantity under the specific conditions of pressure and temperature. sorry I can't help any more, because it's been a long time since I did chemistry and I don't remember atomic weights etc., but I think the concept is what you need more, not someone to actually do your homework.

And skitz is wrong. Sure the gas would fill any container, but depending on its volume the pressure would change. PV=nRT

Answer 2

1 mole of CaCO3 has a molecular weight of 40+12+3*16=100
So, 1 mole of CaCo3 =100g and 4.74g = 0.0474 mole

for the volume V=nRT/P

n=0.0474 R= 8.314 T= 273+26=299K P= 101.325*0.997 Pa

so V= 0.0474*8.314*299/0.997*101325=0.001166m^3

in liters 1.166L

Answer 3

It is going to be the same method as your last question. Try doing it and if you can not someone will show you.

Answer 4

technically at any temp and pressure gas will fill to the size of its container.... that may not be the answer your teacher is looking for but technicallty it is correct based on the properties of gasses