Solved: Mass of CaCO3 to Produce 8.0L CO2 @ STP

[UWMpanther]

[SOLVED] More help on Stoich

Homework Statement

Consider the reaction CaCO3 (s) -> CaO (s) + CO2 (g)
What mass of CaCO3 will produce 8.0L of CO2, measured at STP

I don't know where to begin.

 

[rocomath]

what does STP mean? and what formula do you think you will need to use in order to relate, temperature, pressure, volume, and mass?

remember that

M=\frac{g}{mol}

so

n=\frac{g}{M}=\frac{g}{\frac{g}{mol}}

 

[UWMpanther]

stp meaning standard temp and pressure conditions.

 

[rocomath]

stp meaning standard temp and pressure conditions.

Correct. And so we have 273.15K and 1.00atm.

From here, we need to evaluate the stoichiometric ratio between Calcium carbonate and Carbon dioxide.

 

[UWMpanther]

Ok so the ratio would be

_g CaCO3 x 1mol/100gmol^-1 x 1mol CO2/1mol CaCO3 x 44gmol^-1/1 ?

 

[rocomath]

our formula

PV=nRT

becomes

PV=\frac{mRT}{M}

solving for m (mass of Carbon dioxide)

m=\frac{MPV}{RT}

plugging in our known information ... STP, Volume of Carbon dioxide and it's Molar mass.

from there, you now know the mass of Carbon dioxide and compute how much Calcium carbonate is need to produce 8.0L of Carbon dioxide.

 

[UWMpanther]

Ok so its a multiple choice question. For the variable M would it be the CO2? And R is a constant if I'm not mistaken correct ( I believe .08206 L atm mol^-1)?

 

[rocomath]

M = Molar mass of CO2

R = Gas constant (.08206 L*atm / K*mol)

 

[UWMpanther]

I realized my error after I posted it. Thank you very much for the help!

Ok so then it is:

m= (100g mol CO2 x 1atm x 8L)/(273.15 x 0.08206 Latm/Kmol)

 

[rocomath]

where did 100g mol CO2 come from?

Molar mass of CO2 is 44.01g/mol CO2

 

[UWMpanther]

Ok here's how I solved for it:

m CO2 = (molar mass of CaCO3 x P x V)/(R x T)

after I entered the unkown's I get the answer 36g