(What is the density (in g/L) of gaseous carbon dioxide, CO2, at 0.893 atm and 47°C

Question

Show work please, use ideal law

Answer 1

Hi Dristyn, to answer this question you have to use the ideal gas law as:

d = P x MM / (RT)

P = Pressure (0.893 atm) , MM = Molar Mass CO2 = (44.01 g/mol), R = Ideal gas Constant (0.08206 L x atm / (K x mol) and T = Temperature (47C = 320.15K).

d = (0.893 atm x 44.01 g/mol) / (0.08206 L x atm / (K x mol) x 320.15 K) = 1.50 g/L.

Now how do you get to this form of the ideal gas law:

1. Ideal gas law: PV = nRT
2. Rearrange: n/V = P/(RT)
3. Multiply both sides by the molar mass as m/n. The molar mass is always given in g/mol which is = mass/mol = m/n, as such the ideal gas law becomes: n/V x m/n = P/RT x m/n
4. Simplify to: m/V = P x MM/ (RT) , as such you do not write m/n, MM for molar mass on the right hand side and you cancel out the "n's" on the left hand side.
5. Now, since m/V on the left = d, the density you arrive at: d = P x MM / RT

I hope this helps.