What is the density in g/L of a 14.1 g sample of carbon dioxide gas at 27.2 °C and 3.18 atm?
P = 3.18atm
T= 27.2 oC
= (27.2+273) K
= 300.2 K
Molar mass of CO2,
MM = 1*MM(C) + 2*MM(O)
= 1*12.01 + 2*16.0
= 44.01 g/mol
Lets derive the equation to be used
use:
p*V=n*R*T
p*V=(mass/molar mass)*R*T
p*molar mass=(mass/V)*R*T
p*molar mass=density*R*T
Put Values:
3.18 atm *44.01 g/mol = density * 0.08206 atm.L/mol.K *300.2 K
density = 5.6812 g/L
Answer: 5.68 g/L
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