mass-volume-pressure relationship

[Quincy]

1. The problem statement, all variables and given/known data
What is the volume of a sample of oxygen gas has a mass of 50 grams and is under pressure of 1.20 atm at 27 degrees celsius?

3. The attempt at a solution

Density = Pressure(in pascals)/(specific gas constant * Temperature (in kelvins))

1 atm = 101,325 pascals ~ 1.2 atm = 121,590 pascals
27oCelsius = 300.15 K

Density = (121,590 pascals)/(8.314 * 300.15 K) = 48.72 kg/m3 = 48,720 g/m3

48,720 g/m3 = 50 g/V ~ V = 1.03 x 10-3 m3

[bomba923]

Hint: Ideal Gas Law (PV = nRT)

[Quincy]

So... (1.2 atm)(V) = (3.13 mol)(8.314)(300.15 K) ~ V = 6509 L??

[bomba923]

Not quite --
1) Oxygen is a diatomic gas (O2)
2) Check your units -- your gas constant (and consequently the volume) is off by (about) two orders of magnitude!
_For your units, the gas constant is approximately 0.0821 L*atm/(K*mol)

[Quincy]

(1.2 atm)(V) = (1.56 mol)(0.0821)(300.15 K) ~ V = 32.09 L?

[Quincy]

Bump

[bomba923]

(1.2 atm)(V) = (1.56 mol)(0.0821)(300.15 K) ~ V = 32.09 L?yes, that is correct