What is the Volume of a 50g Oxygen Gas Sample at 1.20 atm and 27°C?

[Quincy]

Homework Statement

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?

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
27^oCelsius = 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?

 

[bomba923]

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

yes, that is correct

 

[jordy102]

Hi, can someone please help me...its quite urgent...I have two vessels, one has capacity of 0.5l and the other 0.15l. The 0.15l is in a vacuum state held constantly at -80C and the 0.5l vessel is at 50mbar at room temperature (20C). I have gas in the 0.5l vessel...I then open the valve and release the gas to the vacuum upon which it immediately desublimes.. until it reaches equilibrium state and then i close the valve and take the smaller vessel away. What conditions hold at equilibrium? and how do I find the mass of desublimed solid?