Posted by Katie on .
Many analytical instruments require liquid nitrogen. While filling an instrument with liquid nitrogen, an analytical chemist slips and spills the contents of the dewer, 29.0 L, onto the floor. Since the boiling point of liquid nitrogen at 1.00 atm is 77.4 K, all the nitrogen boils away to gas very quickly. The density of liquid nitrogen is 804 kg/m^3. What volume of nitrogen gas is produced from the liquid nitrogen spill if the temperature of the room is 25 degrees C at 1.00 atm?
Here is what I would do.
First, your prof may not like this but I prefer to work in g/cc for density; therefore, convert 804 kg/m^3 = 0.804 g/cc.
m = volume x density
mass = 29,000 cc x 0.804 g/cc = ?? grams.
moles N2 = grams/molar mass = n
Then use PV = nRT and solve for volume.