Having some trouble with how to get this problem:
Gas was obtained boiling liquid nitrogen in a 180 L tank. What volume of n2 is released at 0.935 atm of pressure and 25 degrees celcius from a tank of full liquid N2 (density 0.808 g/mL)
If someone could show me how to do this before tomorrow I would be forever grateful
20 minutes later, I figured it out for myself. But if anyone else happens to be googling this question, here's how I got my answer:
180 L = 180000 mL
.808 g/mL = density, so .808 x 180000 = 145440 g / 28.014 (molar mass of N2) = 5191.69 M
V=nRT/P
(5191.69)(.082)(298)
________________ = 135683.56L
(.935)
Gas was obtained boiling liquid nitrogen in a 180 L tank. What volume of n2 is released at 0.935 atm of pressure and 25 degrees celcius from a tank of full liquid N2 (density 0.808 g/mL)
If someone could show me how to do this before tomorrow I would be forever grateful
20 minutes later, I figured it out for myself. But if anyone else happens to be googling this question, here's how I got my answer:
180 L = 180000 mL
.808 g/mL = density, so .808 x 180000 = 145440 g / 28.014 (molar mass of N2) = 5191.69 M
V=nRT/P
(5191.69)(.082)(298)
________________ = 135683.56L
(.935)