Volume of N2

Go to google type "volume n2" and down load N2 of Volume 11, N2 of Volume 14.

Maybe this may help you out. To me this seems french.

If a rough value is good enough, there is approximately a 2000:1 ratio of vapor at one bar to liquid volume (any reasonable pressure) for any liquid. Since the PV product is a constant, divide the 2000 by 9 to get 222. 100M3 vapor at 9 bar/222=0.45M3 of liquid.

• Critical Pressure: 492.3 psia (33.5 atm)
• Density, Liquid @ BP, 1 atm: 50.45 lb/scf " Wikipedia" Same irrespective of Pressure(ALMOST!)

Can't tell what you're asking. It reads as if you mean what mass of liquid N₂ is 100 m³ of liquid N₂. Density of liquid N₂ is about 800 kg/m3 so it's 80 tonne. But 100 m³ of liquid N₂ is a lot so you more likely mean 100 m³ gas. At what temperature and pressure? At say 15°C and 1 bar (abs) density is ~ 1.17 kg/m3 so mass = 117 kg.

Presumably the 9 bar refers to the liquid N₂ but pressure obviously doesn't affect the mass and as MUKULMAHANT said it doesn't affect density much either so volume of liquid is ~ 0.146 m³.

Haste is Waste!

Had you asked in plain English ,we would have reached our goal long back.

Are you asking this?:

How many Kg of liquid Nitrogen would completely fill a 100 cubic metre volume(which had been evacuated earlier) and then the N2 Gas will attain a pressureof 9 atg ?

Every word counts.

Also need to know gas temperature

.... to be exact!

As I understand it, is quite simple.

Remember the formula: Pv=RT. Assuming the temperature will be the same (you will have the "space" at room temperature before and after pressurizing), you would need 900 cubic metres to achieve 9 bar in the 100 cubic metres space.

A better way is to call a Nitrogen provider to ask them. They usually give you the most accurate volume and cost alternatives..