Density of CO2 Vapor
Density of CO2 Vapor
(OP)
I'm trying to write a formula in an Excel spreadsheet to calculate the loss of CO2 through an opening. One part of the equation requires the "Density of CO2 Vapor" in "Lb/ft3".
For the most part I could use a standard value at 70°F, but as it happens, I'm dealing with an area where the temperature could be higher, like closer to 120°F or more.
I believe that at standard temperature and pressure the value would be 0.123607/ft3 (1.98kb/m3). (if this is incorrect don't hesitate to let me know).
If the temperature, in Fahrenheit, is known, how would I determine the density at that temperature?
Thanks for the help.
Dan Marr.
For the most part I could use a standard value at 70°F, but as it happens, I'm dealing with an area where the temperature could be higher, like closer to 120°F or more.
I believe that at standard temperature and pressure the value would be 0.123607/ft3 (1.98kb/m3). (if this is incorrect don't hesitate to let me know).
If the temperature, in Fahrenheit, is known, how would I determine the density at that temperature?
Thanks for the help.
Dan Marr.





RE: Density of CO2 Vapor
Keep in mind that the density of a gas depends upon its pressure as well as its temperature.
Using the combined gas laws:
Density, lb/ft3 = (1/Z)(M/10.73)(P/T)
where:
M = Molecular weight = 44 for carbon dioxide (CO2)
P = absolute pressure, psia
T = degrees Rankine = 459.7 + °F
10.73 = the gas law constant R
Z = the gas compressibility factor at P and T
In most cases, Z=1 for all practical purposes.
Milton Beychok
(Visit me at www.air-dispersion.com)
.
RE: Density of CO2 Vapor
For the formula you supplied, will "P" be 14.5?
RE: Density of CO2 Vapor
not too sure on American units, but just make sure that you're using Pabs and not Pgauge.
Pabs = Pgauge +Patm (psia) and you're good to go.
RE: Density of CO2 Vapor
The density of a gas depends upon the temperature, pressure and molecular weight of the gas.
If the gas is at atmospheric pressure, then P would be 14.697 psia (pounds per square inch absolute) if it is at sea level. If the gas is at some other pressure, then that would be P. For example, if the gas is at 10 psig (pounds per square inch guage), then P would be 14.696 + 10 =24.696 psia again at sea level.
I stress the "sea level" bit, because atmospheric pressure decreases with altitude. In other words, atmospheric pressure will be less than 14.696 psia if you live atop a mountain.
If you live in a metric country, atmospheric pressure is 101,325 Pascals absolute at sea level, which is the same as 1.01325 bar absolute.
Milton Beychok
(Visit me at www.air-dispersion.com)
.
RE: Density of CO2 Vapor
Thanks for the info. I've got the numbers plugged into a spreadsheet, but am not sure it they're right. If you're willing to look at it, I'll try and post it.
Thanks,
Dan Marr
RE: Density of CO2 Vapor
RE: Density of CO2 Vapor
van der Waals Equation
van der Waals equation is:
(p + (n2a/V2))(V - nb) = nRT
Table: Van der Waals Coefficients of Selected Gases
Gas a b
atm dm6/mol dm3/mol
ideal 0.0 0.0
He 0.034 0.0237
Ar 1.345 0.0322
O2 1.360 0.0318
N2 1.390 0.0391
CO2 3.592 0.0427
CH4 2.253 0.0428
H2 0.244 0.0266
Example. The volume of one mole of oxygen molecules is 31.8 cm3 according to the van der Waals coefficient values tabulated. If the molecular diameter is taken as 0.370 nm, an approximate molar volume would be NAd3, or 30.5 cm3.The volume actually occupied by one mole of oxygen gas at 25oC, according to the ideal gas law, is 24465 cm3. The molecules of the gas actually occupy only 0.13% of the total volume occupied by the gas at 25oC.
RE: Density of CO2 Vapor
Did you not mean this?
(p + (n2a/V2))(V - nb) = nRT
Milton Beychok
(Visit me at www.air-dispersion.com)
.
RE: Density of CO2 Vapor
RE: Density of CO2 Vapor
RE: Density of CO2 Vapor
This article above could be helpful.
I'm wondering if someone has the simple p-Z diagram for a range of isotherms from 0°C to 500°C, maybe calculated by S&W EOS?
RE: Density of CO2 Vapor