density of carbon dioxide gas?

Question

Hi everyone, 
Could someone please help me with the density of carbon dioxide gas at –25.2°C and 98.0 kPa? I've tried to find the answer multiple times but haven't been successful. Thank you!

Anonymous · Accepted Answer

Use the ideal gas law PV =nRT. First change it into PV = (m/M)RT (m= mass, M is grams per mole). Since density is m/v, solve:
MPV=mRT 
(MP)/(RT) = m/V
(MP)/(RT) = d
M = 44 g/mol (co2 is  one carbon and two hydrogens)
P = 0.967 atm
R = 0.0821 (latm)/(molk) its the Ideal gas constant
T = 247.95 K
When you plug it in and solve, you get : 2.09 g/L

Anonymous · Answer

The Wikipedia page lists several densities for CO2 at different states.
http://en.wikipedia.org/wiki/Carbon_dioxide
I bet you could do a varient of P1V1T1=P2V2T2, change V to density and figure it out.
CO2 is 1562 kg/m^3 at 1 atm and -78.5C.  
M^3=1000L so it's 1562000grams/1000L, which makes it 1562g/1L.
Convert kPa to atm to make units the same: 98 kPa = 0.9672 atm 
http://www.unitconversion.org/pressure/standard-at...
Now you have:
0.9672 atm (-25.2C) (1562g/1L) = 1 atm (-78.5 C) (x g/1L)
-38071.31(/1L) = -78.5x(/1L)
x = 484.995g/1L, which converts back to:
484.995g/1L (1kg/1000g)(1000L/1m^3) = 484.995kg/m^3
Don't know if it's the correct formula, but the math is sound!
Hope this helps! ?

Anonymous

density of carbon dioxide gas?

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