Posted by **randi** on Wednesday, April 11, 2012 at 2:46pm.

what is the density of carbon dioxide at 26.5 degrees C and 755 mm Hg?

- chemistry -
**DrBob222**, Wednesday, April 11, 2012 at 3:16pm
Use the modified general gas equation.

P*molar mass = density*RT

- chemistry -
**randi**, Wednesday, April 11, 2012 at 10:38pm
if i'm using PV=nRT, and manipulate that formula to V=nRT/P to find the volume, do i use 44.01g as my molar mass of CO2 and convert that to moles to find 'n'? i'm really confused how to do this b/c it's not at STP.

- chemistry ** CAN YOU LOOK AT MY ANSWER, PLEASE, DRBOB222? :) -
**randi**, Wednesday, April 11, 2012 at 11:48pm
the answer i came up w/ is 1.76g/L. is this correct?

- chemistry -
**randi**, Wednesday, April 11, 2012 at 11:55pm
...but i did it a different way. i looked at an example in the textbook, but still don't really understand what i did.

for P, i calculated 0.993 atm

for n, i calculated 0.040 mol CO2

for T, i calculated 299.5 K

then, i calculated 0.040 mol CO2 x 44.01g/1 mol CO2 = 1.76 g CO2 (stoichiometry)

density = 1.76 g/L (but i don't understand how or why i went from 1.76 g CO2 to 1.76 g/L)

i'm very lost!! :(

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