What is the density (g/L) of CO2 at 25oC, 1.8 atm ?
(0.0821 atm L mol-1K-1)298K
dissolved in water with the total pressure of gas (Nitrogen +
water vapor) over the water being 3.00 atm. The temperature is
25oC. What is the concentration of Nitrogen in the
Give your answer in g/L .
The vapor pressure of water at 25.0oC is 23.8 mm Hg.
convert the pressure to mmHg to get the pressure of pure N2
3.00atm x 760mmHg=2280mmHg
subtract the water vapor pressure Ptot =PN2
+PH2O 2280mmHg Tot
-23.8mmHg H2O=2256.2mmHg N2-->2.97atm
(28g/mol x 2.97 atm)/ (0.0821 atmLmol-1K-1)(298K)=
3.40g/L Does this make sense well at STP 28g/22.4L=
1.25g/L but the pressure is tripled so yes.