posted by mel on .
a) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the ideal gas law.
(b) Calculate the pressure exerted by 0.5160 mol N2 in a 1.0000 L container at 24.6°C using the van der Waals equation.
(c) Compare the results. (Write the percentage difference between the results, based on the higher value result.)
Surely you know how to do these. Perhaps you just want to know what answer I get but I don't have the time to work these things unless I have a reason. If you truly don't understand them, explain what kind of problem you are having.
so i plugged int he information that i have from the question... i am using an electronic based hmwk. it says that the answers that i have gotten are wrong... here is what i have come up with....
with using PV=nRT
i got a pressure of 12.6012 atm...
with using the van der w.
i got apressure of 12.2816 rounded
am i even close?
I have 12.61 atm. Is the T given as 24.6 or 24.60? If 24.6 then you are allowed 3 sifnificant figures and the answer would be 12.6 atm. If 24.60, then 12.61 atm would be the answer.
For the van der Waals question I have 12.75 but I think only three s.f. are allowed so that would round to 12.7. Check my arithmetic.
or 12.8 if we round to the nearest whole even number.