Ok I got this problem...(adsbygoogle = window.adsbygoogle || []).push({});

Now I figured Vi = 33.7L and to find Vf, i used the density to determine what volume that 1.10 moles of water would need... 1.10 moles of H2O(g) at 1.00 atm and 100. ºC occupies a volume of 33.7 L. When 1.10 moles of H2O(g) is condensed to 1.10 moles of H2O(l) at 1.00 atm and 100. ºC, 44.73 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate ?E for the condensation of 1.10 moles of water at 1.00 atm and 100. ºC.

Vf = (1.1mol * (2(1.0079) + 15.999)g/mol) * (1 cm^3/0.996g) * (1L/1x10^6 cm^3) = 1.878 x 10^-5 L

Using w = -P delta V or w = -P(Vf-Vi)

I got...

w= -(1.0atm)(1.878 x 10^-5) - 33.7) * 101.3J/(L*atm) = 3413.81J

delta E = 3413.81 J + 44730 J = 48.143kJ

But supposedly I'm wrong... Anything wrong in my reasoning?

**Physics Forums | Science Articles, Homework Help, Discussion**

Dismiss Notice

Join Physics Forums Today!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

The friendliest, high quality science and math community on the planet! Everyone who loves science is here!

# Homework Help: Change in energy for vaporization

**Physics Forums | Science Articles, Homework Help, Discussion**