posted by Viola
The normal boiling point for acetone is 56.5°C. At an elevation of 5300 ft the atmospheric pressure is 630. torr. What would be the boiling point of acetone (ÄHvap = 32.0 kJ/mol) at this elevation?
I need to know how to do this!!
what formula do u use for this? is it
the clausius-claperyron? or no? what is the cl-cl equation for anyway?
Yes, use the Clausis-Clapeyron equation.
What pressure would have to be applied to steam at 325°C to condense the steam to liquid water (ÄH vap = 40.7 kJ/mol)?
do u use the Clausius claperyron for this also???
how do u do this?
Please see the correction I made below to the 6.02 kJ/mol for heat vaporization for water. It's under the screen name of Rachelle. Sorry about the error. Check me out on all of this.