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?

  1. DrBob222

    Yes, use the Clausis-Clapeyron equation.

  2. Viola

    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?

  3. DrBob222

    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.

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