Use the Clausius-Clapeyron equation to estimate the boiling point of water at 24.0 torr pressure. (ΔHvap = 42.30 kJ/mol)

asked by @sarahj72 • about 1 year ago • Chemistry • 5 pts
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1 answer

Hey there! So here we would use the given equation:

ln(P2/P1) = - ΔHcap/R x (1/T2 - 1/T1)

Here T1 will just be normal boiling point of water, which is 100 C (just make sure to convert it to Kelvins), P1 is also the normal pressure, 1 atm, but make sure to use torr for pressure units. 1 amt= 760 torrs.

R is the gas constant which you need to remember. R = 8.314 J/mol K

Plug everything in, P2 is given, solve for T2. Just make sure you either convert the R or ΔH because their units don't agree.

Let us know if you need any further help with this.

answered by @dashab2 • about 1 year ago