Homework Help: AP CHEM

Posted by John on Thursday, January 24, 2008 at 3:24am.

2-propanol has a delta Hvp of 701 J/g and a vapor pressure of 31.6 mmHg at 20.0 degrees C. Estimate the normal boiling point of this alcohol in degrees C.

i used the clasius-clayperon equation and this is what i have so far.

ln (31.6 mmHg/760 mmHg)= (-701 J/g)/8.314 J/g C (1/ T2 - 1/20 C)

is that correct?

AP CHEM - DrBob222, Thursday, January 24, 2008 at 3:39pm
No, you have at least two errors. T must be converted to Kelvin and Hvap must be in J/mol. Therefore, T1 = 273.15 + 20.0 = ?? and Hvap for 2-propanol is 701 J/g x ??grams/mol = ??
AP CHEM - DrBob222, Thursday, January 24, 2008 at 4:04pm
Also, I think the equation should be ln(p2/p1). You have reversed the T1 and T2 but that is ok since you have a negativae sign for Hvap. But P2 should be on top and P1 on bottom.

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