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How do I calculate the normal boiling point of CCl4?

CCl4 has a vapor pressure of 213 torr at 40°C and 836 torr at 80°C. What is the normal boiling point  CCl4?

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J.R. S. | Ph.D. in Biochemistry--University Professor--Chemistry TutorPh.D. in Biochemistry--University Profes...
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Use the Clausius-Claperyon equation and solve for ∆Hvap.
ln P1/P2 = ∆Hvap/R (1/T2 - 1T1)
P1 = 213 torr
T1 = 313 K
P2 = 836 torr
T2 = 353 K
R = 8.314 kJ/mol-K
Solve for ∆Hvap which will have units of kJ/mole
Use the ∆Hvap and plug into the C-C equation again, and solve for T2 using P2 = 760 torr and either set of P and T from the original question.