Problem: Carbon tetrachloride, CCl 4, has a vapor pressure of 213 torr at 40. ˚C and 836 torr at 80. ˚C. What is the normal boiling point of CCl4?

FREE Expert Solution

Clausius-Clapeyron Equation:


lnP2P1=-HvapR[1T2-1T1]


Solve for ΔHvap:


ln836213=-Hvap8.314Jmol·K[1(80+273) K-1(40+273) K]


ln(3.92)=-Hvap8.314Jmol[-3.62×10-4]1.366(8.314Jmol)=-Hvap8.314Jmol[-3.62×10-4](8.314Jmol)

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Problem Details

Carbon tetrachloride, CCl 4, has a vapor pressure of 213 torr at 40. ˚C and 836 torr at 80. ˚C. What is the normal boiling point of CCl4?

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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.