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?

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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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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Clausius-Clapeyron Equation concept. You can view video lessons to learn Clausius-Clapeyron Equation. Or if you need more Clausius-Clapeyron Equation practice, you can also practice Clausius-Clapeyron Equation practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Ochoa's class at UCD.

What textbook is this problem found in?

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