For this problem, we can use the Clausius-Clapeyron Equation:
P1 = vapor pressure at T1
P2 = vapor pressure at T2
ΔHvap = heat of vaporization (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
Carbon tetrachloride, CCl4, was once used as a dry cleaning solvent, but is no longer used because it is carcinogenic. At 57.8 °C, the vapor pressure of CCl4 is 54.0 kPa, and its enthalpy of vaporization is 33.05 kJ/mol. Use this information to estimate the normal boiling point for 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.
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Based on our data, we think this problem is relevant for Professor Capps' class at American Public University System.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry - OpenStax 2015th Edition. You can also practice Chemistry - OpenStax 2015th Edition practice problems.