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. Estimating the Normal Boiling Point of Carbon Tetrachloride

The Normal Boiling Temperature of Carbon Tetrachloride
A substance’s normal boiling point refers to the temperature at which its vapor pressure equals the atmospheric pressure. The liquid then boils. For carbon tetrachloride, (CCl4) this is determined using the vapor temperature and enthalpy to vaporization. At 57.8 °C, the vapor pressure of CCl4 is 54.0 kPa, and its enthalpy of vaporization is 33.05 kJ/mol (Mendelsohn, 2019). The vapor pressure of CCl4 is likely to increase as temperatures rise, while the enthalpy for vaporization will fall. The enthalpy for vaporization will decrease and the vapor pressure of CCl4 increases, making vaporization more energy-friendly. This data can be used to estimate the normal boiling temperature of CCl4 (Mendelsohn 2019, Mendelsohn). As the vapor pressure of CCl4 increases with temperature, it can be assumed that the normal boiling point of CCl4 will be higher than 57.8 °C. Extrapolating the data on vapor pressure, enthaly of vaporization and boiling point can give the usual boiling point for…
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