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Chapter 10: Q10.3-38 E (page 587)

Carbon tetrachloride, \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\), was once used as a dry-cleaning solvent, but is no longer used because it is carcinogenic. At \({\bf{57}}.{\bf{8}}\)°C, the vapor pressure of \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\) is \({\bf{54}}.{\bf{0}}\)kPa, and its enthalpy of vaporization is \({\bf{33}}.{\bf{05}}\)kJ/mol. Use this information to estimate the normal boiling point for \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\).

Short Answer

Expert verified

\({{\rm{T}}_{\rm{2}}}{\rm{ = 349\;K}}\) is the normal boiling point for \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\).

Step by step solution

01

Definition of Boiling

Boiling is an unnatural process in which a liquid is heated and evaporated as a result of continuous heating.

02

Writing the equation of normal boiling points

The normal boiling point corresponds to a pressure of \({\rm{1\;atm}}\).

Now, using Clausius-Clapeyron equation:

Now, \({\rm{54kPa = 0}}{\rm{.53\;atm}}\)

03

Estimating the normal boiling point for \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\)


Solving for \(\frac{{\rm{1}}}{{{{\rm{T}}_{\rm{2}}}}}{\rm{ = 0}}{\rm{.00286}}\)

Therefore, the normal boiling point for \({\rm{CC}}{{\rm{l}}_{\rm{4}}}\)is \({{\rm{T}}_{\rm{2}}}{\rm{ = 349\;K}}\)

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