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------------------------------------------------ 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 using the Clausius-Clapeyron equation below:

\[
\ln \left( \frac{P_2}{P_1} \right) = -\frac{\Delta H_{\text{vap}}}{R} \left( \frac{1}{T_2} - \frac{1}{T_1} \right)
\]

Options:
a) 25.0 °C
b) 66.2 °C
c) 100.2 °C
d) 56.0 °C
e) 76.5 °C

The Clausius-Clapeyron equation can be used to find the normal boiling point of a substance. Since the normal boiling point is the temperature at which a substance boils at 1 atm pressure, we should set P₂ to 1 atm. However, our unit for pressure is given in kPa so we will use 101.3 kPa = 1 atm. Therefore, P₂ = 101.3 kPa. Since the equation is in the form In P₂/P₁ = -∆ᵥₐₚ/R (1/T₂-1/T₁), we will set the left side to In (101.3 kPa/54.0 kPa), ∆ᵥₐₚ to 33.05 kJ/mol (which should be converted to J/mol by multiplying by 1000), and T₁ to 57.8°C (which should be converted to K by adding 273), then solve for T₂. Using this equation, the normal boiling point of CCl₄ comes out to be approximately 76.5 °C.

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