Vapor pressure measurements at various temperature values are given below. Determine the molar heat of vaporization for cyclohexane.

Using the two-point form of the Clausius-Clapeyron equation, calculate the vapor pressure of methanol at 12.0°C given its normal boiling point is 64.6°C and its heat of vaporization is 35.2 kJ/mol.

Using the Clausius-Clapeyron equation, what is the enthalpy of vaporization (ΔHvap) for the reaction A(l) ⇌ B(g) if the equilibrium constant K is 3.2 × 10^(-3) at 0 °C and 8.1 × 10^(-3) at 50 °C?

Which three variables are directly related in the Clausius-Clapeyron equation?

Which of the following cannot be determined using the Clausius-Clapeyron equation?

What is the vapor pressure of SiCl4 in mm Hg at 30.0 °C? (See Problem 11.27.)

Dichloromethane, CH2Cl2, is an organic solvent used for removing caffeine from coffee beans. The following table gives the vapor pressure of dichloromethane at various tem- peratures. Fill in the rest of the table, and use the data to plot curves of Pvap versus T and ln Pvap versus 1/T.

Choose any two temperatures and corresponding vapor pressures in the table given in Problem 11.30, and use those values to calculate ΔHvap for dichloromethane in kJ/mol. How does the value you calculated compare to the value you read from your plot in Problem 11.32?