Using the Clausius-Clapeyron Equation, determine the normal boiling point of a substance whose vapor pressure is 55.1 mm Hg at 35°C and has a ΔHvap of 32.1 kJ/mol.

This table displays the vapor pressure of nitrogen at several different temperatures. Use the data to determine the heat of vaporization and the normal boiling point of nitrogen. Temperature (K) Pressure (torr) 65 130.5 70 289.5 75 570.8 80 1028 85 1718

Methylamine has a vapor pressure of 344 torr at -25 °C and a boiling point of -6.4 °C. What is the ΔHvap for methylamine?

A substance has a normal boiling point of 76 °C and an enthalpy of vaporization (ΔvapH) of 38.7 kJ/mol. Using the Clausius-Clapeyron equation, determine the vapor pressure (in mbar) of this substance at 29 °C.

Benzene has a heat of vaporization of 30.72 kJ/mol and a normal boiling point of 80.1 °C. At what temperature does benzene boil when the external pressure is 577 mbar?

Determine the vapor pressure (in mm Hg) of a substance at 29°C, whose normal boiling point is 76°C and has a ΔHvap of 38.7 kJ/mol.

Ethanol has a heat of vaporization of 38.56 kJ/mol and a normal boiling point of 78.4 °C. Using the Clausius-Clapeyron equation, what is the vapor pressure of ethanol at 15 °C?

The boiling point of liquid A is 75.5 °C at 1 atm (760.0 torr). Its vapor pressure at 15.5 °C is 205 torr. What is its ΔHvap in kJ/mol?

The vapor pressure of SiCl4 is 100 mmHg at 5.4 °C, and the normal boiling point is 57.7 °C. What is the enthalpy of vaporization (ΔHvap) for SiCl4 in kJ/mol?