Multiple Choice
Vapor pressure measurements at various temperature values are given below. Determine the molar heat of vaporization for cyclohexane.
13. Liquids, Solids & Intermolecular Forces
Clausius-Clapeyron Equation
Back13. Liquids, Solids & Intermolecular Forces
Clausius-Clapeyron Equation
- Multiple Choice
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 405 torr?
- Open Question
Which of the temperatures below is most likely to be the boiling point of water at 880 torr?
- Multiple ChoiceA 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.
- Multiple ChoiceBenzene 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?
- Multiple ChoiceUsing 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.
- Multiple ChoiceDetermine 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.
- Multiple ChoiceEthanol 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?
- Multiple ChoiceThe 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?
- Multiple ChoiceThe 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?
- Multiple ChoiceThe vapor pressure of dichloromethane at 260 K is 71 torr. What is the vapor pressure at 310 K, given that ΔHvap = 31.4 kJ/mol?
- Multiple ChoiceThe vapor pressure of dichloromethane, CH2Cl2, at 0°C is 134 mmHg. The normal boiling point of dichloromethane is 40°C. Calculate its molar heat of vaporization using the Clausius-Clapeyron equation.
- Multiple ChoiceUsing 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.
- Multiple ChoiceUsing 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?