Methanol boils at 64.65 °C (337.8 K) under a pressure of 1 bar, and its enthalpy of vaporisation there is 35.3 kJ mol⁻¹. Liquid and vapour are at equilibrium at the boiling point. What is the entropy change when one mole of liquid methanol turns to vapour at its boiling point?

ChemistryMediumHigh School (11–12)Chemical Thermodynamics › Entropy, Gibbs Energy and Spontaneity JEE Main

Methanol boils at $64.65\ ^\circ\text{C}$ ( $337.8\ \text{K}$ ) under a pressure of $1\ \text{bar}$ , and its enthalpy of vaporisation there is $35.3\ \text{kJ mol}^{-1}$ . Liquid and vapour are at equilibrium at the boiling point. What is the entropy change when one mole of liquid methanol turns to vapour at its boiling point?

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← The standard enthalpies of combustion are: ethyne, C₂H₂(g), -1300 kJ mol⁻¹; graphite, -393.5 kJ mol⁻¹; hydrogen, -285.8 kJ mol⁻¹ (the water formed is liquid). What is the standard enthalpy of formation of ethyne, 2 C(graphite) + H₂(g) → C₂H₂(g)?One mole of an ideal monatomic gas (CV = 32 R) is at 400 K and 10.0 bar in a cylinder with insulated walls. The external pressure is suddenly dropped to 2.0 bar and held there, and the gas expands against it until its own pressure is 2.0 bar. What is the final temperature of the gas? →

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