The boiling point of a liquid is 64°C and the enthalpy change for the conversion of this liquid to the gas is 32.21 kJ/mole. What is the entropy change for vaporization, ΔSvap, in J/(mol·K)?

Calculate the change in entropy that occurs in the system when 1.00 mole of isopropyl alcohol (C₃H₈O) melts at its melting point (-89.5 °C). See Table 11.9 for heats of fusion.

Calculate the change in entropy that occurs in the system when 1.50 mol of diethyl ether (C₄H₁₀O) condenses from a gas to a liquid at its normal boiling point (34.6 °C). See Table 12.7 for heats of vaporization.

Calculate entropy of vaporization of 8.4 g of acetic acid (CH₃COOH) with a boiling point of 118 °C, ∆H_vap = 23.7 kJ/mol.

The normal boiling point of Br₂(𝑙) is 58.8 °C, and its molar enthalpy of vaporization is Δ𝐻_vap=29.6kJ/mol. (b) Calculate the value of Δ𝑆 when 1.00 mol of Br2(𝑙) is vaporized at 58.8 °C.