Answer :
Final answer:
The total entropy of vaporization of 35.5g of acetone under 1 atm of pressure can be calculated using the enthalpy of vaporization and the boiling point in kelvins, along with the molecular weight of acetone to convert grams to moles.
Explanation:
The question pertains to the total entropy of vaporization of acetone, which is a measure of the disorder or randomness associated with the phase transition from liquid to gas. To determine the entropy of vaporization (ΔSvap), we use the formula ΔSvap = ΔHvap / Tb, where ΔHvap is the enthalpy of vaporization and Tb is the boiling point in kelvin. Given the molar enthalpy of vaporization for acetone is 29.1 kJ/mol and the boiling point is 56.5°C (or 329.65 K), we first convert the mass of the acetone to moles using its molar mass (58.08 g/mol for C3H6O), and then use the formula to calculate the total entropy change for the given amount of acetone.
