Answer:
-18.54kJ of energy would be released
Explanation:
The enthalpy of crystallization is defined as the heat released when 1 mole of a substance change its state from liquid to solid. The ΔHcrystallization of acetic acid is -11.72kJ/mol (ΔHcrystallization = - ΔHfusion).
To solve this question we must convert the mass of acetic acid to moles in order to find the heat released:
Moles acetic acid -Molar mass: 60.052g/mol-:
95.0g * (1mol / 60.052g) = 1.58 moles
Heat released:
1.58 moles * (-11.72kJ/mol) =
-18.54kJ of energy would be released
