Calculate the amount of heat energy, in units of kilojoules, required to evaporate 35.0 g of ethanol, CH₃CH₂OH, at 78.4 $\degree$C, ethanol's boiling point.(The molar heat of vaporization of liquid ethanol is 3.86 x 10⁴ J/mol.The molar mass of ethanol is 46.07 g/mol.)

Question

Quizplus · Accepted Answer

To find the heat energy required, first convert the mass of ethanol to moles: 35.0 g / 46.07 g/mol = 0.759 moles. Then, multiply the moles by the molar heat of vaporization: 0.759 moles * 3.86 x 10^4 J/mol = 2.93 x 10^4 J. Convert this to kilojoules: 2.93 x 10^4 J / 1000 = 29.3 kJ.

Calculate the Amount of Heat Energy, in Units of Kilojoules °\degree°

Calculate the Amount of Heat Energy, in Units of Kilojoules $\degree$