Calculate the amount of heat energy, in units of kilojoules, required to convert 50.0 g of liquid ethanol, CH₃CH₂OH, at 25.5 $\degree$C to gaseous ethanol at 92.0 $\degree$C.(C_{ethanol liquid} = 2.44 J/g $\degree$C; C_ethan_{ol gas} = 1.42 J/g $\degree$C; molar heat of vaporization of liquid ethanol = 3.86 x 10⁴ J/mol.The boiling point of ethanol is 78.4 $\degree$C and its molar mass is 46.07 g/mol.)

Question

Quizplus · Accepted Answer

**Explanation:**First, calculate the heat required to raise the temperature of the liquid ethanol from 25.5 $\degree$C to its boiling point, 78.4 $\degree$C:Q1 = m * C * (Tb - Ti)Q1 = 50.0 g * 2.44 J/g $\degree$C * (78.4 $\degree$C - 25.5 $\degree$C)Q1 = 6.36 kJNext, calculate the heat required to vaporize the liquid ethanol at its boiling point:Q2 = n * ΔHvapn = 50.0 g / 46.07 g/mol = 1.086 molQ2 = 1.086 mol * 3.86 x 10⁴ J/molQ2 = 42.9 kJFinally, calculate the heat required to raise the temperature of the gaseous ethanol from its boiling point to 92.0 $\degree$C:Q3 = m * C * (Tf - Tb)Q3 = 50.0 g * 1.42 J/g $\degree$C * (92.0 $\degree$C - 78.4 $\degree$C)Q3 = 0.97 kJThe total heat required is the sum of Q1, Q2, and Q3:Qtotal = Q1 + Q2 + Q3Qtotal = 6.36 kJ + 42.9 kJ + 0.97 kJQtotal = 49.3 kJTherefore, the correct answer is A) 49.3 kJ.

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

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