How much energy is required to vaporize 98.6 g of ethanol (C₂H₅OH)at its boiling point,if its ΔH_vap is 40.5 kJ/mol? A) 86.7 kJ B) 11.5 kJ C) 18.9 kJ D) 52.8 kJ E) 39.9 kJ

Question

Quizplus · Accepted Answer

First, calculate the moles of ethanol using its molar mass (approximately 46 g/mol for C2H5OH). For 98.6 g of ethanol, moles = 98.6 g / 46 g/mol ≈ 2.14 mol. Then, multiply the moles by the given ΔHvap (40.5 kJ/mol) to find the energy required: 2.14 mol * 40.5 kJ/mol ≈ 86.7 kJ.

How Much Energy Is Required to Vaporize 98