1. The problem statement, all variables and given/known data How much heat is required to change 1.75 L of Ethyl Alcohol (C2H6O) at -50.0°C to a gas at its boiling point? Ethyl Alcohol V = 1.75 L Ti = -50°C 46 g/mol density = 0.789 g/cm3 boiling point = 78°C specific heat (c)= 2400 J/kg*C° Heat of Vaporization (Lv) = 850*103 J/kg 2. Relevant equations density m = ρV specific heat Q = mcΔT latent heat Q = mLv 3. The attempt at a solution First I determined the mass of the Ethyl Alcohol m = ρV = (0.789 g/cm3) (1750 cm3) = 1380.75 g = 1.38075 kg Then I solve for QNET QNET = (mcΔT)l + mLv QNET = [1.38 kg (2400 J/kg*C°) (78°C - (-50°C)] + [1.38 kg (850*103 J/kg)] = 1.60 * 106 J According to the answer sheet, the answer is 4.24*105 J What am I doing wrong? Thank you in advance! Any and all help is appreciated!