This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Welcome back — missed you this week. Step 1: Determine the molar mass of ethanol (C_2H_5OH). The atomic masses are approximately: C = 12.01 g/mol, H = 1.008 g/mol, O = 16.00 g/mol. The formula for ethanol is C_2H_5OH, which can also be written as C_2H_6O. Molar mass of ethanol = (2 × 12.01) + (6 × 1.008) + (1 × 16.00) Molar mass of ethanol = 24.02 + 6.048 + 16.00 = 46.068 g/mol Step 2: Calculate the number of moles in 1 liter of ethanol. Given that 1 liter of ethanol has a mass of 780 g. Number of moles = MassMolar mass Number of moles = 780 g46.068 g/mol ≈ 16.931 mol Step 3: Calculate the total heat energy released. Given that 1370 kJ of heat energy is released per mole of ethanol. Total heat energy released = Number of moles × Heat released per mole Total heat energy released = 16.931 mol × 1370 kJ/mol Total heat energy released ≈ 23195.67 kJ Rounding to three significant figures (due to the 780 g value): Total heat energy released ≈ 23200 kJ The amount of heat energy released when 1 liter of ethanol is completely burned is 23200 kJ. Send me the next one 📸