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
Step 1: Calculate 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. Molar mass of C_2H_5OH = (2 × 12.01) + (6 × 1.008) + (1 × 16.00) = 24.02 + 6.048 + 16.00 = 46.068 g/mol Step 2: Calculate the mass of 1 litre of ethanol. Given the density of ethanol is 789 g/L and the volume is 1 L. Mass = Density × Volume Mass of ethanol = 789 g/L × 1 L = 789 g Step 3: Calculate the number of moles in 1 litre of ethanol. Moles = MassMolar mass Moles of ethanol = 789 g46.068 g/mol ≈ 17.126 mol Step 4: Calculate the total heat energy released. Given that 1 mole of ethanol releases 1370 kJ of heat energy. Total heat energy released = Moles × Heat released per mole = 17.126 mol × 1370 kJ/mol ≈ 23462.62 kJ Rounding to three significant figures (based on the given density 789 g/L), the heat energy released is: ≈ 23500 kJ The amount of heat energy released when 1 litre of ethanol is completely burnt is 23500 kJ. Send me the next one 📸