You must set up a bomb calorimetry experiment using 1 Liter ofwater as your heat

Question

You must set up a bomb calorimetry experiment using 1 Liter ofwater as your heat sink and combusting a 4.409g sample of propane(C3H8). If the initial and final temperature are 24.9 deg C, and77.96 deg C respectively, what is the molar enthalpy of combustionof ethene? (Assuming the calorimeter itself absorbs no heat, andthe density of water is 1 g/mL). Select from: A. -22,200 kJ/mol B. -2,220 kJ/mol C. -222 kJ/mol D. -222,000 kJ/mol E. -22.20 kJ/mol You must set up a bomb calorimetry experiment using 1 Liter ofwater as your heat sink and combusting a 4.409g sample of propane(C3H8). If the initial and final temperature are 24.9 deg C, and77.96 deg C respectively, what is the molar enthalpy of combustionof ethene? (Assuming the calorimeter itself absorbs no heat, andthe density of water is 1 g/mL). Select from: A. -22,200 kJ/mol B. -2,220 kJ/mol C. -222 kJ/mol D. -222,000 kJ/mol E. -22.20 kJ/mol

Explanation / Answer

Mass of water = volume * density                      = 1000 mL * 1 g/ mL                      = 1000 g . Heat = mass * specific heat * temperature difference         = 1000 g * 4.184 J/g. C * (77.96 - 24.90 ) C        = 222003.04 J        = 222 kJ . Moles of propane = mass/ molar mass                            =4.409 g / 44.09 g/mol                            =0.1 moles . Molar enthalpy of combustion of propane = 222 kJ/ 0.1 moles                                                             = 2220 kJ/mol . Do you require the molar enthalpy of combustion of propane or notethene as mentioned ? For ethene the given data isinsufficient.

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