Question

A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) The bomb had a heat capacity of 500 J/K, and the calorimeter contained 610 g of water. Burning 4.50 g of ethanol, C2H5OH(L) resulted in a rise in temperature from 16.5 °C to 20.9 °C. Calculate the enthalpy of combustion of ethanol, in kJ/mol. (The specific heat capacity of liquid water is 4.184 J/g · K.) Enthalpy of combustion kJ/mol Submit Answer Try Another Version 5 item attempts remaining

Answer 1

Solutions Reaction given C₂ Mg OH (1) +30₂(g) 200 (g) + 3 H₂O (1) Heat released in reaction - heat gained by Colorimeter t water Q = CCAT t mc WAT AT change in temperature TE- Te = (20.9-1605 )°cork 4.4 °c ork Cc Heat capacity calosimerer -5003/k cw Heat capacity water 4.184 Ilgok Q (500 J/K) (4.4k) + (6 logh (4-18 4 3/9k) x (4.4k) 2200 It 11229.86 I Q 13429.86 I - Meny 13.43KI Moles ethanol essed - Mass (u.sog) Molar mass (46gnol) 0.0978 moli Enthalpy of combustion- Heat released moles used 13.43KI 0.0978 mol 137.32 KJ mort = Enthalpy of combustion Here (-)sign is peut heat Note: change temperatuese oC ork. - 137.32 kJ/mol heleased. due same for