High-purity benzoic acid (C6H5COOH; heat of combustion = -3227 kJ mol-1 at constant volume) is a combustion standard for calibrating bomb calorimeters. A 1.221 g sample undergoes combustion in a bomb calorimeter (heat capacity =1365 J °C-1).
a) Write the balanced combustion reaction under standard state conditions (1 mark)
b) What temperature change is observed?
c) If the reaction were performed in a coffee-cup calorimeter under standard state conditions with 1 mole of benzoid acid, estimate the value of the work. (1 mark)
d) Calculate the enthalpy change of the reaction in kJ/mol. (1 mark)
Heat of combustion of benzoic acid = -3227 kJ/mol
Mass of benzoic acid = 1.221g
Heat capacity of the bomb calorimeter,Cbomb = 1365 J/oC = 1.365 kJ/oC
Get Answers For Free
Most questions answered within 1 hours.