1. The problem statement, all variables and given/known data The combustion of 0.1577 g benzoic acid increases the temperature of a bomb calorimeter by 2.51°C. a) Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) A 0.2123-g sample of vanillin is then burned in the same calorimeter, and the temperature increases by 3.25°C. b) What is the energy of combustion per gram of vanillin? C)How about per mol? 2. Relevant equations qv=mCv delta T 3. The attempt at a solution a)26.42 kj/g x 0.1557g= 4.113594 kj=q 4.113594 kj= (0.1577g)(Cv)(2.51 Celsius) -> Cv=10.39240375 kj/celcius b) (0.2123g)(10.39240375 kj/celsius)(3.25 celsius) = 7.17... kj/g ->7.17.../0.2123g = 33.78... c) (33.78 kj/1g) x (152.15g/1 mol)= 5139.627 kj/mol All those are wrong apparently... Help?