Explain why experiments in a bomb calorimeter results in ΔU.

When 0.531 g sample of toluene (C₇H₈) was combusted in a bomb calorimeter the temperature rises 2.635 °C and when 0.425 g sample of phenol (C₆H₆O) was combusted in a bomb calorimeter the temperature rises 1.613 °C. Using the value 42.48 kJ/g for the heat of combustion of toluene, the heat of combustion per mole of phenol was calculated to be 3058 kJ/mol.

Calculate the uncertainty in the calculated value of the molar heat of combustion of phenol if there is an uncertainty of 0.001 °C in each temperature reading and 0.001 g for the mass of the samples.

A sample of aniline C₆H₅NH₂ that weighs 3.630 g  was burned in a bomb calorimeter and the temperature of the calorimeter plus contents increased from 25.60 to 34.40°C. Calculate the heat of combustion per mole of aniline if the total heat capacity of the calorimeter is 15.26 kJ/°C.  

Sucrose (C₁₂H₂₂O₁₁, molar mass = 342.30 g/mol) has a food value of 6.58 kJ/g. Calculate the calorimeter constant for the calorimeter used to combust 1.120 g sucrose  with a temperature increase of 4.72 °C. Express the answer in kJ/°C.

A 5.20-gram sample of candy is placed inside a bomb calorimeter to determine its nutritional value. If the observed temperature increase is 3.01 °C and the heat capacity of the calorimeter is 40.10 kJ • K^-1, calculate the nutritional Calories per gram of the candy.

When 0.750 g of bicyclohexane (C₁₂H₂₂) undergoes combustion in a bomb calorimeter, the temperature rises from 24.9 °C to 30.7 °C. Determine the ΔE_rxn for the combustion in kJ/mol. The heat capacity of the bomb calorimeter, determined in a separate experiment, is 7.69 kJ/°C.