The complete combustion of salicylic acid releases 21.90 kJ of energy per gram of salicylic acid. In a particular bomb calorimeter (initially at room temperature), the combustion of 0.1080 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.60 °C. When a 0.2972-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 4.80 °C. What is the energy of combustion per unit mass of the unknown substance?

When sulfuric acid dissolves in water, a great deal of heat is given off. The enthalpy change for this process is called the enthalpy of solution. To measure it, 175.0 g of water was placed in a coffee-cup calorimeter and chilled to 10.0 °C. Then 49.0 g of pure sulfuric acid, also at 10.0 °C, was added, and the mixture was quickly stirred with a thermometer. The temperature rose rapidly to 14.9 °C. Assume that the specific heat capacity of the resulting sulfuric acid solution is 4.19 J/g °C. Calculate the quantity of thermal energy transferred, Q, for the formation of this solution, and calculate the molar enthalpy of solution in kilojoules per mole of H₂SO4.

A 1.595 g samples of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 23.67 degrees Celsius to 29.44 degrees Celsius. The heat capacity (calorimeter constant) of the calorimeter is 30.29 kJ/degrees Celsius, what is the heat of combustion per gram of the material?

When 1.836 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.41°C to 26.63°C. If the heat capacity of the calorimeter is 4.900 kJ/°C, what is the heat of combustion of sucrose?