Ignition wires heat Thermometer Stirrer sample A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods In an experiment, a 1.0580 g sample of B-D-fructose (C6H12O6) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.284x103 g of water. During the combustion the temperature increases from 26.32 to 29.03 °C. The heat capacity of water is 4.184 J g °C. Water The heat capacity of the calorimeter was determined in a previous experiment to be 991.6 J/oC Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of B-D-fructose based on these data 6 H2O(I)6 CO2(g) Energy CH12O6(s)6O2(g) Insulated Sample dish Burning sample Steel bomb kJ/mol Molar Heat of Combustion outside chamber Combustion (bomb) calorimeter.

The combustion of 0.1559 g benzoic acid increases the temperature of a bomb calorimeter by 2.52°C. Calculate the heat capacity of this calorimeter. (The energy released by combustion of benzoic acid is 26.42 kJ/g.) Heat capacity = kJ/°C A 0.2138-g sample of vanillin (C3H3 O3) is then burned in the same calorimeter, and the temperature increases by 3.22°C. What is the energy of combustion per gram of vanillin? Energy kJ/g %3D Per mole of vanillin? Energy = kJ/mol

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 0.1950 g of salicylic acid, in the presence of excess oxygen, causes the temperature of the calorimeter to rise by 1.40 °C. When a 0.2962-g sample of an unknown organic substance is similarly burned in the same calorimeter, the temperature rises by 3.72 °C. What is the energy of combustion per unit mass of the unknown substance?

A certain chemical reaction releases 269. kJ of heat energy per mole of reactant consumed. Suppose some moles of the reactant are put into a calorimeter (a device for measuring heat flow). It takes 3.21 J of heat energy to raise the temperature of this calorimeter by 1 °C. Now the reaction is run until all the reactant is gone, and the temperature of the calorimeter is found to rise by 5.0 °C. How would you calculate the number of moles of reactant that were consumed? Set the math up. But don't do any of it. Just leave your answer as a math expression. Also, be sure your answer includes all the correct unit symbols. moles consumed = x10 010 X Ś