A 0.500 g sample of the explosive TNT (C7H5N3O6) is completely burned in a bomb calorimeter containing 610. grams of water at an initial temperature of 20.00°C. The heat capacity of the bomb is 421 J.°C -1 and the heat of the reaction is 3374 kJ per mole of TNT. Determine the final temperature ( in ºC) of the water.

A 1.800-g sample of phenol (C6H4O2) was burned in a bomb calorimeter whose total heat capacity is 11.84 kJ/°C. The temperature of the calorimeter plus contents increased from 20.82 °C to 27.81 °C. What is the heat of combustion per gram of phenol?

A 22.1g piece of aluminum (which has a molar capacity of 24.03 J/oC.mol) is heated to 82.4oC and dropped into a calorimeter containing water (specific heat capacity of water is 4.18J/goC) initially at 22.3oC. The final temperature of the water is 25.8oC. Ignoring significant figures, calculate the mass of the water in the calorimeter.

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 1.4710 g sample of maleic acid (C4H4O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1159 g of water. During the combustion the temperature increases from 22.46 to 25.59 °C.   The heat capacity of the calorimeter, not including the surrounding water, was determined in a previous experiment to be 852.2 J/°C.   Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of maleic acid based on these data.   Assuming that no energy is lost to the surroundings, what is the molar heat of combustion of maleic acid, based on these data? (in kJ/mol).   C4H4O4(s) + 3O2(g) → 2 H2O(l) + 4 CO2(g) + Energy

When a 4.31 g sample of liquid octane (C8H18) is burned in a bomb calorimeter, the temperature of the calorimeter rises by 27.3 °C. The heat capacity of the calorimeter, measured in a separate experiment, is 6.2 kJ/•C. The calorimeter also contains 3.00 kg of water, specific heat capacity of 4.18 J/g°C. Determine the heat of combustion of octane in units of kJ/mol octane. Enter your answer numerically and in terms of kJ/mol.

The combustion of 1.00mol of glucose (C6H12O6) liberates 2820 kJ of heat. If 1.64g of glucose is burned in a calorimeter containing 788 g of water, and the temperature of the assembly increases from 20.10oC to 24.16oC, what is the heat capacity of the calorimeter in kJ/oC? MW of glucose is 180 g/mol.

Propane gas (C3H6 (g)) is withdrawn from a 100.0 L cylinder at 25.0 oC and is burned at constant pressure in an excess of oxygen. The pressure in the cylinder falls from 2.25 atm to 1.05 atm.  The liberated heat is then used to raise the temperature of 65.5 L of water from 25.0 oC to 56.7 oC. What % of the heat of combustion was absorbed by the water (d = 1.00 g/mL)?   Specific heat capacity of water = 4.18 J/g/oC Δ Hfo(H2O(l)) = -285.8 kJ/mol,    Δ Hfo(O2(g)) = 0 kJ/mol,    Δ Hfo(CO2 (g)) = -393.5 kJ/mol   Δ Hfo(C3H6 ) = -103.8 kJ/mol

At constant volume, the heat of combustion of a particular compound is -3916.0 kJ/mol. When 1.329 g of this compound (molar mass = 166.62 g/mol) was burned in a bomb calorimeter, the temperature of the calorimeter, including its contents, rose by 7.549 "C. What is the heat capacity (calorimeter constant) of the calorimeter? calorimeter constant: kJ/ "C

A 56.1 g sample of polystyrene, which has a specific heat capacity of 1.880 J-g °C-1 is put into a calorimeter (see sketch at right) that contains 250.0 g of water. The temperature of the water starts off at 24.0 °C. When the temperature of the water stops changing it's 29.8 °C. The pressure remains constant at 1 atm. Calculate the initial temperature of the polystyrene sample. Be sure your answer is rounded to the correct number of significant digits. °C thermometer. insulated container water sample. a calorimeter 區 OU Ar