Toluene, CHs, is used in the manufacture of explosives such as TNT. A 1.500 gram sample of liquid toluene was placed in a bomb calorimeter along with excess oxygen. When the combustion of the toluene was initiated, the temperature of the calorimeter rose from 25.000°C to 26.413°C. The products of the reaction were carbon dioxide and water, and the heat capacity of the calorimeter was 45.06 kJ/°c. Write a balanced thermochemical equation for the combustion of toluene.

Fructose, C6H12O6(s), is a sugar closely related to glucose. A 0.755 g sample of fructose was combusted with excess oxygen in a bomb calorimeter, containing 500.0 g of water. The heat capacity of the empty calorimeter was 208 J/K. The temperature of the calorimeter and the water rose from 22.00°C to 27.12°C due to the combustion reaction, which formed CO₂(g) and liquid water. What is the energy change, AU (in kJ), for the combustion of one mole of fructose under these conditions? O +254 O-15600 -2810 +520 -804

10 A student heats 84.17 mL of water to 95.27°C using a hot plate. The heated water is added to a calorimeter containing 73.92 mL of cold water. The water temperature in the calorimeter rises from 2.15°C to 37.48°C. The specific heat capacity of water is 4.184 J and the density of water is g. °C 1.00 mL Assuming that heat was transferred from the hot water to the cold water and the calorimeter, determine the heat capacity of the calorimeter. J Heat capacity of calorimeter = °C

At constant volume, the heat of combustion of a particular compound, compound A, is −3046.0 kJ/mol.−3046.0 kJ/mol. When 1.753 g1.753 g of compound A (molar mass =112.07 g/mol)=112.07 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter (including its contents) rose by 6.475 ∘C.6.475 ∘C. What is the heat capacity (calorimeter constant) of the calorimeter?     Suppose a 3.771 g3.771 g sample of a second compound, compound B, is combusted in the same calorimeter, and the temperature rises from 25.65 ∘C25.65 ∘C to 29.76 ∘C.29.76 ∘C. What is the heat of combustion per gram of compound B?

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.

4. When 1.00 L of 1.05 M Ba(NO3)2 solution is mixed with 1.00 L of 1.10 M NazSO4 solution at 25.0°C in a coffee-cup calorimeter. The reaction is Ba(NOs)2(aq) + NazSO4(aq) → BaSO4(s) + 2NANO:(aq). The final temperature of the mixture increases to 28.1°C. Calculate the enthalpy change per mole for this process. (Assuming C=4.18 J °C' g' and density of the final solution is 1.05 g/ml).

The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy available from foods. Since the "bomb" itself can absorb energy, a separate experiment is needed to determine the heat capacity of the calorimeter. This is known as calibrating the calorimeter. In the laboratory a student burns a 0.461-g sample of 2-naphthylacetic acid (C12H1002) in a bomb calorimeter containing 1150. g water. The temperature increases from 24.70 °C to 27.20 °C. The specific heat capacity of water is 4.184 J g1 oC-1. The combustion enthalpy is -5779 kJ/mol 2-naphthylacetic acid. C12H1002(s) + 27/2 02(g) –→12 CO2(g) + 5 H20(1) A,H° -5779 kJ/mol Calculate the heat capacity of the calorimeter. heat capacity of calorimeter= orc J/C

A student is attempting to determine the heat capacity of a Styrofoam cup calorimeter by pouring hot water into a Styrofoam cup containing cold water. The student determined the mass of the cold water to be 21.2455 g and its initial temperature to be 20.36 °C. The mass of the hot water was 24.2646 g and its initial temperature as 34.54 °C. The final temperature of the water after mixing was determined to be 24.57°C. The specific heat capacity of the water is 4.184 J/(g•°C). What is the heat capacity of the Styrofoam cup calorimeter? Assume the temperature of the calorimeter is the same temperature as the cold water. 4.184 J/°C 132.5 J/°C