A 1.107-g sample of benzoic acid (HC;H;O:) is burned in an excess of O:(g) in a bomb calorimeter, which is immersed in water. The reaction produces heat that causes the temperature of the water and bomb to increase from 24.96 to 29.20°C. (a) If the heat capacity of the calorimeter is 6.90 KJºC, how many kilojoules of heat are produced by the combustion of 1.107 g of benzoic acid? (b) Calculate the heat of combustion per gram of benzoic acid and the molar enthalpy of combustion of benzoic acid.

A bomb calorimeter has a heat capacity of 2.47 kJ/?. When a 1.00 mol sample of a certain hydrocarbon was burned in this calorimeter, the temperature increased by 2.14?. Calculate the heat of combustion per mole of the hydrocarbon.

An experiment was performed to calculate the heat of solution for potassium fluoride. Use the following data to determine its heat of solution. Assume that the specific heat capacity of the solution produced is the same as that of water, 4.184 J⁄g·°C. Identity of Salt   KF Mass of water in calorimeter (g)   52.42 Mass of salt sample (g)   7.32 Initial temperature of Calorimeter (°C)   20.8 Final temperature of Calorimeter (°C)   30.3 Report your answer in kJ/mol to 3 significant figures.

When 1.091 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, in kJ/mol?

A) When 1.911 grams of sucrose (Molar mass 342.3 g/mol) is burned in a bomb calorimeter, the temperature of the calorimeter increases from 22.410 °C to 26.630 °C. If the heat capacity of the calorimeter is 4.900 kJ/ °C, what is the heat of combustion of sucrose, in kJ/mol? And B) A 90.0 g piece of metal, initially at 98.60 °C, is placed into 120.0 g of water initially at 24.30 °C. If the final temperature of the water is 34.00 °C, what is the specific heat of the metal? (The specific heat of water is 4.184 J/g･ °C).

A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200.g of water  First, a 5.500g tablet of benzoic acid C6H5CO2H is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454kJ/g.) The temperature of the water is observed to rise from 16.00°C to 44.20°C over a time of 10.7 minutes. Next, 5.120g of ethanol C2H5OH are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00°C to 41.79°C. Use this information, to answer the questions below about this reaction:   A "bomb" calorimeter. C2H5OH(l) + 3O2(g) → 2CO2(g)  3H2O(g) Be sure any of your answers that are calculated from measured data are rounded to the correct number of significant digits. Note for advanced students: it's possible the student did not do these experiments sufficiently carefully, and the values you calculate may not exactly…

In a constant‑pressure calorimeter, 55.0 mL of 0.340 M Ba(OH)2 was added to 55.0 mL of 0.680 HCl. The reaction caused the temperature of the solution to rise from 23.90 ∘C to 28.53 ∘C. If the solution has the same density and specific heat as water, what is heat absorbed by the solution? Assume that the total volume is the sum of the individual volumes. (And notice that the answer is in kJ).

When 1.151 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, in kJ/mol?

A 1.261 g sample of a new organic material is combusted in a bomb calorimeter. The temperature of the calorimeter and its contents increase from 25.39 °C to 28.44 °C. The heat capacity (calorimeter constant) of the calorimeter is 27.69 kJ/ °C, what is the heat of combustion per gram of the material? heat of combustion: kJ/g

Consider the combustion of liquid CsHs in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of CsHs is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.632 °C. If -4790 J of heat was produced from the combustion of 0.001561 moles of CsHs, what is the enthalpy change (in kJ/mol) for the combustion of CsHs?