A 0.692 g sample of glucose, C6H12O6 is oxidized (burned) in a calorimeter. The calorimeter contains 575 g of water, and the temperature rises from 21.70°C to 25.22°C. Calculate the molar enthalpy of combustion of glucose.

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…

2) A0.500 g sample of Trinitrotoluene (C7H$N2O6) is burned in a bomb calorimeter containing 610 grams of water at an initial temperature of 20°C. The heat capacity of the calorimeter is 420 J°C and the heat of combustion of Trinitrotoluene is 3374 kJ/mol. Using these data, calculate the final temperature of the water and calorimeter once the reaction is complete.

THERMODYNAMICS: A 1.6 g sample of acetic acid (HC2H3O2) was burned in excess oxygen in a bomb calorimeter. The calorimeter, which alone had a heat capacity of 2.67 kJ/ºC, contained 7 g of water. The temperature of the calorimeter and its contents increased from 23.58°C to 27.95°C. What is AH (in kJ) for the combustion per 1.00 mol of acetic acid? MW of acetic acid is 60 g/mol. (Round off the final answer to ONE decimal place. Do not include the unit.)