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16 July, 11:19

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 0.9973 g sample of isophthalic acid (C8H6O4) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.319*103 g of water. During the combustion the temperature increases from 25.37 to 28.49 °C. The heat capacity of water is 4.184 J g-1°C-1. The heat capacity of the calorimeter was determined in a previous experiment to be 939.3 J/°C. Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of isophthalic acid based on these data.

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  1. 16 July, 11:26
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    find heat released by the burn:

    (2 g) (19.4 kJ/g) = 38.8 kJ released

    find heat gained by the water:

    dH = m C dT

    dH = (2250 g) (4.184 J/g-C) ( + 3.17 C)

    dH = 29,842 Joules

    aka

    dH water = + 29.8 kJ

    find the missing heat given to the calorimeter

    (38.8 kJ released) - (29.8 kJ given to water) = 9.0 kJ given to calorimeter

    What is the heat capacity of the empty bomb calorimeter

    (9.0 kJ given to calorimeter) / (3.17 C rise in temp) = 2.84 kJ / C
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