A bomb calorimeter , or constant volume calorimeter, is a device often used to d

Question

A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of 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 0.419-g sample of 9,10-anthracenedione(C14H8O2) in a bomb calorimeter containing 1080. g of water. The temperature increases from 25.60 °C to 28.00 °C. The heat capacity of water is 4.184 J g-1°C-1.

The molar heat of combustion is 6464 kJ per mole of 9,10-anthracenedione.

Calculate the heat capacity of the calorimeter.

Explanation / Answer

Molar mass of C14H8O2 is 208.2121 g/mol

moles of C14H8O2 = 0.419/208.2121

=2.01*10^-3 moles

heat energy released = 2.01*10^-3*6464

=13 kJ

so, let the head capacity of the calorimeter be x.so,

heat energy lost= heat energy gained

or 4.184*1080*(28-25.6) + x*(28-25.6) = 13000

or x=897.947 J/K

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