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A bomb calorimeter, or constant volume calorimeter, is a device often used to determine the heat...

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Chemistry

A bomb calorimeter, or constant volume calorimeter, is a deviceoften used to determine the heat of combustion of fuels and theenergy content of foods. Since the \"bomb\" itself can absorb energy,a separate experiment is needed to determine the heat capacity ofthe calorimeter. This is known as calibrating the calorimeter. Inthe laboratory a student burns a 0.337-g sample of bisphenol A(C15H16O2) in a bomb calorimeter containing 1040. g of water. Thetemperature increases from 25.90 °C to 28.10 °C. The heat capacityof water is 4.184 J g-1°C-1. The molar heat of combustion is −7821kJ per mole of bisphenol A. C15H16O2(s) + 18 O2(g) 15 CO2(g) + 8H2O(l) + Energy Calculate the heat capacity of the calorimeter.heat capacity of calorimeter = J/°C

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4.5 Ratings (987 Votes)

Number of moles of biphenol = 0.337/(15*12 + 16*1 + 2*16) = 1.478 * 10^-3 moles

Heat energy gained by water q = m * S *dT

                                                       = 1040 * 4.184 * (28.1 - 25.9)

                                                       = 9572.99 J

Heat energy lost by biphenol = 1.478 * 10^-3 * 7821 * 10^3 J

                                                    = 11539.88 J

Remaing heat with caloire meter = 11539.88 - 9572.99

                                                           = 1966.89 J

Heat capacity of calorimeter = 1966.89 / (28.1-25.9) = 894.041 J / 0C
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