heat in combustion as measured by the calorimeter = 60.8 kJ/K x (delta T) = ? kJ released.
?kJ released/deltaH in kJ/mol = #moles.
A constant pressure calorimeter having a heat capacity of 60.8 kJ/K is used to measure the energy released from burning a compound in excess oxygen to form CO2(g) and H2O(l). If the enthalpy of combustion of the compound is -2914.0 kJ/mol and the temperature of the calorimeter rises from 25.14 C to 26.79 C, how many moles of the compound were oxidized?
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