Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074



Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

A bomb calorimetric experiment was run to determine the enthalpy of combustion of ethanol. The reaction is

C2H5OH() + 3 O2(g) → 2 CO2(g) + 3 H2O()

The bomb had a heat capacity of 550 J/K, and the calorimeter contained 650 g of water. Burning 4.20 g of ethanol, C2HsOH() resulted in a rise in temperature from 18.5 °C to 22.3 °C. Calculate ΔU for the combustion of ethanol, in kJ/mosl.

Interpretation Introduction


The change in internal energy for the combustion of ethanol has to be determined.

Concept Introduction:

Sum of all energies transferred as heat in the system


Heat energy required to raise the temperature of 1g of substance by 1K.Energy gained or lost can be calculated using the below equation.


Where, q= energy gained or lost for a given mass of substance (m), C =specific heat capacity,ΔT= change in temperature.



  Specific heat capacity of bomb=550J/K

  Mass of ethanol=4.20g

  Mass of water=650g

  qwater=4.184JK/g(650g)(3.8K)=10334J= 10.334kJ

  qbomb=550J/K×3.8K =2090J=2

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