The molar enthalpy of the combustion is the amount of energy released when 1 mole of the substance combusts in excess oxygen:
.
The energy released can be calculated using the specific heat capacities of tin (0.218 J/g°C) and of water (4.186 J/g°C). Assuming the density of water equal 1 g/mL, the mass of water is 200 g. Therefore:
J.
The number of the moles of butane is its mass divided by its molar mass (58.12 g/mol):
mol.
Finally, the molar enthalpy of combustion of butane is:
J/mol, or 333 kJ/mol
Answer: the molar enthalpy of the combustion of butane is 333 kJ/mol.
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