Write a balanced equation for the combustion of C9H20(l) (nonane)-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l). Given the following standard heats of formation: ΔHf° of CO2(g) is -393.5 kJ/mol ΔHf° of H2O(l) is -286 kJ/mol ΔHf° of C9H20(l) is -229.0 kJ/mol -6172.5 kJ Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of nonane.(Assume standard state conditions and 298 K for all reactants and products.)

Question

Write a balanced equation for the combustion of C9H20(l) (nonane)
-- i.e. its reaction with O2(g) forming the products CO2(g) and H2O(l).

Given the following standard heats of formation:

  • ΔHf° of CO2(g) is -393.5 kJ/mol
  • ΔHf° of H2O(l) is -286 kJ/mol
  • ΔHf° of C9H20(l) is -229.0 kJ/mol

-6172.5 kJ

Calculate the difference, ΔHE(PV) for the combustion reaction of 1 mole of nonane.
(Assume standard state conditions and 298 K for all reactants and products.)

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