Write a balanced equation for the combustion of C7H16(l) (heptane) -- 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 C7H16(l) is -187.8 kJ/mol A) What is the standard heat of reaction (ΔH°) for the combustion reaction of C7H16(l)? B) Calculate the difference, ΔH-ΔE=Δ(PV) for the combustion reaction of 1 mole of heptane.

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Write a balanced equation for the combustion of C7H16(l) (heptane)
-- 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 C7H16(l) is -187.8 kJ/mol


A) What is the standard heat of reaction (Δ) for the combustion reaction of C7H16(l)?

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

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