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The reaction is C7H16(L) + 11O2 = 7CO2 + 8H2O


Heat of combustion for one mole C7H16 is -4.85*10^3 KJ


Using the information given, calculate \(\Delta H\) º for C7H16 in kJ/mol


\(\Delta H\) ºf CO2 = -393.5 kJ/mol


\(\Delta H\) ºf H2O = -285.8 kJ/mol


I was actually able to solve this myself. The heat for formation of one mole c7h16 = -187.4 kJ/mol.


Please mark as completed.

 Mar 24, 2019
edited by Cent0rea88  Mar 24, 2019

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