Hydrocarbon fuels can be produced to form methanol byreactions such as the follo

Question

Hydrocarbon fuels can be produced to form methanol byreactions such as the following, which yields 1-hexane: 6CH3OH (g) --> C6H12(g) + 6H2O (g) Compare the standard heat of combustion at 25 degrees C of6CH3OH (g) which the standard heat of combustion at 25degrees of C6H12 (g) for reaction productsCO2 (g) and H2O (g). Hydrocarbon fuels can be produced to form methanol byreactions such as the following, which yields 1-hexane: 6CH3OH (g) --> C6H12(g) + 6H2O (g) Compare the standard heat of combustion at 25 degrees C of6CH3OH (g) which the standard heat of combustion at 25degrees of C6H12 (g) for reaction productsCO2 (g) and H2O (g). Compare the standard heat of combustion at 25 degrees C of6CH3OH (g) which the standard heat of combustion at 25degrees of C6H12 (g) for reaction productsCO2 (g) and H2O (g).

Explanation / Answer

   We Know that the given Reaction is :       6CH3OH (g)--> C6H12 (g) + 6H2O(g)      6 CH3 OH + 9 O2 ------> 6CO2 + 12 H2O          Hrxn =   H0 (products )   - H0 (Reactants )                       = { -393.5 x 6 + 12 x -285.8 } KJ - 6 ( -238.4KJ)                        = - 4360.2 KJ      C6H12 +  9O2   -------->   6CO2 + 6 H2O         Hrxn =    H0( products )   - H0 (Reactants )                     = { 6 x -393.5 + 6 x -285.8 } KJ - 1x (-123.4 ) KJ                      = - 4199.2 KJ         By Comparing theHeat combustions of CH3OH &C6H12 The Cyclohexane produces moreenergy than methanol      As in the above case 6 moles ofmethanol we have taken for corresponding 1 mole of cyclohexane. It indicates greater the percentage of carbon more will be the energy release.         

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