Method 3

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Madeline Ho 1C
Posts: 37
Joined: Mon Apr 23, 2018 3:00 am

Method 3

Postby Madeline Ho 1C » Mon Jan 28, 2019 6:16 pm

What does it mean when the standard enthalpy of formation of one molecule is more negative than another? For example, in class the standard enthalpy of formation for CO2 was -394 kJ/mol and for CH4 it was -75 kJ/mol. Does this mean CO2 is more stable?

Lia Inadomi 1I
Posts: 62
Joined: Fri Sep 28, 2018 12:15 am

Re: Method 3

Postby Lia Inadomi 1I » Mon Jan 28, 2019 6:48 pm

I think this relates to the strength of the bonds. So when CO2 is formed, it releases more heat because two double bonds are stronger than four single bonds like in CH4.

Jesse Kuehn 1B
Posts: 40
Joined: Wed Nov 14, 2018 12:23 am

Re: Method 3

Postby Jesse Kuehn 1B » Mon Jan 28, 2019 6:51 pm

I believe enthalpy refers to the amount fo energy that goes into the bond formation of that compound, the higher the enthalpy, the more energy that goes into the bond. Higher energy bonds also tend to be more reactive and release more energy so i think a higher enthalpy means less stable.


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