Enthalpy change

2010-12-27 7:23 am
Take reaction between H2 and O2 as an example:
2H2 + O2 ---> 2H2O
In the reaction, hydrogen and oxygen will be broken down into H and O, this is endothermic.
And forming 4 O-H bond is exothermic.
Overall, the exothermic process gives out more energy than the energy required by the endothermic process. So it is exothermic reaction.

My question is "why the energy required for exthermic process gives out more energy than the energy required by the endothermic process?", is it related to something strength of bbond, or others etc...? Similarly, the decomposition of NH3 into N2 and H2 is overall endothermic reaction, as the endothermic process required more energy than that the energy given out by the exothermic reaction, why?
更新1:

Please look deeply to my question.... It is not related to heat loss

回答 (2)

2010-12-28 12:16 am
✔ 最佳答案
It is because of the bonding and the structure of the compound.

If the reaction is exothermic, it means the atoms find a more stable arrangement, i.e. turns to a more stable compound. For example, In a H-H bond, energy is needed to overcome the replusive force because of a short distance between the nucleus. It is similar for O=O. but for a O-H bond, due to the electronegativity of the O atom, it hold the hydrogen atom more efficient, and less energy is need to maintain the bonding. Therefore the reaction 2 H2 + O2 ==> 2 H2O is exothermic.

An endothermic reaction is similar, but in the converse.

2010-12-27 10:19 am
that is mainly due heat loss!! If u assume during normal state!! e.g. in industry a carnot cycle can only provide 30% of efficiency


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