Editing Endothermic process (section)

==Details==
Whether a process can occur spontaneously depends not only on the [[enthalpy]] change but also on the [[entropy]] change ({{math|∆''S''}}) and [[Thermodynamic temperature|absolute temperature]] {{mvar|T}}. If a process is a [[spontaneous process]] at a certain temperature, the products have a lower [[Thermodynamic free energy|Gibbs free energy]] {{math|1=''G'' = ''H'' – ''TS''}} than the reactants (an [[exergonic process]]),<ref name="Oxtoby8th"/> even if the enthalpy of the products is higher. Thus, an endothermic process usually requires a [[Entropy production|favorable entropy increase]] ({{math|∆''S'' > 0}}) in the system that overcomes the unfavorable increase in enthalpy so that still {{math|∆''G'' < 0}}. While endothermic [[phase transition]]s into more disordered states of higher entropy, e.g. melting and vaporization, are common, spontaneous chemical processes at moderate temperatures are rarely endothermic.<ref>{{Cite web |title=Examples of Spontaneous Endothermic Reactions - Chemistry Examples |url=https://www.chemicool.com/examples/spontaneous-endothermic-reactions.html#:~:text=Hence%20reactions%20are%20spontaneous%20only,in%20free%20energy,%20is%20negative.&text=Exothermic%20reactions%20have%20negative%20values,with%20positive%20values%20of%20%CE%94H. |access-date=2024-06-28 |website=www.chemicool.com}}</ref> The enthalpy increase{{math| ∆''H'' ≫ 0}} in a hypothetical strongly endothermic process usually results in {{math|1=∆''G'' = ∆''H'' – ''T''∆''S'' > 0}}, which means that the process will not occur (unless driven by electrical or photon energy). An example of an endothermic and exergonic process is

:<chem>C6H12O6 + 6 H2O -> 12 H2 + 6 CO2</chem>
:<math>\Delta_r H^\circ = +627 \ \text{kJ/mol},\quad  \Delta_r G^\circ = -31 \ \text{kJ/mol}</math>.