Editing Chemical reaction (section)

====Forward reactions====
Reactions that proceed in the forward direction (from left to right) to approach equilibrium are often called [[spontaneous reaction]]s, that is, <math>\Delta G</math> is negative, which means that if they occur at constant temperature and pressure, they decrease the [[Gibbs free energy]] of the reaction. They require less energy to proceed in the forward direction.<ref name="libretext2">{{Cite web |date=2016-08-05 |title=11.5: Spontaneous Reactions and Free Energy |url=https://chem.libretexts.org/Courses/University_of_Kentucky/UK%3A_CHE_103_-_Chemistry_for_Allied_Health_(Soult)/Chapters/Chapter_11%3A_Properties_of_Reactions/11.5%3A_Spontaneous_Reactions_and_Free_Energy#:~:text=The%20forward,form. |access-date=2023-04-11 |website=Chemistry LibreTexts |language=en}}</ref> Reactions are usually written as forward reactions in the direction in which they are spontaneous. Examples:
* Reaction of hydrogen and oxygen to form water.
:{{chem|2H|2}} + {{chem|O|2}} {{eqm}} {{chem|2H|2|O}}
* Dissociation of [[acetic acid]] in water into [[acetate]] ions and [[hydronium ion]]s.
:{{chem|CH|3|COOH}} + {{chem|H|2|O}} {{eqm}} {{chem|CH|3|COO|-}} + {{chem|H|3|O|+}}