# Spontaneity (chemistry)

time-evolution of a system in which it releases free energy and moves to a lower, more thermodynamically stable energy state

The spontaneity of a process refers to whether or not the reaction would occur without an input of energy, because of the value of the reaction's Gibbs free energy.

The Gibbs free energy is given by:

${\displaystyle \Delta G=\Delta H-T\Delta S\,}$

where ${\displaystyle \Delta G}$ refers to the Gibbs free energy, ${\displaystyle \Delta H}$to the enthalpy change, ${\displaystyle T}$ to the temperature (in Kelvin) and ${\displaystyle \Delta S}$ to the entropy change.

If the Gibbs free energy change is 0 or negative, the reaction is said to be spontaneous and can occur without an input of energy into the system. If the Gibbs free energy were above 0, the reaction would not be spontaneous and would require an input of energy in order for it to proceed.

In equilibrium reactions, a reaction one way will be spontaneous, while the reverse reaction will be non-spontaneous. Therefore, using a general formula for equilibria:

${\displaystyle {\ce {A <=> B + C}}}$

If the formation of compounds ${\displaystyle B}$ and ${\displaystyle C}$ from ${\displaystyle A}$ were spontaneous, the formation of compound ${\displaystyle A}$ from ${\displaystyle B}$ and ${\displaystyle C}$ would be non-spontaneous.

An example of a spontaneous process is the conversion of diamond into graphite, because graphite has a more thermodynamically stable structure.[1] An example of a non-spontaneous process would be the combustion of methane in oxygen to form carbon dioxide and water, as this requires an input of energy.[2]

## References

1. "Spontaneous and Nonspontaneous Processes". Retrieved 7 August 2019.
2. "Combustion of Fossil Fuels". Retrieved 7 August 2019.