1 Answer
The Gibbs-Helmholtz equation relates the change in the Gibbs free energy of a system to its temperature and entropy. It provides a way to calculate the change in free energy at different temperatures and is useful in thermodynamics for understanding spontaneous processes.
The equation is:
$$
\Delta G = \Delta H - T\Delta S
$$
Where:
* $\Delta G$ is the change in Gibbs free energy,
* $\Delta H$ is the change in enthalpy,
* $T$ is the absolute temperature (in Kelvin),
* $\Delta S$ is the change in entropy.
### More specifically, the **Gibbs-Helmholtz equation** is often expressed in a differential form:
$$
\left(\frac{\partial G}{\partial T}\right)_P = -S
$$
This form shows that the rate of change of Gibbs free energy with temperature, at constant pressure, is equal to the negative of the entropy.
This equation is important in studying chemical reactions and phase changes, as it allows you to predict whether a reaction is spontaneous at a given temperature.
The equation is:
$$
\Delta G = \Delta H - T\Delta S
$$
Where:
* $\Delta G$ is the change in Gibbs free energy,
* $\Delta H$ is the change in enthalpy,
* $T$ is the absolute temperature (in Kelvin),
* $\Delta S$ is the change in entropy.
### More specifically, the **Gibbs-Helmholtz equation** is often expressed in a differential form:
$$
\left(\frac{\partial G}{\partial T}\right)_P = -S
$$
This form shows that the rate of change of Gibbs free energy with temperature, at constant pressure, is equal to the negative of the entropy.
This equation is important in studying chemical reactions and phase changes, as it allows you to predict whether a reaction is spontaneous at a given temperature.