What is the Difference Between Free Energy and Activation Energy?
🆚 Go to Comparative Table 🆚The main difference between free energy and activation energy lies in their definitions and applications. Here are the key differences:
- Free Energy:
- Free energy, also known as Gibbs free energy, is the amount of energy available for a thermodynamic system to perform work.
- It is used in thermodynamic systems and physical chemistry.
- Free energy considers the impact of changes in entropy on the reaction process.
- Mathematically, it is represented as: $$\Delta G = \Delta H - T \Delta S$$, where $$\Delta G$$ is the change in Gibbs free energy, $$\Delta H$$ is the change in enthalpy, $$T$$ is the temperature, and $$\Delta S$$ is the change in entropy.
- Activation Energy:
- Activation energy is the energy barrier that has to be overcome for a chemical reaction to proceed.
- It is mainly used in chemical reactions and biochemistry.
- Activation energy is the minimum amount of energy required for the reaction to reach its transition state.
- Mathematically, it can be represented as: $$k = A e^{-\frac{Ea}{RT}}$$, where $$k$$ is the rate constant, $$A$$ is the Arrhenius constant, $$R$$ is the gas constant, $$T$$ is the temperature, and $$Ea$$ is the activation energy.
In summary, free energy is the amount of energy available to perform work in a thermodynamic system, while activation energy is the energy barrier that has to be overcome for a chemical reaction to proceed. Free energy is used in thermodynamic systems and physical chemistry, whereas activation energy is mainly used in chemical reactions and biochemistry.
Comparative Table: Free Energy vs Activation Energy
The main difference between free energy and activation energy lies in their definitions and applications in thermodynamics and chemical reactions. Here is a comparison table highlighting the differences between the two:
| Free Energy | Activation Energy |
|---|---|
| The amount of energy available to perform a thermodynamic process. | The energy barrier that has to be overcome by the reactant to produce the products. |
| Represented as ∆G, where ∆G is the change in Gibbs free energy. | Represented as Ea, where Ea is the activation energy. |
| Not affected by catalysts. | Affected by catalysts. |
| Relevant to thermodynamic systems in physical chemistry. | Mainly relevant to chemical reactions in biochemistry. |
In summary, free energy is the amount of energy available for a thermodynamic system to perform work, while activation energy is the energy barrier that has to be overcome for a chemical reaction to proceed.
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