key term - Spontaneity

Definition

Spontaneity refers to the inherent tendency of a system or process to occur naturally, without the need for external intervention or energy input. It is a fundamental concept in chemistry that describes the natural, unforced progression of a reaction or physical change towards a more stable or favorable state.

5 Must Know Facts For Your Next Test

1. Spontaneous processes occur naturally and require no external energy input to proceed, while non-spontaneous processes require the addition of energy to occur.
2. The spontaneity of a process is determined by the change in Gibbs free energy, which takes into account both the change in enthalpy (energy) and the change in entropy (disorder) of the system.
3. Processes with a negative change in Gibbs free energy (∆G < 0) are considered spontaneous, while processes with a positive change in Gibbs free energy (∆G > 0) are non-spontaneous.
4. Entropy is a key factor in determining spontaneity, as systems tend to move towards a state of greater disorder or randomness, which corresponds to an increase in entropy.
5. The spontaneity of a process can be influenced by factors such as temperature, pressure, and the presence of catalysts, which can alter the balance between energy and entropy changes.

Review Questions

• Explain the relationship between spontaneity and the change in Gibbs free energy (∆G) of a process.
  • The spontaneity of a process is directly related to the change in Gibbs free energy (∆G). If ∆G is negative, the process is spontaneous and will occur naturally without the need for external energy input. Conversely, if ∆G is positive, the process is non-spontaneous and will not occur naturally, requiring the addition of energy to proceed. The magnitude of ∆G also indicates the driving force behind the spontaneity, with larger negative values corresponding to more favorable, spontaneous processes.
• Describe how the concepts of enthalpy and entropy contribute to the spontaneity of a process.
  • Spontaneity is determined by the combined effects of enthalpy (energy) and entropy (disorder) changes in a system, as captured by the Gibbs free energy equation: ∆G = ∆H - T∆S. Processes with a decrease in enthalpy (∆H < 0) and an increase in entropy (∆S > 0) will have a negative change in Gibbs free energy (∆G < 0), making them spontaneous. Conversely, processes with an increase in enthalpy (∆H > 0) and a decrease in entropy (∆S < 0) will have a positive change in Gibbs free energy (∆G > 0), rendering them non-spontaneous. The balance between these two factors determines the overall spontaneity of a process.
• Analyze how external factors, such as temperature and the presence of catalysts, can influence the spontaneity of a process.
  • The spontaneity of a process can be influenced by various external factors, such as temperature and the presence of catalysts. An increase in temperature, for example, can affect the balance between enthalpy and entropy changes, potentially shifting the spontaneity of a process. Higher temperatures generally favor processes with an increase in entropy (∆S > 0), making them more spontaneous. Catalysts, on the other hand, can alter the activation energy barriers of a process, facilitating the reaction and making it more spontaneous, even if the overall change in Gibbs free energy remains the same. By understanding how these external factors can influence spontaneity, one can better predict and control the behavior of chemical and physical systems.

Related terms

Entropy:

A measure of the disorder or randomness within a system, which increases as a system moves towards a more spontaneous state.

Gibbs Free Energy:

A thermodynamic quantity that combines the concepts of energy and entropy to determine the spontaneity and feasibility of a process.

Thermodynamics:

The study of the relationships between heat, work, temperature, and energy in a system, which provides the underlying principles for understanding spontaneity.