key term - Spontaneous process

Definition

A spontaneous process is a physical or chemical change that occurs without the need for external energy input once it has been initiated. These processes tend to proceed in the direction of increasing entropy, or disorder, and are often characterized by a natural tendency to move toward equilibrium. Understanding spontaneous processes is crucial when distinguishing between reversible and irreversible processes, as spontaneity is often tied to irreversibility in real-world scenarios.

5 Must Know Facts For Your Next Test

1. Spontaneous processes are typically irreversible, meaning they cannot return to their original state without external influence.
2. The Second Law of Thermodynamics states that the total entropy of an isolated system can never decrease over time, supporting the concept of spontaneity.
3. In exothermic reactions, heat is released, often leading to increased spontaneity due to higher entropy in the surroundings.
4. Not all spontaneous processes happen quickly; some can be slow and take a long time to reach completion despite being spontaneous.
5. Examples of spontaneous processes include the melting of ice at room temperature and the diffusion of gas molecules in a container.

Review Questions

• How does the concept of entropy relate to spontaneous processes, and why is this relationship significant?
  • Entropy plays a central role in determining whether a process is spontaneous. A spontaneous process typically results in an increase in the total entropy of the universe, aligning with the Second Law of Thermodynamics. This relationship signifies that as systems evolve toward equilibrium, they tend to move toward configurations that have higher disorder or randomness, highlighting how spontaneity is fundamentally connected to entropy changes.
• Discuss how Gibbs free energy can be used to predict the spontaneity of a chemical reaction.
  • Gibbs free energy combines enthalpy and entropy into a single value that indicates the spontaneity of a reaction under constant temperature and pressure. If the change in Gibbs free energy (ΔG) for a reaction is negative, it suggests that the process can occur spontaneously. This predictive tool helps chemists understand not only if reactions will proceed but also under what conditions they might do so, allowing for better planning in chemical processes.
• Evaluate how irreversible spontaneous processes differ from reversible ones and provide examples of each.
  • Irreversible spontaneous processes occur naturally without external intervention and cannot simply reverse back to their original states, such as combustion or diffusion. In contrast, reversible processes can be returned to their initial states with no net change in the system or surroundings, like certain phase changes under controlled conditions. This distinction emphasizes that while all reversible processes can happen spontaneously under specific conditions, not all spontaneous processes are reversible, illustrating important thermodynamic principles.

Related terms

entropy: A measure of the disorder or randomness in a system, which tends to increase in spontaneous processes.

Gibbs free energy: A thermodynamic potential that helps predict whether a process will occur spontaneously at constant temperature and pressure; a negative change in Gibbs free energy indicates spontaneity.

equilibrium:

A state in which the forward and reverse processes occur at equal rates, resulting in no net change; spontaneous processes work toward achieving this state.