🧤physical chemistry i review

key term - Spontaneity

Definition

Spontaneity refers to the natural tendency of a process to occur without external influence, often associated with changes in energy and disorder within a system. This concept is deeply connected to the idea of entropy, as spontaneous processes typically lead to an increase in entropy, reflecting the direction in which a system tends to evolve. The relationship between spontaneity and entropy helps to predict the feasibility of reactions and physical transformations.

5 Must Know Facts For Your Next Test

  1. Spontaneous processes are characterized by a decrease in Gibbs free energy ($$\Delta G < 0$$), indicating that the process can occur without input of energy.
  2. The second law of thermodynamics states that for a spontaneous process, the total entropy of an isolated system will either increase or remain constant.
  3. Reactions can be spontaneous in one direction and non-spontaneous in the reverse direction; this is often observed in chemical equilibria.
  4. The temperature can affect spontaneity; some processes that are non-spontaneous at lower temperatures may become spontaneous at higher temperatures due to changes in entropy.
  5. Spontaneity does not imply rapidity; spontaneous processes can occur over various timescales, from instantaneous to very slow.

Review Questions

  • How does the concept of spontaneity relate to changes in entropy during a process?
    • Spontaneity is closely tied to changes in entropy, as spontaneous processes typically lead to an increase in the overall entropy of a system and its surroundings. According to the second law of thermodynamics, for a process to be spontaneous, the total change in entropy must be positive. This means that as a system evolves spontaneously, it moves towards a state of greater disorder or randomness.
  • Discuss how Gibbs free energy can be used to determine whether a chemical reaction is spontaneous or not.
    • Gibbs free energy is a critical factor in assessing spontaneity because it incorporates both enthalpy and entropy changes. A reaction is considered spontaneous if the change in Gibbs free energy ($$\Delta G$$) is negative ($$\Delta G < 0$$). This relationship allows chemists to predict whether reactions will occur under specific conditions by analyzing how enthalpy and entropy contribute to the overall energy balance.
  • Evaluate the implications of temperature on the spontaneity of reactions, particularly concerning endothermic processes.
    • Temperature plays a significant role in determining the spontaneity of reactions, especially for endothermic processes that absorb heat. While endothermic reactions typically have positive enthalpy changes ($$\Delta H > 0$$), they can still be spontaneous if the increase in entropy ($$\Delta S > 0$$) is large enough to overcome the positive enthalpy term when calculating Gibbs free energy. As temperature increases, the impact of entropy on Gibbs free energy becomes more pronounced, potentially making previously non-spontaneous endothermic reactions favorable.