Is it possible for a reaction to be nonspontaneous yet exo-thermic? Explain.

검증된 단계별 안내

Understand the terms: A reaction is exothermic if it releases heat, meaning the enthalpy change (ΔH) is negative. A reaction is nonspontaneous if it does not occur on its own without external input, which is determined by the Gibbs free energy change (ΔG).

Recall the Gibbs free energy equation: ΔG = ΔH - TΔS, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.

Consider the conditions for spontaneity: A reaction is spontaneous if ΔG is negative. If ΔG is positive, the reaction is nonspontaneous.

Analyze the scenario: For a reaction to be exothermic (ΔH < 0) and nonspontaneous (ΔG > 0), the term TΔS must be positive and larger in magnitude than ΔH, meaning the entropy change (ΔS) is positive and significant enough to make ΔG positive.

Conclude: Yes, it is possible for a reaction to be nonspontaneous yet exothermic if the increase in entropy (ΔS) is large enough to make the TΔS term outweigh the negative ΔH, resulting in a positive ΔG.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Spontaneity of Reactions

Spontaneity refers to whether a reaction occurs naturally under given conditions without external influence. A spontaneous reaction has a negative Gibbs free energy change (ΔG < 0). However, spontaneity is not solely determined by enthalpy (heat content) but also by entropy (disorder), which can lead to nonspontaneous reactions even if they release heat.

Exothermic Reactions

Exothermic reactions are those that release heat to the surroundings, resulting in a negative change in enthalpy (ΔH < 0). While these reactions often favor spontaneity, they can still be nonspontaneous if the increase in entropy is insufficient to overcome the energy barrier, particularly at lower temperatures or under specific conditions.

Gibbs Free Energy

Gibbs free energy (G) combines enthalpy and entropy to determine the spontaneity of a reaction. The equation ΔG = ΔH - TΔS shows that a reaction can be exothermic (ΔH < 0) but still have a positive ΔG if the entropy change (ΔS) is negative or not large enough to offset the enthalpy term, resulting in a nonspontaneous process.