Reactions in which a substance decomposes by losing CO are called decarbonylation reactions. The decarbonylation of acetic acid proceeds according to: CH₃COOH(l) → CH₃OH(g) + CO(g) By using data from Appendix C, calculate the minimum temperature at which this process will be spontaneous under standard conditions. Assume that ΔH° and ΔS° do not vary with temperature.

검증된 단계별 안내

Identify the reaction: CH_3COOH(l) → CH_3OH(g) + CO(g).

Use the Gibbs free energy equation: ΔG° = ΔH° - TΔS°.

For spontaneity, set ΔG° < 0, which implies ΔH° < TΔS°.

Calculate ΔH° for the reaction using standard enthalpies of formation: ΔH° = ΣΔH°_f(products) - ΣΔH°_f(reactants).

Calculate ΔS° for the reaction using standard entropies: ΔS° = ΣS°(products) - ΣS°(reactants).

비슷한 문제에 대한 검증된 영상 답변:

이 영상 해법은 위 문제에 도움이 된다고 튜터들이 추천한 것입니다.

영상 길이:

11m

주요 개념

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

Gibbs Free Energy

Gibbs Free Energy (ΔG) is a thermodynamic potential that helps predict the spontaneity of a reaction at constant temperature and pressure. A reaction is spontaneous when ΔG is negative, which can be calculated using the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy.

Enthalpy and Entropy

Enthalpy (ΔH) is a measure of the total heat content of a system, while entropy (ΔS) quantifies the degree of disorder or randomness in a system. In the context of decarbonylation reactions, understanding how these two thermodynamic properties change during the reaction is crucial for determining the conditions under which the reaction becomes spontaneous.

Standard Conditions

Standard conditions refer to a set of specific conditions used as a reference point in thermodynamics, typically defined as 1 bar of pressure and a specified temperature, often 25°C (298 K). When calculating thermodynamic properties like ΔH and ΔS, it is essential to ensure that the values used are consistent with these standard conditions to accurately assess the spontaneity of the reaction.