Discussion Overview
The discussion centers around the reversibility of substitution reactions, specifically examining the reaction between hydrogen and copper(II) chloride to form copper and hydrochloric acid. Participants explore the conditions under which such reactions may or may not be reversible, considering factors like Gibbs energy and the activity of the involved elements.
Discussion Character
- Debate/contested
- Technical explanation
- Mathematical reasoning
Main Points Raised
- Some participants propose that the reaction H2 + CuCl2 = Cu + 2HCl may not be reversible because copper is less active than hydrogen, suggesting that copper cannot substitute hydrogen in hydrochloric acid.
- Others reference Gibbs energy and its relation to the rates of direct and reverse reactions, indicating that both entropic and enthalpic contributions must be considered to assess reversibility.
- A participant mentions specific Gibbs energy values for HCl and CuCl2, arguing that the Gibbs energy of HCl is significantly more negative, which implies that the reaction is difficult to reverse at room temperature.
- There is a repeated emphasis on the need to analyze the Gibbs energy to understand the feasibility of the reverse reaction.
Areas of Agreement / Disagreement
Participants express differing views on the reversibility of the reaction, with no consensus reached. Some support the idea that the reaction is not reversible due to the activity of copper, while others focus on Gibbs energy calculations that may suggest otherwise.
Contextual Notes
Participants reference specific Gibbs energy calculations and the significance of entropic and enthalpic contributions, but the discussion does not resolve the assumptions or conditions under which these calculations apply.
Who May Find This Useful
This discussion may be of interest to those studying chemical thermodynamics, reaction kinetics, or substitution reactions in chemistry.
