Why Does the Equilibrium Constant Depend Only on Temperature?

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Discussion Overview

The discussion centers on the reasons why the equilibrium constant (K) is dependent solely on temperature, rather than on the concentrations or partial pressures of reactants and products. Participants explore the implications of this dependency in the context of chemical equilibrium and reaction quotients.

Discussion Character

  • Technical explanation, Conceptual clarification, Debate/contested

Main Points Raised

  • One participant questions why the equilibrium constant K remains unchanged with variations in concentrations of products or reactants, given its definition as the ratio of product concentrations to reactant concentrations.
  • Another participant clarifies that while the reaction quotient Q changes with the addition of products or reactants, the system will adjust until Q equals K, which describes the equilibrium state.
  • A subsequent participant seeks to understand if the ratio of products to reactants remains constant once the system reaches equilibrium, indicating confusion about the nature of K and Q.
  • Further clarification is provided that the system adjusts itself to reach equilibrium, and that the reaction quotient is more complex than a simple ratio, suggesting a need for deeper understanding of these concepts.

Areas of Agreement / Disagreement

Participants express differing views on the relationship between K and Q, with some seeking clarification on the concepts while others emphasize the distinction between equilibrium and non-equilibrium states. The discussion remains unresolved regarding the specific implications of these relationships.

Contextual Notes

There are indications of confusion regarding the definitions and implications of K and Q, as well as the nature of equilibrium adjustments. Participants have not fully agreed on the interpretations of these concepts.

Scharles
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why the equilibrium constant only depending on temperature but not concentration and partial pressure ?

Since K= [product]/[reactants], why the value of K remain the same as [product]or [reactant] increase ?
 
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When you add products or reactants Q - so called reaction quotient, defined identically as K - changes its value. However, after that system will react and concentrations of products and reactants will change till Q=K. K describes system at equilibrium, Q describes system at any moment.
 
Last edited by a moderator:
isn't mean that the ratio of [products] / [reactants] remain unchanged after the system is adjusted to equilibrium ??
 
Scharles said:
isn't mean that the ratio of [products] / [reactants] remain unchanged after the system is adjusted to equilibrium ??

System is not adjusted, system adjusts itself. It is not just ratio of products/reactants we are talking about, but reaction quotient, which is more complicated than simple ratio. And finally this is not a correct phrase and I have troubles trying to decipher what you are asking about. Please elaborate.
 
Last edited by a moderator:

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