Why Does the Equilibrium Constant Depend Only on Temperature?

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The equilibrium constant (K) is defined by the ratio of concentrations of products to reactants at equilibrium and remains constant at a given temperature, regardless of changes in concentration or partial pressure. When products or reactants are added, the reaction quotient (Q) changes, but the system will adjust until Q equals K, restoring equilibrium. This adjustment reflects the dynamic nature of chemical reactions, where the system self-regulates to maintain the equilibrium constant. The relationship between K and temperature is crucial, as K varies with temperature changes but remains unaffected by concentration shifts. Understanding these principles clarifies how equilibrium is established and maintained in chemical systems.
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.
 
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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.
 
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