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Himal kharel
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I recently studied that equilibrium constant is independent of concentration. But if you multiply both sides of equation by any number, equilibrium constant changes. Isn't this contradictory?
The equilibrium constant contradiction refers to a discrepancy between the value of the equilibrium constant calculated using different methods or experimental conditions. This can occur due to experimental errors, assumptions made in calculations, or limitations of the model used.
The equilibrium constant (Kc) is calculated by taking the ratio of the concentrations of products to reactants at equilibrium, each raised to their respective stoichiometric coefficients. This is based on the law of mass action, which states that the ratio of the concentrations of reactants and products at equilibrium is constant at a given temperature.
There are several factors that can lead to an equilibrium constant contradiction, such as experimental errors in measuring concentrations, assumptions made in calculations (such as assuming ideal behavior of gases or neglecting the effects of ionic strength), or limitations of the model used to describe the system.
In some cases, an equilibrium constant contradiction can be resolved by improving experimental techniques or accounting for additional factors in calculations. However, in some cases, the contradiction may be due to limitations of the model used and cannot be fully resolved.
An equilibrium constant contradiction may call into question the validity of results or calculations, as it indicates a discrepancy between different methods or experimental conditions. It is important to carefully consider the potential sources of error and limitations when interpreting the results of equilibrium constant calculations.