Answer:
changing the temperature
Explanation:
In general, a reaction is said to be at equilibrium when the rate of consumption of the reactants equals the rate of formation of products. The dynamics of this state can be represented in terms of the 'equilibrium constant', Keq which is the ratio of the concentration of products to that of the reactants.
Consider a hypothetical reaction:
A ↔ B
[tex]Keq = \frac{[B]}{[A]}[/tex]
Based on the above equation, the value of Keq should increase if the concentration of B i.e. the product is decreased. However, if concentration of B is decreased then based on Le Chatelier's principle, the equilibrium will shift in a direction to produce more of B such that a new equilibrium is established and Keq remains undisturbed. This is also the case for changes in pressure.
It is only by changing the temperature does the value of Keq change.
