When q > k, the amount of the products must <u>decrease </u>and the amount of the reactants must <u>increase </u>until equilibrium is established. The reaction will proceed toward the <u>reactants</u>
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What is equilibrium?</h3>
In a reversible chemical reaction, chemical equilibrium is the state in which there is no net change in the quantity of reactants or products. When a chemical reaction is reversible, the products react with the original reactants as soon as they are created.
There is no net change in the quantity of the chemicals involved when the two opposing reactions are in equilibrium because they are occurring at identical rates, or velocities. At this point, the reaction may be deemed to be finished, meaning that the maximum amount of reactants to products has been converted under the given reaction conditions. It is possible to formulate the equilibrium conditions quantitatively.
For example, for the reversible reaction A ⇋ B + C, the velocity of the reaction to the right, , is given by the mathematical expression (based on the law of mass action) = (A), where is the reaction-rate constant and the symbol in parentheses represents the concentration of A. The velocity of the reaction to the left, , is = (B)(C). At equilibrium, = , therefore:
or
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