chemical equilibrium class 11
Chemical equilibrium is a state in which the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations of the reactants and products remain constant over time. In other words, chemical equilibrium is a dynamic state where both forward and reverse reactions occur at the same rate, resulting in no net change in the concentrations of reactants and products.
The rules of thermodynamics, in particular the second law, which stipulates that all spontaneous processes move towards a state of maximum entropy or disorder, control chemical equilibrium. As reactants in a chemical process are transformed into products, the system's entropy, or disorder, rises. When a system reaches equilibrium, its maximum entropy or disorder is present, and its Gibbs free energy—a measure of the energy available to do work—minimizes.
The equilibrium constant, denoted by K, is a measure of the extent to which a chemical reaction reaches equilibrium. The equilibrium constant is defined as the ratio of the concentrations of products to the concentrations of reactants, each raised to their stoichiometric coefficients. The equilibrium constant is a thermodynamic property that depends only on the temperature of the system and not on the initial concentrations of reactants and products.
If the value of the equilibrium constant is greater than 1, it indicates that the forward reaction is favored, and at equilibrium, the concentration of products is greater than the concentration of reactants. If the value of the equilibrium constant is less than 1, it indicates that the reverse reaction is favored, and at equilibrium, the concentration of reactants is greater than the concentration of products. If the value of the equilibrium constant is equal to 1, it indicates that the forward and reverse reactions are proceeding at the same rate, and the concentrations of reactants and products are equal at equilibrium.
The principle of Le Chatelier's is another important concept related to chemical equilibrium. Le Chatelier's principle states that when a system in equilibrium is subjected to a stress, such as a change in temperature, pressure, or concentration, the system will respond in such a way as to counteract the stress and restore equilibrium. For example, if the temperature of a system in equilibrium is increased, the system will respond by shifting the equilibrium in the direction that consumes heat, in order to counteract the temperature increase.
There are several factors that can affect the position of the equilibrium, including temperature, pressure, and concentration. Changes in temperature affect the equilibrium constant, as the equilibrium constant is temperature-dependent. An increase in temperature favors the endothermic reaction, while a decrease in temperature favors the exothermic reaction. Changes in pressure affect the equilibrium position in a system containing gases, as the volume of the system changes with pressure. An increase in pressure favors the side of the equilibrium with fewer moles of gas, while a decrease in pressure favors the side with more moles of gas. Changes in concentration affect the equilibrium position, as the equilibrium constant is concentration-dependent. An increase in the concentration of a reactant will shift the equilibrium towards the products, while an increase in the concentration of a product will shift the equilibrium towards the reactants.
chemical equilibrium is a dynamic state where the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations
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