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Learn the definition, equation, and facts of chemical equilibrium, a condition in which a reversible reaction reaches a steady state with no net change in reactants and products. Find out how the equilibrium constant and the standard Gibbs free energy are related to the reaction.
- Equilibrium Constant
Other articles where equilibrium constant is discussed:...
- Equilibrium Constant
In a chemical reaction, chemical equilibrium is the state in which both the reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system.
Science. Chemistry archive. Unit 7: Chemical equilibrium. About this unit. This unit is part of the Chemistry library. Browse videos, articles, and exercises by topic. Equilibrium constant. Learn. The equilibrium constant K. Calculating equilibrium constant Kp using partial pressures. Practice. Factors that affect chemical equilibrium. Learn.
Learn about chemical equilibrium, a state where the forward and reverse reactions of a system occur at the same rate. Explore topics such as dynamic equilibrium, equilibrium constants, reaction quotients, Le Chatelier's principle, and Gibb's free energy.
A chemical reaction is in equilibrium when there is no tendency for the quantities of reactants and products to change. The direction in which a chemical reaction is written (and thus which components are considered reactants and which are products) is arbitrary. Consider the following two reactions:
A reaction is at equilibrium when the amounts of reactants or products no longer change. Chemical equilibrium is a dynamic process, meaning the rate of formation of products by the forward reaction is equal to the rate at which the products re-form reactants by the reverse reaction.
Chemical equilibrium is a dynamic process consisting of forward and reverse reactions that proceed at equal rates. At equilibrium, the composition of the system no longer changes with time. The composition of an equilibrium mixture is independent of the direction from which equilibrium is approached.
