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When a chemical reaction is at equilibrium, any disturbance of the system, such as a change in temperature, or addition or removal of one of the reaction components, will "shift" the composition to a new equilibrium state. This is the only unambiguous way of verifying that a reaction is at equilibrium.
Equilibrium chemistry is concerned with systems in chemical equilibrium. The unifying principle is that the free energy of a system at equilibrium is the minimum possible, so that the slope of the free energy with respect to the reaction coordinate is zero.
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. Writing equilibrium constant expressions. 7 questions.
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. [1]
Chemical equilibrium, condition in the course of a reversible chemical reaction in which no net change in the amounts of reactants and products occurs. A reversible chemical reaction is one in which the products, as soon as they are formed, react to produce the original reactants.
In a chemical equilibrium, the forward and reverse reactions occur at equal rates, and the concentrations of products and reactants remain constant. If we run a reaction in a closed system so that the products cannot escape, we often find the reaction does not give a 100% yield of products.
This unit explores the how and why of chemical equilibrium. Learn about reversible reactions, the equilibrium constant, Le Châtelier's principle, solubility equilibria, and more. Practice what you’ve learned and study for the AP Chemistry exam with more than 80 AP-aligned questions.
Worked example: Calculating an equilibrium constant from initial and equilibrium pressures
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.
In this lecture, we discuss the nature of chemical equilibrium and of the chemical equilibrium constant. We start to consider how external factors can “push” the equilibrium in one direction or the other.
