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An equilibrated system that contains products and reactants in a single phase is a homogeneous equilibrium; a system whose reactants, products, or both are in more than one phase is a heterogeneous equilibrium.
It is also possible to achieve chemical equilibrium in a reaction involving substances in more than one phase of matter. An example of such heterogeneous equilibrium is the decomposition of calcium carbonate for the production of lime, a process that involves the application of heat.
The examples of a heterogeneous equilibrium are solid Calcium carbonate on decomposition to produce CaO solid and CO 2 gas here in the phase of reactants and products are different. Similarly solid Ferrous oxide with Gaseous carbon monoxide produces solid iron and gaseous carbon dioxide.
Describe examples of systems involving two (or more) simultaneous chemical equilibria; Calculate reactant and product concentrations for multiple equilibrium systems; Compare dissolution and weak electrolyte formation
30 Ιαν 2023 · These types of changes are examples of heterogeneous equilibrium. For this type of equilibrium, the equilibrium constant is expressed by the partial pressure rather than by the ratio of pressure and concentration. For example, the dissolution of oxygen in water and the equilibrium constant are usually written in this way:
15 Αυγ 2020 · A heterogeneous reaction is one where one or more states within the reaction differ (the Greek word "heteros" means "different"). For example, the formation of an aqueous solution of lead(II) iodide creates a heterogeneous mixture dealing with molecules in both the solid and aqueous states:
In thermodynamics, a heterogeneous equilibrium is an equilibrium state that involves a phase change of the system. In such an equilibrium, the system is not in thermal equilibrium with its surroundings; that is, the system is at a temperature different from that of the surroundings.
