Explain in short homogeneous equilibrium and heterogeneous equilibrium?
Question: Explain in short homogeneous equilibrium and heterogeneous equilibrium?
In a homogeneous equilibrium, all reactants and products are in the same phase (i.e., all are either gases, liquids, or solids). The reactants and products are uniformly distributed throughout the system, and their concentrations remain constant over time, as the forward and reverse reactions proceed at the same rate. Examples of homogeneous equilibria include the dissociation of gases, such as the reaction between nitrogen dioxide and dinitrogen tetroxide.
In contrast, a heterogeneous equilibrium involves reactants and products in different phases (i.e., one or more are gases, while others are liquids or solids). The reaction occurs at the interface between the different phases, and the rate of the reaction is influenced by factors such as surface area and concentration. An example of a heterogeneous equilibrium is the reaction between solid calcium carbonate and gaseous carbon dioxide to form solid calcium oxide and gaseous water vapor.
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