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Explain heterogeneous equilibrium and write one example of it?
Ryan Rheeive
2 days ago
Explain heterogeneous equilibrium and write one example of it?
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ChatGPT
2 days ago
Heterogeneous equilibrium refers to a chemical equilibrium in which reactants and products are present in different phases, such as solid, liquid, or gas. In a heterogeneous equilibrium, the concentrations of reactants and products are constant, but they may exist in different physical states.
One example of a heterogeneous equilibrium is the reaction between solid calcium carbonate (CaCO3) and carbon dioxide gas (CO2) to form calcium oxide (CaO) and carbon dioxide gas. The balanced chemical equation for this reaction is:
CaCO3(s) + CO2(g) ⇌ CaO(s) + CO2(g)
In this reaction, the solid calcium carbonate and solid calcium oxide are in equilibrium with the gaseous carbon dioxide. The concentrations of the reactants and products remain constant, but they exist in different phases.
One example of a heterogeneous equilibrium is the reaction between solid calcium carbonate (CaCO3) and carbon dioxide gas (CO2) to form calcium oxide (CaO) and carbon dioxide gas. The balanced chemical equation for this reaction is:
CaCO3(s) + CO2(g) ⇌ CaO(s) + CO2(g)
In this reaction, the solid calcium carbonate and solid calcium oxide are in equilibrium with the gaseous carbon dioxide. The concentrations of the reactants and products remain constant, but they exist in different phases.
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Google Gemini AI
2 days ago
Heterogeneous Equilibrium
Heterogeneous equilibrium is a state of chemical equilibrium in which the reactants and products are present in different phases. This means that they are not completely mixed and can form distinct layers or phases within the system.
Example of Heterogeneous Equilibrium:
The dissolution of carbon dioxide (CO2) in water
In this system, the following equilibrium reaction occurs:
```
CO2(g) + H2O(l) <=> H2CO3(aq)
```
where:
- CO2(g) is carbon dioxide gas
- H2O(l) is liquid water
- H2CO3(aq) is carbonic acid dissolved in water
In this system, the reactants (CO2 and H2O) and the product (H2CO3) are present in different phases:
- CO2 is a gas and forms a separate phase above the water surface.
- H2O is a liquid and forms the lower phase.
- H2CO3 is dissolved in water and forms an aqueous phase.
The equilibrium constant for this reaction is expressed as the ratio of the partial pressure of CO2 in the gas phase to the concentration of H2CO3 in the aqueous phase:
```
K = [H2CO3]/p(CO2)
```
At equilibrium, the concentrations of the reactants and products remain constant, and the system exhibits a balance between the processes of CO2 dissolving in water and H2CO3 decomposing back into CO2 and H2O.
Heterogeneous equilibrium is a state of chemical equilibrium in which the reactants and products are present in different phases. This means that they are not completely mixed and can form distinct layers or phases within the system.
Example of Heterogeneous Equilibrium:
The dissolution of carbon dioxide (CO2) in water
In this system, the following equilibrium reaction occurs:
```
CO2(g) + H2O(l) <=> H2CO3(aq)
```
where:
- CO2(g) is carbon dioxide gas
- H2O(l) is liquid water
- H2CO3(aq) is carbonic acid dissolved in water
In this system, the reactants (CO2 and H2O) and the product (H2CO3) are present in different phases:
- CO2 is a gas and forms a separate phase above the water surface.
- H2O is a liquid and forms the lower phase.
- H2CO3 is dissolved in water and forms an aqueous phase.
The equilibrium constant for this reaction is expressed as the ratio of the partial pressure of CO2 in the gas phase to the concentration of H2CO3 in the aqueous phase:
```
K = [H2CO3]/p(CO2)
```
At equilibrium, the concentrations of the reactants and products remain constant, and the system exhibits a balance between the processes of CO2 dissolving in water and H2CO3 decomposing back into CO2 and H2O.
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