Chemistry Exam > Chemistry Questions > CO2(g) + C(s) 2CO(g) is an example of ______...
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CO2(g) + C(s) ⇌ 2CO(g) is an example of _____________
- a)homogeneous equilibrium
- b)heterogeneous equilibrium
- c)neither homogeneous nor heterogeneous
- d)both homogeneous and heterogeneous
Correct answer is option 'B'. Can you explain this answer?
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CO2(g) + C(s) 2CO(g) is an example of _____________a)homogeneous equi...
In heterogeneous equilibrium, the reactants and products are present in two or more physical States or phases. Here carbon dioxide is present in the gaseous state while carbon is present in the solid state, so it is an example of heterogeneous equilibrium.
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CO2(g) + C(s) 2CO(g) is an example of _____________a)homogeneous equi...
Heterogeneous equilibrium
In a chemical reaction, the reactants and products can be either in the same phase (homogeneous) or in different phases (heterogeneous). The given reaction: CO2(g) + C(s) ⇌ 2CO(g) involves reactants and products in different phases, which makes it an example of a heterogeneous equilibrium.
Explanation:
Definition:
A heterogeneous equilibrium is a type of chemical equilibrium in which the reactants and products of a reaction are present in different phases.
Reactant and Product Phases:
In the given reaction, CO2(g) is a gas, C(s) is a solid, and 2CO(g) is also a gas. The reactants and products are present in different phases: gas and solid. Therefore, the reaction is an example of a heterogeneous equilibrium.
Visual Representation:
CO2(g) + C(s) ⇌ 2CO(g)
Interpretation:
The forward reaction involves the reactant CO2(g) and solid C(s) to produce 2CO(g) as products. The reverse reaction involves the reactant 2CO(g) to produce CO2(g) and C(s) as products.
Phase Change:
In the forward reaction, the reactant CO2(g) is a gas and the reactant C(s) is a solid. During the reaction, the solid carbon (C) combines with the gaseous carbon dioxide (CO2) to form gaseous carbon monoxide (CO). This phase change from solid to gas and gas to solid indicates a heterogeneous equilibrium.
Presence of Different Phases:
The presence of different phases (gas and solid) in the reactants and products of the reaction indicates a heterogeneous equilibrium. This means that the reaction does not occur entirely in one phase, but involves a mixture of phases.
Therefore, the given reaction CO2(g) + C(s) ⇌ 2CO(g) is an example of a heterogeneous equilibrium.
In a chemical reaction, the reactants and products can be either in the same phase (homogeneous) or in different phases (heterogeneous). The given reaction: CO2(g) + C(s) ⇌ 2CO(g) involves reactants and products in different phases, which makes it an example of a heterogeneous equilibrium.
Explanation:
Definition:
A heterogeneous equilibrium is a type of chemical equilibrium in which the reactants and products of a reaction are present in different phases.
Reactant and Product Phases:
In the given reaction, CO2(g) is a gas, C(s) is a solid, and 2CO(g) is also a gas. The reactants and products are present in different phases: gas and solid. Therefore, the reaction is an example of a heterogeneous equilibrium.
Visual Representation:
CO2(g) + C(s) ⇌ 2CO(g)
Interpretation:
The forward reaction involves the reactant CO2(g) and solid C(s) to produce 2CO(g) as products. The reverse reaction involves the reactant 2CO(g) to produce CO2(g) and C(s) as products.
Phase Change:
In the forward reaction, the reactant CO2(g) is a gas and the reactant C(s) is a solid. During the reaction, the solid carbon (C) combines with the gaseous carbon dioxide (CO2) to form gaseous carbon monoxide (CO). This phase change from solid to gas and gas to solid indicates a heterogeneous equilibrium.
Presence of Different Phases:
The presence of different phases (gas and solid) in the reactants and products of the reaction indicates a heterogeneous equilibrium. This means that the reaction does not occur entirely in one phase, but involves a mixture of phases.
Therefore, the given reaction CO2(g) + C(s) ⇌ 2CO(g) is an example of a heterogeneous equilibrium.
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CO2(g) + C(s) 2CO(g) is an example of _____________a)homogeneous equilibriumb)heterogeneous equilibriumc)neither homogeneous nor heterogeneousd)both homogeneous and heterogeneousCorrect answer is option 'B'. Can you explain this answer?
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