Final answer:
The equilibrium constant expression for the given reaction is K = [P4]^6 [O2]^30 / [P4O10].
Step-by-step explanation:
The equilibrium constant expression for the given reaction is expressed as:
K = [P4]^6 [O2]^30 / [P4O10]
Where [P4] represents the concentration of P4, [O2] represents the concentration of O2, and [P4O10] represents the concentration of P4O10.
, equilibrium refers to a state in a chemical reaction where the rates of the forward and reverse reactions are equal, and the concentrations of reactants and products remain constant over time. At equilibrium, there is no net change in the amounts of reactants and products, even though both reactions continue to occur.
The concept of equilibrium is described by the law of mass action, which states that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants, each raised to the power of its coefficient in the balanced chemical equation.
A general chemical reaction at equilibrium can be represented as follows:
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+
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⇌
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+
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aA+bB⇌cC+dD
where
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A and
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B are reactants,
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C and
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D are products, and
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,
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,
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,
a,b,c, and
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d are coefficients representing the stoichiometry of the reaction.
Key points about equilibrium include:
Dynamic Process: Equilibrium is a dynamic process, meaning that reactions are still occurring. The forward and reverse reactions continue, but at the same rate, leading to a constant concentration of reactants and products.
Equilibrium Constant (
�
K): The equilibrium constant, often denoted as
�
K, is a ratio of the concentrations of products to reactants, each raised to the power of its coefficient. The expression for
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K depends on the specific chemical reaction.
Shifts in Equilibrium: Changes in temperature, pressure, or concentrations of reactants or products can cause the system to shift toward the formation of more products or more reactants. Le Chatelier's Principle describes how a system at equilibrium responds to changes in conditions.
Homogeneous and Heterogeneous Equilibria: In a homogeneous equilibrium, all the reactants and products are in the same phase (e.g., all gases or all aqueous solutions). In a heterogeneous equilibrium, the reactants and products are in different phases.