Final answer:
An reaction mixture's composition of 0.439 doesn't suggest it being at equilibrium. For a reaction at equilibrium, the concentrations of reactants and product remain constant, and the reaction quotient (Q) equals the equilibrium constant (K). To confirm if the reaction is at equilibrium or not, we need to compare Q to K.
Step-by-step explanation:
The question relates to the concept of chemical equilibrium, which suggests that the concentrations of substancs in a reaction mixture do not change over time. This happens when the rate of the forward reaction is equal to the rate of the reverse reaction. However, the initial composition of a mixture given as a number (0.439 in this case) doesn't provide substantial information to suggest it being at equilibrium or not, as we need to compare this to the reaction's equilibrium constant (K) to determine if the mixture is at equilibrium or not.
In a given reaction, initial reactant concentrations decrease and product concentrations increase as the reaction proceeds toward equilibrium in the forward direction. This happens till we achieve a state where the concentrations of reactants and product remain constant, and the reaction quotient (Q) equals the equilibrium constant (K). If Q is lesser or greater than K initially, the reaction will accordingly move forward or in reverse till equilibrium is established. Hence, it is incorrect to state just from the mixture composition number 0.439 that the reaction is initially at equilibrium.
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