When are more products of a reaction available initially than at equilibrium?
A. K = 0
B. Q < K
C. Q = K
D. Q > K
To determine when there are initially more products available than at equilibrium in a chemical reaction, we need to consider the reaction quotient, Q, and the equilibrium constant, K.
Q is a measure of the relative concentrations of reactants and products at any given point during the reaction. It is calculated by substituting the current concentrations of reactants and products into the equilibrium expression of the reaction.
K, on the other hand, is the equilibrium constant and represents the concentrations of reactants and products at equilibrium. It is determined at a specific temperature and remains constant under those conditions.
Now, let's consider the options and see which one indicates that more products are available initially than at equilibrium:
A. K = 0: If K is equal to zero, it means that the reaction does not proceed in the forward direction to produce products. It implies that there are no products available initially or at equilibrium. Therefore, this option does not indicate more products initially than at equilibrium.
B. Q < K: This option indicates that the reaction has fewer products initially than at equilibrium. Q is smaller than K, which suggests that the reaction has not yet reached the equilibrium concentration of products. Thus, this option is not the correct answer.
C. Q = K: If Q is equal to K, it means that the reaction is already at equilibrium. In this case, the concentrations of reactants and products do not change, and there are no more products available initially than at equilibrium. So, this option does not describe the scenario we are looking for.
D. Q > K: This option indicates that the reaction has more products available initially than at equilibrium. Q being greater than K means that the reaction has shifted towards the products, resulting in higher product concentrations than at equilibrium. Therefore, the correct answer is D. Q > K.
In conclusion, when the reaction quotient, Q, is greater than the equilibrium constant, K (D. Q > K), there are more products available initially than at equilibrium.