When this reaction comes to equilibrium, will the concentrations of the reactants or products be greater? Does the answer to this question depend on the initial concentrations of the reactants and products? A(g)+B(g) ⇌ 2 C(g) K_c = 1.4⨉10^-5

Verified step by step guidance

1. Identify the equilibrium constant expression for the reaction: \( K_c = \frac{[C]^2}{[A][B]} \).
2. Recognize that the equilibrium constant \( K_c \) is very small (\( 1.4 \times 10^{-5} \)), indicating that the reaction favors the reactants.
3. Understand that a small \( K_c \) value means that at equilibrium, the concentration of products \([C]\) will be much smaller compared to the concentrations of reactants \([A]\) and \([B]\).
4. Conclude that the concentrations of the reactants \([A]\) and \([B]\) will be greater than the concentration of the product \([C]\) at equilibrium.
5. Note that the answer does not depend on the initial concentrations of the reactants and products, as \( K_c \) is a constant at a given temperature.

Key Concepts

Chemical Equilibrium

Chemical equilibrium occurs when the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products. At this point, the system is dynamic, meaning that reactions continue to occur, but there is no net change in concentration. Understanding this concept is crucial for analyzing how concentrations shift in response to changes in conditions.

Equilibrium Constant (Kc)

The equilibrium constant (Kc) quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. A small Kc value, such as 1.4x10^-5, indicates that at equilibrium, the concentration of reactants is much greater than that of products. This value helps predict the direction of the reaction and the relative amounts of substances present at equilibrium.

Le Chatelier's Principle

Le Chatelier's Principle states that if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract that change and restore a new equilibrium. This principle is essential for understanding how initial concentrations of reactants and products can influence the final equilibrium concentrations, as shifts in equilibrium can occur based on these initial conditions.