Question

If an equilibrium is product-favored, is its equilibrium constant large or small with respect to \(1 ?\) Explain.

Short answer

The equilibrium constant is large for a product-favored equilibrium.

Step-by-step solution

Understanding Equilibrium Constant

The equilibrium constant, denoted as \( K \), is a number that expresses the ratio of the concentration of products to reactants at equilibrium. It is defined by the equation \( K = \frac{[products]}{[reactants]} \).

Definition of Product-Favored Equilibrium

An equilibrium is product-favored if, at equilibrium, the concentration of the products is significantly greater than the concentration of the reactants. This implies that the reaction tends to produce more products than reactants.

Analyzing Equilibrium Constant Value

If an equilibrium is product-favored, then the concentration of products is high, and that of reactants is low. This means the numerator in the equilibrium constant expression \( K = \frac{[products]}{[reactants]} \) is larger than the denominator, resulting in a large value of \( K \).

Relation to One

Since a product-favored reaction has a large value of \( K \), which indicates a larger concentration of products than reactants, \( K \) is much larger than \( 1 \). Therefore, the equilibrium constant is large with respect to \( 1 \) for a product-favored equilibrium.

Key concepts

Product-Favored Equilibrium

In chemical reactions, the term product-favored indicates a scenario where, at equilibrium, the concentration of products surpasses that of reactants. This means the reaction naturally tends to form more products. To visualize this, consider baking cookies. A product-favored situation would mean that after baking and cooling, you have more cookies than leftover ingredients.

The equilibrium constant, denoted as \( K \), helps us understand whether a reaction is product-favored. This constant is calculated using the ratio \( \frac{[\text{products}]}{[\text{reactants}]} \). If \( K \) is large, it suggests the products side is dominant, indicating a product-favored equilibrium.

Understanding whether an equilibrium is product- or reactant-favored is essential in predicting reaction outcomes. It helps chemists control and optimize reactions to yield the most desired products.

Reaction Products and Reactants

In a chemical reaction, reactants are substances initially present, while products are substances formed as the reaction progresses.

Consider a simple analogy with a kitchen recipe. The reactants are your raw ingredients, like flour and sugar, while the products are the final baked cookies. During the reaction, the reactants undergo changes to form the products.

In equilibrium reactions, both reactants and products are present, and their concentrations remain steady over time. The equilibrium constant \( K \) reflects their ratio at equilibrium. If a reaction heavily favors products, it means more products are produced relative to the reactants. Conversely, if a reaction favors reactants, there are fewer products relative to the initial substances.

Analyzing the roles of products and reactants is key for predicting and managing chemical processes.

Equilibrium Reactions

Equilibrium reactions are dynamic processes where the rate of the forward reaction equals the rate of the reverse reaction. As a result, the concentrations of reactants and products reach a state where they no longer change over time, although both reactions are still occurring.

This balance is not static but dynamic; it can be compared to a scenario where runners on a track keep exchanging positions but maintain an overall constant formation. At equilibrium, neither the reactants nor the products disappear completely, but their concentrations remain steady.

The equilibrium constant \( K \) quantifies this balance. A large \( K \) value means more products are present at equilibrium (product-favored), while a small \( K \) indicates more reactants (reactant-favored).

Understanding equilibrium reactions allows chemists and scientists to predict the concentration of different components in a reaction. This understanding is crucial for various applications, from industrial manufacturing to pharmaceutical development.