This reaction has an equilibrium constant of K_p = 2.2⨉10⁶ at 298 K. 2 COF₂(g) ⇌ CO₂(g) + CF₄(g) Calculate K_p for each reaction and predict whether reactants or products will be favored at equilibrium.
a. COF₂ (g) ⇌ 1/2 CO₂(g) + 1/2 CF₄(g)

Verified step by step guidance

1. Identify the relationship between the original reaction and the new reaction. The new reaction is obtained by dividing the original reaction by 2.
2. Understand that the equilibrium constant for a reaction that is multiplied or divided by a number can be calculated by raising the original equilibrium constant to the power of that number. In this case, since the reaction is divided by 2, the new K_p will be the square root of the original K_p.
3. Calculate the new K_p for the reaction COF₂ (g) ⇌ 1/2 CO₂(g) + 1/2 CF₄(g) by taking the square root of the original K_p (2.2⨉10⁶).
4. Compare the new K_p value to 1 to predict the direction of the equilibrium. If K_p > 1, the reaction favors the formation of products at equilibrium.
5. Conclude that since the new K_p is greater than 1, the reaction COF₂ (g) ⇌ 1/2 CO₂(g) + 1/2 CF₄(g) will favor the formation of products (CO₂ and CF₄) at equilibrium.

Key Concepts

Equilibrium Constant (Kp)

The equilibrium constant, Kp, quantifies the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is expressed in terms of partial pressures for gaseous reactions. A large Kp value indicates that products are favored at equilibrium, while a small Kp suggests that reactants are favored.

Reaction Stoichiometry

Reaction stoichiometry refers to the quantitative relationship between reactants and products in a chemical reaction, as represented by the balanced chemical equation. It is essential for calculating the equilibrium constant for different stoichiometric coefficients, as changing these coefficients alters the expression for Kp, affecting the equilibrium position.

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict the direction in which the reaction will shift when the concentrations of reactants or products are altered, thereby influencing the favorability of reactants or products at equilibrium.