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.
c. 2 CO₂(g) + 2 CF₄(g) ⇌ 4 COF₂(g)

Verified step by step guidance

1. Identify the relationship between the given reaction and the reaction in part c. The reaction in part c is the reverse of the given reaction and also doubled.
2. Recall that the equilibrium constant for the reverse reaction is the inverse of the equilibrium constant for the forward reaction. Therefore, calculate the inverse of K_p for the given reaction.
3. Since the reaction in part c is also doubled, raise the inverse of K_p to the power of 2 to account for the stoichiometry change.
4. Compare the magnitude of the new K_p value to 1. If K_p is greater than 1, the products are favored at equilibrium; if K_p is less than 1, the reactants are favored.
5. Predict whether reactants or products will be favored at equilibrium based on the calculated K_p value for the reaction in part c.

Key Concepts

Equilibrium Constant (Kp)

The equilibrium constant (Kp) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium for a given reaction at a specific temperature. It is calculated using the partial pressures of gases involved in the reaction. A large Kp value (greater than 1) indicates that products are favored at equilibrium, while a small Kp value (less than 1) suggests that reactants are favored.

Reaction Quotient (Q)

The reaction quotient (Q) is a measure of the relative amounts of products and reactants at any point in a reaction, not just at equilibrium. It is calculated in the same way as Kp but uses the current concentrations or partial pressures. By comparing Q to Kp, one can predict the direction in which the reaction will proceed to reach equilibrium: if Q < Kp, the reaction will shift to the right (toward products), and if Q > Kp, it will shift to the left (toward reactants).

Le Chatelier's Principle

Le Chatelier's Principle states that if a dynamic equilibrium is disturbed by changing the conditions (such as concentration, pressure, or temperature), the system will adjust to counteract the change and restore a new equilibrium. This principle helps predict how a change in concentration of reactants or products will affect the position of equilibrium, guiding the understanding of whether reactants or products will be favored in a given reaction.