This reaction has an equilibrium constant of K_p = 2.26⨉10⁴ at 298 K. CO(g) + 2 H₂(g) ⇌ CH₃OH(g) Calculate K_p for each reaction and predict whether reactants or products will be favored at equilibrium. a. CH₃OH(g) ⇌ CO(g) + 2 H₂(g)

Verified step by step guidance

1. 1. The given reaction is CO(g) + 2 H2(g) ⇌ CH3OH(g) with Kp = 2.26⨉10^4. The reaction in part a is the reverse of the given reaction. In the reverse reaction, the equilibrium constant is the reciprocal of the original equilibrium constant. So, for the reaction CH3OH(g) ⇌ CO(g) + 2 H2(g), the equilibrium constant Kp' = 1/Kp.
2. 2. To determine whether reactants or products will be favored at equilibrium, compare the value of Kp' to 1. If Kp' > 1, the products are favored. If Kp' < 1, the reactants are favored.
3. 3. Since Kp' is the reciprocal of Kp, and Kp is greater than 1, Kp' will be less than 1.
4. 4. Therefore, for the reaction CH3OH(g) ⇌ CO(g) + 2 H2(g), the reactants will be favored at equilibrium because Kp' < 1.
5. 5. In summary, to solve problems like this, first determine the relationship between the given reaction and the reaction of interest. Then, use this relationship to find the equilibrium constant for the reaction of interest. Finally, compare the equilibrium constant to 1 to determine whether reactants or products are favored at equilibrium.

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 larger Kp value indicates that products are favored at equilibrium, while a smaller Kp suggests that reactants are favored.

Le Chatelier's Principle

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

Reaction Direction and Equilibrium

The direction of a reaction at equilibrium can be determined by comparing the equilibrium constant (Kp) of the forward and reverse reactions. If Kp for the forward reaction is greater than 1, products are favored; if less than 1, reactants are favored. In this case, calculating Kp for the reverse reaction allows us to predict the favored side at equilibrium.