At 900 K, the following reaction has 𝐾_𝑝 = 0.345: 2 SO₂(𝑔) + O₂(𝑔) ⇌ 2 SO₃(𝑔) In an equilibrium mixture the partial pressures of SO₂ and O₂ are 0.135 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO₃ in the mixture?

The equilibrium constant, Kp, is a dimensionless number that expresses the ratio of the partial pressures of products to reactants at equilibrium for a given reaction at a specific temperature. For the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g), Kp is calculated using the formula Kp = (P_SO3^2) / (P_SO2^2 * P_O2), where P represents the partial pressures of the gases involved. A Kp value less than 1 indicates that at equilibrium, the reactants are favored over the products.

Partial pressure is the pressure exerted by a single component of a gas mixture. According to Dalton's Law of Partial Pressures, the total pressure of a gas mixture is the sum of the partial pressures of each individual gas. In this context, knowing the partial pressures of SO2 and O2 allows us to calculate the partial pressure of SO3 at equilibrium using the equilibrium constant.

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. In this case, understanding how the equilibrium shifts can provide insights into the relationship between the partial pressures of the reactants and products.