Final answer:
To calculate the value of Kp for the equilibrium 2 SO₃(g) ↔ 2 SO₂(g) + O₂(g), use the equation Kp = Kc(RT)^(Δn), where Kp is the equilibrium constant in terms of partial pressures, Kc is the equilibrium constant in terms of concentrations, R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas involved in the reaction. Plugging in the given values, we find that Kp = 0.336.
Step-by-step explanation:
To calculate the value of Kp for the equilibrium 2 SO₃(g) ↔ 2 SO₂(g) + O₂(g), we need to use the equation Kp = Kc(RT)^(Δn), where Kp is the equilibrium constant in terms of partial pressures, Kc is the equilibrium constant in terms of concentrations, R is the ideal gas constant, T is the temperature in Kelvin, and Δn is the change in the number of moles of gas involved in the reaction.
In this case, Δn = (2 + 1) - (2) = 1. Substituting the values into the equation, we get Kp = Kc(RT)^1. Plugging in the values Kc = 4.08 x 10⁻³ and T = 1000 K, we can calculate Kp by multiplying Kc by (RT): Kp = 4.08 x 10⁻³ x (0.08206 L atm/mol · K)(1000 K) = 0.336.