Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute
At equilibrium.

Question

Consider the equilibrium system: N₂O₄(g) ⇌ 2 NO₂(g) for which K_p = 0.1134 at 25 °C and Δ_rH° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N₂O₄ was present inside the container,compute

Consider the equilibrium system: N<sub>2</sub>O<sub>4</sub>(g) ⇌ 2 NO<sub>2</sub>(g) for which K<sub>p</sub> = 0.1134 at 25 °C and Δ<sub>r</sub>H° = 58.03 kJ/mol.Assuming that the total pressure inside the container is 1.00 atm at equilibrium and that initially only N<sub>2</sub>O<sub>4</sub> was present inside the container,compute At equilibrium. A) 0.398 atm B) 0.113 atm C) 0.602 atm D) 0.285 atm E) 0.715 atm

At equilibrium.

Quizplus · Accepted Answer

Using the ideal gas law, we can express the equilibrium partial pressures in terms of the equilibrium mole fractions. Let x be the mole fraction of NO₂(g) at equilibrium. Then, the equilibrium mole fractions are: [NO₂(g)] = 2x [N₂O₄] = 1 - 2x Using the equilibrium constant expression: K_p = [NO₂(g)]^2/[N₂O₄] = (2x)^2/(1-2x) At equilibrium, the partial pressure of NO₂(g) is 2xPtotal, where Ptotal = 1.00 atm. Similarly, the partial pressure of N₂O₄(g) is (1-2x)Ptotal. Using the ideal gas law, we can convert partial pressures to concentrations: [NO₂(g)] = 2xPtotal/RT [N₂O₄] = (1-2x)Ptotal/RT Substituting into the equilibrium constant expression and solving for x: 0.1134 = (2xPtotal/RT)^2/[(1-2x)Ptotal/RT] 0.1134 = 4x^2/(1-2x) 0.1134 - 0.1134x + 4x^2 = 0 (2x - 0.285)(1-14x) = 0 The positive root, x = 0.142, corresponds to the mole fraction of NO₂(g) at equilibrium. Therefore, the partial pressures at equilibrium are: [NO₂(g)] = 2xPtotal = 0.285 atm [N₂O₄] = (1-2x)Ptotal = 0.715 atm Thus, the answer is D) 0.285 atm.

Consider the Equilibrium System: N2O4(g)⇌ 2 NO2(g)for Which Kp =

Consider the Equilibrium System: N₂O₄(g)⇌ 2 NO₂(g)for Which K_p =