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The reaction PCl3(g) + Cl2(g) ? PCl5(g) has Kp = 0.0870 at
Chapter 10, Problem 88AE(choose chapter or problem)
Problem 88AE
The reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) has Kp = 0.0870 at 300 °C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2, and 0.20 atm PCl5 at this temperature. (a) Use the reaction quotient to determine the direction the reaction must proceed to reach equilibrium. (b)Calculate the equilibrium partial pressures of the gases. (c) What effect will increasing the volume of the system have on the mole fraction of Cl2 in the equilibrium mixture? (d) The reaction is exothermic. What effect will increasing the temperature of the system have on the mole fraction of Cl2 in the equilibrium mixture?
Questions & Answers
QUESTION:
Problem 88AE
The reaction PCl3(g) + Cl2(g) ⇌ PCl5(g) has Kp = 0.0870 at 300 °C. A flask is charged with 0.50 atm PCl3, 0.50 atm Cl2, and 0.20 atm PCl5 at this temperature. (a) Use the reaction quotient to determine the direction the reaction must proceed to reach equilibrium. (b)Calculate the equilibrium partial pressures of the gases. (c) What effect will increasing the volume of the system have on the mole fraction of Cl2 in the equilibrium mixture? (d) The reaction is exothermic. What effect will increasing the temperature of the system have on the mole fraction of Cl2 in the equilibrium mixture?
ANSWER:
(a) The reaction quotient can be calculated using the equation Q = [PCl5]/[PCl3][Cl2] = 0.20/ (0.50)(0.50) = 0.40. Since Q is greater than Kp, the reaction will proceed to the left to reach equilibrium.
(b) The equilibrium partial pressures of the ga