What are the equilibrium partial pressures of PCl3, Cl2, and PCl5, respectively?
Express your answers numerically in atmospheres with three digits after the decimal point, separated by commas.
An Equilibrium Study: Phosphorus Trichloride/Phosphorus Pentachloride Equilibrium
For the exothermic reaction
PCl3(g)+Cl2(g)→PCl5(g)
Kp = 0.180 at a certain temperature.
A flask is charged with 0.500 atm PCl3 , 0.500 atm Cl2, and 0.300atm PCl5 at this temperature.
What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5, respectively? Express your answers...
The equilibrium PCl5(g) ⇄ PCl3(g) + Cl2(g) is established at 250oC. At equilibrium the partial pressures of the components are 0.020 Atm (PCl5), 1.28 Atm (PCl3), and 1.28 Atm (Cl2). If the partial pressure of Cl2 is suddenly increased to 2.15 Atm, what is the partial pressure of PCl5 after equilibrium has been reestablished?
Consider the following reaction between phosphorus trichloride and chlorine gases to make phosphorus pentachloride gas: PCl3(g) + Cl2(g) --> PCl5(g) Kp = 24.2 at 250 Celsius If the initial partial pressures of PCl3 and Cl2 are 0.43 and o.87 atm, respectively, and no PCl5 is initially present, what is partial pressure of the Cl2 when equilibrium is achieved? Simplifying assumptions cannot be made; quadratic solution is required. A. 0.00 atm B. 2.30 atm C. 0.47 atm D. 0.03 atm E....
The equilibrium partial pressures for the reaction Cl2 (g) + PCl3 (g) ↔ PCl5 (g) at 300 K are PCl2 = 0.75 atm, PPCl3 = 0.45 atm, and PPCl5 = 0.73 atm. The value of Kp is __________. A. 0.15 B. 0.048 C. 4.7 D. 2.16
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride according to the following equilibrium: PCl3(g)+Cl2(g)⇌PCl5(g) A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K . At equilibrium, the partial pressures of the three gases are PPCl3 = 0.121 atm ,PCl2 = 0.159 atm , and PPCl5 = 1.60 atm A. What is the value of Kp at this temperature? B. Does the equilibrium favor reactants or...
The following reaction has equilibrium constant of Kp = 11.5 atm at 300 oC: PCl5(g) PCl3 (g) + Cl2 (g). A flask was charged with pure PCl5 (g) and allowed to achieve the equilibrium, at which partial pressure of PCl5 (g) was 1.50 atm. Find (a) total pressure at equilibrium (b) partial pressures of PCl3 (g) and Cl2(g), (c) initial pressure of PCl5.
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride gas:PCl3(g)+Cl2(g)→PCl5(g).A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K. At equilibrium the partial pressures of the three gases are PPCl3 = 0.123atm , PCl2 = 0.158atm , and PPCl5 = 1.20atm .Calculate Kc for this reaction at 450 K.
Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride according to the following equilibrium: PCl3(g)+Cl2(g)⇌PCl5(g) A 7.5-L gas vessel is charged with a mixture of PCl3(g) and Cl2(g), which is allowed to equilibrate at 450 K . At equilibrium, the partial pressures of the three gases are PPCl3 = 0.129 atm , PCl2 = 0.159 atm , and PPCl5 = 1.20 atm . 1. What is the value of Kp at this temperature? Express the equilibrium constant to...
The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121 at certain temperature. A vessel is charged with PCl5 giving an initial pressure of 0.123 atm. PCl5 (g) ⥦ PCl3 (g) + Cl2 (g) a) Calculate equilibrium partial pressure of PCl3 b) Calculate total pressure at equilibrium
Phosphorus pentachloride decomposes at high temperatures. PCl5(g) ⇆ PCl3(g) + Cl2(g) An equilibrium mixture at some temperature consists of 3.51 g PCl5 4.86 g PCl3 3.59 g Cl2 in a 1.00-L flask. If you add 1.31 g of Cl2, how will the equilibrium be affected? (Shift left, shift right, or no change) What is the new equilibrium of PCl5?
An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has partial pressures of 217.0 Torr, 13.2 Torr, and 13.2 Torr, respectively. A quantity of Cl2(g)is injected into the mixture, and the total pressure jumps to 263.0 Torr at the moment of mixing. The system then re-equilibrates. The chemical equation for this reaction is PCl3(g)+Cl2(g)↽−−⇀PCl5(g Calculate the new partial pressures,pP, after equilibrium is reestablished.p pcl5 , pcl2 , ppcl3.