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
The equilibrium partial pressures for the reaction Cl2 (g) + PCl3 (g) ↔ PCl5 (g) at...
1. The equilibrium constant, Kp, for the following reaction is 0.497 at 500 K: PCl5(g) <----> PCl3(g) + Cl2(g) Calculate the equilibrium partial pressures of all species when PCl5(g) is introduced into an evacuated flask at a pressure of 1.00 atm at 500 K. PPCl5 = atm PPCl3 = atm PCl2 = atm 2. The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K: NH4I(s) <----> NH3(g) + HI(g) Calculate the equilibrium partial pressure of HI when...
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.
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.
For the reaction PCl5(g) ↔ PCl3(g) + Cl2(g) the value of K = 15.4 at 497.0 K. Calculate the equilibrium partial pressures (in bar) of all species at 497.0 K if the initial pressures were P(PCl5(g)) = 0.700 bar, P(PCl3(g)) = 0.320 bar, and P(Cl2(g)) = 0.000 bar.
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 EquilibriumFor the exothermic reactionPCl3(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.
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?
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...
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 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.
The equilibrium constant Kp for the reaction PCl5(g) <---> PCl3(g) + Cl2(g) is 1.15 at 25 degrees Celsius. The reaction starts with a mixture of 0.177 atm PCl5, 0.223 atm PCl3, and 0.111 atm Cl2. When this mixture comes to equilibrium at 25 degrees Celsius, what are the equilibrium pressures of each component?