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. 0.40 atm
Consider the following reaction between phosphorus trichloride and chlorine gases to make phosphorus pentachloride gas: PCl3(g)...
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...
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 pentachloride is formed when phosphorus trichloride and chlorine react. PCl3(g) + Cl2(g) ⇌ PCl5(g) The equilibrium constant for the reaction is KC = 38.0 at 233 °C. If 0.510 mol of phosphorus trichloride is added to 0.238 mol of chlorine in a 1.11-L reaction vessel at this temperature, what is the equilibrium concentration (in mol/L) of phosphorus pentachloride? Report your answer to THREE significant figures.
Revie Phosphorus trichloride gas and chlorine gas react to form phosphorus pentachloride according to the following equilibrium: What is the value of Kp at this temperature? Express the equlibrlum constant to three significant figures. PCl3 (9) +Cla (9) PCls (g) A7.5-Lgas vessel is charged with a mixture of PCls(9) equilibrate at 450K. At equilibrium, the partial pressures of the three gases are Ppci, 0.124 atm, Pa, 0.159 atm, and PpcCls 1.40 atm and Cl2 (g), which is allowed to VAXD...
Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: PCl5(g) ⇌ PCl3(g) + Cl2(g) At 250° 0.250 M PCl 5 is added to the flask. If K c = 1.80, what are the equilibrium concentrations of each gas? [PCl5] = 2.27 M, [PCl3] = 2.02 M, and [Cl2] = 2.02 M [PCl5] = 1.80 M, [PCl3] = 1.80 M, and [Cl2] = 1.80 M [PCl5] = 0.0280 M, [PCl3] = 0.222 M, and [Cl2] = 0.222 M...
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.
Consider the reversible reaction. PCl5↽−−⇀PCl3+Cl2PCl5↽−−⇀PCl3+Cl2 Are the concentrations of phosphorus pentachloride, PCl5,PCl5, and phosphosphorus trichloride, PCl3,PCl3, constant or changing at equilibrium? The concentration of PCl5PCl5 is constant, and the concentration of PCl3PCl3 is changing at equilibrium. The concentration of PCl5PCl5 is changing, and the concentration of PCl3PCl3 is constant at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are constant at equilibrium. The concentrations of both PCl5PCl5 and PCl3PCl3 are changing at equilibrium. which one is correct please explain
phsophorous trichloride and phosphorous pentachloride equilibrate in the presence of molecular chlorine according to PCl3 (g) +Cl2 (g)->PCl5 (g) Kc = 2.01 at 500k If a 1.000L reaction vessel is charged with .300 mol of PCl5(g) and allowed to equilibrate at this temperature, what would be the partical pressure of PCl5(g) please help need this to study for a test tomorrow. I know I have to use the ice table in there somewhere but that is about it.
Phosphorus pentachloride can dissociate into phosphorus trichloride and chlorine: PCs (8) PC13(8) + Cl2(8) At 250.°C, the equilibrium constant for this dissociation reaction is 2.15. (a) If 12.00 g of phosphorus pentachloride is placed in a 11.90-L vessel and heated to 250°C, what is the partial pressure of phosphorus trichloride when equilibrium is attained? (Enter your answer to 3 significant figures.) atm (b) What fraction of phosphorus pentachloride is dissociated at equilibrium? (Enter your answer to 3 significant figures.)