a.) Calculate the partial pressure in bar of phosphorus pentachloride produced in a system in which phosphorus trichloride and chlorine gases are initially each at a partial pressure of 3.00 bar and allowed to reach equilibrium. The reaction is run at a temperature in which the equilibrium constant = 1.12. Note: This K value is for the reaction written as: PCl3(g) + Cl2(g) ----> PCl5(g)
b.) Strontium-90 is a radionuclide that is a legacy of nuclear weapons development and testing. It is particularly dangerous because it takes the place of calcium in bone marrow, and has a half life of 28.1 years. Suppose 1.20 micrograms were absorbed by a human. How many micrograms will remain after 34.0 years?
c.) The chemical decomposition of reactant species A is followed in a spectrophotometer to determine its decreasing concentration with time. The following data is taken:
time(min) [A] mmol/L --------------------------- 0 90.0 10 66.58 20 49.26 30 36.44 40 26.96 ---------------------------
Determine the order of the reaction and the rate constant. If the
reaction turns out to be first order, report its half-life in
minutes. If it turns out to be second order, report its rate
constant in L/mmol-min.
a.) Calculate the partial pressure in bar of phosphorus pentachloride produced in a system in which...
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.
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....
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 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...
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
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.
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.)
Phosphorus pentachloride, PCl5, an important reagent in organic chemistry for converting alcohols to alkyl chlorides (ROH ---> RCl), is hydrolyzed in water to form phosphoric acid and hydrogen chloride. In the gaseous state, however, PCl5 can decompose at 250oC according to the following reaction PCl5(g) <---> PCl3(g) + Cl2(g), for which K = 0.0240 If a 2500.-L vessel containing 3250. kg of PCl3(g) with a constant chlorine pressure of 3.525 atm is allowed to reach equilibrium, how many kilograms of...
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...