1. Chemistry - Answer Check

    The two common chlorides of Phosphorus, PCl3 and PCl5, both important in the production of other phosphorous compounds, coexist in equilibrium as shown in the balanced chemical reaction below: PCl3 (g) + Cl2 (g) PCl5 (g) At 250 C, an equilibrium mixture in

    asked by Anonymous on May 18, 2016
  2. chem

    PCL5=PCl3+Cl2 a. Initially 0.72 mole PCl5 are placed in 1.50 L flask. At equilibrium, there is 0.16 mole PCl3 in the flask. What is the equilibrium concentration of the PCl5? b. What is the equilibrium concentration of the Cl2? c.What is the equilibrium

    asked by chemdummy79 on November 19, 2012
  3. chem sorry the last one did not have the question

    A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes according to the equation:

    asked by laura on December 6, 2011
  4. chem

    A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes according to the equation:

    asked by laura on December 6, 2011
  5. chemistry

    how would you begin this question? An empty 15.0 L cylinder, .500 moles of gaseous PCl5 are added and allowed to reach equilibrium. The concentration of PCl3 is found to be .0220M. (Temp at 375K) PCl3(g) + Cl2(g) --> PCl5(g) i need to fine how many moles

    asked by Anonymous on April 29, 2007
  6. Chemistry

    The equilibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5 (g) ↔ PCl3 (g) + Cl2 (g) A vessel is charged with PCl5, giving an initial pressure of 0.123 atm. At equilibrium, the partial pressure of PCl3 is __________ atm. I have

    asked by Zack on April 20, 2018
  7. Chem II

    PCl5 dissociates according to the reaction: PCl5(g) ↔ PCl3(g) + Cl2(g). One mole of PCl5 was placed in one liter of solution. When equilibrium was established, 0.5 mole of PCl5 remained in the mixture. What is the equilibrium constant for this reaction?

    asked by Sam on March 1, 2012
  8. Chemistry

    When a sample of PCl5(g) (0.02087 mol/L) is placed in 83.00 L reaction vessel at 491.0 °C and allowed to come to equilibrium the mixture contains 103.0 grams of PCl3(g). What is the equilibrium concentration (mol/L) of Cl2(g)? PCl5(g) = PCl3(g)+Cl2(g)

    asked by Drew on April 15, 2010
  9. Chem 2

    Phosphorus pentachloride decomposes according to the chemical equation PCl5PCl3 +Cl2 A 0.260 mol sample of PCl5(g) is injected into an empty 2.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium. Please

    asked by Anonymous!! on March 31, 2014
  10. Chemistry

    Phosphorus pentachloride decomposes according to the chemical equation: PCl5(g) PCl3(g)+Cl2(g) Kc = 1.80 at 250 degrees Celsius A 0.352 mol sample of PCl5(g) is injected into an empty 4.45 L reaction vessel held at 250 °C. Calculate the concentrations of

    asked by Laura on March 9, 2013
  11. chemistry

    For the exothermic reaction PCl3(g)+Cl2(g)⇌PCl5(g) K = 0.160 at a certain temperature. A flask is charged with 0.507 bar PCl3 , 0.507 bar Cl2, and 0.304 bar PCl5 at this temperature. What are the equilibrium partial pressures of PCl3 , Cl2, and PCl5,

    asked by Miranda on February 6, 2018
  12. CHEMISTRY

    Equilibrium Equation with Partial Pressures PCl3(g) +Cl2(g) PCl5(g)? 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

    asked by Kylie on March 9, 2012
  13. Chemistry

    Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) PCl3(g)+Cl2(g) Kc=1.80 at 250 degrees Celsius A 0.222 mol sample of PCl5(g) is injected into an empty 3.25 L reaction vessel held at 250 °C. Calculate the concentrations of

    asked by J on March 3, 2013
  14. Chemistry

    PCl5 --> PCl3 + Cl2 A 0.318 mol sample of PCl5(g) is injected into an empty 4.15 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.

    asked by Jordyn on April 22, 2014
  15. Chem II

    The equilibrium constant, Kp for the reaction PCl5 PCl3 + Cl2 is 1.05 at 250 degrees C. The reaction is started with PCl5, PCL3 and Cl2 at 0.177, 0.223, and 0.111 atm at 250 degrees C. When the reaction comes to equilibrium, the pressure of _________ PCl3

    asked by Ken on June 17, 2008
  16. CHEM

    A 0.229 mol sample of PCL5 is injected into an empty 3.20 L reaction vessel held at 250 degrees celsius. Calculate the concentration of PCl5 and PCl3 at equilibrium. Kc=1.80 M PCl5 -------> PCl3 + Cl2

    asked by Mer on February 11, 2014
  17. Chemistry

    Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) ⇌ PCl3(g) + Cl2(g) A 0.304 mol sample of PCl5(g) is injected into an empty 4.75 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at

    asked by Dee on April 2, 2013
  18. chemistry

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium. PCl5(g)PCl3(g)+Cl2(g)

    asked by elona on April 20, 2011
  19. HELP!!!!!!!!!

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium. PCl5(g)PCl3(g)+Cl2(g)

    asked by elona on April 20, 2011
  20. Chmistry

    pcl3(g) cl2(g) ¨

    asked by Marie on April 17, 2015
  21. chem

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium. PCl5(g)PCl3(g)+Cl2(g) Can you

    asked by elona on April 19, 2011
  22. Chemistry

    PCl3 (s) + Cl2 (g) -> PCl5 (s) 1. WHAT VOLUME OF Cl2 would react with 1.4g of PCl3 to make PCl5? 2. IF YOU WANTED to make 10g of PCl5, what volume of Cl2 would you need? 3. WHAT IS THE MAXIMUM MASS of PCl5 that could be made from 360cm3 of cl2? I am very

    asked by 0oooooooo0 on September 27, 2017
  23. chm152

    PCl3 + Cl2 = PCl5 Kc=26 @ 250 degree Celcius 1.0 mol of PCl3 , 1.0 mol of Cl2 , and 5.0 mol of PCl5 are placed in a 10.0L flask at 250 C and allowed to come to equilibrium. What is the concentration, in M,of cl2 of at equilibrium? Choose one answer. a. 3.4

    asked by ami on March 27, 2010
  24. chemistry

    Please help me with this question For the system, PCl5 (g) --> PCl3 (g) + Cl2 (g) K= 26 @ 3000C In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: PCl5 = 0.012 atm PCl3 = 0.90 atm Cl2 = 0.45 atm Is the

    asked by Jack on March 9, 2008
  25. Chemistry

    Please help me with this question For the system, PCl5 (g) --> PCl3 (g) + Cl2 (g) In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: PCl5 = 0.012 atm PCl3 = 0.90 atm Cl2 = 0.45 atm Is the system at

    asked by Jack on March 9, 2008
  26. CHM 152

    Consider the following equilibrium: PCl3 + Cl2 = PCl5 Kc=26 @ 250 degree Celcius 1.0 mol of PCl3 , 1.0 mol of Cl2 , and 5.0 mol of PCl5 are placed in a 10.0L flask at 250 C and allowed to come to equilibrium. What is the concentration, in M, of at

    asked by AMI on March 26, 2010
  27. Chemistry

    An equilibrium mixture of PCl5(g), PCl3(g), and Cl2(g) has a partial pressure 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. The appropriate chemical

    asked by Kat on March 6, 2012
  28. chemistry

    Introduced into a 1.50L container is 0.100mol PCl5(g). The flask is held at 227degreesC until equilibrium is established. What are the partial pressures and the total pressures of the gases in the flask at the equilibrium. PCl5(g)PCl3(g)+Cl2(g) I got a

    asked by elona on April 20, 2011
  29. Chemistry

    Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.206 mol sample of PCl5(g) is injected into an empty 3.30 L reaction vessel held at 250 °C. Calculate the concentrations of

    asked by Katherine on September 30, 2013
  30. chemistry

    A reaction starts with 1.00 mol each of PCl3 and Cl2 in a 1.00-L flask. When equilibrium is established at 250 degree Celsius in the reaction PCl3(g)+ Cl2(g)--> PCl5(g), the amount of PCl5 present is 0.82 mol. What is Kc for this reaction?

    asked by Shanice on October 26, 2010
  31. chemistry equilibriums

    At a certain temperature, 2.00 moles of phosphorus(V) chloride, PCl5, was placed in a 1.0 L vessel and permitted to react as shown: PCl5 (g) PCl3 (g) + Cl2(g) At equilibrium, the container held 0.40 PCl5. What is the numerical value of Kc for the system as

    asked by chem on December 29, 2010
  32. chemistry

    Please help me with this question For the system, (the previous post i forgot to post the Kp) PCl5 (g) --> PCl3 (g) + Cl2 (g) In a 5.0 L flask, the gaseous mixture consists of all three gasses with partial pressures as follows: PCl5 = 0.012 atm PCl3 = 0.90

    asked by Jack on March 9, 2008
  33. chemistry

    Phosphorus pentachloride decomposes according to the chemical equation PCl5(g) -----> PCl3 (g)+ Cl2(g) Kc= 1.80 at 250 degrees C A 0.463 mol sample of PCl5(g) is injected into an empty 4.80 L reaction vessel held at 250 °C. Calculate the concentrations of

    asked by Sarah on March 10, 2012
  34. Chemistry

    1.5 mole of PCl5 are heated at constant temperature in a closed vessel of 4 litres capacity.At the equilibrium,PCl5 is 35percent dissociated into PCl3 and Cl2.calculate the equilibrium constant.

    asked by Chador on June 11, 2017
  35. cemestry

    a sample of pcl5 weighing 2.69 placed in 1.0 l flask and completely vaporized at a tem of 250 c the pressur at this tempreture was 1.0 atm if pcl5 dissociated are partual pressur of pcl5 pcl3 and cl2 at condition

    asked by biran on August 8, 2018
  36. cemestry

    a sample of pcl5 weighing 2.69 placed in 1.0 l flask and completely vaporized at a tem of 250 c the pressur at this tempreture was 1.0 atm if pcl5 dissociated are partual pressur of pcl5 pcl3 and cl2 at condition

    asked by biran on August 8, 2018
  37. Chem/math question - from Sam

    For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5. PCl5(g) = PCl3(g) + Cl2(g) Suppose that 2.510 g of PCl5 is placed in an evacuated 470. mL bulb, which is then heated to 600. K. (a) What would be the pressure of PCl5 if it did

    asked by Writeacher on January 16, 2009
  38. Chemistry

    a 1.00-mol sample of phosphorus pentachloride placed in 10.0-L reaction flask and allowed to come to equilibrium at 250 degrees celsius; PCL5(g) = PCL3(g) Cl2(g) if the amount of chlorine in the equilibrium mixture is0.470 mol, calculate (a) the

    asked by MIndy on October 19, 2011
  39. mosab bin omair

    We examine the following reaction at 250C: PCl5(g) ⇌ PCl3(g) + Cl2(g). At equilibrium we find [PCl5] = 3.4 x 10-5 M, [PCl3] = 1.3 x 10-2 M, and [Cl2] = 1.0 x 10-4 M. Calculate the

    asked by yazan on January 9, 2017
  40. chem

    A sample of PCl5 weighing 2.69 grams is placed in a 1.000 liter flask and vaporized completely at 250 o C. The final pressure observed at this temperature is 1.000 atmospheres. Note that some, but not all of the PCl5 decomposes according to the equation:

    asked by laura on December 6, 2011
  41. ap chemistry

    a 0.76 mol sample of pcl5 is placed in a 500 ml reaction vessel. what is the concentration of pcl5 when the reaction pcl5(g) ⇀↽ pcl3(g) + cl2(g) has reached equilibrium at 250◦c (when kc = 1.8)

    asked by amanda on February 1, 2014
  42. Chemistry

    At a certain temperature, .5 mol of PCl5 was placed in a .25 L vessel and permitted to react as shown PCl5 (g) --> PCl3 (g)+ Cl2 (g) At equilibrium, the container held .1 mol of PCl5. What is the value of "K"?

    asked by Alex on August 20, 2012
  43. Chemistry

    At 25C, an equilibrium mixture of gases con- tains 0.00680 mol/L PCl3, 0.0290 mol/L Cl2, and 0.00500 mol/L PCl5. PCl5(g) ⇀ ↽ PCl3(g) + Cl2(g) What is the equilibrium constant for the reaction? How would I do this? I'm so confused!

    asked by Sara on April 27, 2014
  44. Chemistry

    The initial concentration for the compounds involved in the reaction displayed were determined to be [PCl5(g)] = 0.4107 mol/L, [PCl3(g)] = 0.3463 mol/L, [Cl2(g)] = 0.04085 mol/L. Calculate the value of the equilibrium constant (Kc) at 191.0 °C if the

    asked by marmar on September 30, 2013
  45. CHEMISTRY

    The initial concentration of PCl5 was 0.1983 M. It was allowed to decompose at some temperature until equilibrium had been attained (see reaction below). What must be the equilibrium concentration of PCl3? PCl5(g) ↔ PCl3(g) + Cl2(g) Kc = 0.0580 a. 0.1162

    asked by Chemistry on April 6, 2014
  46. Chemistry

    You wish to know the enthalpy change for the formation of liquid PCl3 from the elements shown below. P4(s) + 6 Cl2(g)--> 4 PCl3(l) ΔH°f = ? The enthalpy change for the formation of PCl5 from the elements can be determined experimentally, as can the

    asked by Kat on May 2, 2011
  47. Chemistry

    I am unsure of how to approach this question, any help would be greatly appreciated! "2.085g of PCl5 were heated to 250°C in a 500mL vessel: PCl5 (g) ⇌ PCl3 (g) + Cl2 (g) Calculate the initial concentration of PCl5. At equilibrium the concentration of

    asked by ChemGeek on May 27, 2012
  48. chem

    For the reaction: PCl3(g) + Cl2(g) --> PCl5(g) at 85 degreeC, Kp = 1.19 If one starts with 2.00 atm pressure of PCl3, 1.00 atm pressure of Cl2 and no PCl5, what is the partial pressure of PCl5(g) at equilibrium?

    asked by jack on March 12, 2008
  49. Chemistry

    If 0.500 mol each of phosphorus trichloride and chlorine are injected into a 1.00-L container at 60oC, find the equilibrium concentrations of all three species in the equilibrium mixture. PCl5(g) PCl3(g) + Cl2(g) K - 12.5 at 60oC This is my ICE Table...

    asked by Anonymous on January 5, 2018
  50. Chemistry-

    PCl5 (g) PCl3 (g) +Cl2 what is the property that might be observed in order to determine when equlibrium has been reached? The question is a little vague. Is the property visual or some other property? I don't think vision (color) will work for PCl5 is a

    asked by Mike on May 2, 2007
  51. Chemistry: Equilibrium

    So, I think I'm doing everything right and even checking my math, but it keeps showing up as wrong. If someone can help me and go into detail,including the quadratic formula, I would appreciate it: Phosphorus pentachloride decomposes according to the

    asked by Jessica on October 14, 2015
  52. chemistry

    For the reaction below, Kp= 28.63 at 800 K. Calculate the equilibrium partial pressures of the reactants and products if the initial pressures are PpCl5=0.5600 atm and PpCl3= 0.4700 atm PCl5(g) PCl3(g) + Cl2(g) PCl5=?? PCl3=?? Cl2=??

    asked by brun on November 5, 2012
  53. Chemistry

    For the following reaction at 600. K, the equilibrium constant, Kp is 11.5. PCl5(g) PCl3(g) + Cl2(g) Suppose that 3.314 g of PCl5 is placed in an evacuated 460. mL bulb, which is then heated to 600. K. (a) What would be the pressure of PCl5 be if it did

    asked by Anonymous on March 9, 2010
  54. chemistry

    Given the equilibrium system PCL5(g) PCl3(g) + Cl2(g) K = 12.5 at 60 degrees celsius. A 1.0 L reaction vessel is analyzed and found to contain 3.2 mol Cl2(g), 1.5 mol PCl3(g) and 2.0 mol PCl5(g). Show that the reaction mixture has not yet reached

    asked by ChemMaster98 on March 31, 2008
  55. chemistry

    Given the equilibrium system PCl5(g) PCl3(g) + Cl2(g) K = 12.5 at 60 degrees Celsius. A 1.0-L reaction vessel is analyzed and found to contain 3.2 mol Cl2(g), 1.5 mol PCL3(g) and 3.0 mol PCl5(g). Show that the reaction mixture has not yet reached

    asked by Walter on April 9, 2008
  56. Chemistry

    If the equilibrium concentrations are [PCl5] = 1.0M, [Cl2] = 0.10M, what is the equilibrium constant value? PCl5(g) PCl3(g) + Cl2(g) Would you mind showing the calculations Please. I've been working on this problem over an hour now. Not certain if I am

    asked by Cathy on January 20, 2013
  57. chemistry

    What is the percent yield for the reaction PCl3(g) + Cl2(g) --> PCl5(g) if 119.3 g of PCl5 are formed when 61.3 g of Cl2 react with excess PCl3? I don't understand how to set this up?

    asked by dan on July 14, 2011
  58. Chemistry

    Initially, 1.68 mol of PCl5(g) and 0.36 mol of PCl3(g) are in mixed in a 2.00 l container. It is later found that 1.44 mol of PCl5 are present when the system has reached equillibrium. Calculate the value of the equllibrium. This is what I did: Equation:

    asked by Lena on July 19, 2009
  59. Chemistry

    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 1.46 atm at 500 K. PPCl5 =

    asked by Kayla23 on March 22, 2015
  60. AP CHEMISTRY

    The equilibrium constant for the reaction PCl3(g) + Cl2(g) ⇀↽ PCl5(g) is 35000 at 760 ◦C. At equilibrium, the partial pressure of PCl5 was 150 bar and that of PCl3 was 8.12 bar. Calculate the equilibrium partial pressure of Cl2. Answer in units of

    asked by Lou on February 9, 2016
  61. college chemistry

    For the following reaction: PCl5(g) PCl3(g) + Cl2(g) Kc=.058 If the initial concentration of PCl5(g) is .160M, calculate the equilibrium concentrations of all the components. (use quadratic)

    asked by Jerrett on March 24, 2010
  62. Chemistry

    The equilibrium constant, K, for the following reaction is 1.54×10-2 at 506 K: PCl5(g) PCl3(g) + Cl2(g) An equilibrium mixture of the three gases in a 15.7 L container at 506 K contains 0.207 M PCl5, 5.64×10-2 M PCl3 and 5.64×10-2 M Cl2. What will be

    asked by Daniel on November 26, 2016
  63. equilibrium constant (Kp)

    What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) -->

    asked by k on July 20, 2011
  64. chemistry

    What is the equilibrium constant "Kp" at 200 C for the reaction below: P4(s) + 6 Cl2(g) -->

    asked by l on July 20, 2011
  65. Chemistry

    A concentration of PCL5(g),4,0 mol/L, verifies that the process PCl5(g) = PCl3(g) + Cl2(g) is achieved with a degree of balance of 20% Calculate the equilibrium of the reaction constant

    asked by Kelly on January 20, 2016
  66. Chemistry

    A concentration of PCl5(g), 4,0 mol/L, it appears that the proceeding PCl5(g) => PCl3(g) + Cl2(g) is achieved with a degree of balance of 20%. In these conditions, calculate the value of chemical equilibrium

    asked by Matt on January 20, 2016
  67. AP chem

    The equilibrium constant for the reaction PCl3(g) + Cl2(g) ⇀↽ PCl5(g) is 35000 at 760 ◦C. At equilibrium, the partial pressure of PCl5 was 160 bar and that of PCl3 was 9.85 bar. Calculate the equilibrium partial pressure of Cl2. Answer in units of

    asked by martha on November 28, 2018
  68. AP Chemistry

    The equilibrium constant for the reaction PCl3(g) + Cl2(g) PCl5(g) is 35000 at 760◦C. At equilibrium, the partial pressure of PCl5 was 110 bar and that of PCl3 was 9.98 bar. Calculate the equilibrium partial pressure of Cl2. Answer in units of bar

    asked by Gabriella on November 27, 2013
  69. General Chemistry II

    The equillibrium constant (Kp) for the interconversion of PCl5 and PCl3 is 0.0121: PCl5(g) --> PCl3(g) + Cl2(g) A vessel is charged with PCl5, giving a initial pressure of 0.123 atm. At equillibrium, the partial pressure of PCl3 is _____ atm.

    asked by Rosi on January 28, 2012
  70. college chem

    In the reaction PCl5(g) ---> PCl3(g) + Cl2 (g) 0.200 mol of PCl5 is introduced into a 2.00 liter vessel. At equilibrium, the concentration of Cl2 is found to be 0.0500 molar. Find Kc for the reaction.

    asked by josh on March 8, 2010
  71. CHM 152

    Consider the following equilibrium: PCl5 = PCl3+ Cl2 5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of are present at equilibrium.

    asked by AMI on March 26, 2010
  72. AP Chemistry

    2 Questions (Multi-choice and T/F, though not sure if they're right, and these 2 questions have no correspondence to each other) 1.) a.) Consider the following system at equilibrium where Kc = 1.20E-2 and H° = 87.9 kJ/mol at 500 K. PCl5 (g) PCl3 (g) + Cl2

    asked by Ian on February 13, 2015
  73. Chemistry

    Consider the reaction: PCl3(g) + Cl2(g) PCl5(g). If [PCl3] = 0.78 M, [Cl2] = 0.44 M, and [PCl5] = 0.88 at equilibrium, what is the value of K? A.0.39 B.1.4 C.2.6 D.0.72 Thanks!

    asked by Hannah on March 22, 2012
  74. Chemistry

    A sample of gaseous PCl5 was introduced into an evacuated flask so that the pressure of pure PCl5 would be 0.54 atm at 425 K. However, PCl5 decomposes to gaseous PCl3 and Cl2, and the actual pressure in the flask was found to be 0.85 atm. Calculate Kp for

    asked by Margaret on February 14, 2013
  75. Chemistry

    PCl5 --> PCl3 + Cl2 (Kp = 630 at 546 K) A system is prepared by placing equimolar amounts of the three gases shown in the equation above in a suitable rigid container held at constant volume. Equilibrium is established at 546 K. (A) When equilibrium is

    asked by Molly on April 25, 2011
  76. chemistry

    In the gaseous phase PCl5 dissociates according to the following equilibrium: PCl5⇌PCl3+Cl2 and Kc=0.8 at 613K .Determine the equilibrium composition when 0.12 moles/L of the three compounds are mixed at 613K.

    asked by Anonymous on July 10, 2016
  77. chem

    Given these two reactions, how do I calculate ΔH for the third one? P4(s) + 6 Cl2(g) -> 4 PCl3(g) ΔH= -1148 kJ P4(s) + 10 Cl2(g) -> 4 PCl5(g) ΔH = -1500 kJ PCl3(g) + Cl2(g) -> PCl5(g) ΔH = ?

    asked by adrian on November 19, 2014
  78. chemistry calculations

    At some temperature,the reaction PCl3(g) +Cl2(g) ====PCl5(g) is at equilibrium when the concentration of PCl3, Cl2, and PCl5 are 10, 9.0, and 12mol/L, respectively. Calculate the value of Kc for this reaction at that temperature.

    asked by =) on August 31, 2014
  79. chemistry calculations

    At some temperature, the reaction PCl3(g)+Cl2(g)====PCl5(g) is at equilibrium when the concentration of PCl3, Cl2, and PCl5 are 10, 9.0, and 12 mol/L, respectively. Calculate the value of Kc for this reaction at that temperature.

    asked by =) on August 19, 2014
  80. Chemistry

    PCl5 is introduced into an evacuated chamber and comes to equilibrium (see Problem 16.37), at 250◦C and 2.00 atm. The equilibrium gas contains 40.7% Cl2 by volume. (a1) What are the partial pressures of the gaseous components at equilibrium? (a2) From

    asked by Joe johnson on June 24, 2015
  81. Chemistry

    Consider the following equilibrium: PCl3 (g) + Cl2 (g) yields PCl5 (g) delta H= -92KJ The concentration of PCl3 at equilibrium may be increased by: decreasing the temp (think this is it) adding Cl2 to the system the addition of neon the additio of PCl4

    asked by Robby on February 10, 2013
  82. Chemistry

    You are given the following data. P4(s) + 6 Cl2(g) 4 PCl3(g) ΔH = -1225.6 kJ P4(s) + 5 O2(g) P4O10(s) ΔH = -2967.3 kJ PCl3(g) + Cl2(g) PCl5(g) ΔH = -84.2 kJ PCl3(g) + 1/2 O2(g) Cl3PO(g) ΔH = -285.7 kJ Calculate ΔH for the following reaction. P4O10(s)

    asked by Britni on February 15, 2010
  83. chem

    You are given the following data. P4(s) + 6 Cl2(g) 4 PCl3(g) H = -1225.6 kJ P4(s) + 5 O2(g) P4O10(s) H = -2967.3 kJ PCl3(g) + Cl2(g) PCl5(g) H = -84.2 kJ PCl3(g) + 1/2 O2(g) Cl3PO(g) H = -285.7 kJ Calculate H for the following reaction. P4O10(s) + 6

    asked by mel on December 1, 2007
  84. chemistry equilibrium

    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

    asked by james on October 2, 2015
  85. Chemistry

    How many kilojoules are absorbed when 266 g of PCl5 reacts? PCl5(g)→PCl3(g)+Cl2(g)ΔH=+67kJ

    asked by Cara on April 6, 2016
  86. chemistry

    The percentage yield for the reaction PCL3+Cl2-->PCL5 is 83.2%. What mass of PCL5 is expected from the reaction of 73.7g of PCL3 with excess chlorine?

    asked by Brennan on January 13, 2015
  87. chemistry

    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

    asked by james on October 2, 2015
  88. chemistry

    A 0.239 mol sample of PCl5(g) is injected into an empty 2.85 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.

    asked by layla on May 3, 2015
  89. chemistry

    Given the equilibrium system PCL55(g) PCL3(g) + Cl2(g) k = 12.5 at 60 degrees Celsius. A 1.0-L reaction vessel is analyzed and found to contain 3.2 mol Cl2(g), 1.5 mol PCl3(g) and 2.0 mol PCl5(g). Show that the reaction mixture has not yet reached

    asked by Claus on April 3, 2008
  90. chemistry

    A 0.411 mol sample of PCl5(g) is injected into an empty 4.65 L reaction vessel held at 250 °C. Calculate the concentrations of PCl5(g) and PCl3(g) at equilibrium.kc=1.80 at 250c

    asked by muna on November 10, 2013
  91. chemistry

    A system initially contains 0.100 mol each of the three species sealed in a 10.0 L container. The temp was raised to a temp where the equilibrium constant Kc, is 12.6 for PCl3(g) + Cl2(g)-->

    asked by Anonymous on September 10, 2014
  92. chemistry

    A system initially contains 0.100 mol each of the three species sealed in a 10.0 L container. The temp was raised to a temp where the equilibrium constant Kc, is 12.6 for PCl3(g) + Cl2(g)-->

    asked by Anonymous on September 10, 2014
  93. chemistry

    Using the Le Chatelier's principle, predict the direction of the net reaction in each of the following equilibrium systems, as a result of increasing the pressure at constant temperature. a)N2(g) + O2(g) ==> 2NO(g) PCl3(g) + Cl2(g) COCl2(g)

    asked by karl on June 14, 2010
  94. Chemistry

    For each of these reactions, indicate the property which might be observed in order to determine when equilibrium has been reached. a) PCl5(g) PCl3(g) + Cl2(g) b) CaCO3(s) CaO(s) + CO2(g) c) H2O(l) H2O(g) d) Cl2(g) + 2H2(g)  H2(g) + 2HCl(g) e)

    asked by Billy Bob on March 29, 2012
  95. Chemistry

    For each of these reactions, indicate the property which might be observed in order to determine when equilibrium has been reached. a) PCl5(g) PCl3(g) + Cl2(g) b) CaCO3(s) CaO(s) + CO2(g) c) H2O(l) H2O(g) d) Cl2(g) + 2H2(g)  H2(g) + 2HCl(g) e)

    asked by Billy Bob on March 29, 2012
  96. chemistry: equilibrium

    predict shift in equilibrium position and effect on amount of chlorine gas when volume is doubled at constant temperature. PCl3 (g) + Cl2(g) -> PCl5 (g)

    asked by i on January 11, 2018
  97. Chemistry

    In the reaction, PCl3 + Cl2 ------> PCl5 the concentration of the reactants at equilibrium were each determined to be 7.2 mol/L, and the product at 0.050 mol/L. Calculate the equilibrium constant (rounding to 2 significant figures and using scientific

    asked by James on September 13, 2015
  98. Chemistry

    The value of the equilibrium constant, Kc, at a certain temperature is 4.20 x 10-2. Would the reaction as represented by the chemical equation favor reactants or products? Enter Product or Reactant. PCl5(g) = PCl3(g)+Cl2(g)

    asked by Angel on February 27, 2010
  99. Idontgetit

    At 565 K the value of Kp for the equilibrium represented by the balanced equation is 2.00 x 10-1. Calculate the value of Kc at the same temperature. Express answer in scientific notation. PCl3(g)+Cl2(g) = PCl5(g) ____ x 10 _____

    asked by Chemistry on October 2, 2013
  100. chemistry

    Phosphorus trichloride gas and chlorine gas reacts to form phosphorus pentachloride gas: PCL3(g) +CL2(g) = PCL5(g). A vessel is CHARGED WITH A MIXTURE OF PCL3(g) and CL2(g), which is allowed to equilibrate at 450K. At equlibrium the partial pressures of

    asked by MIndy on October 19, 2011