# -Suppose K= 4.5x10^-3 at a certain temperature for the reaction : PCl5 PCl3+ Cl3, what must be the concentration of Cl2 under these conditions? -Chromate ion, Cro4^-2, is used as a qualitative test for lead(II) ion, forming a birght yello

36,802 results
1. ## 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?

2. ## 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

3. ## chemistry

Given overall reaction: P4 + 10Cl2 ---> 4PCl5 Delta H for the reaction = ? PCl5 -----> PCl3 + Cl2 Delta H = +157 kJ P4 + 6Cl2 ----> 4PCl3 Delta H = -1207 kJ Calculate the Delta H for the overall reaction.

4. ## 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.

5. ## chemistry plse help

Use the standard reaction enthalpies given below to determine Î”H°rxn for the following reaction: P4(g) + 10 Cl2(g) â†’ 4PCl5(s), Î”H°rxn = ? Given: PCl5(s) â†’ PCl3(g) + Cl2(g), Î”H°rxn= +157 kJ P4(g) + 6 Cl2(g) â†’ 4 PCl3(g),

6. ## 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

7. ## Chemistry

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

8. ## 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

9. ## 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

10. ## 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!

11. ## 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

12. ## 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

13. ## 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

14. ## Chemistry

Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine,

15. ## Chemistry

a) Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine,

16. ## 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

17. ## 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

18. ## 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

19. ## 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:

20. ## Chemistry

For the following reaction at 600. K, the equilibrium constant, Kp, is 11.5. PCl5(g) equilibrium reaction arrow PCl3(g) + Cl2(g) Suppose that 2.030 g of PCl5 is placed in an evacuated 535 mL bulb, which is then heated to 600. K. (a) What would be the

21. ## Chemistry

At 760◦C, Kc= 33.3 for the reaction PCl5(g)⇀↽PCl3(g) + Cl2(g) If a mixture that consists of 0.31 mol PCl3 and 0.22 mol Cl2 is placed in an 8 L reaction vessel and heated to 760◦C, what is the equilibrium composition of PCl5?Answer in units of

-Suppose K= 4.5x10^-3 at a certain temperature for the reaction : PCl5 PCl3+ Cl3, what must be the concentration of Cl2 under these conditions? -Chromate ion, Cro4^-2, is used as a qualitative test for lead(II) ion, forming a birght yello precipitate of

23. ## 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

24. ## 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

25. ## 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

26. ## Chmistry

pcl3(g) cl2(g) ¨

27. ## 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?

28. ## 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?

29. ## 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.

30. ## 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

31. ## 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

32. ## 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 =

33. ## 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

34. ## 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)

35. ## 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

36. ## 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

37. ## mosab bin omair

We examine the following reaction at 250ÃƒÂ¯Ã¢â‚¬Å¡Ã‚Â°C: PCl5(g) ÃƒÂ¢Ã¢â‚¬Â¡Ã…â€™ 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

38. ## chem

For the gaseous equilibrium represented below, it is observed that greater amounts of PCl3 and Cl2 are produced as the temperature is increased. PCl5(g) PCl3(g) + Cl2(g) a) What is the sign of S° for the reaction? Explain. b) What change, if any, will

39. ## Chemistry

a) Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine,

40. ## Chemistry

a) Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine,

41. ## Chemistry

In the reaction PCl3 + Cl2 ---> PCl5. If the rate doesn't increase when the concentration of PCl3 is doubled and the rate increases by a factor of four when the concentration of Cl2 is doubled, how would I write the rate law for the reaction?

42. ## chem

Using LeChatelier's principle, predict the direction of the net reaction in each of the following system as a result of decreasing the volume of the chamber for the reaction mixture. Where does the direction shifts? a.) N2(g)+ O2(g)= 2NO(g) b.)

43. ## 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,

44. ## 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.

45. ## 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

46. ## 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

47. ## equilibrium constant (Kp)

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

48. ## 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:

49. ## chemistry

a) Tetraphosphorus (P4), commonly known as white phosphorus, forms different compounds with chlorine (Cl2) depending on the amount of chlorine present. If chlorine is limited, phosphorus trichloride (PCl3) is formed. If there is an excess of chlorine,

50. ## 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.

51. ## 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)

52. ## 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

53. ## 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:

54. ## 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

55. ## 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)

56. ## science

Given the following reaction, with Kp=1.05 at 250 degrees C what is Kc? The reaction is PCl5 to PCl3+Cl2

57. ## Chemistry

write a sentence for the following reaction PCl5(s)=PCl3(s)+Cl2(g)

58. ## chemistry

If the temperature of the system PCl5 (g) =PCl3 (s) + Cl2 (g) + 92.5 kj. is increased, predict the direction of th Le Chatelier's shift.

59. ## 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

60. ## 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:

61. ## Chemistry

If P4 (white phosphorous) forms different compounds with chlorine (Cl3) depending on the amount of chlorine present (limited chlorine forms PCl3 and chlorine in excess forms PCl5) design an experiment that could be performed to verify each synthesis

62. ## 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

63. ## 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.

64. ## 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.

65. ## 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

66. ## 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

67. ## 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

68. ## 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)

69. ## 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

70. ## 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?

71. ## 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

72. ## 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)

73. ## 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

74. ## 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

75. ## 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

76. ## 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"?

77. ## chemistry

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

78. ## 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

79. ## 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=??

80. ## 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?

81. ## 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

82. ## 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!

83. ## 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

84. ## 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.

85. ## 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

86. ## chemistry

For the gaseous equilibrium represented below, it is observed that greater amounts of PCl3 and Cl2 are produced as the temperature is increased. PCl5 (g) PCl3 (g) + Cl2 (g) a) what is the sign of delta S for the reaction? Provide a legitimate rationale for

87. ## 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)

88. ## Chemistry

Kp=1.78 at 250 degrees for the decomposition reaction, PCl5(g)->PCl3(g)+Cl2(g. Calculate the percentage of reactant that remains if 10.0 moles of starting material are placed in a closed vessel at this temperature and 2.00 atm pressure. Also, determine the

89. ## 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

90. ## 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

91. ## 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

92. ## 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

93. ## 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

94. ## 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 = ?

95. ## 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...

96. ## 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

97. ## 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

98. ## 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

99. ## 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

100. ## chemistry

Given the following data: 4PCl5(s) ¨ P4(s) + 10Cl2(g) ƒ¢H = +1774 kJ P4(s) + 6Cl2(g) ¨ 4PCl3(l) ƒ¢H = -1278.8 kJ Find the ƒ¢H of the following reaction: PCl5(s) ¨ PCl3(l) + Cl2(g)