# Pure phosgene gas (COCl2), .03mole, was placed in a 1.5 L container. It was heated to 800k, and at equilibrium the pressure of CO was found to be .497 atm. Calculate the equilibrium constant Kp for the reaction CO(g) +

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1. ## Chemistry

Pure phosgene gas (COCl2), .03mole, was placed in a 1.5 L container. It was heated to 800k, and at equilibrium the pressure of CO was found to be .497 atm. Calculate the equilibrium constant Kp for the reaction CO(g) + Cl2(g) = COCL2(g)
2. ## Chemistry

Pure phosgene gas (COCl2), .03mole, was placed in a 1.5 L container. It was heated to 800k, and at equilibrium the pressure of CO was found to be .497 atm. Calculate the equilibrium constant Kp for the reaction CO(g) + Cl2(g) = COCL2(g)
3. ## Chemistry

pure phosphene gas 3x10^-2 mol was placed in a 1.5L container. it was heated to 800K. at equilibrium the pressure of CO was found to be 0.497atm. calculate the Kp for the reaction: CO + Cl2 <---> COCl2
4. ## Chemistry

the initial pressure of phosgene gas (COCl2), was 1.31 atm. it was heated, and at equilibrium the pressure of CO was found to be .547 atm. what are the equilibrium pressures of Cl2 and COCl2? CO +Cl2=COCl2 i've done it twice and keep getting the wrong
5. ## chemistry

Phosgene (COCl2) is an extremely poisonous gas that was used extensively in World War I as a chemical warfare agent. At 300oC, phosgene decomposes to carbon monoxide and chlorine with a Kp = 6.8 x 10-2. Calculate the pressure in the vessel at equilibrium
6. ## Chem

Consider 1.40 mol of carbon monoxide and 3.20 mol of chlorine sealed in a 8.00 L container at 476 oC. The equilibrium constant, Kc, is 2.50 (in M-1) for CO(g) + Cl2(g) ↔ COCl2(g) Calculate the equilibrium molar concentration of CO. So I tried this
7. ## Chemistry

Need help in AP chemistry on Equilibrium When heated, hydrogen sulfide gas decomposes according to the equation 2 H2S(g) ⇄ 2 H2(g) + S2(g) A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is
8. ## HARD CHEM QUESTION- any help appreciated

Phosgene (COCl2) is a poisonous gas that dissociates at high temperature into two other poisonous gases, carbon monoxide and chlorine with equilibrium constant Kp = 0.0041 at 600 K. Find the equilibrium composition of the system after 0.124 atm of COCl2 is
9. ## Chemistry

A chemist wants to prepare phosgene, COCl2, by the following reaction: CO(g) + Cl2(g) COCl2(g) He places 2.60 g of chlorine, Cl2, and an equal molar amount of carbon monoxide, CO, into a 10.00 L reaction vessel at 395 °C. After the reaction comes to
10. ## 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 =
11. ## Chemistry

The Kp for the production of phosgene is 18.0. If one mole each of CO and Cl2 are mixed at the total pressure of 1 atm, what will be the partial pressure (in atm) of COCl2 after equilibrium is reached, CO(g) + Cl2(g)-->COCl2(g)
12. ## Chemistry

A container is filled with CO2(g) and heated to 1000K. The gas pressure at this temperature is 0.50 atm. Graphite (C) is then added to the container and some of the CO2 is converted to CO according to the reaction below. The final equilibrium total gas
13. ## chemistry

A sample of only solid ammonium chloride was heated in a 1 L container at 500 C. At equilibrium, the pressure of NH3 (g) was found to be 1.75 atm. what is the equilibrium constant, Kc, for the decomposition at this temperature? R= .08206 L atm/K Mol NH4CL
14. ## Chemistry

Nitrogen gas (N2) reacts with hydrogen gas (H2) to form ammonia (NH3). At 200 oC in a closed container, 1.1 atm of nitrogen gas is mixed with 2.1 atm of hydrogen gas in an otherwise empty container. At equilibrium, the total pressure is 2.2 atm. Calculate
15. ## Chemistry Equilibrium Constant

The initial pressures for I2 (g), H2(g), and HI(g) were Pi2 = 0.100 atm, Ph2 = 0.200 atm, and Phi = 0 atm, respectively. After the system came to equilibrium, the pressure of I2 (g) became very low, PI2 = 1.00 x 10^-5 atm. Calculate the equilibrium
16. ## chemistry

Phosgene is a potent chemical warfare agent that is now outlawed by international agreement. It decomposes by the reaction CoCl2(g)=>Co(g) + Cl2(g), Kc=8.3×10^-4.calculate [CoCl2] when 0.100mol CoCl2 decomposes and reach equilibrium in a 10L flask
17. ## Chemistry

At T = 25 degrees Celsius, the reaction No2 <-> 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium
18. ## Chemistry

At T = 25 degrees Celsius, the reaction No2 <-> 2NO +O2 has an equilibrium constant K=5.0*10^-13. Suppose the container is filled with NO2 at an initial pressure of 0.25 atm. Calculate the partial pressure of NO at equilibrium
19. ## Chemistry

A 10.0-g sample of solid NH4Cl is heated in a 5.00-L container to 900.°C. At equilibrium the pressure of NH3(g) is 1.51 atm. NH4Cl(s) mc011-1.jpg NH3(g) + HCl(g) The equilibrium constant, Kp, for the reaction is:
20. ## Chemistry Equilibrium

1.15 g oh h2O (density 1.00 g/ml) is introduced into an empty 1.00 L container. The seled container is heated to 412 K and .150 moles of O2 (g) is present at equilibrium. A. Wrte the equilibrium expression for the reaction above. B. Calculate the
21. ## Chemistry

If the reaction Fe2N(s) + 3/2H2(g) -> 2Fe(s) +NH3(g) comes to equilibrium at a total pressure of 1 bar, analysis of the gas shows that at 700. and 800.K, PNH3/PH2=2.165 and 1.083 respectively, if only H2(g) was initially present in the gas phase and
22. ## Chemistry

When 0.20 mol of hydrogen gas and 0.15 mol of iodine gas are heated at 723 K until equilibrium is established, the equilibrium mixture is found to contain 0.26 mol of hydrogen iodide. The equation for the reaction is as follows. H2(g) + I2(g) ↔ 2HI(g)
23. ## chemistry

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the
24. ## chemistry

For reactions in solution, molar concentrations are usually used in equilibrium constant expressions (designated by K or Kc). In gases, partial pressures can also be used (designated by Kp). Equilibrium partial pressures of NOCl, NO and Cl2 in a container
25. ## 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
26. ## Chemistry

Carbon monoxide and chlorine gas react to form phosgene: CO(g)+Cl2(g)⇌COCl2(g) Kp = 3.10 at 700 K If a reaction mixture initially contains 319torr of CO and 220torr of Cl2, what is the mole fraction of COCl2 when equilibrium is reached?
27. ## Chemistry

Hydrazine, N2H4 can be made (on paper) by reaction of molecular nitrogen and molecular hydrogen, 2 H 2 ( g ) + N 2 ( g ) --> N 2 H 4 ( g ) and suppose that the equilibrium constant Kp has the value 1×10^–3. (a) A stoicheometric mixture of H2 and N2
28. ## chemistry

For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.15 g of SO3 and 0.107 g of O2. 1) How many grams of SO2 are in the vessel? ---------------------------- A flask is charged with 1.500 atm of N2O4(g)
29. ## Chemistry

Write the equilibrium expression, and calculate Kp for the reaction under the conditions described: 2NaHCO3 (s) --> <--- Na2CO3 (s) + H2O (g) + CO2 (g) 100 g of solid NaHCO3 was placed in a previously evacuated rigid 5.00 L container and heated to
30. ## Chemistry

Write the equilibrium expression, and calculate Kp for the reaction under the conditions described: 2NaHCO3 (s) --> <--- Na2CO3 (s) + H2O (g) + CO2 (g) 100 g of solid NaHCO3 was placed in a previously evacuated rigid 5.00 L container and heated to
31. ## chemistry

Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g)
32. ## (1-16)Chemistry - Science

Consider the reaction: SO2 (g) + NO2 (g) ==> SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 The reaction vessel is charged initially with all four gases, each at a pressure of 0.5 atm. After
33. ## chemistry

The following reaction is at equilibrium at a pressure of 1 atm, in a closed container. NaOH(s) + CO2(g) NaHCO3(s); ΔH°rxn < 0 Which, if any, of the following actions will decrease the concentration of CO2 gas present at equilibrium? A. lowering
34. ## 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)
35. ## chemistry

SO2Cl2(g) SO2(g) + Cl2(g) The Kp for the reaction is 2.18 at 648 K. A sample of SO2Cl2 is placed in a container and heated to 648 K while the total pressure is kept constant at 9.00 atm. Calculate the partial pressures of the gases at equilibrium.
36. ## chemisrty

Q6) A 10 L container contains a mixture of 0.8 g of He and 8 g of Ar at 0 oC. a) (1 pt) Calculate the total pressure of the gas mixture. b) (1 pt) Calculate the partial pressure of each gas in the gas mixture. c) (1 pt) If the initial total pressure of the
37. ## Chemistry

The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) I'm sorry.. English is a second language for me. After
38. ## chemistry

can you explain me how to do this question. any help would be much appreciated. 1) If 0.025 mol of COCl2(g) is placed in a one liter container at 400c, 16.0% of the CoCl2 is dissociated when equilibrium is established. COCl2(g)-> Co(g)+Cl2(g) calculate
39. ## chemistry

I was having trouble with this problem. initial pressure for the compounds involved in the reaction displayed were determined to be P(CO(g)) = 0.5794 atm, P(H2O(g)) = 0.5662 atm, P(CO2(g)) = 0.7950 atm, P(H2(g)) = 0.2754 atm. Calculate the value of the
40. ## chemistry

1.0 mol of nitrogen oxide NO and 1.0 mol of oxygen were mixed in a container and heated to 450 oC. At equilibrium the number of moles of oxygen was found to be 0.70 mol. The total pressure in the vessel was 4.0 atm. Calculate the value of Kp for the
41. ## Chemistry

CaCO3(s) <--> CaO(s) + CO2 (g) A 5.9-gram sample of CaCO3 (molar mass = 100.) is placed in an evacuated 2.00L container and heated to 200^oC. Equilibrium is reached when 5.15% of the CaCO3 has decomposed. 1)Write the Kp expression for this reaction
42. ## Chemistry

I have been stuck on this question please help me solve it? The following reaction is used in some self-contained breathing devices as a source of O2(g). 4KO2(s)+2CO2(g)⇌2K2CO3(s)+3O2(g)Kp=28.5at25∘C Suppose that a sample of CO2(g) is added to
43. ## chemistry

Calculate the value of the equilibrium constant (Kp) for the reaction shown, if F(g) was found to be 96.80 % decomposed at 1000 K when its initial pressure was 4.638 atm. The initial pressure of the reaction products is 0 atm. 2F(g) = F2(g)
44. ## Chemistry

When solid CO2 (dry ice) is allowed to come to equilibrium in a closed constant volume container at room temperature (300K), 1. the pressure rises until it reaches 1 atm 2. the pressure rises until a liquid-gas equilibrium is reached. 3. the pressure does
45. ## CHEMISTRY

1.0 mol of nitrogen oxide NO and 1.0 mol of oxygen were mixed in a container and heated to 450 oC. At equilibrium the number of moles of oxygen was found to be 0.70 mol. The total pressure in the vessel was 4.0 atm. Calculate the value of Kp for the
46. ## Chemistry

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.
47. ## Chem

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.
48. ## Chemistry

Enough SO3 is added to an evacuated container so its initial pressure is 4.00 atm. Calculate the mole fraction of O2 in the equilibrium mixture if the total pressure at equilibrium is 5.00 atm.
49. ## Chemistry

Consider the heterogeneous equilibrium process shown below. C(s) + CO2(g) 2 CO(g) At 700.°C, the total pressure of the system is found to be 3.87 atm. If the equilibrium constant KP is 1.52, calculate the equilibrium partial pressures of CO2 and CO.
50. ## Chemistry

3H2(g)+N2(g)=2NH3(g) Suppose the equilibrium constant Kp = 0.003337 for the reaction above. If the equilibrium mixture contains partial pressures H2 = 0.400 atm and N2 = 0.350 atm. What is the equilibrium partial pressure of NH3 in atm?
51. ## Chemistry

A mixture containing 0.5 mol of H2 (g) and 0.5 mol of I2 (g) was introduced into a 10L container at a temperature of 448 C. At this temperature the equilibrium constant Kp is 50. i. What is the total pressure in the container before the reaction starts and
52. ## Chemistry

A mixture containing 0.5 mol of H2 (g) and 0.5 mol of I2 (g) was introduced into a 10L container at a temperature of 448 C. At this temperature the equilibrium constant Kp is 50. i. What is the total pressure in the container before the reaction starts and
53. ## (1-17)Chemistry - Science

Consider the reaction: SO2 (g) + NO2 (g)  SO3 (g) + NO (g) At T = 1000 K, where the reaction is exothermic with an equilibrium constant K = 9.00 If the reaction vessel is instead charged initially with SO3(g) and NO(g), each at a partial pressure
54. ## Chemistry***

A mixture containing 19.8 moles of H2 and 7.2 mole of I2 was allowed to reach equilibrium in a 5 L closed vessel at ToC according to the equation: H2 (g) + I2 (g) 2HI (g) At equilibrium, 14 moles of H2 was present. The equilibrium constant for this
55. ## 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
56. ## Chemistry

A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred. Reaction (a): 2 FeSO4(s)--> Fe2O3(s) + SO3(g) + SO2(g) Reaction (b): SO3(g)--> SO2(g) + 1/2 O2(g) After equilibrium was reached, the
57. ## Gen Chm II

Determine the pressure-based Keq for the reaction: 2SO2(g) + O2(g)<--->2SO3(g) given that 1.00×10−2 moles of SO2 and 2.00×10−2 moles of O2 were initially placed in a 2.00 L reaction chamber. The chamber contained 7.5×10−3 moles
58. ## science

A mixture of nitrogen gas, hydrogen gas and ammonia gas reacts by: N2(g) + 3H2(g) = 2NH3(g) If the total pressure in the reaction vessel is 50.0 atm ans the equilibrium mixture contains by volume: N2= 96.143% H2= 0.3506% NH3= 3.506% what is the equilibrium
59. ## AP Chemistry

In 1.33L container, 4.20 AB3, is heated to 400C, and 2.98x10-2(negative 2) moles of A is present at equilibrium. AB3(g) <----> A(g)+ 3B(g) (28.23amu) (a.) Write the expression for K (b.) Calculate the equilibrium concentration of the following gases
60. ## Chemistry

The initial pressure for the compounds involved in the reaction shown were determined to be P(Br2(g)) = 0.5417 atm, P(Cl2(g)) = 0.6962 atm, P(BrCl(g)) = 0.3442 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium pressure
61. ## Chemistry

The Kp for the following equilibrium system is 4.31 x 10‒4 at 375°C : N2(g) + 3H2(g) ↔ 2NH3(g). If 0.862 atm of N2 and 0.373 atm of H2 were mixed in a constant-volume flask and heated to 375°C, which of the following would be closest to the
62. ## Chemsitry

Consider the equilibrium A(g)=2B(g)+3C(g) at 25 degrees Celsius. When A is loaded into a cylinder at 10 atm and the system is allowed to come to equilibrium, the final pressure is found to be 12.13 atm. What is the standard gibbs free energy of reaction
63. ## CHEMISTRY

The equilibrium constant for the reaction, SO2(g)+ NO2(g) <----> NO(g)+ SO3(g) has been experimentally determined as a function of temperature. The results are presented in the table below. T (°F) KC 285 662 752 156 842 93.4 932 59.6 1022 40.2 If
64. ## chemistry(check my work)

Calculate the value of the equilibrium constant (Kp) for the reaction displayed if the following equilibrium pressure data were measured at 25.00 °C: P(H2(g)) = 0.2282 atm, P(I2(g)) = 0.1646 atm, P(HI(g)) = 5.462 atm. H2(g)+I2(g) = 2HI(g) is it like this,
65. ## chemistry

An equilibrium mixture contains N2O4, (P= 0.30 ) and NO2 (P= 1.1 ) at 350 K. The volume of the container is doubled at constant temperature. Calculate the equilibrium pressure of when the system reaches a new equilibrium. Calculate the equilibrium pressure
66. ## chemistry(check my work)

The initial pressure for the compounds involved in the reaction displayed were determined to be P(SO2(g)) = 0.5932 atm, P(O2(g)) = 0.4886 atm, P(SO3(g)) = 0.09287 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium
67. ## Chemistry

A mixture containing the same number of moles of SO2 and O2 is placed in a 2L container at 900K. The initial pressure is 1.90Atm. A reaction occurs leading to the formation of SO3: 2SO3 + O2 <--> 2SO3 After equilibrium is established the TOTAL
68. ## Chemistry

The equilibrium constant Kc for the following reaction is equal to 0.20 at 250°C. Calculate the equilibrium constant Kp for the reverse reaction at the same temperature. COCl2 (g) = CO (g) + Cl2 (g) My Answer: To find the reverse reaction of Kc, it should
69. ## Chemistry

If the equilibrium constant K equals .05, and the reaction C3H8=C3H6 + H2 (all gases), starts with pure C3H8 and is allowed to reach equilibrium at 200 K at a total pressure of 2 bar. Calculate the partial pressure of H2 at equilbirum.
70. ## chem

The following reaction is used in some self-contained breathing devices as a source of O2. 4KO2(s) + 2C02(g)---> 2K2CO3(s) + 3O2(g) Suppose that a sample of CO2(g) is added to an evacuated flask containing KO2(s) and equilibrium is established. The
71. ## Chemistry

Another Equilibrium Question! The following reaction is at equilibrium in a closed 20.0-L container. At equilibrium, the pressures of NH3 and HCl are both equal to 0.00552 atm, and the mass of NH4Cl (s) is 35.4 g. Calculate the equilibrium pressure of NH3
72. ## Chemistry

A student ran the following reaction in the laboratory at 651 K: 2 NH3(g) N2(g) + 3 H2(g) When she introduced 8.75E-2 moles of NH3(g) into a 1.00 Liter container, she found the equilibrium concentration of H2(g) to be 0.119 M. Calculate the equilibrium
73. ## Chemistry

A student ran the following reaction in the laboratory at 650 K: H2(g) + I2(g) 2 HI(g) When she introduced 0.204 moles of H2(g) and 0.229 moles of I2(g) into a 1.00 Liter container, she found the equilibrium concentration of I2(g) to be 5.77E-2 M.
74. ## Chemistry

Consider the reaction A+B->C+3D. A solution was prepared by mixing 50 ml of .001 M of A, 100 ml of .002 M of B, 10 ml of 1 M of C, and 75 ml of .0015 M of D. At equilibrium, the concentration of D was measured and found to be .0006 M. Calculate the
75. ## chemistry(just to double check)

The initial pressure for the compounds involved in the reaction displayed were determined to be P(SO2(g)) = 0.5932 atm, P(O2(g)) = 0.4886 atm, P(SO3(g)) = 0.09287 atm. Calculate the value of the equilibrium constant (Kp) at 1000 K if the equilibrium
76. ## chemistry

sulfur trioxide gas dissociates into sulfer dioxide gas and oxygen gas at 1250 degrees C. In an experiment, 3.6 moles of sulfur trioxide were placed into an evacuated 3.0-L flask. THe concentration of sulfur dioxide gas measured at equilibrium was found to
77. ## Chemistry

A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial pressures: P(SO2)=0.35 atm, P(SO2Cl2)=0.19 atm, P(Cl2)=0.24 atm. Kp=91 for the equilibrium system: SO2 (g) + Cl2 (g) -> SO2Cl2 (g) Is
78. ## Chemistry

Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now calculate the work done if this
79. ## chem

A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25°C, and the following equilibrium is achieved. N2O4(g)-> 2 NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.504 atm. (a) What is the equilibrium partial
80. ## Chemistry

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) --> C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C
81. ## Chemistry

The equilibrium constant Kp for the reaction below at 700°C is 0.76 atm. CCl4(g) C(s) + 2 Cl2(g) Determine the initial pressure of carbon tetrachloride that will produce a total equilibrium pressure of 1.20 atm at 700°C
82. ## Chemistry

The Haber process is used to synthesize ammonia (NH3) from N2 and H2. The change in standard Gibbs free energy is ΔG°rxn = -16 kJ/mol A. Calculate the equilibrium constant for this reaction B. Calculate the ΔGrxn when you have 2 atm of NH3 (g),
83. ## chemistry

at 22°C the equilibrium constant, Kc, for the following reaction is 4.66 x 10-3. (1) If 0.800 mol of N2O4 were injected into a closed 1.00-L container at 22°C, how many moles of each gas would be present at equilibrium? (b) If the volume were halved (to
84. ## chemistry

the reaction between H2 and O2 reaches equilibrium in a closed container according to the following balanced equation: 4HCl+O2=2H2O+2Cl2 the volume of the container is 5dm3 calculate the equilibrium constant (Kc) for this reactin
85. ## Chemstry

For the reaction A(g) + B(g) <==> C(g) + D(g) the equilibrium constant K is defined as K = Y(sub y) * Y(sub D) / (Y (sub A) * Y(sub b)) where y is the molar fraction of the gas phase of a species At 620.00 K, the equilibrium constant is 1.100.
86. ## chemistry

1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K. CO + Cl2 +++> COCl2 kp = 22.5 Calculate partial pressure of COCl2. i get about 30.9. but its wrong. i solved for x,
87. ## chemistry

1.30 mol each of CO} and Cl2 are introduced into an evacuated 1.80 L flask, and the following equilibrium is established at 668 K. CO + Cl2 +++> COCl2 kp = 22.5 Calculate partial pressure of COCl2. i get about 30.9. but its wrong. i solved for x,
88. ## Chem

At 850 C, the equilibrium constant Kp for the reaction: C(s)+CO2(g) >< 2CO(g) has a value of 10.7. If the total pressure in the system at equilibrium is 1.000 atm, what is the partial pressure of carbon monoxide.
89. ## science

Pure PCL5 is introduced into an evacuated chamber and comes to equilibrium at 247C and 2 atm. The equilibrium gaseous mixture contain 40% chlorine by volume. Calculate Kp for the reaction.
90. ## Chemistry

Consider the following decomposition reaction of ammonium carbonate ((NH4)2CO3): (NH4)2CO3 (s)  2 NH3 (g) + CO2 (g) + H2O (g) In one experiment at 25.0°C, a sample of pure (NH4)2CO3 is placed in an evacuated 2.00 L vessel. At equilibrium, the total
91. ## chemistry help plz

Le chatelier's principle? co(g)+cl2(g)=cocl2(g)is reversible and ,after a certain amount of time ,will reach equilibrium.Explain,using Le chatelier's principle,what effect: 1)increasing the pressure (at constant temperature) 2)increasing the temperature
92. ## Chemistry

Consider an ideal gas encloesd in a 1.00 L container at an internal pressure of 10.0 atm. Calculate the work, w, if the gas expands against a constant external pressure of 1.00 atm to a final volume of 20.0 L. w = ____ J now calculate the work done if this
93. ## Chemistry

For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.340 mol of F2 is added to this equilibrium mixture, calculate the
94. ## chemistry

For the reaction below at a certain temperature, it is found that the equilibrium concentrations in a 4.87-L rigid container are [H2] = 0.0496 M [F2] = 0.0116 M [HF] = 0.429 M. H2(g) + F2(g) <==> 2 HF(g) If 0.185 mol of F2 is added to this
95. ## Chemistry

For the following reaction at a certain temperature: 2( ) 2( ) ( ) 2 H F HF g g g +  it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2]=0.0500 M, [F2]=0.0100 M, and [HF]=0.400 M. If 0.200 mol F2 is added to this
96. ## chemistry

For the following reaction at a certain temperature, it is found that the equilibrium concentrations in a 5.00 L rigid container are [H2] = 0.0500 M, [F2] = 0.0100 M, and [HF] = 0.400 M. If 0.261 mol of F2 is added to this equilibrium mixture, calculate
97. ## Chemistry

At elevated temperatures, SbCl5 gas decomposes into SbCl3 gas and Cl2 gas as shown by the following equation: SbCl5(g)<=> SbCl3(g) + Cl2(g) 1. What is the concentration in moles per liter of SbCl5 in the container before any decomposition occurs? 2.
98. ## chem

Fluorine and krypton react to form binary compounds when a mixture of the two gases is heated to 500C in a nickel reaction vessel. A 100mL nickel container is filled with fluorin and krypton to partial pressures of 1.24 atm and 10.10 atm, respectively at a
99. ## Chemistry

Consider the following equilibrium at 1000K: 2SO2 (g) + O2 (g) ¡ê 2SO3 (g) A study of this system reveals that there are 3.5E-3 moles of sulfur dioxide gas, and 4.8E-3 moles of oxygen gas present in a 11.0L flask at equilibrium. The equilibrium constant
100. ## chemistry

a flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 degrees celsius and allowed to reach equilibrium.when equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) what are the