1. Chem

    Given the reaction: SO2(g) + NO2(g) = NO(g) + SO3(g) H = -42.6Kj How will the concentration of SO3 at equilibrium be effected by the following: a) Adding more NO2(g) b) Removing some NO(g) c) Increasing the temperature
  2. chemistry

    I am a bit confused with this proble because the concentration of SO3 at equilibrium. Any help would be appreciated. Given the reaction: SO2(g) + NO2(g) ⇌ NO(g) + SO3(g) ∆H = -42.6 kJ. How will the concentration of SO3(g) at equilibrium be
  3. Chemistry

    SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50 moles of NO2 are added to the
  4. Chem Equilbirum

    SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. ---How many moles/liter of NO2 would have to be added to the
  5. Chemistry

    SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. ---How many moles/liter of NO2 would have to be added to the
  6. Chemistry

    The equilibrium constant is 16 for the gas phase reaction SO2 + NO2 <--> SO3 + NO at a certain temperature. If 3.0 moles each of SO2 and NO2 are placed together in an empty 1.0 liter flask and the system is allowed to come to equilibrium at this
  7. Chemistry

    Given the following equation: SO2 + NO2 <--> SO3 + NO At 25 Celcius, 2.00 mol of each of SO2 and NO2 are introduced into a 1.0L sealed flask. When euilibrium is reached, it is found that [NO2] = 1.30 mol/L [SO3] = 1.30 mol/L -- Calculate the
  8. Chemistry

    At a given temperature, analysis of an equilibrium mixture represent below is given as: SO2(g) + NO2(g) <--> SO3(g) + NO(g) Where [SO2]=4.0M, [NO2]=0.50M, [SO3]= 3.0M, [NO]=2.0M. Find the value of Keq
  9. General Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.90. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.53 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium.
  10. Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) at equilibrium. SO2(g)
  11. Chemistry

    At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases. K=(.5+x)^2/(.5-x^2) solve for
  12. Chem.

    10. Suggest how two very different variables could be manipulated to increase the percent yield of sulphur trioxide. The equation for the reaction follows. 2 SO2(g) + O2(g)>>> 2 SO3(g) + energy Ok, I really don't know this one. Can you please
  13. Chemistry, equilibrium molarity

    At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases. This is what I've done so
  14. 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
  15. chem: equilibrium

    In which direction does the equilibrium shift for the following reaction? SO2(g) + NO2 (g) <-> SO3(g0 + NO(g) + 42 KJ a. temperature increases b. pressure increases c. [SO2] increases d. [NO2] increases e. temperature decreases f. [No] increases Im
  16. apchemistry

    The numerical value of the concentration equilibrium constant for the gaseous reaction 2 SO2 + O2 *) 2 SO3 is 0.5 at temperature T. When a reactionmix- ture is brought to equilibrium, [O2] is found to be 2.0 M and [SO3] is found to be 10 M. What is the
  17. Chemistry

    Without detailed equilibrium calculations, estimate the equilibrium concentration of SO3 when a mixture of 0.134 mol of SO2 and 0.067 mol of O2 in a 275 mL flask at 300oC combine to form SO3. 2 SO2(g) + O2(g) = 2 SO3(g) Kc = 6.3x10^9 I tried doing an ICE
  18. ap chemistry

    At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2 SO2(g) + O2(g) *) 2 SO3(g) What concentration of SO3 would be in equilibrium with 0.250moles of SO2 and 0.853 moles of O2 in a 1.00 liter container at this temperature? Note:
  19. ap chem

    At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2 SO2(g) + O2(g) *) 2 SO3(g) What concentration of SO3 would be in equilibrium with 0.250moles of SO2 and 0.578 moles of O2 in a 1.00 liter container at this temperature? Note:
  20. (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
  21. Chemistry

    For the reaction, 2SO2(g) + O2(g) ¨ 2SO3(g) + heat, at equilibrium, what will be the effect on the net amount of SO3 present if the temperature of the container is increased? A) The concentration of SO3 decreases. B) The concentration of SO3 increases.
  22. (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
  23. Chemistry

    At a particular temperature, 13.4 mol of SO3 is placed into a 3.8-L rigid container, and the SO3 dissociates by the reaction given below. 2 SO3(g) <-> 2 SO2(g) + O2(g) At equilibrium, 3.6 mol of SO2 is present. Calculate K for this reaction.
  24. Chemistry

    At a particular temperature, 13.7 mol of SO3 is placed into a 3.9-L rigid container, and the SO3 dissociates by the reaction given below. 2 SO3(g) 2 SO2(g) + O2(g) At equilibrium, 3.8 mol of SO2 is present. Calculate K for this reaction.
  25. Chemistry(Urgent, please respond, thanks!!)

    1) For the reaction system, 2 SO2(g) + O2(g) = 2 SO3(g), Kc has a value of 4.62 at 450.0 K (Kelvin). A system, at equilibrium has the following concentrations: (SO3) = 0.254 M; (O2) = 0.00855 M. What is the equilibrium concentration of SO2? Is set this up
  26. chemistry

    Consider the following chemical equilibrium: SO3(g) --> SO2(g) + 1/2 O2(g) and Delta H = 98.9J a. Predict weather the forward or reverse reaction will occur when the equilibrium is disturbed by: i. adding oxygen gas ii. compressing the system at
  27. chemistry

    An equilibrium mixture of SO2,SO3 and O2 gases is maintained in a 11.5 L flask at a temp at which Kc=55.2 for the rxn: 2SO2 + O2 <> 2SO3. If the # of moles of SO2 and SO3 are =, how many moles of O2 are present? I let SO2 and SO3 =x and O2=y. Since
  28. Gen Chem

    Consider the reaction: 2 SO2(g) + O2(g) ↔ 2 SO3(g). If, at equilibrium at a certain temperature, [SO2] = 1.50 M, [O2] = 0.120 M, and [SO3] = 1.25 M, what is the value of the equilibrium constant?
  29. Chemistry

    An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following reaction. 2
  30. P. Chemistry

    The equilibrium 2 SO2(g) + O2(g) 2 SO3(g) has the value K = 2.5 1010 at 500. K. Find the value of K for each of the following reactions at the same temperature. (a) SO2(g) + 1/2 O2(g) SO3(g) K = (b) SO3(g) SO2(g) + 1/2 O2(g) K = (c) 3 SO2(g) + 3/2 O2(g) 3
  31. chem

    At a certain temperature, a 19.0-L contains holds four gases in equilibrium. Their masses are: 3.5 g SO3, 4.6 g SO2, 14.0 g N2, and 0.98 g N2O. What is the value of the equilibrium constant at this temperature for the reaction of SO2 with N2O to form SO3
  32. chemistry

    All the following species are best described by writing at least two Lewis structures EXCEPT a. O3. b. SO2. c. NO2- d. SO3-2 e. SO3.
  33. Chemistry

    Consider the reaction: N2O4(g) <--> 2NO2(g) delta H^o =58.576kJ; Keq =0.87 at 55degrees celsius What is the effect of each of these changes upon the concentration of N2O4 at equilibrium? a)increasing the temperature b)increasing the volume c) adding
  34. 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
  35. chemistry

    An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following reaction. 2
  36. tommy

    At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) SO3(g) + NO(g) If all four gases had initial concentrations of 0.870 M, calculate the equilibrium concentrations of the gases.
  37. Chemistry

    At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) <==> SO3(g) + NO(g)\ If all four gases had initial concentrations of 0.550 M, calculate the equilibrium concentrations of the gases.
  38. AP Chem

    At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) SO3(g) + NO(g) If all four gases had initial concentrations of 0.580 M, calculate the equilibrium concentrations of the gases.
  39. chemistry

    At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g)= SO3(g) + NO(g) If all four gases had initial concentrations of 0.840 M, calculate the equilibrium concentrations of the gases.
  40. Chemistry

    At a particular temperature, K = 3.75 for the following reaction. SO2(g) + NO2(g) SO3(g) + NO(g) If all four gases had initial concentrations of 0.520 M, calculate the equilibrium concentrations of the gases
  41. Chemistry

    An equilibrium mixture of the following reaction was found to have [SO3] = 0.391 M and [O2] = 0.125 M at 600 °C. What is the concentration of SO2? 2 SO2 (g) + O2 (g) ====== 2 SO3 (g) Keq = 4.34 at 600 °C
  42. Chemistry

    Can we use O2 to identify NO and SO2 from each other? Is it because NO+O2-->NO2; NO2 - brownish gas and 2SO2+O2--2SO3;SO3-blue in colour? Or what is the reason?
  43. Chemistry

    Calculate Kp at 298K for the reaction SO2 + NO2--->SO3 + NO
  44. Chemistry

    The reaction NO2(g) + NO2(g) → N2O4(g) is second order with a rate constant of 0.044 /M·s at a particular temperature and pressure. If the initial concentration of NO2(g) is 0.100 M, what is the concentration of NO2 after 20 minutes?
  45. chemistry

    balance: SO2(g)+O2(g)------->SO3(g) the concentration of SO2 and O2 are determined to be [0.06] and [0.03] if the following reaction has a Kc of 3.6x10^2, what is the concentration of SO3???? any work would be much appreciated thank you!!
  46. chemistry

    At 298K, Go = -141.8 kJ for the reaction 2 SO2 + O2 in equilibrium with 2 SO3 Calculate the change in Gibbs free energy (in kJ) at the same temperature when P (SO2) = 0.505 bar, P (O2) = 0.80 bar and P (SO3) = 1.317 bar. (R = 8.314 J/K mol)
  47. chem class

    The value of Keq for the following reaction is 0.25: SO2 (g) + NO2 (g)<~> SO3 (g) + NO (g) The value of Keq at the same temperature for the reaction below is __________. 2SO2 (g) + 2NO2 (g)<~> 2SO3 (g) + 2NO (g) answer is 0.25 how do i figure
  48. Chemistry

    Sulfur trioxide, SO3, is made from the oxidation of SO2, and the reaction is represented by the equation 2SO2 + O2 2SO3 A 25-g sample of SO2 gives 18 g of SO3. The PERCENT YIELD of SO3 is?
  49. Chemistry

    For the teaction system, 2SO2(g) + O2(g) <--> 2SO3(g), Kc has a value of 4.62 at 450.0K. A system, at equilibrium, has the following concentrations: [SO3] = 0.254 M, [O2] = .00855 M. What is the equilibrium concentration of SO2(g)? The correct answer
  50. Chem

    At 930 K, Kp = 0.30 for the following reaction. 2 SO2(g) + O2(g)=>2 SO3(g) Calculate the equilibrium partial pressures of SO2, O2, and SO3 produced from an initial mixture in which the partial pressures of SO2 and O2 = 0.51 atm and the partial pressure
  51. Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 M
  52. Chemistry

    For the reaction NO2(g) + NO(g) = N2O3(g) If at particular temperature, K was 575 and equilibrium concentration of N2O3(g) was 2.5 M, calculate the equilibrium concentrations of NO2(g) and NO(g) if they both had the same initial concentrations. i have my
  53. College Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 M
  54. Chemistry

    At a particular temp, K = 1.6 x 10^-5 for the reaction: 2SO3(g) <-> 2SO2(g) + O2 (g) If 4 mol of SO2 and 2 mol of O2 are placed into a 2.0L flask, calculate the equilibrium concentrations of all species. I set up an ICE table with SO3 to start with
  55. chem

    Consider the following chemical equilibrium: SO3(g) --> SO2(g) + 1/2 O2(g) and Delta H = 98.9J i. adding oxygen gas ii. compressing the system at constant temperature iii. adding argon gas iv. removing sulfur dioxide gas v. decreasing the temperature
  56. AP Chemistry

    I'm so sorry to bother you guys again! Stuck on two other questions: 1. In the following equilibrium: NaCl(s) Na+(aq) + Cl–(aq), would adding more NaCl(s) increase the Cl-(aq) concentration? Explain why. My thoughts: I thought that it wouldn't increased
  57. Chemistry

    What will happen to the number of moles of SO3 in equilibrium with SO2 and O2 in the following reaction in each of the following cases? 2 SO3(g) equilibrium reaction arrow 2 SO2(g) + O2(g) ΔH° = 197 kJ (a) Oxygen gas is removed. increase decrease
  58. chemistry(Please check)

    1)Which thermochemical equation and data does not agree with the other two written? a) 2NO (g)+ O2 (g) ->2 NO2 (g) deltaH=-169.8 b) NO (g) + 1/2 O2 (g) -> NO2 (g) delta H = -56.6 c) 4 NO2 (g) -> 4 NO (g) + 2 O2 (g) delta H = +226.4 d)all three
  59. Chemistry

    Sulfur trioxide decomposes into sulfur dioxide and oxygen in an equilibrium. You have a 3.00 L vessel that is charged with 0.755 mol of SO3. At equilibrium, the amount of SO3 is 0.250 mol. 2 SO3 (g) ----> 2 SO2 (g) +O2 (g) A) calculate the equilibrium
  60. Analytical Chem

    Equilibrium involving SO2(g), O2(g) & SO3(g) is important in sulfuric acid production. When a 0.0200 mol sample of SO3 is introduced into an evacuated 1.52 L vessel at 900 K, 0.0142 mol, SO3 is found to be present at equilibrium. What is the value of Kp
  61. Chemistry

    For 2 SO2(g) + O2(g) equilibrium reaction arrow 2 SO3(g), Kp = 3.0 104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.21 g of SO3 and 0.183 g of O2. How many grams of SO2 are in the vessel?
  62. AP Chem

    NO2 + H2 <-> NO + H2O [H2] = .30 mol/L [NO2] = .20 mol/L [NO] = [H20] = .70 mol/L @ 1000K A. What is the mole fraction of NO in the equilibrium mixture? B. Calculate Kc C. Determine Kp in terms of Kc D. If system is cooled to a lower temperature, 35%
  63. chemistry

    How will the following system at equilibrium shift in each of the following cases? 2 SO3(g) <--> 2 SO2(g) + O2(g) H° = 197 kJ (a) SO2(g) is added (b) the pressure is decreased by increasing the volume of the container (c) the pressure is increased
  64. chemical equilibrium

    At a certain temperature, Kc = 0.914 for the reaction NO2 (g) + NO (g) <----> N2O (g) + O2 (g) Equal amounts of NO and NO2 are to be placed in a 5.00 L container until the N2O concentration at equilibrium is 0.050 M. How many moles of NO and NO2 must
  65. Chemistry

    Why is sulfur dioxide (SO2) a better reducing agent than carbon dioxide (CO2) or nitrogen dioxide (NO2)? I really don't know how to answer your question. It's much like asking why the sky is blue, etc. You can look up the reduction potentials of SO2 vs CO2
  66. Chemistry

    the reaction is CO + SO3 <=> CO2 + SO2, the rate law for this reaction is rate=k[SO3] and the mechanism is SO3 -> SO2 + O CO + O -> CO2 Which is the slow step? I have to find catalysts and intermediates and is O both catalyst and intermediate?
  67. Chemistry

    Consider the following reaction: 2 SO2 (g) + O2 (g)----> 2 SO3 (g) If 285.3 mL of SO2 is allowed to react with 158.9 mL of O2 (both measured at 315 K and 50.0 mmHg), what is the limiting reactant and theoretical yield of SO3 in moles? If 187.2 mL of SO3
  68. AP Chemistry

    At a certain temperature, the equilibrium constant Kc is 0.154 for the reaction 2SO2(g) + O2(g)<-> 2SO3(g) What concentration of SO3 would be in equilibrium with 0.250 moles of SO2 and 0.885 moles of O2 in a 1.00 liter container at this temperature?
  69. CHEMISTRY

    A chemist studying the equilibrium N2O4(g)<----->2NO2(g) controls the temperature so that keq ( equilibrium constant)= 0.028. At one equilibrium position, the concentration of N2O4 is 1.5 times greater than the concentration of NO2. Find the
  70. math

    how much oxygen is required to convert total so2 into so3 tell me the percentage ratio of so2:o2 the reaction is so2+1/2o2=so3
  71. Chemistry

    An equilibrium mixture at 852 K is found to contain 3.61 x 10^ - 3 mol/L SO3. Calculate the equililbrium , constant , keq for the reaction where SO2 an O2 are reactants and SO3 is the produce.
  72. chemistry

    What happens to the concentration of SO2(g) when the total pressure on the equilibrium reaction 2 SO2(g) + O2(g) <---> 2 SO3(g) is increased (by compression)? I thought it remained the same but that was incorrect.
  73. chemistry 112

    the formation of SO3 from so2 and o2 is an intermediate step in the manufacture of sulfuric acid, and it is also responsible for the acid rain phenomenon. the equilibrium constant Kp for the reaction is 0.13 at 830 degree celcius. in one experiment, 2.00
  74. chemistry

    6. Determine Keq for the reaction: 2 SO2 (g) + O2(g) 2 SO3(g), given that 1.00 x 10-2 moles of SO2 and 2.00 x 10-2 moles of O2 were placed in a 2.00L reaction chamber. The chamber contained 7.5 x 10-3 moles of SO3 when equilibrium was established at 727oC.
  75. Chemistry

    At 900 K the following reaction has Kp=0.345; 2 SO2(g) + O2 (g) -> 2 SO3 (g) In an equilibrium mixture the partial pressures of SO2 and O2 are 0.145 atm and 0.455 atm, respectively. What is the equilibrium partial pressure of SO3 in the mixture?
  76. Chemistry

    The following reaction is a step in the commercial production of sulfuric acid. 2SO2(g) + O2(g) 2SO3(g) The equilibrium constant is very high at room temperature, but the reaction is very slow. It must be run at high temperatures to achieve a reasonable
  77. Chemistry(Please check)

    For the reaction, 2 SO2(g) + O2(g) == 2 SO3(g), at 450.0 K (Kelvin) the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations, (SO3) = 0.254 M and (O2) = 0.00855 M, and (SO2) = 0.500 M. In which direction
  78. Chem 2

    The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4? N2O4(g) 2 NO2(g)
  79. chemistry

    The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4?      N2O4(g) 2 NO2(g)
  80. Chemistry

    Use the equations with the enthalpy information given below to calculate the ÄH° for the reaction: S(s) + O2(g) --> SO2(g) S(s) + 3/2 O2(g) --> SO3(g) ÄH° = -395kJ 2 SO2(g) + O2(g) --> 2 SO3(g) ÄH° = -198.2 kJ
  81. Chemistry

    I am having great difficulty with the following questions. Any and all help will be greatly appreciated. I have read the chapter and even looked up online tutorials. I still do not understand it. 2 NO (G) + O2 (G) > 2 NO2 (G) Write the equilibrium
  82. 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)
  83. Chemistry(Please help)

    For the reaction, 2 SO2(g) + O2(g) == 2 SO3(g), at 450.0 K (Kelvin) the equilibrium constant, Kc, has a value of 4.62. A system was charged to give these initial concentrations, (SO3) = 0.254 M and (O2) = 0.00855 M, and (SO2) = 0.500 M. In which direction
  84. Chemistry

    Consider the following mixture of SO2(g) and O2(g).If SO2(g) and O2(g) react to form SO3(g),draw a representation of the product mixture assuming the reaction goes to completion. What is the limiting reactant in the reaction? If 96.0 g of SO2 reacts with
  85. Pchem

    2 NO2(g) N2(g) + 2 O2(g) The ¥ÄH¡Æ for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if NO2 is added to the reaction mixture at constant temperature and volume? (Select all that apply.) And here's the options. The
  86. Equilibrium

    An equilibrium mixture at 852 K is found to contain 3.61*10^-3 mol/L of SO2, 6.11*10^-4 mol/L of O2, and 1.01*10^-2 mol/L of SO3. Calculate the equilibrium constant Keq, for the reaction where SO2 and O2 are reactants and SO3 is the product. Equation would
  87. Chemistry Equilibrium

    For the reaction NO2(g) + NO(g) N2O(g) + O2(g) Kc = 0.914. Equal amounts of NO and NO2 are to be placed into a 5.00 L container until the N2O concentration at equilibrium is 0.0446 M. How many moles each of NO and NO2 must be placed into the container?
  88. chemistry

    An equilibrium mixture of SO2,SO3 and O2 gases is maintained in a 11.5 L flask at a temp at which Kc=55.2 for the rxn shown below. If the number of moles of SO3 in the flask at equilibrium is twice the num of moles of SO2, how much O2 is present in the
  89. Chemistry

    2 NO(g) + O2 (g) <==> 2 NO2 (g) Given that Kp=7.96×1012 for the reaction above and the following starting conditions: Initial Concentrations p(NO)=0.775 atm p(NO2)=0.000 atm p(O2)=0.789 atm Determine the equilibrium concentration of NO2.
  90. 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
  91. Chemistry

    Consider this equilibrium: N2O4(g) + heat NO2(g). Initially, a 1.0 L container is filled with 2.0 mol of NO2. As the system approaches equilibrium, what happens to the rate of reaction of NO2 breaking down?
  92. Chemistry

    Consider this equilibrium: N2O4(g) + heat NO2(g). Initially, a 1.0 L container is filled with 2.0 mol of NO2. As the system approaches equilibrium, what happens to the rate of reaction of NO2 breaking down?
  93. Chemistry

    The reaction, 2 SO3(g) == 2 SO2(g) + O2(g) is endothermic. Predict what will happen if the temperature is increased. A. the pressure decreases B. more SO3(g) is produced C. Kc increases D. Kc decreases E. none of the above I chose that Kc will increase.
  94. Chemistry

    For 2 SO2(g) + O2(g) 2 SO3(g), Kp = 3.0 104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.58 g of SO3 and 0.136 g of O2. How many grams of SO2 are in the vessel?
  95. chemistry

    each of the following species except____, the electronic structure may be adequately described by 2 resonance formulas. NO2 C6H6 SO2 O3 SO3 -2charge
  96. Chemistry

    Sulfur dioxide reacts with oxygen to form sulfur trioxide according to the equation 2SO2(g) + O2(g) <-> 2SO3(g) Samples of sulfur dioxide, oxygen, and sulfur trioxide were added to a flask of volume 1.40 dm^3 and allowed to reach equilibrium at a
  97. chemistry

    A mixture of SO3,SO2 and O2 gases is maintained in 10litre flask at which the Kc for reaction is 100 . If number of moles of SO2 and SO3 are equal then how many moles of O2 present.
  98. chemistry

    Balance the equation: SO2 + NO2 → SO3 + NO im confused, isnt this already balanced since both sides have equal number of atoms
  99. "le Chat. Principle" #2

    Hi, there are 5 questions and I was wondering if you could check them for me. Thanks! 3. The hypothetical equilibrium reaction represented by the equation that follows. QA(s) + 2 X(g)>>>Q(l) + X2A(g) + energy This reaction can be shifted to
  100. Chemistry

    Given the reaction system; 2 NO (g) + O2 (g) -> 2 NO2 (g) Write a brief explanation for each of the following statements in terms of the collision model and/or reactions mechanisms. (1)Increasing the concentration of NO (g)makes the reaction go faster.