1. Chemistry 2

    If 2.0 mol of NO and 1.0 mol Cl2 are placed into a 1.0L flask, calculate the equilibrium concentrations of all species
  2. chemistry

    A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be ____ M.
  3. math

    rules find 1/4 of the input find 1/8 of the input input output 16 ___ 20 ____ 80 ____ 32 ____ 40 ____ 18 ____
  4. Organic Chemistry Lab

    a)If the Keq for the esterification of acetic acid with isopentyl alcohol is 3.0, what is the maximum amount of isopentyl acetate that can be recovered at equilibrium if a 1:1 mole ratio of alcohol was used? b)If a 1:5 mole ratio was used? c) 5:1 mole
  5. Chemistry

    Hydrogen iodide decomposes according to the following equation: H2(g) + I2(g) ⇌ 2HI(g) A 2.50 L equilibrium mixture contains 0.0875 mol H2, 0.020 mol I2, and 3.72 mol HI. Determine the new equilibrium concentrations after 1.25 mol HI are added to the
  6. chemistry

    What information does an equilibrium constant give about a reaction? A. It tells how long it takes the reaction to reach equilibrium. B. It tells how much energy is required for the reaction to happen. C. It tells what the rate constant of the reaction is
  7. science

    What information does an equilibrium constant give about a reaction? A. It tells how long it takes the reaction to reach equilibrium. B. It tells how much energy is required for the reaction to happen. C. It tells what the rate constant of the reaction is
  8. Chemistry

    Calculate the concentrations of Cd+2 , Cd(CN)4^-2 and CN at equilibrium when dissolvs 0.42 moles of Cd(NO3)2 (2.50 mol/L) Kf for Cd(NO3)2 = 7,1x10^16.
  9. Chemistry

    Calculate the concentrations of Cd ⁺ ², [Cd (CN)₄-²] and CN at equilibrium when they dissolve mole of 0.42 Cd (in the ₃)²⁺ 2.50 M. Given: Kf = 7, 1 x 10 ^16
  10. chemistry

    A 0.10-mol sample of H2(g) and a 0.10-mol sample of Br2(g) are placed in a 2.0-L container. The reaction H2(g) + Br2(g) <----> 2 HBr(g) is then allowed to come to equilibrium. A 0.20 mol sample of HBr is placed into a second 2.0-L sealed container at
  11. Chem

    The initial concentration for the compounds involved in the reaction displayed were determined to be [NO2(g)] = 1.243 mol/L, [N2O4(g)] = 0.2578 mol/L. Calculate the value of the equilibrium constant (Kc) at 500.0 K if the equilibrium concentration of
  12. 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
  13. Chemistry

    Hi Please help Initial [Fe3+] = 0.00050 M Initial [SCN-] = 0.0010 M Equilibrium [Fe(SCN)2+] = 5.7 x 10-5 Find [Fe3+]E and [SCN-]E (in mol/L) Find K. Balanced equation is: Fe3+ + SCN- -> Fe(SCN)2+ (reversible) I know I can get K if I have the equilibrium
  14. Physics (Fill in the Blanks)

    1. The last stage of a giant star is ____ 2. The path of a satellite is called ____ 3. The size of the Sun is the result of the "tug of war" between two opposing processes, nuclear fusion and ____ contraction Thanks :)
  15. chemistry

    2 HI(g)--><--H2(g) + I2(g) When a sufficiently large sample of HI(g) is introduced into an evacuated vessel at 643 K, the equilibrium concentration of I2(g) is found to be 0.248 M. Calculate the concentration of HI in the equilibrium mixture. M.
  16. Spanish 2

    Fill in the blank with the correct form of the present perfect. You do not need capital letters or accents for this. 1.) Los chicos_____hecho la tarea. 2.) Maria ____ ____ (limpiar) 3.) Usted ha ____(ver) la pelicula? 4.) Yo he ____(comer) los tacos. 5.)
  17. Chemistry

    What's the difference between the pressure of a system and the partial pressures in relation to Le Chatelier's principles? I know that when the pressure of the system is increased, it goes to the side with less moles/particles and when decreased it will go
  18. Chemistry

    At 25°C, K = 0.090 for the following reaction. H2O(g) + Cl2O(g) equilibrium reaction arrow 2 HOCl(g) Calculate the concentrations of all species at equilibrium for the following case. 1.3 mol pure HOCl is placed in a 1.6 L flask [HOCl]________
  19. CHEMISTRY

    An equilibrium mixture of the following reaction was found to have = 0.0325 at 1200 degrees C. What is the concentration of I? I2(g)<->2I (g) Keq=1.3×10−2 at 1200
  20. chemistry

    consider the following equilibrium. 4NH3(g) +3O2(g)<-> 2N2(g) + 6H2O(g) suppose 0.30mol of NH3 and 0.40mol of oxygen are added to a 5.0L container. If x mol of water is present at equilibrium, what is the equilibrium concentration of oxygen?
  21. English

    I would like to know if this grammatically correct. When there is change in reactant, product, and temperature the equilibrium position will shift in a direction that tends to decrease that change in situations. When the concentration of one of the
  22. science

    I posted this before but i realized i posted somethings that were wrong. mosquito larvae can tolerate extremely low dissolved oxygen concentrations, yet cannot survive at temperatures above 25 degrees celcius. how might you account for dissolved oxygen
  23. Chemistry

    At 25 °C, an aqueous solution has an equilibrium concentration of 0.00147 M for a generic cation, A (aq), and 0.000735 M for a generic anion, B2–(aq). What is the equilibrium constant, Ksp, of the generic salt A2B(s)?
  24. chem 12

    consider the following equilibrium 2NOCl(g)--- 2 NO(g) + Cl2(g) Initally 1.00 mol of NO and 1.00 mol of Cl2 are placed in a 5.00L container. Calculate the initial concentrations of NOCl, NO and Cl2 NO= 0.20 mol/L Cl2= 0.20 mol/l NOCl=0 At equilibrium it is
  25. chemistry abs spectrum and wavelength

    Hello, can someone please help me? I'm stuck on a question: I'm doing an analysis of the absorbance of FeSCN2+ at it's max wavelength (i.e. 450nm where abs=0.154)The species I used to make the solution tested were Fe(NO3)3, HNO3, and KSCN. Now, the
  26. Adding letters instead of numbers

    Is anybody smarter than a fifth grader on this problem? I'm not able to help my son with this homework problem. e g g + e g g --------- p a g e a=____ e=____ g=____ p=_1___ How we started: p = 1, and g is greater than 5. Thanks!
  27. chemistry-electrochem

    Determine the equilibrium constant, Keq, for the reaction 5.3 10–19 18.30 1.7 1054 1.9 1018 5.7 10–55 this is an assignment question- as writen, no values, nothing. any help
  28. Physical Chemistry

    A 100 amino acid folded protein (F) is in equilibrium with it’s unfolded (U) (or denatured) form. Let ΔrH(std) =+347 kJ mol-1 and ΔrS(std) =-1010 J K-1 mol-1 for the equilibrium (F U) at 25℃. (a) Calculate the concentration of protein in
  29. chemistry

    at 327 degrees C, the equilibrium concentrations are [CH3OH]=0.15M, [CO]=0.24M, and [H2]=1.1M for the reaction: CH3OH(g)<-->CO(g)+2H2(g) Calculate Kp at this temperature
  30. Math 7 - Dividng and Multiplying Integers

    Find the missing integer for each problem. 1. +18 / ____ = -9 2. ___ / -5 = -6 3. -24 / ____ = +2 4. +18 / ____ = -3 / = dividing My Answers: 1. -2 2. +30 3. +12 4. -6 Are my answers are correct???? Please answer! Thank You! :)
  31. health safety and nutrition

    The mineral ____ and vitamins ____ and ____ regulate bone and tooth formation. A) calcium, K, E B) iron, A, D C) magnesium, C, B12 D) calcium, A, D
  32. 3rd grade math

    write the missing fraction or mixed number for each number line 0,1/3,2/3,1,____,____,____,______,2 1/3 3
  33. Chemistry

    Using the concentration of CH3COOH (0.8326M) and the equilibrium concentration of H3O+ (3.2x10-3), complete the reaction table for vinegar. Then calculate the acidity constant. Reaction table is given Ch3COOH + H2O --CH3COO- + H3O+ Initial. Change
  34. chemistry

    I keep getting the wrong answer for this one can someone help. The initial concentration for the compounds involved in the reaction displayed were determined to be [NOCl(g)] = 0.1738 mol/L, [NO(g)] = 0.1991 mol/L, [Cl2(g)] = 0.000005938 mol/L. Calculate
  35. 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
  36. Chemistry

    If the pH of a solution is 6, what are the hydrogen- and hydroxide-ion concentrations? The PH of a 0.1 M MCl (M+ is an unknown cation) was found to be 4.7. Write the net ionic equation for the hydrolysis of M+ and its corresponding equilibrium expression
  37. Chemistry

    I posted this last night, A 0.500L vessel initially contains 0.0125 mol of H2S2 . Find the equilibrium concentrations of H2 and S2. Kc = 1.67 x 10^-7 2 H2S <--> 2 H2 + S2 I have come up with this equation so far, but I am lost now because I don’t
  38. chemistry

    what is the equilibrium concentration of acetate ion if the equilibrium concentration of acetic acid is .40 M, the pH is 3.85, and Ka is 1.8E-05?
  39. Chemistry

    I'm having trouble with the following question, any help would be greatly appreciated. A voltaic cell consists of a Zn/Zn^2+ half-cell and a Ni/Ni^2+ half-cell at 25 C . The initial concentrations of Ni^2+ and Zn^2+ are 1.30 M and 0.100 M , respectively.
  40. 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
  41. chemistry

    If 1.00 mol of iodine and 0.50 mol of chlorine are initially placed into a 2.00 L reaction vessel at 25 degrees celsius, find the concentrations of all entities at equilibrium
  42. Chemistry

    Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 723.0 K: [N2(g)] = 2.936 mol/L, [H2(g)] = 2.933 mol/L, [NH3(g)] = 3.443 mol/L. N2(g)+3H2(g) = 2NH3(g)
  43. chemistry

    23) The equilibrium constant for the gas phase reaction 2NH3 (g) <-> N2 (g) + 3H2 (g) is Keq = 230 at 300 °C. At equilibrium, __________. A) reactants predominate B) products predominate C) only products are present D) roughly equal amounts of
  44. chemistry

    Using the concentration of CH3COOH (0.8326M) and the equilibrium concentration of H3O+ (OJ = 31.6x10^-6 and milk = 3.16x10^-8), complete the reaction table for vinegar. Then calculate the acidity constant. Please show all work in solving the problem.
  45. Chemistry

    A 0.170-mole quantity of CoCl2 is added to a liter of 1.20 M NH3 solution. What is the concentration of Co2 ions at equilibrium? Assume the formation constant (Kf) of Co(NH3)62 is 5.0× 1031 M–6. I don't really know how to start. At first I thought about
  46. Spanish 1

    5. No, ____ me gusta ir a la escuela a. nada b. no c. pues d. ni B? 9. No me gusta ____ nadar ____ dibujar. a. si/si b. si/ni c. ni/ni d. ni/tampoco D? Thanks -MC
  47. Chem

    I am having problems with these two questions. 1.The value of the equilibrium constant (Kp) as represented by the first chemical equation is 1.58 x 102 at 727 °C. Calculate the value of the equilibrium constant (Kp) for the second equation at the same
  48. General Chemisty

    3. Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 723.0 K: [N2(g)] = 2.936 mol/L, [H2(g)] = 2.933 mol/L, [NH3(g)] = 3.443 mol/L. N2(g)+3H2(g) = 2NH3(g)
  49. MATH

    PLEASE EXPLAIN HOW TO FIND THE COMMON RATIO FOR THE GEOMETRIC SEQUENCE 16, 40. 100,____, ____ AND 81,54, ______,______,______
  50. chem 12

    2H2S(g)---2H2(g) + S2 delta H=220KJ k eq is 0.40 a 10.0L vessel containing 2.0 mol of H2S, 2.2 mol of H2, and 2.5 mol of S2 Calculate a trail k eq value to see whether the reaction is at equilibrium. trail k eq =(h2)^2(S2)/(H2S)^2 = (0.22)^2(0.25)/(0.2)^2
  51. chem 12

    2H2S(g)---2H2(g) + S2 delta H=220KJ k eq is 0.40 a 10.0L vessel containing 2.0 mol of H2S, 2.2 mol of H2, and 2.5 mol of S2 Calculate a trail k eq value to see whether the reaction is at equilibrium. trail k eq =(h2)^2(S2)/(H2S)^2 = (0.22)^2(0.25)/(0.2)^2
  52. Biochemistry

    1. Given the following equation: Glycerol-3-phosphate glycerol + Pi Go’ = -9.7 kJ/mol At equilibrium the concentrations of both glycerol and inorganic phosphate are 1 mM. Under these conditions, calculate the final concentration of glycerol-3-phosphate.
  53. chemistry

    Gaseous CO2 decomposes to form the gaes CO and O2. At 20.0 degrees Celsius, =2.0*10^-8. 2.0 mol carbon dioxide is placed in a 5.0 L flask. What are the equilibrium concentrations of each species. My attempt to get the answer: Balanced equation: 2CO2-->
  54. English

    A(n) ____ will be sent to all our representatives in Latin AMerica advising them how to handle the problem ingenious? Some of lifes rewards are ____ others are a long time coming instantaneous None of us could figure out how the ____ magician had managed
  55. College Chemistry

    The initial concentration for the compounds involved in the reaction shown were determined to be [CH4(g)] = 0.6616 mol/L, [H2O(g)] = 0.8127 mol/L, [CO(g)] = 0.9566 mol/L, [H2(g)] = 0.7688 mol/L. Calculate the value of the equilibrium constant (Kc) at 1200
  56. chemistry

    A diprotic acid solution H2A has a molarity of .95 M. the concentrations of the species present at equilibrium are as follows: [H+] = .25 M, [HA-]=.25M, [A^2-] =4.6x10^-4 M. what are the first and second ionization constants for this acid?
  57. biology,chemistry,physics

    the contact process prepares purest form of sulphuric acid 2so2+o2=2so3 calculate its kp if following concentrations are found at equilibrium so2=0.59,o2=0.05 and so3=0.259
  58. Chemistry

    How do I calculate the amount of grams of Na2HPO4 and NaH2PO4 to prepare 200 mL of a buffer with an 8.25 pH so the sum of the concentrations of HPO4 and H2PO4 ions is 0.5 M? Does this involve writing a Ka expression and equilibrium? I am confused and
  59. Chemistry

    How do I calculate the amount of grams of Na2HPO4 and NaH2PO4 to prepare 200 mL of a buffer with an 8.25 pH so the sum of the concentrations of HPO4 and H2PO4 ions is 0.5 M? Does this involve writing a Ka expression and equilibrium? I am confused and
  60. a level chemistry

    two most abundant atmospheric gases react to a small extent at 298K in the presence of a catalyst to achieve dynamic equilibrium: N2(g) + O2(g) ->/<- 2NO(g) Kp= 0.30 Partial pressure of N2 and O2 = 0.78atm 1dm3 flask and equilibrium established after
  61. chemistry abs spectrum and wavelength analysis

    Hello, can someone please help me? I'm stuck on a question: I'm doing an analysis of the absorbance of FeSCN2+ at it's max wavelength (i.e. 450nm where abs=0.154)The species I used to make the solution tested were Fe(NO3)3, HNO3, and KSCN. Now, the
  62. physics

    Two ropes pull on a ring. One exerts a 63 N force at 30.0°, the other a 63 N force at 60.0° (a) What is the net force on the ring? Magnitude ____ N Direction ____ ° (b) What are the magnitude and direction of the force that would cause the ring to be in
  63. Chemistry

    the equilibrium constant Kc for the reaction H2 + Co2 to H2O + CO is 4.2 t 1650°C initially .80 mol of H2 and 0.8 mol Co2 are injected into a 5.0 flask. Calculate the concentration of each species at equilibrium
  64. Equilibrium constant

    Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A solution is made containing initial [SO2Cl2]= 0.022M . At equilibrium, [Cl2]= 1.7×10−2M Calculate the value of the equilibrium constant.
  65. chemistry

    Carbon monoxide gas and hydrogen gas are mixed in a two liter flask. The reaction produces methanol gas as the only product. At equilibrium the Keq is 1.1 x 10-5. The flask initially held 6 grams of hydrogen and the equilibrium concentration of hydrogen is
  66. Chemistry

    Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 1200 K: [Br2(g)] = 0.0001151 mol/L, [Br(g)] = 0.00004423 mol/L. Br2(g) = 2Br(g)
  67. Chemistry

    Calculate [Fe^2]+ when the cell reaction reaches equilibrium? A voltaic cell is constructed based on the following reaction and initial concentrations: Fe^2+,( 0.0055 M ) + Ag+,( 2.5 M ) ----> Fe^3+,( 0.0055 M ) + Ag(s) Calculate [Fe^2]+ when the cell
  68. 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
  69. Algebra

    What is the pattern for the next three numbers for -1, 2, -4, 8 ____, ____, ____? Thanks!
  70. Math

    Fill in the blanks. 56 ÷ 7 = ____ ones ÷ 7 = ____ ones = ____
  71. Algebra help please

    Simplify I am using parenthesis to separate , if i write the whole prob as is, it runs together a + 9 (3a - 18) _____ ________ 36 - a^2 (3a + 27) possible answers i can choose from 1 ____ a + 6 1 ____ a - 6 - 1 ____ a - 6 - 1 ___ a + 6 I am thinking it is
  72. Chemistry

    Dinitrogen tetraoxide decomposes to give nitrogen dioxide. Calculate the equilibrium concentration of NO2 at 100oC if the equilibrium constant is 0.200 and [N2O4] = 0.800M. N2O4(g) ¡ê 2 NO2(g)
  73. CHEMISTRY

    Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) Qc
  74. CHEMISTRY

    Method for getting correct answer? Thank you! Initially there were equilibrium concentrations of 0.1887 M A, 0.1042 M B. Which of the equations below is correct if the pressure decreased by a factor of 2.40? Use the reaction below. 6A(g) ↔ 5 B(g) a.
  75. 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.
  76. Chemistry

    Zinc, copper, lead, and mercury ions are toxic to Atlantic salmon at concentrations of 6.42 × 10–2 mM, 7.16 × 10–3 mM, 0.965 mM, and 5.00 × 10–2 mM, respectively. What are the corresponding concentrations in milligrams per liter? Concentration of
  77. chemistry

    the equilibrium constant for the synthesis of HBr(g0 from hydrogen and bromine gas is 2.18*10 exponent 6 at 730 degrees celcius.if 3.75 mol of HBr(g) is put into a 15L reaction vessel,calculate the concentration of H2,Br2 and HBr at equilibrium
  78. chemistry

    a chemist puts 6 moles of nitrogen gas and 7 moles hydrogen gas into an evacuated 1 liter container. The system reaches equilibrium at a certain temperature according to the process outlined above. when the system is at equilibrium the chemist determines
  79. 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
  80. 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
  81. Chemistry

    For a reversible reaction where A + B (both arrows) C + D, the equilibrium constant is represented by kc = 5.3 = (c)(d)/(A)[B]. Initially A and B are present at 2.00 M each. What is the final concentration of A once equilibrium is reached. I made an ICE
  82. English

    1.the trip led to an argument between Helen and ____ a.I b.me 2. It was ____ who demanded an apology from the newspaper. a.we b.us 3. We appreciated ____ writing a personal letter to explain his stand on the issue. a.his b.him 4. The most outspoken critics
  83. 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
  84. 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
  85. CHEMISTRY HELP!

    Consider the following reactions and their equilibrium constants. (NO(g) + 0.5Br2(g) <===> NOBr(g) Kp = 5.3 2NO(g) <===> N2(g) + O2(g) Kp = 2.1 x 1030 Use these equations and their equilibrium constants to determine the equilibrium constant for
  86. Chemistry

    Bromine and chlorine gas react to give bromine monochloride (BrCl) according to Br2(g)+Cl2(g)⇌2BrCl(g) Given initial concentrations [Br2]=1.50 mol L-1, [Cl2]=0.90 mol L-1 and [BrCl]=0 and K=7 determine (to two decimal places) the equilibrium
  87. Chem Class

    The equilibrium constant for reaction 1 is K.....? how do i figure out problems like this? do i check which ones cancel out? The equilibrium constant for reaction 1 is K. The equilibrium constant for reaction 2 is ___? (1) SO2 (g) + (1/2) O2 (g) (right and
  88. 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.
  89. 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
  90. chemistry

    is there any way to know if its products or reactants..? The equilibrium constant for the gas phase reaction N2 (g) + 3H2 (g) (2 arrows: one to right, one to left.) 2NH3 (g) is Keq = 4.34 × 10^-3 at 300°C. At equilibrium, __________. A) reactants
  91. Chemistry

    Did I answer this equilibrium question correctly? 2CO(g) + O2(g) <-> 2CO2(g) 1) How will increasing the concentration of CO shift the equilibrium? a] to the right [i chose this] b] to the left c] no effect 2] how will increasing the concentration of
  92. chemistry

    Suppose you have the following reaction at equilibrium: N2(g) + 3H2(g) = 2NH3(g), ΔH = −22 kcal/mol What changes are expected to occur if the temperature of the system was decreased. You may select multiple answers. The concentration of NH3(g)
  93. chemistry

    Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?
  94. chemistry

    Calculate each of these equilibrium concentrations based on the reaction below. 2 NO(g) + O2(g) 2 NO2(g) K = 1.71 1012 (a) [NO] = 0.0048 M; [O2] = 0.000057 M; [NO2] = ? (b) [NO] = 0.0026 M; [O2] = 0.000023 M; [NO2] = ?
  95. 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
  96. 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.
  97. chemistry

    Malic acid is a weak diprotic organic acid with K1 = 4.0x 10-4 and K2 = 9.0 x 10-6. (a) Letting the symbol H2A represent malic acid, write the chemical equations that represent K1 and K2 . Write the chemical equation that represents K] xK2 . (b)
  98. Chemistry Class

    Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g) <- A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol ofN2O4 remains. Keq for this reaction is ?. hOw can i set
  99. Chemistry

    Consider the following equilibrium: At equilibrium, 4.0 × 10-2mol H2, 4.0 × 10-2mol CO, 1.0 × 10-2mol H2O and 1.0 × 10-2mol C were present in a 1.0L container. What is the value of Keq? a) 0.063 b) 16 c) 0.16 d) 6.3 I got b, but I'm not too certain
  100. AP Chem

    At a particular temperature, K = 1.00 102 for the following reaction. H2(g) + I2(g) 2 HI(g) In an experiment, 1.23 mol H2, 1.23 mol I2, and 1.23 mol HI are introduced into a 1.00 L container. Calculate the concentrations of all species when equilibrium is