For a reaction that has an equilibrium constant of 9 × 10–9, which of the following statements must be true? A) ∆G° is positive. B) ∆G° is negative. C) ∆H° is negative. D) ∆H° is positive. E) ∆S° is positive

33,523 results
  1. Chemistry chemical equilibrium

    1.25 mol of NOCl was placed in a 2.50 L reaction chamber at 427 celciciu degre . After equilibrium was reached, 1.1 mole of NOCl remained. Calculate the equilibrium constant Kc for the reaction

  2. Chemistry

    The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium and will remain in an un

  3. AP Chemistry

    For the system 2SO2(g) + O2(g) 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L container. The system is allowed to

  4. chemistry

    Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change D. Increase the value of

  5. 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

  6. Chemistry

    Given the two reactions 1.PbCl2 Pb^2+ + 2 Cl^-, K1= 1.82×10^−10 2. AgCl Ag^+ + Cl^-, K2 = 1.15×10−4 what is the equilibrium constant Kfinal for the following reaction? PbCl2+ 2 Ag^+ 2AgCl+ Pb^2+ This is what i have soo far: PbCl2Pb2+ + 2Cl- K1=

  7. 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)

  8. 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 heated to

  9. chemistry

    How is the reaction quotient used to determine whether a system is at equilibrium? The reaction is at equilibrium when Q > Keq. At equilibrium, the reaction quotient is undefined. The reaction quotient must be satisfied for equilibrium to be achieved. The

  10. Chemistry

    The equilibrium constant, Kc is 3.2 x10 -34 at 25C for the reaction 2 HCl(g) H2(g) + Cl2(g). what is The equilibrium expression, Kc for the reaction

  11. Chemistry

    Which of the following statements is true regarding the dissolution of a salt in a solvent? A. Precipitates are included in the equilibrium constant. B. An equilibrium constant can be describes that is the product of the concentrations of the ions to the

  12. chemistry

    Which of the following statements is not true? 1.Chemical equilibria are examples of reversible processes. 2.When multiple reaction steps are in equilibrium, then the equilibrium constant for the net reaction is the product of the individual reactions.

  13. Chemistry

    In the industrial synthesis of ammonia, the equilibrium constant expression may be written as: Keq= [NH3]^2/[N2][H2]^3 Calculate the value of this equilibrium constant, if the equilibrium concentration of nitrogen in the reaction mixture at 600°C if [N2]

  14. chemistry

    For the reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), removing some of the product, Fe3O4(s), would: Answer A. Increase the value of the equilibrium constant, K B. No change C. Decrease the value of the equilibrium constant, K D. Shift the

  15. Chemistry

    If the reaction SO2(g) +0.5O2(g) SO3(g) has the equilibrium constant Kc =56, then what is the Kc value for the following reaction? 2SO3 (g) 2SO2 (g) + O2(g) A. -112 B. 3.2 * 10^-4 C. 56 D. 8.9*10^-3 I think the answer would be C because the amount of

  16. chem

    a.) At equilibrium, the molar concentrations for reactants and products are found to be [I2] = 0.50 M,[Cl2] = 0.60 M, and [ICl] = 5.0 M. What is the equilibrium constant (Kc) for this reaction? b.) The concentration of I2 is increased to 1.5 M, disrupting

  17. Chemistry

    For the reaction 2NH3(g) 3H2(g) N2(g) at 472oC equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37x10^_8 M. What is the equilibrium constant for the reverse reaction?

  18. chemistry

    For the following reaction, 2SO3(g) = 2SO2(g) + O2(g), the equilibrium constant, Kp, is 1.32 at 627 degrees Celsius. What is the equilibrium constant for the reaction: SO3(g) = SO2(g)+ 1/2 O2(g)

  19. Chemistry

    The reaction of iron and water vapor results in an equilibrium reaction, 3 Fe(s) + 4 H2O(g) ¡ê Fe3O4(s) + 4 H2(g) and an equilibrium constant of 4.6 at 850¡ÆC. What is the concentration of Hydrogen present at equilibrium if the reaction is initiated

  20. chemistry

    For the reaction 2CO(g)+O2 《=》2CO2 with equilibrium constant Kc. Suppose the equation is rewritten as CO + 1/2O2 《=》CO2 with an equilibrium constant Kc'.what is the relationship between Kc and Kc'

  21. Chemistry

    An aqueous solution of 0.25 M silver nitrate, AgNO3, and 0.25 M iron(II) nitrate, Fe(NO3)2, are allowed to come to equilibrium in the following chemical reaction: Ag+(aq) + Fe2+(aq) Fe3 + (aq) + Ag(s) If the equilibrium constant, Kc, for the reaction is

  22. Chemistry

    Which of the following statements is true regarding the dissolution of a salt in a solvent? A. Precipitates are included in the equilibrium constant. B. An equilibrium constant can be describes that is the product of the concentrations of the ions to the

  23. Science

    The following reaction: 2SO3 (g) ! 2SO2 (g) + O2 (g) has an equilibrium constant equal to 0.23 M. If the following concentrations are present: [SO2] =0.480 M, [O2] = 0.561 M, [SO3] = 0.220 M, is the reaction at equilibrium? If not, which way must it shift

  24. Chemistry

    Consider the following reaction: CO(g)+2H2(g)⇌CH3OH(g) This reaction is carried out at a specific temperature with initial concentrations of [CO] = 0.27 M and [H2] = 0.49 M. At equilibrium, the concentration of CH3OH is 0.11 M. Find the equilibrium

  25. chem

    Given the concentrations, calculate the equilibrium constant for this reaction: I2(g) + Cl2(g)---> 2ICl(g) At equilibrium, the molar concentrations for reactants and products are found to be I2 = 0.50M, Cl2 = 0.60M, and ICl = 5.0M. What is the equilibrium

  26. Chemistry

    One enzyme- catalyzed reaction in a biochemical cycle has an equilibrium constant (K1) that is 10 times the equilibrium constant (K2) of a second reaction. If the standard Gibbs energy of the former reaction is - 300 kJ mol-1, what is the standard reaction

  27. Chemistry

    At a given temperature, the elementary reaction A B in the forward direction is first order in A with a rate constant of 2.60 x 10^-2 s^-1. The reverse reaction is first order in B and the rate constant is 8.50 x 10^-2 s^-1. What is the value of the

  28. chem

    When the concentration of I2 is increased to 1.5 M, the ratio of products to reactants is 28. The equilibrium constant for the reaction is 83. In which direction will the reaction shift to regain equilibrium?

  29. science

    For the reaction mc011-1.jpg at 472°C equilibrium is established when [H2] =0.0200M, [N2] = 0.0100M and [NH3] = 5.37 x 10-8M. What is the equilibrium constant for this reaction

  30. Chem II

    The equilibrium constant of a reaction is 12.6. If the rate constant of the reverse reaction is 5.1 x 10 -2 the rate constant for the forward reaction is _____ 0.32 0.16 0.64 0.08 I don't even know where to start on this question. Any direction will help

  31. Chemistry

    The equilibrium constant, Keq, is defined as the ratio of the concentrations of products to reactants. What is the equilibrium constant for the following reaction: ClNO2 (g) + NO (g) ↔ NO2 (g) + ClNO (g)

  32. Chemistry

    The equilibrium constant for the reaction H2 + I2 --> 2HI, is 54 at 425 degrees C. If the equilibrium mixture contains 0.030 M HI and 0.015 M I2, calculate the equilibrium concentration of H2.

  33. 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

  34. 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

  35. chm

    The equilibrium constant for the equation 2 H2(g) + CO(g) CH3OH(g) Is 19 at a certain temperature. If there are 3.11 x 10-2 moles of H2 and 5.79 x 10-3 moles of CH3OH at equilibrium in a 6.75 L flask. What is the concentration of CO? At 1280 °C the

  36. 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

  37. chemistry

    Which of the following can we predict from an equilibrium constant for a reaction? 1 The extent of a reaction 2 Whether the reaction is fast or slow 3 Whether a reaction is exothermic or endothermic a. 1 only b. 2 only c. 3 only d. 1 and 2 only e. 1 and 3

  38. Chemistry

    If the equilibrium constant for a particular chemical reaction is 1 x 10^-3, what does this tell us? A. At equilibrium, there are more products than reactants. B. At equilibrium, there are more reactants than products. C. At equilibrium, there are 1 x

  39. 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.

  40. Chemistry

    SO this is my first time doing this... lol i need help on an AP chemistry question for equilibrium. A 0.500 L tank contains 3.00 g of NO(g) at 750. K. The equilibrium constant for the reaction below at this temperature is 3.4 x 10 -3 2NO(g) ⇌ N2(g) +

  41. 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

  42. 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

  43. Chemistry

    Consider the reaction HCHO(g) *) H2(g) + CO(g). 1.0 mol of HCHO, 1.0 mol of H2 and 1.0 mol of CO exist in equilibrium in a 2.0 L reaction vessel at 600C. a) Determine the value of the equilibrium constant Kc for this system. 2.0 moles of HCHO and 1.0 mol

  44. 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

  45. Chemistory

    The reaction has an equilibrium constant of = 0.154. If 6.60 of , 4.30 of , and 11.60 of are added to a reaction vessel with a volume of 5.30 , what net reaction will occur? A-The reaction will proceed to the left to establish equilibrium. B-The reaction

  46. 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. Suppose the feed

  47. 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 constant

  48. Idontgetit

    The value of the equilibrium constant, Kc, at a certain temperature is 2.50 x 102. If the reaction quotient for a mixture of these species at the same temperature is found to be 7.37 x 100, would the mixture yield more products, more reactants or is it at

  49. 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

  50. Idontgetit

    The value of the equilibrium constant, Kc, at a certain temperature is 2.56 x 10-1. If the reaction quotient for a mixture of these species at the same temperature is found to be 9.90 x 10-4, would the mixture yield more products, more reactants or is it

  51. Idontgetit

    The value of the equilibrium constant, Kc, at a certain temperature is 2.56 x 10-1. If the reaction quotient for a mixture of these species at the same temperature is found to be 9.90 x 10-4, would the mixture yield more products, more reactants or is it

  52. chemistry

    given the equilibrium constant for the following reaction at 500 K, 2 NO (g) + O2 (g) 2 NO2 (g) Kc = 6.2x10^5 calculate the equilibrium constant for the reaction expressed as partial pressures, Kp. the answer is 1.51x10^4. How do i get this?

  53. Chemistry

    At 2000°C the equilibrium constant for the reaction is Kc = 2.4 ✕ 103. 2 NO(g) equilibrium reaction arrow N2(g) + O2(g) If the initial concentration of NO is 0.160 M, what are the equilibrium concentrations of NO, N2, and O2? I do not even know how to

  54. Chemistry(Please check answer)

    The equilibrium constant for the reaction, H2(g) + I2(g) == 2 HI(g) is 54.9 at 699.0 K (Kelvin). What is the equilibrium constant for 4 HI(g) == 2 H2(g) + 2 I2(g) under the same conditions? Note: the == indicates the equilibrium double arrow Since the

  55. Chemistry

    Use the data in the table to calculate the equilibrium constant for the following reaction. HCOOH(aq)+ OH −(aq) equilibrium reaction arrow HCOO−(aq)+ H2O(l) HCOO is 5.9e-11 (Kb) HCOOH is 1.7e-4 (Ka) Not sure how to find the equilibrium constant given

  56. CHEMISTRY

    the equilibrium composition of a reaction is 1.522mol CO, 1.566mol H2, 0.478mol CH4 and 0.478mol H2O and the volume of the reaction vessel is 10Litres. -What is the equation for the reaction? -Calculate the equilibrium constant for both the forward and

  57. 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

  58. Chemistry

    A chemist trying to synthesize a particular compound attempts two different synthesis reactions. The equilibrium constants for the two reactions are 23.3 and 2.2 X 10^4 at room temp. However, after 15minutes the chemist finds that the reaction with the

  59. chemistry

    I am given the following reaction: 2NH3(g) -------> N2(g) + 3H2(g) My question is: 6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium mixture

  60. chemistry

    I am given the following reaction: 2NH3(g) -------> N2(g) + 3H2(g) My question is: 6.4 mols of ammonia gas has been put into a 1.7 L flask and has been permitted to reach equilibrium in accordance to the reaction listed above. If the equilibrium mixture

  61. chemistry

    What effect does raising the temperature of the reaction chamber at a constant pressure have on the following reaction at equilibrium? 2NO2(g) N2O4(g) + heat A. The equilibrium shifts toward the reactants because the reverse reaction is endothermic. B. The

  62. Chemistry 3A

    An aqueous solution contains the ions B, C, and D that are in equilibrium with one another according to the reaction B (aq) + C (aq) ->/

  63. Chemistry

    Cu(s) | Cu2+(0.10M) || H+ (0.20M), MnO4-(0.35M), Mn2+(0.15M) | C(s) Determine the cell potential. ii. Is this reaction spontaneous? Prove using ∆G. iii. The equilibrium constant can also be found from Standard Cell Potentials. Eventually the cell will

  64. Chemistry

    . The reaction of iron and water vapor results in an equilibrium reaction, 3 Fe(s) + 4 H2O(g) Fe3O4(s) + 4 H2(g) and an equilibrium constant of 4.6 at 850 degree C. What is the concentration of water present at equilibrium if the reaction is initiated with

  65. Chemistry

    Ka for a weak acid HA = 3.46x10^-8, calculate K for the reaction of HA with OH- HA + OH- = A- + H2O This is an equilibrium question, but I do not understand how to find the equilibrium constant K, from the equilibrium constant of an acid, Ka

  66. Chemistry

    8. For the reaction H2(g)+I2(g)„\2HI(g); [H2] = 0.95 M; [I2] = 0.78 M; [HI] = 0.27 M. Calculate the equilibrium constant K and describe the direction (forward or reverse) of the reaction. Will adding a catalyst to the reaction alter the direction of the

  67. chem

    Reaction H2 +I2 yields 2HI All three gases are initially at 0.1atm/ upon reaching equilibrium it is found that H2 pressure droped by 55% what is the equilibrium constant for this reaction.

  68. chemistry

    Equilibrium constant K for some reaction at temperature 300K was found to be 100 .Calculate equilibrium for same reaction at 400K if R= 8.23 change in enthalpy is 5000J

  69. Chemistry

    Consider the reaction 2 SO2 + O2 in equilibrium with 2 SO3 . At 25°C Ho = -197.78 kJ and So = -187.95 J/K. Using this information, calculate the equilibrium constant for the reaction at 50°C. (R = 8.314 J/K) Enter your answer using TWO significant

  70. 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

  71. chemistry

    For the reaction 2CO(g)+O2 《=》2CO2 with equilibrium constant Kc. Suppose the equation is rewritten as CO + 1/2O2 《=》CO2 with an equilibrium constant Kc'.what is the relationship between Kc and Kc'

  72. chemistry

    Determine the expression for the equilibrium constant for this equilibrium reaction: 2NO(g) + 2CO(g) (arrows)(in equilibrium with) N2(g) + 2CO2(g) PLease help anyone i really apreciate it Beccy

  73. Chem, help please

    Consider the reaction N2 + 3H2 in equilibrium with 2 NH3 . At 25°C Ho = -92.22 kJ and So = -198.53 J/K. Using this information, calculate the equilibrium constant for the reaction at 226°C. (R = 8.314 J/K) Enter your answer using TWO significant figures.

  74. chemistry

    The equilibrium constant Kc for the reaction C D + E is 7.90 * 10^-5. The initial composition of the reaction mixture is [C]=[D]=[E]=1.10*10^-3. What is the equilibrium concentrations of C, D, and E? C=? D=? E=?

  75. chemistry... HELPP

    Chemistry Equilibrium Constant PLEASE Help!? In an experiment, equal volumes of 0.00150 M FeCl3 and 0.00150 M NaSCN were mixed together and reacted according to the equation: Fe3+ (aq) + SCN– (aq) Fe(SCN)2+ (aq) The equilibrium concentration of FeSCN

  76. chem

    1) If more reactant is added to a gaseous reaction at equilibrium, what will happen to the value of the equilibrium constant? a. it will increase b. it will decrease c. it will remain the same d. it can either increase or decrease 2) Which of the following

  77. science

    When Q < K, what can you conclude about the reaction? A. The reaction is not yet at equilibrium, and the reaction will proceed in the forward direction. B. The reaction is not yet at equilibrium, but the direction of the reaction must be experimentally

  78. chemistry

    We have the following equilibrium: 2 A(aq) ⇄ B(aq). At equilibrium we measure [A] = 0.056 M and [B] = 0.21 M. Calculate the equilibrium constant for the reaction as written.

  79. chemistry

    For the reaction 2A(g) + B(aq) + 3C(l) D(s) + 3E(g), the concentrations at equilibrium are found to be: A: 2.3x10^3 Pa B: 1.8x10^-2 M C: 15.8M D: 12.5M E: 5.6x10^4 Torr Find the numerical value of the equilibrium constant that would appear in a

  80. chemistry

    the equilibrium constant is the ration of product concentration to reactant concentration at equilibrium. a reaction will likely go to completion if the equilibrium constant is what?

  81. chemistry

    If the equilibrium constant for the conversion of isobutane to n-butane is 2.5 what is the value of the equilibrium constant for the reverese reaction?

  82. Chem -Bob Pursley Please Help!

    Consider the following reaction: 2 HI (g) → H2 (g) + I2 (g) Assume that an experiment is carried out in which the starting concentration of HI (g) is 0.100 mol/L. No products are present at the beginning of the reaction. When equilibrium is established,

  83. 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

  84. chemistry

    A classic experiment in equilibrium studies dating from 1862 involved the reaction in solution of ethanol and acetic acid to produce ethyl acetate and water. The reaction can be followed by analyzing the equilibrium mixture for its acetic acid content. In

  85. Chemistry

    1. The equilibrium constant of the balance reaction below is 1.6 x 10-2 at 25 oC and 2.7 x 10-5 at 125 oC. AB (g) + C (g)  3D (g) Which of the following is wrong for this reaction? a) Adding catalyst does not change the equilibrium constant of the

  86. chemistry

    The following reaction: SO2 (g) SO3 (g) + NO (g) having reached a state of equilibrium, was found to contain 0.40 M SO3, 0.30 M NO, 0.15 M NO2, and 0.20 M SO2. Calculate the equilibrium constant for this reaction. Describe the direction ad extent of a

  87. Chemistry

    If the equilibrium constant for a reaction A + B C + D is K, which is true of the equilibrium constant K* for the reaction C + D A + B under the same conditions? A) K* = K B) K* = 1/K C) K* = 1 - K D) K* = 1 - (1/K) E) K* = 1 + K

  88. chem

    What is constant about the equilibrium constant? A. The reversibility of the reaction at equilibrium is constant. B. The ratio of products to reactants at equilibrium is constant. C. The concentrations of products present at equilibrium are constant. D.

  89. chemistry

    Choose all of the following statements about the equilibrium constant K that are true: (a) If the K value for a reaction is > 1 then Go must be negative for this reaction (b) A large value for K implies there is a strong driver for the reaction to proceed

  90. chemistry

    The correct interpretation of the equation below is:? Fe3+(aq) + SCN¨C(aq)¡ú FeSCN2+(aq) A. The reaction is incomplete because the product is still charged. B. A heterogeneous equilibrium exists because of the charged ions. C. The equilibrium constant

  91. chemistry

    The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> FeSCN2+(aq) A. At equilibrium, the rate of the forward reaction equals the rate of the reverse reaction. B. The equilibrium constant is Kc = [Fe3+][SCN–][FeSCN2+] C. A

  92. chemistry

    The correct interpretation of the equation below is: Fe3+(aq) + SCN–(aq) --> and

  93. Chemistry

    For the reversible, one-step reaction A + B ARROW C + D, the forward rate constant is 35.9 1/(M·h) and the rate constant for the reverse reaction is 25.4 1/(M·h). The activation energy was found to be 33.0 kJ/mol for the forward reaction and 45.6 kJ/mol

  94. Chemisty

    For the reaction: 2NO(g) + H2(g) N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of H2 is 3.00

  95. Chemisty

    For the reaction: 2NO(g) + H2(g) N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of H2 is 3.00

  96. Science

    For the reaction: 2NO(g) + H2(g) N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. This reaction takes place at 25°C. At this temperature the concentration of NO is found to be 1.75 mol/L, the concentration of H2 is 3.00

  97. chemistry

    A 2.30 mole quantity of NOCl was initially in a 1.50 L reaction chamber at 400°C. After equilibrium was established, it was found that 20.0 percent of the NOCl had dissociated: 2NOCl(g) 2NO(g) + Cl2(g) Calculate the equilibrium constant Kc for the

  98. Chemistry

    Consider the reaction 2 SO2(g) + O2(g) in equilibrium with 2 SO3(g) . At 25°C delta H° = -197.78 kJ and delta S° = -187.95 J/K. Using this information, calculate the equilibrium constant for the reaction at -32°C. (R = 8.314 J/K) Enter your answer

  99. 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

  100. chemistry

    Consider the reaction: 2H2S(g)⇌2H2(g)+S2(g) An equilibrium mixture of this reaction at a certain temperature was found to have [H2S]= 0.542M , [H2]= 2.64×10−2M , and [S2]= 7.54×10−3M . What is the value of the equilibrium constant at this

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