An equilibrium mixture contains 2.0cm 3 of 1.00mol dm-3 of h2so4. Calculate the number of moles of H+ in this acid??? ???

76,119 results
  1. 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

  2. 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

  3. Chemistry

    Consider the following equilibrium process at 700°C: 2H2 + S2 ↔ 2H2S Analysis shows that there are 2.50 moles of H2, 1.35x10^-5 mole of S2, and 8.70 moles of H2S present in a 12.0-L flask. Calculate the equilibrium constant Kc for the reaction.

  4. science

    I am doing a titration lab and need help with a problem. (i used .100M H2SO4)(I used 10.0 ml of Ba(OH)2 solution and added 50.0 ml of distilled water making 60.0 ml total.) 1. Use the titration results to calculate the moles of H2SO4 that were used to

  5. Chemistry

    I'm working on a problem that says: A 4.00 gram sample of a mixture of CaO and BaO is placed in a 1.00 L vessel containing Co2 at a pressure of 730 torr and a temperature of 25C. The CO2 reacts with the CaO and BaO forming CaCO3 and BaCO3. When the

  6. Chemsitry

    The equilibrium between three substances, a, B and c is shown below. A(g) + B(g) C(g) Initially there were 0.1 mol of a and 0.2 mol of B in the reaction mixture. a and B reacted together to produce an equilibrium mixture containing 0.04 mol of c. The total

  7. Chemistry (please help me!)

    H2(g) + CO2(g) H20(g) + CO(g) When H2(g) is mixed with CO2(g) at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured: [H2]=0.20 M [CO2]=0.30 M [H2O]=[CO]=0.55M a) What

  8. CHEMISTRY

    for the reaction system H2 + X2 2HX Kc = 24.4 at 300 K a system made up fron these components which is at equilibrium contains 0.150 moles of H2 and 0.600 moles of HX in a 3.00 liter. calculate the number of moles of X2 present at equilibrium.

  9. Chemistry

    3. Calculate the amount of isopentyl acetate that should be present in the reaction mixture at equilibrium based on 300 mmol of acetic acid and 150 mmol of isopentyl alcohol as starting quantities. Use equilibrium constant of 4.2 for this calculation.

  10. Chemistry

    A 5.00L reaction vessel is filled with 1.00mol of H2, 1.00mol of I2, and 2.50mol of HI. If equilibrium constant for the reaction is 129 at 500k, what are the equilibrium concentrations of all species? H2(g) + I2(g) 2HI(g) Kc = 129

  11. Chemistry

    Calculate the number of moles of H2SO4 in 500ml of 0.324M H2SO4 solution and calculate the number of grams of H2SO4 in 500ml of 0.324M H2SO4 solution

  12. 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

  13. Chemistry

    When one mole of ammonia is heated to a given temperature, 50% of the compound dissociates and the following equilibrium is establised. NH3(g) 1/2N2(g) + 3/2H2(g) (note: is my sad attempt at the equilibrium symbol) What is the total number of moles of gas

  14. Chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization curve is 1.5x10^-4

  15. 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.

  16. chemistry

    Subject – equilibria Pure ethanoic acid (25.0cm3, CH3COOH), pure ethanol (35.0 cm3, C2H5OH) and pure water (20.0cm3, H2O) were mixed in a sealed flask at room temperature. The flask was placed in a heated water bath and maintained at 323K until

  17. UNM

    In an air-conditioned room at 19.0C , a spherical balloon had the diameter of 50.0cm . When taken outside on a hot summer day, the balloon expanded to 51.0cm in diameter. What was the temperature outside? Assume that the balloon is a perfect sphere and

  18. Chemistry

    Initially there were 1.0mol of a and 0.2 mol of b in the reaction mixture.a and b reacted together to produce an equilibrium mixture containing 0.04mol of c.the total volume of the mixture was 2.00dm^3. A.Calculate the number of moles of (a) and (b) at

  19. Chemsitry II

    mole fraction is equal to partial pressure divided by the total pressure Total pressure= sum of partial pressure use PV=nRT where n= number of moles equation become PV/RT=n make sure to convert the temperature to Kelvin and to use 0.0821 for R. V=volume,

  20. Chemistry

    An equilibrium mixture in a 10.0 L flask contains 7.0 mol HI(g) and 1.0 mol each of I2(g) and H2(g). If 2.5 mol H2, 5.0 mol I2 and 2.0 mol HI are added to that equilibrium mixture how many moles of each gas will be present when equilibrium is

  21. chemistry

    Calculate ∆T for the reaction. Assume the initial temperature of both reactants is 25.0◦C. Calculate the volume of the reaction mixture. Calculate the mass of the reaction mixture. Assume the density of the mixture is 1.03 g mL^(-1). Calculate the heat

  22. chemistry

    Can one calculate the number of moles of air? If so, calculate the number of moles in 1 kg of air (making sure your calculation, units and assumptions are fully explained); If not, explain why it is not possible to calculate the number of moles of air.

  23. Chemistry

    Consider the gas-phase equilibrium A ⇌ B. In a series of experiments, different initial amounts of A and B are mixed together, and the mixture in each case is allowed to come to equilibrium. Which one of these experiments would yield values for the

  24. chemistry

    I am given the following reaction: 2NH3(g) -----> N2(g) + 3H2(g) 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 has 4.2 mols of

  25. Chemistry

    A water chemist obtained a 250 ml sample from a nearby lake and fixed the oxygen on-site with alkaline solutions of MnSO4 and KI-NAN3. Returning to the laboratory, a 200 ml sample was analyzed by acidifying the sample with conc H2SO4 and then titrating

  26. Chemistry

    5.88 moles of nitrogen and 16.2 moles of oxygen are mixed and heated at 2000C° until equilibrium is established ,11,28 moles of nitric oxide are formed . Calculate the value of equilibrium constant?

  27. Chemistry

    a mixture of methane CH4 and ethane C2H6 is stored in a container at 294 mmHg. The gases are burned in air to form CO2 and H2O. If the pressure of CO2 is 346mmHg at the same temp and volume as the original mixture, calculate the ratio of moles of CO2

  28. AP CHEM!

    IM SO CONFUSED PLEASE HELP! H2 +CO2-->H2O + CO When H2 is mixed with CO2 at 2,000K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured. [H2]= 0.20mol/L [CO2]= 0.30mol/L

  29. CHem Part 2

    Part of the SO2 that is introduced into the atmosphere by combustion of sulfur containing compounds ends up beingh converted to sulfuric acid. 2SO2 (g) + O2 (g) ---> 2H2SO4 (aq) How much sulfuric acid can be formed from 5 moles of SO2, 2 moles of O2 and an

  30. CHEMISTRY: URGENT DRBob222

    A mixture of 0.50 mol of ethanoic acid and 1.00 mol of ethanol was shaken for a long time to reach equilibrium. The whole mixture was titrated quickly with 1.00 mol dm3 sodium hydroxide and 80cm3 of alkali were required. 1. Write an equation for the

  31. Chemistry

    Consider the gas-phase equilibrium A ⇌ B. In a series of experiments, different initial amounts of A and B are mixed together, and the mixture in each case is allowed to come to equilibrium. Which one of these experiments would yield values for the

  32. Chemistry

    A mixture of 0.5 mole of ethanoic acid and 1 mole of ethanol was allowed to reach equilibrium at room temperature. The equilibrium mixture was quickly titrated and 40cm3 of 2moldm-3 sodium hydroxide was used in the titration. a) Why is the reaction

  33. Chemistry

    Determination of the solubility product of PbI2. From the experimental data we obtain [I-] directly. To obtain Ksp for PbI2, we must calculate [Pb2+] in each equilibrium system. This is most easily done by constructing an equilibrium table. We first find

  34. AP CHEMISTRY

    An experiment was carried out to determine the value of the equilibrium constant Kc for the reaction. Total moles of Ag+ present = 3.6 x 10-3 moles Total moles of NH3 present = 6.9 x 10-3 moles Measured concentration of Ag(NH3)2+ at equilibrium= 3.4* 10-2

  35. Optics

    A converging lens of focal length f1 = +22 .5cm is placed at a distance d = 60 .0cm to the left of a diverging lens of focal length f2 = −30.0cm. An object is placed on the common optical axis of the two lenses with its base 45.0cm to the left of the

  36. Chemistry

    5.88 moles of nitrogen and 16.2 moles of oxygen are mixed until the equilibrium is established 11.28 moles of nitric acid are formed calculate the value of equilibrium constant

  37. Chemistry

    5.88 moles of nitrogen and 16.2 moles of oxygen are mixed until the equilibrium is established, 11.28 moles of nitric oxide are formed calculate the value of equilibrium constant

  38. Chemistry

    Calculate the ratio of moles of CO2 produced to moles of the original gas mixture? A mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mmHg. The gases are burned in air to form CO2 and H2O. If the pressure of CO2 is 351 mmHg

  39. Chemistry

    Calculate the ratio of moles of CO2 produced to moles of the original gas mixture? A mixture of methane (CH4) and ethane (C2H6) is stored in a container at 294 mmHg. The gases are burned in air to form CO2 and H2O. If the pressure of CO2 is 351 mmHg

  40. chem 221 #3

    during the preparation of synthetic banana oil lab. Calculate the amount of isopentyl acetate that should be present in the reaction mixture at equilibrium based on 300 mmol of acetic acid and 150 mmol of isopentyl alcohol as starting quantities. Use

  41. chemistry

    Initially, there are 33 moles of A and 0 moles of B. How many moles of A and B will be present after the system reaches equilibrium? a) 33 moles A; 0 moles B b) 0 moles A; 33 moles B c) 3 moles A; 30 moles B d) equal amounts of A and B The answer is given

  42. AP Physics C

    when a block is pulled out to x=+4.0cm, we must apply a force amgnitude 360N to hold it there. we pull the block to x=11cm and then realease it. how much work does the spring do on the block as the block moves from xi=+5.0cm to a)x=+3.0cm, b)x=-3.0cm,

  43. Chemistry

    What mass of solid potassium sulfate, K2SO4, is used to make up exactly 100.0cm^3 of 0.100 mol/dm^3 SO4^2-? This should be a very easy, 1-mark question but for some reason I can't wrap my head around it. moles = mass/Mr, so all you gotta do is moles x

  44. Chemistry

    Consider the following reaction: CO2 (g) + H2 (g) CO (g) + H2O (g) Calculate the value of the equilibrium constant, Kc, for the above system, if 0.1908 moles of CO2, 0.0908 moles of H2, 0.0092 moles of CO, and 0.0092 moles of H2O vapour were present in a

  45. chemistry

    Calculate (a) the moles and (b) the mass of magnesium carbonate at the start if 0.2 moles of sulfuric acid is added to the magnesium carbonate and the excess sulfuric acid made up to a 250 cm3 solution. 25 cm3 of this solution required 0.03 moles of sodium

  46. 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.

  47. 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? Note:

  48. Chemistry

    Calculate the concentrations of S2O8 2-, I-, S2O32 2- in moles per litre of reaction mixture given the following: 20mL of 0.1 M (NH4)2S2O8 added to: 20mL of 0.2M KI 10mL of 0.01M Na2S2O3 5mL 0.2% starch Also, calculate -(delta)S2O8 2- that is, how much

  49. chemistry

    Suppose that the reaction of Fe3+ and SCN- produces Fe(SCN)2 (+). 5.00mL of 2.0mM Fe3+ is mixed with 5.00 mL of 2.0mM SCN-. The student finds the equilibrium concentrations of Fe(SCN)2(+) to be 0.3mM. 1.) What is the initial number of moles of each species

  50. chemistry

    n one experiment, a mixture of 1.000 mol acetic acid and 0.5000 mol ethanol is brought to equilibrium. A sample containing exactly one-hundredth of the equilibrium mixture requires 28.80mL 0.1040M Ba(OH)2 for its titration. Calculate the equilibrium

  51. CHEMISTRY

    An equilibrium mixture contains 2.0cm 3 of 1.00mol dm-3 of h2so4. Calculate the number of moles of H+ in this acid??? ???

  52. CHEMISTRY

    An equilibrium mixture contains 2.0cm 3 of 1.00mol dm-3 of h2so4. Calculate the number of moles of H+ in this acid??? ???

  53. 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

  54. AP Chem - to Dr. Bob

    I don't understand how to even start this problem: A mixture of H2(g), O2(g), and 2 mL of H2O is present in a 0.5 L rigid container at 25 degrees Celsius. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1146 mmHg.

  55. chemistry

    1(a) when 25.0ml of 0.500 mol.dm3 H2SO4(AQ) SOLUTION IS added to 0.025dm3 of 1.00 moldm3 KOH SOLUTION , THE TEMPERATURE OF THE REACTION MIXTURE RISES FROM 23.50 CELCIUS TO 30.17 CELCIUS . THE SPECIFIC HEAT CAPACITY AND DENSITY OF WATER 4.20j.g.celcius and

  56. 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

  57. Chemistry - check answer

    A 20.0 L reaction vessel contains 0.016 moles CO2, 1.05 moles of CO, and 2.00 moles of C. The mixture is approaching the following equilibrium: CO2(g) + C(s) 2CO(g) a) Calculate the reaction quotient Q. b) If value of K is 1.17, predict which direction the

  58. Chemistry (Equilibrium)

    Consider the following equilibrium system at 900°C: H20(g) + CO(g) H2(g) + CO2(g) Initially 5.0 moles of H2O and 4.0 moles of CO were reacted. At equilibrium, it is found that 2.0 moles of H2 are present. How many moles of H2O remain in the mixture? Would

  59. chm152

    Consider the following equilibrium: 5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of Cl2 are present at equilibrium. Choose one

  60. CHM 152

    Consider the following equilibrium: PCl5 = PCl3+ Cl2 5.0 moles of are placed in a 10.0 L flask at 200 C and allowed to come to equilibrium. Analysis shows that 1.0 mole of is present in the equilibrium mixture. How many moles of are present at equilibrium.

  61. chemistry

    A reaction mixture of 4.0 mL of 0.002 M SCN- and 5.0 mL of 0.002 M Fe3+ is diluted to 10.0 mL with 0.1 M HNO3 to form the blood-red FeNCS2+ complex. The equilibrium molar concentration of the FeNCS2+ determined from a standardization curve is 1.5x10^-4

  62. 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

  63. chemistry

    Ideal Mixed Gas Law problems 1. What is the pressure generated by a mixture of 25.6 g SO2 and 12.6 g Ne in a container of 72.45 L and temperature of 131 K? 2. What is the pressure of a mixture of 5.80 moles Kr and 2.71 moles Xe in a container with a volume

  64. chemistry

    1) 14 moles of Ar 12 moles of N2 2 moles of BF3 If the total number of mol present in the mixture visualized is 1.43, calculate the number of mol of N2. 2) 11 moles of N2 4 moles of CSH4 If the total number of mol present in the mixture visualized is 1.68,

  65. 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

  66. 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

  67. Chemistry

    At 1200 K a gaseous mixture contains 0.30 moles of carbon monoxide, 0.10 moles of hydrogen, 0.20 moles of water vapor and 0.059 moles of methane in a 1.00 liter container. Determine whether or not equilibrium has been reached for the following reaction:

  68. chemistry

    50.0cm^3 of 2.0 mol dm^-3 aluminium sulphate,Al2(SO4)3 solution Calculate the number of moles of ions.

  69. Chemistry

    Pure ethanoic acid (25.0cm3, CH3COOH), pure ethanol (35.0 cm3, C2H5OH) and pure water (20.0cm3, H2O) were mixed in a sealed flask at room temperature. The flask was placed in a heated water bath and maintained at 323K until equilibrium was established.

  70. Chemistry Question!!

    When 1.00 g of gaseous I2 is heated to 1000. K in a 1.00 L sealed container, the resulting equilibrium mixture contains 0.830 g of I2. Calculate Kc for the dissociation equilibrium below. I2 2 I What I did was converted the initial I2 into moles then

  71. Physical Chemistry

    When 1.00 g of gaseous I2 is heated to 1000. K in a 1.00 L sealed container, the resulting equilibrium mixture contains 0.830 g of I2. Calculate Kc for the dissociation equilibrium below. I2 2 I What I did was converted the initial I2 into moles then

  72. Chemistry

    Two moles of pure ammonia were injected into a 2.00L flask at a certain temperature. The equilibrium mixture: 2NH3(G)-->N2(G) + 3H2(G)

  73. Chemistry

    The equilibrium constant for the reaction 2SO2 + O2 2SO3(all are gases) at a certain const temperature is 846.4mol/dm^3. At equilibrium in a 1dm^3 vessel, 0.5 moles of SO2, 0.1 moles of O2, and 4.6 moles of SO3 were found. How many moles of oxygen must be

  74. CHEM- need help ASAP

    An equilibrium mixture in a 10.0 L flask contains 7.0 mol HI(g) and 1.0 mol each of I2(g) and H2(g). If 2.5 mol H2, 5.0 mol I2 and 2.0 mol HI are added to that equilibrium mixture how many moles of each gas will be present when equilibrium is

  75. AP Chem - to Dr. Bob

    I don't understand how to even start this problem: A mixture of H2(g), O2(g), and 2 mL of H2O is present in a 0.5 L rigid container at 25 degrees Celsius. The number of moles of H2 and the number of moles of O2 are equal. The total pressure is 1146 mmHg.

  76. physical science

    calculate the number of moles of H2SO4 wich were added to the NaOH solution

  77. Chemistry

    Question : 4 moles of A(g) is added to a fixed volume container and left until they arrive at the equilibrium status. 2A(g) A2(g) At 127 C total pressure of the equilibrium system is 8.314*10^5 Pa and the density of the mixture of gas is 10 kg/m^3 . If the

  78. 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

  79. chemistry

    calculate number of moles of h2so4 needed to react with 25.0ml of .20M liOH

  80. Chemistry

    Calculate the number fo moles of NaOH(aq) needed to react completely with 125 mL fo 6.00 M H2SO4(aq)

  81. chemestry

    i don't know how to solve this problem,could anyone is here to give me the correct solution.It will be good for me. In a reactor of 1.5 L the same amount of C and H2O was introduced. When the reaction: C(s) + H2O ⇄ CO + H2 reaches the equilibrium at 1273

  82. Chemistry

    A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800C. Calculate the equilibrium partial pressures of H2 Cl2 and HCl if the total pressure is 2.00 atm. For the reaction Kp is 193 at 2800C. H2(g) +Cl2(g) = 2HCl (g) I know that I need to find

  83. Chemistry

    a mixture of methane CH4 and ethane C2H6 is stored in a container at 294 mmHg. The gases are burned in air to form CO2 and H2O. If the pressure of CO2 is 346mmHg at the same temp and volume as the original mixture, calculate the ratio of moles of CO2

  84. Chemistry

    A volume of 10cm^3 of 2M H2SO4 is placed in a volumetric flas of 250cm^3 and filled to the mark with distilled water. What is the molar conc. of the H2So4 in the flask? After I found how many moles there are in 10cm^3, which is 0.02 mol, what is my next

  85. Chemistry

    A mixture of salt way in 13.78g contains CACO3 with gaseous impurity it was heated to a constant mass and the resolve was reacted with H2SO4 to form 6.78g of CASO4. Calculate the percentage purity of the calcium trizoncarbonate four I'm the mixture (ca=40,

  86. 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 pressure drops to

  87. AP Chemistry

    Given: N2O4 (g) « 2NO2 (g) @ 25 degrees celcius, Kc is 5.84 x 10^-3. (A) Calculate the equilibrium concentrations of both gases when 4.00 grams of N2O4 is placed in a 2.00 L flask at 25 degrees celcius. (B) What will be the new equilibrium concentrations

  88. PHYSICS (REALLY DIFFICULT PLEASE HELP)

    At a temperature of 18.0°C of 23.0cm^3 of a certain gas occupies has pressure of 103 kPa. (a) What volume would the gas occupy at a temperature of 0.00°C and pressure of 101kPa? (b) 1.00 moles of a certain gas occupies a volume of 22.4 litres at 0.00°C

  89. PHYSICS (PLEASE HELP ME ASAP)

    At a temperature of 18.0°C of 23.0cm^3 of a certain gas occupies has pressure of 103 kPa. (a) What volume would the gas occupy at a temperature of 0.00°C and pressure of 101kPa? (b) 1.00 moles of a certain gas occupies a volume of 22.4 litres at 0.00°C

  90. Chemistry

    Calculate the equilibrium constant for the equilibrium knowing that there are 2 moles of O2 H2, 6 moles of O2 and 3 moles of H2O in a jar reactor 2L? 2 H2 + O2 = 2 H2O

  91. 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

  92. chem101

    The equilibrium under investigation is : H2CO3(aq) * H2O(l) + CO2(g) How does the pulling and pushing of the plunger affects the equilibrium? Is it consistent with LeChatelier's principle? my answer is that if you push you increase the pressure volume

  93. Chem

    A mixture of 2.5 moles of H2O and 100 g of C are placed in a 50.0 L container and allowed to come to equilibrium in the following reaction: C(s) + H2O(g)  CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040 M. What is the

  94. Chemistry 30

    A mixture of 2.5 moles of H2O and 100 g of C are placed in a 50.0 L container and allowed to come to equilibrium in the following reaction: C(s) + H2O(g)  CO(g) + H2(g) The equilibrium concentration of hydrogen gas is found to be 0.040 M. What is the

  95. chem

    Determination of the solubility product of PbI2. From the experimental data we obtain [I-] directly. To obtain Ksp for PbI2, we must calculate [Pb2+] in each equilibrium system. This is most easily done by constructing an equilibrium table. We first find

  96. 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

  97. Chemistry (11th grade)

    we have the following equation- 2HCl+CuSO4 yields H2SO4+CuCl2. the question is if 7 moles of HCl react, how many moles of H2SO4 will be produced?

  98. Chemistry

    for the reaction 2NaOH + h2SO4 yieda 2H2O + Na2SO4 if .80 moles of NaOH are used, how many moles of H2SO4 must be used?

  99. 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

  100. 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

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