1. General Chemistry

    NH4+ + NO2- = N2 + 2H2O A reaction is run, and the liberated N2 gas is collected in a previously evacuated 500 mL container. After the reaction has gone on for 750 seconds, the pressure of N2 in the 500 mL container is 2.77 x 10^-2 atm , and the
  2. Chemistry

    The following reactions is a first order reaction with respect to nitrite ion and its rate constant is 0.0030/s. In a solution that is 10.0 M NO2-, what is the half-life of the reaction? NH4+ + NO2- -->N2 + 2H2O
  3. College Chemistry

    Given the following equilibrium constants, Ka (NH4^+)=5.6*10^-10 Kb (NO2^-)=2.2*10^-11 Kw=1.00*10^-14 determine the equilibrium constant for the reaction below at 25*C. NH4^+(aq)+NO2^-(aq)f HNO2(aq)+NH3(aq)
  4. Chemistry

    The half-life of the following first order reaction is 231 seconds. What percent of the original concentration of nitrite ion remains after 10.0 minutes? NH4+ + NO2- --> N2 + 2H2O
  5. Chemistry

    Ammonium ion (NH4^+) reacts with nitrite ion (NO2^-) to yield nitrogen gas and liquid water. The following initial rates of reaction have been measured for the given reactant concentrations. Expt. # [NH4^+] [NO2^-] Initial rate (M/hr) 1 0.010 0.020 0.020 2
  6. chei

    .0815moles NO are reacted with .0789moles O2 gas to from NO2 gas according to the following equation: 2NO + O2 = 2NO2 determine the molar amounts of NO, O2, and NO2 after complete reaction.
  7. chemistry

    .0815moles NO are reacted with .0789moles O2 gas to from NO2 gas according to the following equation: 2NO + O2 = 2NO2 determine the molar amounts of NO, O2, and NO2 after complete reaction.
  8. chemistry

    .0815 moles NO are reacted with .0789moles O2 gas to form NO2 gas according to the following equation: 2NO +O2=2NO2 determine the molar amounts of NO, O2 and NO2 after complete reaction.
  9. chemistry

    .0815 moles NO are reacted with .0789moles O2 gas to form NO2 gas according to the following equation: 2NO +O2=2NO2 determine the molar amounts of NO, O2 and NO2 after complete reaction.
  10. chem

    an 18.9g sample of copper and an 82.0 mL of 16.0mol/L nitric acid are allowed to react. Brown nitrogen dioxide gas is generated. find the maximum mass of NO2 that could be produced. if 22.6g of the gas is actually produced, find the percentage yield of the
  11. Chemistry

    So, they give me a word equation, where I am suppose to try and create a balanced equation for it. Ammonium phosphate and barium hydroxide react to form ammonium hydroxide and barium phosphate. 2(NH4)3PO4 + 3BaOH2 → 6NH4OH + Ba3(PO4)2 [I was thinking
  12. Chemistry!!!!

    1. For a reaction mechanism to be plausible, what 2 criteria must be met? 2. The reaction between CO and NO2 to produce NO and CO2 is thought to occur in 2 steps. NO2 + NO2 ====> NO + NO3 NO3 + CO =====> NO2 + CO2 The experimental rate law is,
  13. Chemistry!!!!

    1. For a reaction mechanism to be plausible, what 2 criteria must be met? 2. The reaction between CO and NO2 to produce NO and CO2 is thought to occur in 2 steps. NO2 + NO2 ====> NO + NO3 NO3 + CO =====> NO2 + CO2 The experimental rate law is,
  14. Chemistry

    A container at room temperature is filled with equal moles of O2(g), NO2(g) and He(g). The gases slowly leak through a pinhole in the container. After some gas has effused, which relationship is true about the partial pressures of the gas remaining in the
  15. Science - Chemistry

    If the rate law of a chemical reaction is k[NH4+]2[NO2–], what is the order of the reaction? 1. The order of the reaction cannot be determined. 2. 3 3. 1 4. 2
  16. PChem

    For the gas phase reaction 2NO2 + F2 ¨ 2NO2F, the rate constant is k= 38 dm3/mol-s at 27 oC. The reaction is first-order in NO2 and first-order in F2. A) Calculate the number of moles of NO2, F2, and NO2F after 10.0 s if 2.00 mol of NO2 is mixed with
  17. 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
  18. Chemistry

    When 442 mg of NO2 is confined to a 150. mL reaction vessel and heated to 300°C, it decomposes by a second-order process. In the rate law for the decomposition of NO2, k = 0.54 1/(M·s). A) what is the initial reaction rate? B) what is the reaction rate
  19. chemistry

    Nitric acid can be produced by the reaction of gaseous nitrogen dioxide with water. 3 NO2(g) + H2O(ℓ) −→ 2 HNO3(ℓ) + NO(g) If 900 L of NO2 gas react with water, what volume of NO gas will be produced? Assume the gases are measured under the same
  20. science

    The equilibrium constant for the gas phase reaction N2O4 ⇀↽ 2 NO2 at a certain temperature is K = 0.0466. If the initial concentrations are [N2O4] = 1.0 M, [NO2] = 0.0 M, what are the final concentrations of [N2O4] and [NO2], respectively? 1.
  21. chemistry

    Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo missions to the moon. In a closed container the gas N2O4(g) decomposes to nitrogen dioxide, NO2(g). The equilibrium constant,k, for this reaction is 0.87 at 55 degrees Celsius. A vessel
  22. chemistry

    Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 23°C and 0.94 atm, the density of this gas mixture is 2.6 g/L. What is the partial pressure of each gas? NO2 N2O4
  23. chemistry

    Which of the following equations correctly describes the relationship between the rate at which NO2 and Cl2 are consumed in the following reaction? 2 NO2(g) + Cl2(g) → 2 NO2Cl(g) A. -d(NO2)/dt = 1/2 [d(Cl2)/dt] B. -d(NO2)/dt = 2 [d(Cl2)/dt] C.
  24. science

    Which of the following equations correctly describes the relationship between the rate at which NO2 and Cl2 are consumed in the following reaction? 2 NO2(g) + Cl2(g) → 2 NO2Cl(g) A. -d(NO2)/dt = 1/2 [d(Cl2)/dt] B. -d(NO2)/dt = 2 [d(Cl2)/dt] C.
  25. chemistry

    water vapor and nitrogen dioxide gas NO2 are cimbined to manufacture ammonia. a by product of this reaction is oxygen gas. write a balanced equation for this reaction. i do not understand this at all please help me figure it out
  26. Chem

    Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g) 2NO(g) + O2(g) > 2NO2 (g) 3NO2(g) + H2O(l) > 2HNO3(aq) + NO(g) What mass of NH3 must be used to produce
  27. chemistry

     If we combine nitrous oxide (NO, laughing gas) with oxygen (O2) we produce nitrogen dioxide (NO2) according to the following reaction: 2NO + O2→ 2NO2 How many grams of NO2 will be produced when 5.00 moles of NO react?
  28. Chemistry

    I've tried to answer some -The reaction mechanism for a reaction is as follows… Step 1 O3 (g) + NO2 (g)→ NO3 (g) + O2 (g) slow Step 2 NO3 (g) + NO2 (g) → N2O5 (g) fast a. Write the overall reaction equation. b. Identify the molecularity of
  29. Chemistry

    Nitric acid can be produced by the reaction of gaseous nitrogen dioxide with water. 3 NO2(g) + H2O(ℓ) −→ 2 HNO3(ℓ) + NO(g) If 916 L of NO2 gas react with water, what volume of NO gas will be produced? Assume the gases are measured
  30. chemistry

    A reaction mixture of N2O4 and NO2 absorbs the heat given off in the combustion of 6.35 L CH4 measured at 24.7 C and 812 Torr. How many moles of N2O4 can be converted to NO2 as a result? CH4 + 2O2 --> CO2 + 2H2O Delta H = -890.3 KJ N2O4 --> 2NO2
  31. chemistry ap

    Nitric acid can be produced by the reaction of gaseous nitrogen dioxide with water. 3 NO2(g) + H2O(ℓ) −→ 2 HNO3(ℓ) + NO(g) If 734 L of NO2 gas react with water, what volume of NO gas will be produced? Assume the gases are measured
  32. Chemistry

    The following reaction mechanism has been proposed for a reaction: (slow) NO2 + NO2-> NO3 + NO (fast) NO3 + CO -> CO2 + NO2 A. Write the equation for the overall reaction from the mechanism above. B.Write the rate law for the reaction
  33. Chemistry

    The following reaction mechanism has been proposed for a reaction: (slow) NO2 + NO2-> NO3 + NO (fast) NO3 + CO -> CO2 + NO2 A. Write the equation for the overall reaction from the mechanism above. B.Write the rate law for the reaction
  34. Chemistry

    The following reaction mechanism has been proposed for a reaction: (slow) NO2 + NO2-> NO3 + NO (fast) NO3 + CO -> CO2 + NO2 A. Write the equation for the overall reaction from the mechanism above. B.Write the rate law for the reaction
  35. 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?
  36. Chemistry

    A reaction requires 22.4 L of gas at STP. You have 30.5 L of gas at 101.5 kPa and 373 K. Which of the following statements is true? (Use the ideal gas law: PV = nRT where R = 8.31 L-kPa/mol-K.) You will have excess gas for the reaction. You will have
  37. AP Chem (Thank you for help)

    Hey guys! Stuck on some Redox Reactions. I tried my best to put as much work as I could, but I'm super stuck on these ones. Thanks for any help: 1) Balance the equation as written, what is the coefficient for O2? NH4+ + O2-->NO2− + H2O (in basic
  38. chemistry

    2 NO2(g) N2(g) + 2 O2(g) The ΔH° for the reaction above is -66.4 kJ. The system is initially at equilibrium. What happens if N2 is added to the reaction mixture at constant temperature and volume? The reaction absorbs energy. The reaction releases
  39. Chemistry

    Imagine that you have a 6.00L gas tank and a 3.00L gas tank. You need to fill one tank with oxygen and the other with acetylene to use in conjunction with your welding torch. If you fill the larger tank with oxygen to a pressure of 125atm , to what
  40. chemistry

    Hydorgen peroxide may be prepared by the following reactions: 2NH4HSO4 ---> H2+(NH4)2S2O8 (NH4)2S2O8+2H2O ----> 2NH4HSo4+H2O2 What mass of ammonium hydrogen sulfate, Nh4HSo4 is initially required to prepare 2.00 mole of H2O2? What mass of H2O is
  41. Chemistry (equilibrium)

    In the following equilibrium system, N2O4(g) <--> NO2(g), what happens to the color of the gas if the forward reaction speeds up? What happens if the reverse reaction speeds up? What happens if the forward and reverse reaction happen at the same
  42. 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] = ?
  43. 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] = ?
  44. Chemistry

    In 20 s, the concentration of NO2 decreases from 450 mM to 320 mM in the reaction 2 NO2 --> 2 NO + O2 (a) Determine the rate of reaction of NO2 (b) Determine the rate of formation of O2 (c) What is the unique rate of the reaction?
  45. AP Chemistry

    Given: 2N2(g) +O(2) --> 2N2O(g) Kc =1.2x10^(-35) N2O4(g) --> 2NO2(g) Kc = 4.6x10^(-3) 1/2N2(g) + O2(g) --> NO2(g) Kc= 4.1x10^(-9) Calculate Kc for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give nitrogen tetroxide gas.
  46. Chem

    Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g) + 5O2(g) > 4NO(g) + 6H2O(g) 2NO(g) + O2(g) > 2NO2 (g) 3NO2(g) + H2O(l) > 2HNO3(aq) + NO(g) What mass of NH3 must be used to produce
  47. Chemistry

    Is the Conversion of NO2 to HNO3 endo- or exothemic? Calculate the enthalpy and free energy change for the reaction 4NO2 + o2 + 2H2O-----> 4HNO3 in the aqueous phase.
  48. Chemistry

    Is the Conversion of NO2 to HNO3 endo- or exothemic? Calculate the enthalpy and free energy change for the reaction 4NO2 + o2 + 2H2O-----> 4HNO3 in the aqueous phase.
  49. Analytical chemistry

    A Kjeldahl analysis was preformed upon a 0.055 g sample of impure biguanide (C2H7N5, fw=101.1). The liberated ammonia, collected in 40 mL of 4% boric acid was titrated with 19.51 mL of 0.1060 M HCl. Calculate the percentage of biguanide in the sample.
  50. someone correct my work please? fun, fun chemistry

    Okay. I'm very, very confused. The initial question is: predict the products of the electrolysis of a 1 mol/L solution sodium chloride. This is my work: The four different possible equations are: 2H2o + 2e- -------> H2 + 2OH- (V= -0.83) O2 + 4H+ + 4e-
  51. 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
  52. chem

    Is ammonium hydroxide a strong or weak base and how do you know that? Technically there is no such thing as ammonium hydroxide. NH3 gas (ammonia gas) dissolves easily in water and produces the NH4^+ and the OH^- from the reaction with water. It is a weak
  53. 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)
  54. Chemistry

    Ammonium carbonate decomposes upon heating according to the balanced equation: (NH4)2CO3(s) -> 2NH3(g)+CO2(g)+H2O(g) Calculate the total volume of gas produced at 27.0 degrees C and 2.03 atm from the reaction of 1.4kg of (NH4)2CO3. What is the pressure
  55. Chemistry 2

    The mechanism for the reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be the following. NO2 + NO2 NO3 + NO Slow NO3 + CO NO2 + CO2 Fast What would be the overall balanced equation to this reaction?
  56. chemistry

    When ammonia gas is burned in oxygen the products formed are water and nitrogen monoxide gas. Write the balanced equation showing this reaction NH4 + O2 --> H2O + NO i am stuck balancing this
  57. Chemistry

    The reform reaction between steam and gaseous methane () produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen.
  58. Chemistry

    O3 + NO --> O2 + NO2 (all in gas state) Calculate the change in enthalpy for the reaction at room temp. using the following data ^Hf: O3 = 143 NO = 90 NO2 = 33 So, I have 143+90--> X + 33. I don't know what the enthalpy of O2 is. I assume you simply
  59. Chemistry (redox reaction)

    Which reaction is a redox reaction? 1. HCI+H2O=H3O^+ +CI^- 2. H2SO4+2KOH=K2SO4+2H2O 3. CH4+2O2=CO2+2H2O 4. Fe^2+ +2OH^- =Fe(OH)2 I chose number 3, is this correct?
  60. Equilibrium

    The following reaction has an equilibrium constant (Keq) of 160. 2 NO2(g) <--> 2 NO(g) + O2(g) What will be the reaction quotient (Q) and in which direction will the reaction proceed if the partial pressure of NO2 is 5.0*10^-4 atm, NO is 0.080 atm,
  61. chemistry

    1) All of the following are oxidation-reduction reactions except (a) 2Al(s) + Fe2O3(s) ---> A12O3(s) + 2Fe(s) (b) (NH4)2Cr2O7(s) ---> Cr2O3(s) + N2(g) + H2O(1) (c) Cu(s) + 2H2SO4(aq) ---> CuSO4(aq) + SO2(g) + 2H2O(1) (d) Hg(NO3)2 + 4KI --->
  62. 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?
  63. 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?
  64. chemistry

    When copper is dissolved in nitric acid, a brown gas (NO2) is evolved, either by direct production of NO2 or by production of NO which is oxidized to NO2 by O2. Provide a Lewis drawing and resonance structures for the nitrate anion.
  65. Chemistry-Enthalpies of formation

    "Synthesis gas" is a mixture of carbon monoxide and hydrogen that is used to synthesize a variety of organic compounds. One reaction for producing synthesis gas is 3CH4 + 2H2O + CO2 = 4CO + 8H2 Using enthalpies of formation, calculate the enthalpy change
  66. AP chemistry

    The mechanism for the reaction of nitrogen dioxide with carbon monoxide to form nitric oxide and carbon dioxide is thought to be NO2+NO2 > NO3+NO slow NO3+CO > NO2+CO2 fast Write the rate law expected for this mechanism. What is the overall balanced
  67. Chemistry

    Given a sample of gas (2.49 g) with a volume of 752 mL at 335K and 1.98 atm, what is the gas, SO2 or NO2? PV=nRT (1.98atm)(0.752L)= X (0.08206L-atm/mol-K)(335K) X = 0.0541634989 mol= g/gfm 2.49/X= 0.0541634989 X = 45.97 NO2 has 46g, whereas SO2 is 64.1g.
  68. Chemistry

    When the rate of the reaction 2NO+O2=2NO2 was studied, the rate was found to double when the O2 concentration alone was doubled but to quadruple when the NO concentration alone was doubled. Which of the following mechanisms accounts for these observations?
  69. Chemistry

    At 573 K, gaseous NO2(g) decomposes, forming NO(g) and O2(g). If a vessel containing NO2(g) has an initial concentration of 1.9 × 10−2 mol/L, how long will it take for 75% of the NO2(g) to decompose? The decomposition of NO2(g) is second-order in
  70. chemistry

    In a 1L beaker, 203mL of 0.307 M ammonium chromate was mixed with 137mL of 0.269 M chromium(iii) nitrite. 3(NH4)2CrO4 + 2Cr(NO2)3 -> Cr2(CrO4)3 + 6NH4NO2 If the percent yield of the reaction was 88.0 %, what mass of solid product was isolated?
  71. chemistry

    In a 1L beaker, 203mL of 0.307 M ammonium chromate was mixed with 137mL of 0.269 M chromium(iii) nitrite. 3(NH4)2CrO4 + 2Cr(NO2)3 -> Cr2(CrO4)3 + 6NH4NO2 If the percent yield of the reaction was 88.0 %, what mass of solid product was isolated?
  72. Chemistry

    The mechanism for the reaction described by 2N2O5(g) ---> 4NO2(g) + O2(g) is suggested to be (1) N2O5(g) (k1)--->(K-1) NO2(g) + NO3(g) (2) NO2(g) + NO3(g) --->(K2) NO2(g) + O2(g) + NO(g) (3) NO(g) + N2O5(g) --->(K3) 3NO2(g) Assuming that [NO3]
  73. Chemistry

    Given…Overall reaction: 2 NO2 (g) + F2 (g) → 2 NO2F (g) Rate = k[NO2][F2] a. Can this be a single step reaction? b. Postulate a mechanism using experimental data and chemical intuition come up with a mechanism that fits.
  74. physics 30

    Given the reaction 3 NO2(g) + H2O(l) ¨ 2 HNO3(l) + NO(g) ƒ¢rH = -72.0 kJ, calculate the molar enthalpy of reaction, rH for: 1) NO2(g) 2) H20 (l) 3) HNO3 (l) 4) NO (g) Express you answer in Kj/mol
  75. Chemistry

    Check my answer please? A reaction requires 22.4 L of gas at STP. You have 45.0 L of gas at 100 kPa and 373 K. Which of the following statements is true? The gas constant is 8.31 L-kPa/mol-K. You will have an excess of gas and the reaction will occur.
  76. Chemistry

    What mass of NO2 is formed by the complete reaction of 2 mol O3 with excess NO in the reaction? O3 + NO --> O2 + NO2 I know the molar mass of O3 is 48 g/mol and NO2 46 g/mol a) 23.0 g b) 46.0 g c) 92.0 g d) 96.0 g
  77. 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.
  78. Chem

    At 25°C the following heats of reaction are known: 2C2H2 + 5O2 ---> 4CO2 + 2H2O; ΔH = -2600 kJ C + O2 ---> CO2 ; ΔH = -394 kJ 2H2 + O2 ---> 2H2O; ΔH = -572 kJ At the same temperature, calculate ΔH for the following reaction: 2C + H2 --->
  79. Chemistry

    A 5.00L reaction vessel contains hydrogen at a partial pressure of 0.588atm and oxygen gas at a partial pressure of 0.302atm. The equation is 2H2(g)+O2(g)-> 2H2O(g). Suppose the gas mixture is ignited and the reaction produces the theoretical yield of
  80. Chemistry

    Identify the following chemical equations by type. 1. If an electric discharge produces 800 cm3 of ozone (O3), how many cm3 of oxygen (O2) are required? 3O2(g) ---> 2O3(g) 2. When 75.0 dm3 of O2 react with an excess of glucose (C6H12O2), according to
  81. 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
  82. Chemistry

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

    How much energy will be liberated upon the combustion of 12.5 grams of ethene? C2H4(g) + 3O2(g) ----> 2CO2(g) + 2H2O(g) Delta H = -1387.4 kj
  84. ap chemistry

    Calculate the standard reaction enthalpy for the reaction NO2(g) ! NO(g) + O(g) Given: O2(g) ! 2O(g) H = +498.4 kJ/mol NO(g) + O3(g) ! NO2(g) + O2(g) H = −200 kJ/mol 3O2(g) ! 2O3(g) H = +285.4 kJ/mol
  85. Chemistry

    One reaction of iron with hydrochloric acid is represented by the following thermochemical equation. Fe(s) + 2HCl(aq) ? FeCl2(aq) + H2(g); (Delta)H°= –87.9 kJ How much heat is liberated at constant pressure if 0.215 g of iron reacts with 40.4 mL of
  86. Chem

    2NH3 <--> NH4+ + NH2- In liquid ammonia the reaction represented above occurs. In the reaction, what does the NH4+ act as? A catalyst? And acid & a base? the conjugate acid of NH3? The reducing agent? The oxidizing agent?
  87. Chemistry

    What volume of gas can be produced in a lab where pressure is 16.0 psi and temperature is 25 C if you collect it over water from the reaction of 50g of ammonium sulfate with 50g of aluminum hydroxide. The equation for the reaction is: 3(NH4)2SO4 + 2Al(OH)3
  88. Chem Check Please!!!

    1) Assuming the following reaction proceeds in the forward direction, 3 Sn4+(aq) + 2 Cr(s) ---> 3 Sn2+(aq) + 2 Cr3+(aq) a.Sn4+(aq) is the reducing agent and Cr(s) is the oxidizing agent. b.Cr(s) is the reducing agent and Sn2+(aq) is the oxidizing agent.
  89. Chemistry

    for the redox reaction given in the chemical equation Pb(OH)4^2- (aq) + ClO- (aq) --> PbO2 (s) + Cl- (aq) For the oxidation half reaction I got Pb(OH)4^2- (aq) --> PbO2 (s) + 2H2O (l) + 2e- For the reduction half reaction I got 2e- + 2H2O(l) +
  90. 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?
  91. Chemistry

    The first step of the synthesis is described by the reaction below. When 1.750 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4 , the theoretical yield of FeC2O42H2O is _______grams. Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq) FeC2O42H2O(s) +
  92. chemistry 1c

    The first step of the synthesis is described by the reaction below. When 2.000 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4, the theoretical yield of FeC2O42H2O is grams. Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq) FeC2O42H2O(s) + (NH4)2SO4(aq) +
  93. chemistry

    The first step of the synthesis is described by the reaction below. When 1.000 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4, the theoretical yield of FeC2O42H2O is grams. Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq) FeC2O42H2O(s) + (NH4)2SO4(aq) +
  94. chemistry ASAP please!!

    The reaction of CO(g) + NO(g) is second-order in NO2 and zero-order in CO at temperatures less than 500K. (a) Write the rate law for the reaction. (b) How will the reaction rate change if the NO2 concentration is halved? (c) How will the reaction rate
  95. Chemistry

    The first step of the synthesis is described by the reaction below. When 1.750 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4, the theoretical yield of FeC2O42H2O is____ grams. Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq)----> FeC2O42H2O(s) +
  96. Chemistry

    The first step of the synthesis is described by the reaction below. When 2.000 g of Fe(NH4)2(SO4)2 6H2O is mixed with 13 mL of 1.0 M H2C2O4, the theoretical yield of FeC2O42H2O is ______ grams. Fe(NH4)2(SO4)26H2O(s) + H2C2O4(aq)--> FeC2O42H2O(s) +
  97. Chemistry

    At 700 K, the equilibrium constant for the reaction NO2(g) « 2NO(g) + O2(g) is Kc = 4.79×10-3 (M), and the rate constant for the reaction 2NO(g) + O2(g) ® NO2(g) is k = 3.13×10^3 M^-2s^-1. What is the rate constant for the reaction NO2(g) ® 2NO(g) +
  98. Chemistry

    From the following data, calculate ΔH° for the reaction O3(g) +NO(g)----->O2(g)+NO2 (g) Compound ΔH°f (kJ/mol) O3 142.7 NO 90.3 O2 0 NO2 33.2
  99. CHEM

    Consider the reaction, 3 NO2(g) + H2O(l) ® 2 HNO3(aq) + NO(g), where DH = – 137 kJ. How many kilojoules are released when 92.3 g of NO2 reacts?
  100. chemistry

    2. What is the reduction half-reaction for the following unbalanced redox equation? Cr2O72– + NH4+ Cr2O3 + N2 A.) Cr2O3 -> Cr2O7^2– *B.) Cr2O72– -> Cr2O3 C.) NH4+ -> N2 D.) N2 -> NH4+ 3. Which oxidation-reduction reactions are best