# The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) „_ 2 NO2(g) The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7 x

17,082 results
1. ## chemistry

The standard molar entropy value of N2 (g) is 191.5 J/K-mol, of O2 (g) is 205.0 J/K-mol and of NO2 (g) is 240.0 J/K-mol. From these values we can calculate the Delta S for the reaction N2 (g) + 2 O2 (g) produces 2 NO2 (g) to be a. – 156.5 J/K b. 636.5

2. ## 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] is governed

3. ## 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

4. ## chem

For the elementary reaction NO 3 + CO → NO2 + CO 2 the molecularity of the reaction is __________, and the rate law is rate = __________. A) 2, k[NO 2][CO 2] B) 2, k[NO 3][CO]/[NO2 ][CO 2] C) 4, k[NO 3][CO][NO 2][CO 2] D) 4, k[NO 2][CO 2]/[NO 3][CO] E)

5. ## 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

6. ## 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

7. ## Chemistry

Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2 (g)+ H2O (l) --> 2HNO3 (l) + NO (g) Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of the reactant in excess

8. ## Chemistry

The reaction of NO and O2 produces NO2. 2 NO(g) + O2(g) „_ 2 NO2(g) The reaction is second-order with respect to NO(g) and first-order with respect to O2(g). At a given temperature, the rate constant, k, equals 4.7 x 10^2 M^¡V2s^¡V1. What is the rate

9. ## Chem

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

10. ## chemistry

Balance the following redox reaction occurring in acidic solution Cu(s) + NO3-(aq)--> Cu2+(aq) +NO2(g) This is what I have done so far Cu-->Cu2+ + 2e- 2H + NO-3 --> NO2 + H2O Need help please

11. ## Calculus

4. At high temperatures, nitrogen dioxide, NO2, decomposes into NO and O2. If y(t) is the concentration of NO2 (in moles per liter), then at 600 degrees K, y(t) changes according to the reaction law dy/dt = −. 05y2 for time t in seconds. A. Express y in

12. ## chem

For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) Later during the reaction, the rate of consumption of N2O5 was determined to be 0.0080 M/s. What was the rate of formation of NO2 and of O2 at this point in time?

13. ## Chemistry due soon

If the following reaction: NO(g) + 1/2O2(g) NO2(g) has the following enthalpy change: H° = -56 kJ/mol What is the enthalpy of the decomposition reaction of 2 moles of NO2? A. 112 kJ B. 56 kJ C. -56 kJ D. -112 kJ i think the answer is d

14. ## 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?

15. ## Chem

O3 + NO --> O2 + NO2 Write the rate law equation for the reaction. Explain how you obtained your answer. Experiment 1: [O3] .0010 [NO] .0010 Rate of formation of NO2 x Experiment 2: [O3] .0010 [NO] .0020 Rate of formation of NO2 2x Experiment 3: [O3] .0020

16. ## chem

For the reaction 3NO2 + H2O  2HNO3 + NO, how many grams of HNO3 can form when 1.00 g of NO2 and 2.25 g of H2O are allowed to react? This is a limiting reagent problem. 1. Write the equation. You have done that and it is balanced. 2. Convert 1.00 g NO2 and

17. ## chemistry

How many grams of NO2 will be produced when 5.00 moles of NO react? I have 5 moles of NO2 produces 5 moles of NO (1:1ratio) mass (g)=5 moles times 16.02g/mol=80.1g

18. ## chemistry

For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) The experimental data for this reaction is : t = 0.0 s [N2O5] = 0.80 M [NO2] = 0.0 M [O2] = 0.0 M t = 20.0 s [N2O5] = 0.60 M [NO2] = 0.40 M [O2] = 0.10 M How much N2O5 was consumed during the 20.0 s time

19. ## 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 the

20. ## Chemistry

Consider the reaction for the production of NO2 from NO: 2 NO(g) + O2(g) = 2 NO2(g) a)If 84.8L of O2(g), measured at 35 degrees Celsius and 632mm Hg, is allowed to react with 158.2g of NO, find the limiting reagent. b) If 97.3L of NO2 forms, measured at 35

21. ## 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

22. ## Chemistry

Each molecule of NO2, nitrogen dioxide, consists of 1 atom of N and 2 atoms of O. If you have 0.155 g. of NO2, how many molecules of NO2 do you have ? If you could, please include steps as to how to do the problem. Thank you

23. ## 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

24. ## 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

25. ## chemistry help

predict the geometries of the complexes from these reactions: 1- [pt(NO2)cl3)]2- + NH3 --> [pt(NO2)(NH3)cl2]-1 +cl- 2-cis-[pt(RNH2)2(NH3)(NO2)]+1 + cl- --> Pt(RNH2)(NH3)(NO2)Cl + RNH2

26. ## chem

Which of the following is true about the following reaction when an amount of NO₂ (g) is added to the equilibrium reaction? N₂O₄ (g) ⇄ 2 NO₂ (g)

27. ## Inorganic chemistry

Nitrogen dioxide reacts with carbon monoxide to produce nitrogen monoxide and carbon dioxide. NO2(g) + CO(g) ==>NO(g) + CO2(g) A proposed mechanism for this reaction is 2No2(g) = NO3(g) + NO(g) (fast,equilibrium) NO2(g) + CO(g) ==> NO2(g) + CO2(g) (slow)

28. ## 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

29. ## Chemistry

Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen 14) monoxide and oxygen according to the following chemical equation. 2 NO2(g) → 2 NO(g) + O2(g). A sample of NO2(g) is initially placed in a 2.50-L reaction vessel at

30. ## chemistry

a flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 degrees celsius and allowed to reach equilibrium.when equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. (a) what are the

31. ## chemistry

The following kinetic data were obtained for the reaction: NO2(𝑔)+O3(𝑔)→NO3(𝑔)+O2(𝑔) Experiment: Initial [NO2](M): Initial [O3](M): Initial Rate(M/s): 1 0.21 0.70 6.3 2 0.21 1.39 12.5 3 0.38 0.70 11.4 Find the reaction order for each reactant

32. ## science

For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) The experimental data for this reaction is : t = 0.0 s [N2O5] = 0.80 M [NO2] = 0.0 M [O2] = 0.0 M t = 20.0 s [N2O5] = 0.60 M [NO2] = 0.40 M [O2] = 0.10 M What is the average rate of reaction during this

33. ## chemical equilibrium

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

34. ## 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. 1.0 M ;

35. ## 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

36. ## Limiting Reactant (Chemistry)

What is the limiting reactant for the following reaction if there are 3.4 moles of Ca(NO2)2 and 2.4 moles of Li3PO4? 3Ca(NO2)2 + 2Li3PO4 --> 6LiNO2 + Ca3(PO4)2 A)Ca(NO2)2 B) Li3PO4 C) LiNO2 D) Ca3(PO4)2

37. ## Chemistry

The gram-formula mass of NO2 is defined as the mass of one mole of a. one mole of NO2 b. one molecule of NO2 c. two moles of NO d. two molecules of NO Explain why.

38. ## 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?

39. ## Chem 2

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

40. ## 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?

41. ## Chemistry Help!

The reaction is O3 + NO arrow O2 + NO2 If 0.740 g O3 reacts w/ 0.670g of NO, how many grams of NO2 will be produced? I've tried to solve this. but I can't seem to get the right answer

42. ## 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, R=k[NO2]2

43. ## Chemistry

The decomposition of dinitrogen tetroxide produces nitrogen dioxide: N2O4 (g) ---> 2 NO2(g) ΔG°= 2.80 kJ/mol Find the minimum partial pressure of N2O4 at which the reaction is spontaneous if P(NO2)=2.00 bar and T=298 K.

Using this data, 2 NO(g) + Cl2(g) == 2 NOCl(g) Kc = 3.20 X 10-3 NO2(g) == NO(g) + ½ O2(g) Kc = 3.93 calculate a value for Kc for the reaction, NOCl (g) + ½ O2 (g) == NO2 (g) + ½ Cl2 (g) I do not understnad how I am suppose to use the Kc values given if

45. ## 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

46. ## Chemistry

Nitrogen dioxide decomposes at 300°C via a second-order process to produce nitrogen 14) monoxide and oxygen according to the following chemical equation. 2 NO2(g) → 2 NO(g) + O2(g). A sample of NO2(g) is initially placed in a 2.50-L reaction vessel at

If the following reaction: NO(g) + 1/2O2(g) NO2(g) has the following enthalpy change: H° = -56 kJ/mol What is the enthalpy of the decomposition reaction of 2 moles of NO2? A. 112 kJ B. 56 kJ C. -56 kJ D. -112 kJ i think the answer is d

48. ## Chemistry

The reaction between nitric oxide (NO) and oxygen to form nitrogen dioxide (NO2) is a key step in photochemical smog formation. 2 NO(g) + O2(g) 2 NO2(g) (a) How many moles of NO2 are formed by the complete reaction of 0.404 mole of O2? (b) How many grams

49. ## 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?

50. ## 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] = ?

51. ## 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?

52. ## 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?

53. ## Chemistry Equilibrium

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

54. ## Chemistry

Question 6: 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 (If that was jumbled up i Dont understand?

55. ## 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.

56. ## 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?

57. ## chemistry

For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) After the reaction had run for a while, 0.40 M of N2O5 was consumed. What was the molarity of the NO2 and O2 made?

58. ## Chem

The brown color associated with photochemical smog is due to NO2(g). This is involved with the following equilibrium in the atmosphere: 2 NO2(g) N2O4. Predict the signs of the enthalpy and entropy changes for this reaction. If the equation is at

59. ## chemistry

how do i solve the following problem? Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300°C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of Disappearance of NO2 for this

60. ## chemistry

how do i solve the following problem? Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300°C, [NO2] drops from 0.0100 to 0.00650 M in 100 s. The rate of Disappearance of NO2 for this

61. ## 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. -d(NO2)/dt

62. ## 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, R=k[NO2]2

63. ## 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

64. ## 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 each step.

65. ## 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

66. ## 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.

67. ## 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

68. ## 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, and O2 is

69. ## Chemistry

When a sample of NO2(g) (849.9 grams) is placed in 390.0 L reaction vessel at 961.0 K and allowed to come to equilibrium the mixture contains 248.2 grams of NO(g). What is the concentration (mol/L) of NO2(g)? 2NO2(g) = 2NO(g)+O2(g) I keep getting .0212 or

70. ## Chemistry

Please help me! I don't know how to do this at all. Calculate the enthalpy for the reaction: NO (g) + O (g) → NO2 Given the following known reactions: NO(g)+O3 (g)→NO2 (g)+O2 (g) 03 (g)→1.5O2 (g) O2 (g)→2O(g) ΔH°=-198.9kJ ΔH°=-142.3kJ

71. ## 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?

72. ## Chemistry

NO(g) + CO2(g) NO2(g) + CO (g) ƒ´H¢X = ¡V100 kJ Which of the following will favor the forward reaction?Why? A) add NO B) remove NO2 C) decrease the volume of the container D) raise the temperature E) add CO

73. ## egweg

For the reaction: 2 N2O5 (g) → 4 NO2 (g) + O2 (g) Later during the reaction, the rate of consumption of N2O5 was determined to be 0.0080 M/s. What was the rate of formation of NO2 and of O2 at this point in time?

74. ## 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) +

75. ## Chem II Oxidation Reduction

NO2 ----> NO2^-1 + NO3^-1 which N do you use? I have N being +4 on the reactant side, then as a +3 on for the NO2^-1 and +5 for the NO3^-1. Do you add the N's together on the product side? Then what about the rest of the equation? You leave out all the O,

76. ## chem

A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25°C, and the following equilibrium is achieved. N2O4(g)-> 2 NO2(g) After equilibrium is reached, the partial pressure of NO2 is 0.504 atm. (a) What is the equilibrium partial

77. ## 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. -d(NO2)/dt

78. ## 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

79. ## 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] = ?

80. ## 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?

81. ## 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

82. ## 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

83. ## chemistry

*This is part of an exam. so please don't give full solution* just trying to bump ahead of a block. The decomposition of NO2 at room temperature exhibits the following variation in concentration with time: The concentration of NO2 is expressed in

84. ## chemistry

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

85. ## Chemistry

92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate. N2O4 (g) --> 2NO2 (g) The mixture of N2O4 and NO2 resulting from the reaction occupies 36.0 liters at a total pressure of 773 mmHg and 45 °C. A. Let x equal the moles of N2O4 that

86. ## AP Chem

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

87. ## 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

88. ## chemistry

hi, I have redone this question. Is this right. How many grams of NO2 will be produced when 5.00 moles of NO react? 5 moles of NO2 produces 5 moles of NO (1:1ratio) mass(g) = 5 moles * 46g/mol = 230g

89. ## 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.

90. ## chemistry

Hi, I can't figure out how to start this one. I know I need to figure out the proportions or something of that sort. Any help is greatly appreciated Thanks! Calculate ƒ¢H for the reaction NO(g) + O(g) ¨ NO2(g) given the following: NO(g) + O3(g) ¨

91. ## 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.

92. ## 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.

93. ## 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.

94. ## 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.

95. ## chemistry

predict the geometries of the complexes from these reactions: 1- [pt(NO2)cl3)]2- + NH3 --> [pt(NO2)(NH3)cl2]-1 +cl- 2-cis-[pt(RNH2)2(NH3)(NO2)]+1 + cl- --> Pt(RNH2)(NH3)(NO2)Cl + RNH2

96. ## chemistry

predict the geometries of the complexes from these reactions: 1- [pt(NO2)cl3)]2- + NH3 --> [pt(NO2)(NH3)cl2]-1 +cl- 2-cis-[pt(RNH2)2(NH3)(NO2)]+1 + cl- --> Pt(RNH2)(NH3)(NO2)Cl + RNH2

97. ## Chemistry

Part 1: Each molecule of NO2, nitrogen dioxide, consists of 1 atom of N and 2 atoms of O. If you have 0.155 g. of NO2, how many molecules of NO2 do you have ? 2030000000000000000000 was the correct answer Part 2: How many atoms of N do you have ?

98. ## Science

The rate law for the reaction NO + O2 > NO2 is R=k[NO][O2]. what will be the effect on the reaction rate if the partial pressure of NO is doubled? What will the effect be if the partial pressure of O2 is tripled? My answer: More NO2 would be produced if NO

99. ## Chemistry

What is the correct rate law for the following reaction? 2 NO2(g) + F2(g) → 2 NO2F(g) rate = kf(NO)2 rate = -kf(NO2)2(F2) rate = kf(NO2)2(F2) rate = -kf(F2) Not enough information is available to determine the rate law.

100. ## Chemistry

As an environmental chemist, you want to find the Kc for the following reaction: 2 NO2 (g) ⇌ N2 (g) + O2 (g) Kc = ? Use the following data to find the unknown Kc : ½ N2(g) + ½ O2(g) ⇌ NO (g) Kc = 4.8 x 10-10 2 NO2(g) ⇌ 2 NO (g) + O2 (g) Kc = 1.1 x