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- The overall reaction of hydroxide radical with hydrogen gas occurs as follows: OH (g) + H2(g) – H20(g) + H'(g) Part A This reaction plays a significant role in the chemistry of the earth's atmosphere by eventually converting OH to HO, through the subsequent reaction of H with O2. HO2 is involved in the destruction of stratospheric ozone (J. Phys. Chem. A, 2006, 110. 6978). Determine the activation energy for the reaction of OH with H, reaction. O 16.4 kJ mol The rate constants for the reaction of OH with H2 were found to be 1.83x10' L mol s'at 107. °C and 5.68×10° L mol's at 37. C. -1 O -85.9 kJ mol -1 O -16.4 kJ mol O 54.8 kJ mol O 65.9 kJ mol25) Consider the following set of reactions. Assume that A, B, C and D are atoms. (1) A + A → B (2) А-В + С-D А-С-D-B (3) A + B-C → A-B-C Order these reactions in terms of increasing significance of the orientation probability (that is the A in the Arrhenius equation). А. (1) (2) < (3) В. (3) < (2) <(1) C. (1) < (3) <(2) D. (1) = (2) = (3) E. (1) < (2) = (3)The overall reaction of hydroxide radical with hydrogen gas occurs as follows: OH'g) + H,(g) – H0(g) + H'(g) Part A This reaction plays a significant role in the chemistry of the earth's atmosphere by eventually converting OH to HO, through the subsequent reaction of H with O,. HO, is involved in the destruction of stratospheric ozone (J. Phys. Chem. A, 2006, 110, 6978). Determine the activation energy for the reaction of OH with H, reaction. The rate constants for the reaction of OH with H, were found to be 5.54x10 L mol s at 36. C and 1.09x10 L molrs at -27. °C. -20.9 kJ mol1 O 18.3 kJ mol1 O 25.1 kJ mol O -18.3 kJ mol O 25.1 kJ mol
- In a study of the formation of HI from its elements,H₂(g)+I₂(g)→ 2HI(g) equal amounts of H₂ and I₂ were placed in a container, whichwas then sealed and heated.(a) On one set of axes, sketch concentration vs. time curves for H₂ and HI, and explain how Qchanges as a function of time.(b) Is the value of Qdifferent if [I₂] is plotted instead of [H₂]?2. The following sequence of steps has been proposed for the overall reaction between H₂ and Br₂ to form HBr: (1) Br2(g) 2Br(g) (2) Br(g) + H₂(g) HBr(g) + H(g) (3) H(g) + Br(g) HBr(g) Write the overall balanced equation and show that the overall Qc is the product of the Qc's for the individual steps.2) Suppose that we have 100 cm' of water (p = 1g.cm"), which is D;0 in a proportion of %3! 0.015% (D stands for deuterium, or H). a) Compute the energy (in J) that would obtain from this sample if all the deuterium were to be consumed in the reaction H + H - 'H+p, which is known to release an energy output of 4.0 MeV. b) As an alternative, compute the energy (in J) that would be released if two-thirds of the deuterium were fused (according to the previous reaction) to form 'H, which then combines with the remaining one third according to the reaction H+ 'H → *He +n, known to release an energy output of 17.6 MeV. c) Which of the processes a) or b) produces more energy? Given: N = 6.022x10" mot P. ->
- The nitric oxide molecule undergoes photodissociation in the upper atmosphere.The balanced reaction for the combustion of ethane is shown in the table. You allow 3.9 mol of ethane (C2H6) to react with 5.0 mol oxygen (02). Complete the following ICF table, which may be done using the Simulation, to indicate the amounts of all chemical species for the initial, change, and final conditions. Drag the appropriate amounts to their respective targets.This equation is related to Kinetic Isotope Effect. Subject Chemistry The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCs) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1)ClO(g)+O3(g)⟶Cl(g)+2O2(g)Δ?∘rxn=−122.8 kJ (2)2O3(g)⟶3O2(g)Δ?∘rxn=−285.3 kJ (3)O3(g)+Cl(g)⟶ClO(g)+O2(g) Δ?∘rxn= ?The 1995 Nobel Prize in Chemistry was shared by Paul Crutzen, F. Sherwood Rowland, and Mario Molina for their work concerning the formation and decomposition of ozone in the stratosphere. Rowland and Molina hypothesized that chlorofluorocarbons (CFCS) in the stratosphere break down upon exposure to UV radiation, producing chlorine atoms. Chlorine was previously identified as a catalyst in the breakdown of ozone into oxygen gas. Using the enthalpy of reaction for two reactions with ozone, determine the enthalpy of reaction for the reaction of chlorine with ozone. (1) CIO(g) + 0;(g) Cl(g) + 20,(g) AHxn = -122.8 kJ AHan = -285.3 kJ (2) 203(g) → 30,(g) (3) 0,(g) + Cl(g) → CIO(g) + 0,(g) AHn = ?SEE MORE QUESTIONS