A suggested mechanism for the gas phase decomposition of nitrous oxide is:step 1:NgÐ —Nz + 0N₂O + O N₂ + O2step 2:(a) Identify the molecularity of each step in the mechanism.step 18step 2(b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leaveit blank.8(c) Identify any intemediates and/or catalysts in this mechanism.Catalyst: Enter formula. If none, leave box blank:Intermediate: Enter formula. If none, leave box blank:The following mechanism has been proposed for the gas phase reaction of nitrogen monoxide with bromine.step 1:NO + Br₂ → NOBr₂NOBr₂ + NO 2 NOBrstep 2:(a) Identify the molecularity of each step in the mechanism.step 1step 2(b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leaveit blank.(c) Identify any intermediates and/or catalysts in this mechanism.Catalyst: Enter formula. If none, leave box blank:Intermediate: Enter formula. If none, leave box blank:

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A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1: Nz0 — Nz + 0 N₂O + O N₂ + O₂ step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leav it blank. + (c) Identify any intemediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate: Enter formula. If none, leave box blank:

A suggested mechanism for the gas phase decomposition of nitrous oxide is: step 1: Nz0 — Nz + 0 N₂O + O N₂ + O₂ step 2: (a) Identify the molecularity of each step in the mechanism. step 1 step 2 (b) Write the equation for the net reaction. Use the smallest integer coefficients possible. If a box is not needed, leav it blank. + (c) Identify any intemediates and/or catalysts in this mechanism. Catalyst: Enter formula. If none, leave box blank: Intermediate: Enter formula. If none, leave box blank:

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions

Section: Chapter Questions

Problem 89IL: The oxidation of iodide ion by the hypochlorite ion in the presence of hydroxide ions I(aq) +...

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The peroxydisulfate ion (S2O8-2) reacts with the iodide ion in aqueous solution via the reaction: S2O82-(aq) + 3I- → 2SO4(aq)+ I3-(aq). An aqueous solution containing 0.050 M of S2O8-2 ion and 0.072 M of I- is prepared, and the progress of the reaction followed by measuring [I-]. The data obtained is given in the table below. Time (s) 0.00 400.0 800.0 1200.0 1600.0 [I‑] (M) 0.072 0.057 0.046 0.037 0.029 Determine the average rate of disappearance of I- between 400.0 s and 800.0 s in M/s. Determine the average rate of disappearance of I- in the initial 400.0 s in M/s. Determine the average rate of disappearance of I- between 1200.0 s and 1600.0 s in M/s. Determine the concentration of S2O82- remaining at 400 s in M. Determine the concentration of S2O82- remaining at 800 s in M. Determine the concentration of S2O82- remaining at 1600 s in M.
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