4. N₂Os(g) decomposes according to the following reaction: 2N2O5(g) → 4NO₂(g) + O₂(g) The experimentally observed rate l

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4 N Os G Decomposes According To The Following Reaction 2n2o5 G 4no G O G The Experimentally Observed Rate L 1 (98.13 KiB) Viewed 28 times

4. N₂Os(g) decomposes according to the following reaction: 2N2O5(g) → 4NO₂(g) + O₂(g) The experimentally observed rate law is: Rate = k[N₂05] The following mechanism has been proposed for the reaction. Show that the mechanism is consistent with the observed rate law. N₂O5 + NO 1 K-1 NO₂ NO + N₂O5 3 K₂ K3 NO₂ + NO NO₂ 3 + NO + O 3NO₂ -A[N₂05] At 2 2HI(g) = 5. In the gas phase, hydrogen and iodine react to form hydrogen iodide according to the following chemical equilibrium: H₂(g) + 1₂(g) In one experiment, 2.000 mol each of hydrogen and iodine are placed in a 10.00 L reaction vessel held at 730 K. At equilibrium, the concentration of 12 was determined to be 0.0440 mol L.¹. Determine the value of the equilibrium constant Kc, for this reaction. What is the value of K₂?