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Atomic chlorine elimination may occur via the single step mechanism shown below. CI (g) + O2...
Atomic chlorine reconstitution may also occur via the single step mechanism shown below. CIO (g) + O (g) = CI (g) + O2 (g) What is the rate law for the reaction? O Rate = k[O] Rate = k Rate = k[CIO] Rate = k[CIO][O]
Atomic chlorine reconstitution may also occur via the single step mechanism shown below. CIO (g) + O (g) = Cl (g) + O2 (g) Which of the following is true for the reaction? O If temperature is increased, the activation energy of the reaction decreases O Neither is true O If the activation energy of the reaction is decreased, extent increases O Both are true
Determine the reaction type and write the complete mechanism for the elimination shown below. CI 100 C rxn type
Consider the mechanism below. Step 1: O, (g) + Br (g) BrO (g) + O, (g) Step 2: Bro (g) + O (g) Br (g) + 0 (s) Overall Reaction: 03 (g) +O (g) → 2 02 (g) The catalyst in this reaction is a) O3 b) BrO c) Br d) O2 6.
10. Consider the reaction that takes place via the mechanism below; STEP I: NO2(g) + CO(g) - NO(g) + CO2(e) (fast) STEP II: NO) + Cl2(e) - NOC12(e) (slow) Determine; (a) The reaction intermediate(s) (2 points) command (b) The rate determining step (2 points)
Atoms A and Z may form either single bonds or double bonds. Shown is an energy diagram for the formation of a single bond between A and Z from the individual atoms in the gas phase. AIR) Zle) A-Zig) Which diagram below corresponds to the reaction Alg) Zia) - AZ(9)? AZ A . ZR Ad Which dlagram below corresponds to the reaction A(g) +Z(g) - A-Z(g)? AEZIR) All Zig) AR) AR) + ZIR) Energy Aigle!
Overall rate In the question below the correct answer is B, how does that show agreement with the overall reaction which does not have any concentration of CL present? Questions 42-44 refer to the following information. When free Cl(g) atoms encounter O(8) molecules in the upper atmosphere, the following reaction mechanism is proposed to occur. Cl(g) +03(g) → C10(g) +02(g) CIO(g) + 03(g) → Cl(g) + 2 O2(g) 203(g) → 302(g) slow step fast step overall reaction AH-285 kJ/mol 42....
PIOS 4. Dintrogen pentoxide, N205, decomposes as shown below: 2 N205 (g) ---> 4 NO2(g) + O2(g) The reaction is first order and a plot of the concentration of N2O5 as a function time for an experiment at 55 °C is shown below. What are (i) the half-life: and (ii) the rate constant for reaction at 55 °C? [N205) vs time 0.0200 LE 0.015 (N205 0.010 0.005 O 100 200 300 400 500 600 700 timers 5. A possible mechanism...
Fill in the Blanks Consider the already balanced chemical reaction shown below: KCLO2(s)KCl(s) + O2(g) The oxidation state of K in KCLO2(s) = The oxidation state of Cl in KCLO2(s) = The oxidation state of O in KCLO2(s) = The oxidation state of K in KCl (s) = The oxidation state of Cl in Kcl(s) = The oxidation state of O in O2(g) = The element being oxidized is (K, CI, O) The element being reduced is (K, CI, O)
Help with this mechanism. Q4. (10 pts) Draw a mechanism for the reaction shown below, including all arrows and intermediates. Include both Steps 1 and 2 Step 1: Cl 0 Cl , DMSO; 1 hour at -78 °C Form 0 ond o Step 2: add EtgN; allow to rise from -78 °C to room temperature over 2h t Et3D 3