2NO2(g) + F2(g) -> NO2F(g) H°rxn = -284 kJ/molrxn NO2(g) and F2(g) can reactto produce NO2F(g), as represented above. A proposed mechanism for the reaction has two elementary steps, as shown below. Step 1: NO2 + F2 -> NO2F + F          (slow) Step 2: NO2 + F -> NO2F         (fast) a.) Write a rate law for the overall reaction that is consistent with the proposed mechanism. b.) On the incomplete reaction energy diagram below, draw a  curve that shows the following two details. The relative activation energies for the two elementary steps  The enthalpy change of the overall reaction

Which of the following is true concerning the reaction energy diagram below: Reaction progress O The reaction produces 3 reaction intermediates. O The overall reaction is exothermic. O The 3rd elementary step is the rate-determining step. O The reaction mechanism includes 4 elementary steps. Energy

Based on the provide elementary steps below, determine the net reaction. NO2Cl(g) ---->  NO2(g) + Cl (g) elementary step 1 NO2Cl(g) + Cl (g) ----> NO2(g) + Cl (g) elementary step 2

question 8

For the reaction   2NO + Cl2  ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above            NO + Cl2  NOCl2     fast equilibriumNOCl2 + NO  2NOCl     slow            2NO  N2O2     fast equilibriumN2O2 + Cl2  2NOCl     slow            Cl2  2Cl     slowCl + NO  NOCl     fast            NO + Cl2  NOCl + Cl     slowCl + NO  NOCl     fast

(39 of 41) According to the reaction mechanism in Question 37, please identify all reaction intermediates. A H₂O I H 1) CH3MgBr 2) H3O+ CH3 B OH D F OH X 5 CH3 E H L -H G

8. Thallium (1) is oxidized by cerium (IV) as follows: TI+ + 2 Ce+ → T1³+ + 2Ce³+ The elementary steps are as follows: 1. Ce4+ + Mn²+ Ce³+ + Mn³+ 2. Ce4+ + Mn³+ Ce³+ + Mn4+ 3. TI+ + Mn4+ → T1³+ + Mn²+ a) Add all reactants and products and obtain the overall reaction. b) Identify the catalyst and intermediate. c) Determine which is the rate determining step if the rate law for the reaction is Rate = k(Ce4+][ Mn²+]

A reaction has the following proposed mechanism: A2(g) + B(s)-> A₂B(s) (fast) A₂B(s)-> A(g) + AB(s) (slow) AB(s) + C(g) -> AC(g) + B(s) (fast) A(g) + C(g) -> AC(g)(fast) For this mechanism, the species B would best be classified as a(n) O heterogeneous catalyst homogeneous catalyst intermediate transition state structure product of the overall reaction

The reaction Cl2(g) + CHCl3(g) --> CCl4(g) + HCl(g) proceeds through the following mechanism: Cl2(g) --> 2 Cl(g)Cl(g) + CHCl3(g) --> HCl(g) + CCl3(g)Cl(g) + CCl3(g) --> CCl4(g) (a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [Cl2] [CHCl3]Rate = k [Cl2]2 [CHCl3]     Rate = k [Cl2] [CHCl3]2Rate = k [Cl2]1/2 [CHCl3] Rate = k [Cl2] [CHCl3]1/2 Rate = k [Cl2]2 Rate = k [Cl2]2 [CHCl3]1/2 (b) What would the rate law be if the first step of this mechanism were rate-determining? Rate = k [Cl2] [CHCl3] Rate = k [Cl2]2 [CHCl3]     Rate = k [Cl2] [CHCl3]2 Rate = k [Cl2]1/2 [CHCl3] Rate = k [Cl2] [CHCl3]1/2 Rate = k [Cl2]2 Rate = k [Cl2]2 [CHCl3]1/2 Rate = k [Cl2]