3.) A proposed mechanism for the formation of N2Os (g) from NO2 (g) and 03 (g) is NO2(g) + 03 (9) NO3(g) + O2(g) NO(g) + O2(g) N₂05 (9) Determine the rate law expression for the production of N2Os (g) given this mechanism.

3.) A proposed mechanism for the formation of N2Os (g) from NO2 (g) and 03 (g) is NO2(g) + 03 (9) NO3(g) + O2(g) NO(g) + O2(g) N₂05 (9) Determine the rate law expression for the production of N2Os (g) given this mechanism.

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

Section14.7: Reaction Mechanisms

Problem 2.2ACP

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The rate of photodecomposition of the herbicide piclo- ram in aqueous systems was determined by exposure to sunlight for a number of days. One such experiment produced the following results. (Data from R.T. Hedlun and C.R. Youngson, “The Rates of Photodecomposition of Picloram in Aqueous Systems," Fate of Organic Pesticides in tbe Aquatic Environment, Advances in Chemistry Series, #111, American Chemical Society (1972), 159—172.) Exposure Time, t (days) [Pidoram] (mol L_1) 0 4.14 X 10-6 7 3.70 X 10-6 14 3.31 X 10-6 21 2.94 X 10~6 28 2.61 X 10~6 35 2.30 X 10-6 42 2.05 X 10-6 49 1.82 X 10"6 56 1.65 X 10-6 Determine the order of reaction, the rate constant, and the half-life for the photodecomposition of picloram.
23.1b On the basis of the following proposed mechanism, account for the experimental fact that the rate law for the decomposition 2 N₂O5(g) → 4 NO₂(g) + O₂(g) is v=k[N₂O5]. (1) N₂O5NO2 + NO3 (2) NO₂ + NO3 → NO₂ + O₂ + NO (3) NO+N₂O5 → NO₂ + NO₂+NO₂ 23.2a A slightly different mechanism for the decomposition of N₂O5 from that in Exercise 23.1b has also been proposed. It differs only in the last step, which is replaced by (3) NO+NO3 →→ NO₂+NO₂ k3 Show that this mechanism leads to the same overall rate law. k₁, k₁ k₂ k3 23.2b Consider the following mechanism for the thermal decomposition of R₂: (1) R₂ → R+R (2) R+ R₂ → PB+R' (3) R' → PA+R (4) R+R PA + PB where R₂, PA, PB are stable hydrocarbons and R and R' are radicals. Find the dependence of the rate of decomposition of R₂ on the concentration of R₂. 16
The acid-catalyzed hydrolysis of sucrose occurs by the fol-lowing overall reaction whose kinetic data are given below:C₁₂H₂₂O₁₁(s) H₂O(l) →C₆H₁₂O₆(aq) C₆H₁₂O₆(aq) (a) Determine the rate constant and the half-life of the reaction.(b) How long does it take to hydrolyze 75% of the sucrose?(c) Other studies have shown that this reaction is actually sec-ond order overall but appears to follow first-order kinetics.(Such a reaction is called a pseudo–first-order reaction.) Sug-gest a reason for this apparent first-order behavior.
The mechanism for the reaction described by nust. A common d(a stronger whch ont of ice prhct NO,(g) + CO(g) → CO,(g) + NO(g) coor on be c is suggested to be (1) 2NO,(g) –→ NO,(g) + NO(g) k1 -> k2 (2) NO,(g) + CO(g) → NO,(g) + CO,(g) d[CO2] k[NO2]? %3D The experimental rate law for the production of [CO2] = k1 [NO2J² or dt d[NO3] 0 ), is this a valid mechanism? i.e show Assuming that [NO3] is governed by a steady state ( dt that using elementary reactions 1 and 2, the experimental rate law can found. (Hint write out all the ways d[NO3] = ? d[C02] = ? ) %3| and %3D dt that [NO3] and [CO2] are created and destroyed, dt owing clecre cel at 25 C NiC C)Cu a062 0.62 V 0.00 V 4. 460 V
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2.8b A second-order reaction of the type A + 2 B → P was carried out in a solution that was initially 0.075 mol dm−3 in A and 0.030 mol dm−3 in B. After 1.0 h the concentration of A had fallen to 0.045 mol dm−3 . (a) Calculate the rate constant. (b) What is the half-life of the reactants?
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A suggested mechanism for the decomposition of peroxide (H2O2) is H2O2(aq) ->>> 2OH(aq) H2O2(aq) + OH(aq) H2O()+ HO2(g) HO2(g) + OH(aq)) → H2O(l) + O2 (g) ->> Based on the mechanism which statement is true? (1) The rate law is rate = k[H202] (2) the molecularity of the slow reaction is 4 (4) OH2 is an intermediate (3) OH is a catalyst A Moving to the next question prevents changes to this answer. MacBook Pro fast slow fast
The following mechanism has been proposed for the gas phase reaction of H2 with ICl: H2 (g) + ICl(g) ---> HI (g) + HCl (g) HI (g) + ICl(g) ---> I2 (g) + HCl(g) (a) write the balanced equation for the overall reaction. (b) identify any intermediates in the mechanism. Group of answer choices A.) a) H2(g) + 2 ICl(g) --------> I2(g) + 2 HCl(g) b) HCl B.) a) H2(g) + 2 ICl(g) --------> I2(g) + 2 HCl(g) b) ICl C.) a) H2(g) + 2 ICl(g) --------> I2(g) + 2 HCl(g) b) HI D.) a) H2(g) + 2 ICl(g) + HI(g) --------> HI(g) + I2(g) + 2 HCl(g) b) HCl
The gas-phase decomposition of ozone is thought to oc- cur by the following two-step mechanism. Step 1: 03(8) = 02(8) + O(g) (fast) Step 2: 0(8) + O,(8) → 202(8) (slow) (a) Write the balanced equation for the overall reaction. (b) Derive the rate law that is consistent with this mecha- nism. (Hint: The product appears in the rate law.) (c) Is O a catalyst or an intermediate? (d) If instead the reaction occurred in a single step, would the rate law change? If so, what would it be?
The mechanism for the reaction described by the equation CH,NC(g) CH, CN(g) is suggested to be k1 (1) A(g) + M(g) = A" (g) + M(g) k-1 k2 * (2) А (g) → B(g) where A(g) is CH, NC(g), M(g) is any gas molecule, A* (g) is CH,NC*(g) (an energized gas molecule), and B(g) is CH,CN(g). Assuming that [A* ] is governed by steady-state conditions, derive the rate law for the production of CH, CN(g) in terms of [A], [M], and the appropriate k values.