Consider the oxidation of nitrogen monoxide with the observed rate law below. Rate = k(No)°C02J %3D 2 NO (g)+ O2cg) →2N2 (g) The proposed two-step mechanism is: I. NO (g) + Oz ( = NO3 NO 3 cg) (Fast, reversible) I NO3 c9) + NO lg) → 2 NO2 (9) (Slow) D. Write rate laws for the elementary steps. Give the molecularity for each step. E. Using rate laws from part d., determine a reasonable rate law for the overall process, including values for reaction orders. Is the mechanism reasonable and consistent with the observed rate law? Fully explain and show ALL work.

Consider the oxidation of nitrogen monoxide with the observed rate law below. Rate = k(No)°C02J %3D 2 NO (g)+ O2cg) →2N2 (g) The proposed two-step mechanism is: I. NO (g) + Oz ( = NO3 NO 3 cg) (Fast, reversible) I NO3 c9) + NO lg) → 2 NO2 (9) (Slow) D. Write rate laws for the elementary steps. Give the molecularity for each step. E. Using rate laws from part d., determine a reasonable rate law for the overall process, including values for reaction orders. Is the mechanism reasonable and consistent with the observed rate law? Fully explain and show ALL work.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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The reaction described by H, (g) + 1,(g) → 2 HI(g) has an experimentally determined rate law of rate = k [H2][I2] Some proposed mechanisms for this reaction are: Mechanism A (1) H, (g) + L,(g) 2 HI(g) (one-step reaction) Mechanism B (1) 1,(g) =2 1(g) (fast, equilibrium) k_1 (2) H, (g) + 2 I(g) –→ 2 HI(g) (slow) Mechanism C (1) I, (g) = 2 I(g) (fast, equilibrium) k_ k, (2) I(g) + H, (g) –→ HI(g)+H(g) (slow) (3) H(g)+I(g) → HI(g) (fast) Which of these mechanisms are consistent with the observed rate law? O mechanism A O mechanism B O mechanism C In 1967, J. H. Sullivan showed that this reaction was dramatically catalyzed by light when the energy of the light was sufficient to break the I-I bond in an I, molecule. Which mechanism or mechanisms are consistent with both the rate law and this additional observation? O mechanism B O mechanism C O mechanism A
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The reaction 2 N205(g) → 4 NO2(g) + O2(g) was studied and the rate of change of the concentration of O2 was found to be 3.65 mol L 15-1. Calculate the reaction rate (in mol L1s1). Reaction rate = i mol L-1s-1. eTextbook and Media Save for Later Attempts: 0 of 3 used Submit Answer
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Identify the molecularity of each elementary reaction in the table below. elementary reaction 2NO(g) + Br₂(g) 2NOBr(g) N₂O(g) → N₂(g) + 0(g) CH₂ CH₂ Br(aq) + OH(aq) CH₂CH₂OH(aq) + Br (aq) molecularity Ounimolecular Obimolecular O Cannot be determined. Ounimolecular Obimolecular O termolecular O quadrimolecular O termolecular O quadrimolecular Cannot be determined. unimolecular Obimolecular O Cannot be determined. O termolecular O quadrimolecular X G
tab esc slock ||| = OKINETICS AND EQUILIBRIUM Writing the rate law implied by a simple mechanism with an initi.... Suppose the formation of dinitrogen pentoxide proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) + O₂ (g). -NO₂(g) + O₂(g) k₁ 2 NO₂ (g) + NO₂ (g) → N₂O5 (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. Write the balanced chemical equation for the overall chemical reaction. BE 1 Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Explanation Q A @ 2 Check W S X # 3 E 0 rate = k 14 D $ 4 rate constant > R F % 5 © Stv T MacBook Pro 6 G We Y & 7 H 0-0 U 00 Ⓒ2022 McGraw Hill LLC. All R You * 00 00 8 S a (
Mechanism Suppose a reaction occurs with the following mechanism. All are elementary steps. Step 1: 0₂(9) 20(g) fast K₂ Step 2: O(g) + N₂(g) Step 3: O(g) + N(g) گی 3 NO(g) + N(g) slow very fast K3, NO(g) $ 4 % 5 6 What is the rate law for the rate-determining step? Rate =k,[0₂]² Rate = kr[O]² Rate-k,[O][N] Rate = kf[0₂]/k,[0]² Rate = k₂[O][N₂] Rate = K[0₂] & 7 What is the rate law for the forward reaction in step 1? Rate = kr[O]² Rate = kr[0₂] Rate =k+[0₂1² Rate = kr[0₂1² Rate = kf[0]² Rate =k+[0₂] What is the overall rate law for this reaction? Rate = k[N₂][0₂][N][0] MacBook Pro 8 ( 9 ☆ 88
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