What is the molecularity of the rate-determining step in the proposed mechanism? A) unimolecular H2(g) + 2NO(g) → N2O(g) + H2O(g) Step 1 (slow) B) bimolecular C) termolecular N20(g) + H2(g) → N2(g) + H2O(g) Step 2 (fast) D) Cannot be determined from given mechanism

What is the molecularity of the rate-determining step in the proposed mechanism? A) unimolecular H2(g) + 2NO(g) → N2O(g) + H2O(g) Step 1 (slow) B) bimolecular C) termolecular N20(g) + H2(g) → N2(g) + H2O(g) Step 2 (fast) D) Cannot be determined from given mechanism

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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Options for part a: Unimolecular, bimolecular, termolecular
Determine the rate law for the formation of oxygen predicted by this mechanism. (Assume the steady-state approximation is valid for any reaction intermediates.) k₁ CIO + CIO + M (CIO)₂ → CIOO + Cl (CIO)2 + sunlight k3 C100 + M k4 →→ Cl + O₂ 2x (C1 + 03 net: 2 033 0₂ → CIO + O₂) (this reaction occurs twice in the mechanism)
The reaction 2 H₂O₂ --> 2 H₂O + O₂ follows the mechanism: Step 1: H₂O2 (aq) + I¯‍(aq) --> H₂O(1) + 10¯(aq) SLOW Step 2: 10 (aq) + H₂O2(aq) --> H₂O(1) + O2(g) + l'(aq) FAST What is the molecularity of Step 2? bimolecular cannot be determined unimolecular termolecular
N2O4 -> 2NO2 The rate law is most likely: options: Rate = k[N2O4 ]1 Rate = k[N2O4 ]1[NO2]2 Rate = [NO2]2 Rate = [N2O4 ]1
Consider the following reaction mechanism for the addition of HCl to propene in the gas phase. The overall reaction is just HCI + CH3CH=CH2 → CH;CH2CH3, but the experimentally observed rate law is more complicated than that stoichiometry would suggest. 2 HCl 2 (HCI), k_1 k2 HCI + CH3CH = CH, 2 complex k_2 (HCI)2 + complex → CH3CHCICH3 (Here (HCl)2 is an HCl dimer and “complex" represents some intermediate species of unknown structure.) Assume that the third step is rate determining, and that the first two steps both remain in equilibrium throughout the reaction. d[CH;CHCICH3] Please write Derive an expression for the rate of formation of CH3CHCICH,' dt your final expression in the boxes. HINT: Be sure to use the equilibrium assumption, and not the steady state approximation. Your final rate law should NOT include the concentrations of any intermediates.
Based on the information below, determine the rate law. N2 + O2 --> 2 NO [N2] (M) [O2] (M) initial rate (M/s) Exp 1 0.040 0.020 707 Exp 2 0.040 0.010 500 Exp 3 0.010 0.010 125
For the reaction H2(g) + C2H4(g) ⟶⟶C2H6(g) A series of experiments were conducted as sown in the Table. If the rate law were found to be : rate = k[H2][C2H4] what is the missing initial rate (marked with a "?" in the Table)?
2 N₂O5(g) - → 4 NO₂(g) + O₂(g) Consider the decomposition of dinitrogen pentoxide shown above. In order to determine the rate of this reaction, we can measure the concentration of N2O5 at various time intervals throughout the reaction. The data and graph of [N205] verses time are shown below. Time (3) 0 200 400 600 800 1000 1200 1400 1600 1800 2000 M/sec (C) Which of the following is true as the reaction proceeds to longer times? Rate slows down because the concentration of reactant is smaller. Rate speeds up because the concentration of reactants is smaller. The rate slows down because the concentration of reactants is larger. Rate slows down because the concentration of product is larger. Rate speeds up because the concentration of product is larger. [N₂O₂] (M) 1.00 0.88 0.78 0.69 0.61 0.54 0.48 0.43 0.38 0.34 0.30 75- [NgO3] (M) 9 25 (A) What is the average rate of consumption of N2O5 in the first 400 seconds? NOTE: The sign is important! M/sec (B) What is the average rate of…
Consider the proposed mechanism for the reaction described by the equation 2NO2(g) + Br2(g) – 2NO2Br(g): (1) NO2(g) + Br2(g) – NO2B12(g) (fast) (2) NO2B12(g) – NO2B1(g) + Br(g) (slow) (3) Br(g) + NO2(g) → NO2B1(g) (fast) Which of the following is the properly-expressed rate law for the overall reaction that is consistent with the proposed mechanism? (Select one.) Rate = k [NO2(g))? [Br2(g)] O Rate = k [Br(g)] [NO2(g)] O Rate = k [NO2(g)] [Br2(g)] Rate = k [NO2Br2(g)]
Question 4 Calculate the frequency factor (A). Studies have shown that the reaction occurs via the following mechanism. ki Cl2O4 k-1 Step 1: 2 Cl02 (fast equilibrium) k2 Step 2: C2O4 + OH- → ClO;¯+HCIO2 (slow) k3 Step 3: HCIO2 + OH → ClO2¯+H2O (fast) Question 5: Identify the intermediate/s and the rate-determining step. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 → ClO3¯+HC1O2 Step 2: C204 + OH- (slow) k3 Step 3: HC1O2 + OH- ClO2- + H2O (fast) Question 6 Is the proposed mechanism consistent with the experimentally determined rate law? Show your solution to justify your answer. ki 2 ClO2 2 C2O4 k-1 Step 1: (fast equilibrium) k2 Step 2: C204 + OH- → ClO3¯+ HCIO2 (slow) k3 Step 3: HCIO2 + OH- → ClO2-+ H2O (fast) Question 7 Draw the transition state for Step 3. Identify the bond/s forming/breaking.
Q2: Nitramide decomposes in water according to the chemical equation, kobs N₂O + H₂O 0,N-NH, The observed rate law is the following, The proposed mechanism is: O,N-NH, = 1² +11 d[N₂0] dt = kobs [0,N – NH2] [H+] O,N-NH + H* N₂O O,N-NH H* + OH H₂O Fast Is the reaction mechanism consistent with the observed rate law? If so, what is the relationship between kobs and the rate constants of the individual steps? Fast Equilibrium + он Slow
for the following mechanism proposed wfor the decomposition of hydrogen peroxide using potassium bromide (see image) which of the following reactuin intermediates