Consider the following mechanism for the decomposition of dinitrogen monoxide: N₂O(g) → N₂(g) + O(g) - (1) N₂O(g) + O(g) → N₂(g) + O₂(g) (2) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. O yes O no 0

Consider the following mechanism for the decomposition of dinitrogen monoxide: N₂O(g) → N₂(g) + O(g) - (1) N₂O(g) + O(g) → N₂(g) + O₂(g) (2) Write the chemical equation of the overall reaction: Are there any intermediates in this mechanism? If there are intermediates, write down their chemical formulas. Put a comma between each chemical formula, if there's more than one. O yes O no 0

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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9:53 AM Tue Nov 21 Question 18 of 20 Step 1 (slow) H₂O2(aq) + (aq) H2O(l) + IO-(aq) Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I¯(aq). What is the rate law for this reaction? Step 2 (fast) H₂O2(aq) + 10 (aq) → H₂O(l) + O2(g) + (aq) A) rate= K[H₂O₂] B) rate= K[H₂O₂]² C) rate= K[H₂O₂] [1] D) rate = K[H₂O₂] [10] E) rate = K[H₂O₂]²[1]/[H₂O] Tap here or pull up for additional resources 36% Submit
H2 reacts with ClF. Someone thinks this is the mechanism: H2(g) + ClF(g) → HCl(g) + HF(g) HCl(g) + ClF(g) → Cl2(g) + HF(g) (a) Write the balanced equation for the overall reaction. (b) Identify any intermediates in the mechanism, if any. (c) identify and catalysts in the mechanism, if any. (d) Write rate laws for each elementary reaction in the mechanism. (e) If the first step is slow and the second one is fast, what rate law do you expect to be observed for the overall reaction?
Consider the following reaction: 4 HBr(g) + O2(g) 2 H2O(g) + 2 Br2(g)(a) The rate law for this reaction is first order in HBr(g) and first order in O2(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 8.80e+03, what is the reaction rate when [HBr(g)] = 0.00429 M and [O2(g)] = 0.00758 M?Rate = _______ M/s.(c) What is the reaction rate when the concentration of HBr(g) is doubled, to 0.00858 M while the concentration of O2(g) is 0.00758 M?Rate = _______ M/s
[4] Consider the following mechanism for the reaction of nitric oxide and hydrogen: kı 2NO(g)+ H2(g) → N;O(g) + H¿O(g) slow k2 N,0(g) + H2(g) → N2(g) + H2O(g) fast (a) Write an equation for the overall reaction. (b) Write the theoretical rate law for the above mechanism. (c) Is a catalyst involved in the above mechanism? If so, what is it? (d) Are there any reaction intermediates? If so, list them.
The following mechanism has been proposed for the atmospheric destruction of ozone, O3 (g):O3 (g) + NO (g) --> O2 (g) + NO2 (g) (slow)NO2 (g) + O (g) --> NO (g) + O2 (g) (fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
The overall reaction of ozone reacting to form oxygen has been proposed to occur in a reaction mechanism of: Step 1: O3(g)-→O2(g) + O(g) Step 2: O3(g) + O(g) →202(g) What is the role of O(g) and what is the overall balanced equation? Periodic Table and Datasheet Select one: O a. O(g) is an intermediate; 203(g) + O(g) →302(g) + O(g) O b. O(g) is a catalyst; 203(g) + O(g)→302(g) + O(g) O c. O(g) is an intermediate; 203(g) → 302(g) O d. O(g) is a catalyst; 203(g)→302(g) Which statement best describes general equilibrium?
The following mechanism has been proposed for the reaction of H2 (g) and NO (g): H2 (g) + NO (g) → H2O (g) + N (g) (Slow)N (g) + NO (g) → N2 (g) + O (g) (Fast)H2 (g) + O (g) → H2O (g) (Fast)a) Write the equation for the overall balanced reaction. b) Write the rate law predicted by this reaction mechanism.
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +F₂ (g) → NO₂F (g)+F (g) 2 F (g) + NO₂ (g) → NO₂F (g) 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. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = & rate constant k₁ k₂
The chemistry of smog formation includes NO3 as an intermediate in several reactions. If Δ[NO3] / Δt is –21.58×104 mM/min in the following reaction, what is the rate of appearance of NO2? NO3(g)+NO(g)---->2NO2(g) Δ[NO2]/Δt= mM/min What is the rate of change in [NO2] in the following reaction if Δ[NO3] / Δt is –22.56×10–1 mM/min? 2NO3(g)---->2NO2(g)+O2(g) Δ[NO2]/Δt= mM/min
Suppose the reaction between nitric oxide and bromine proceeds by the following mechanism: step elementary reaction 1 NO (g) + Br₂ (g) → NOBr₂ (g) k₁ k₂ 2 NOBr₂ (g) + NO (g) → 2NOBr (g) 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. Write the experimentally- observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. 0 rate = k rate constant 010 X Ś
Consider the following reaction in aqueous solution: 5Br-(aq) +BrO3-(aq) +6H+(aq)→ 3Br2(aq) + 3H2O(l) If the rate of disappearance of Br–(aq) at a particular moment during the reaction is 2.5 x 10–4 mol L–1 s–1, what is the rate of appearance of Br2(aq) at that moment? Question 2 options: a) 2.1 x 10–4 mol L–1 s–1 b) 1.5 x 10–4 mol L–1 s–1 c) 7.2 x 10–4 mol L–1 s–1 d) 9.4 x 10–4 mol L–1 s–1
Consider the following reaction: O2(g) + 2 NO(g) 2 NO2(g)(a) The rate law for this reaction is first order in O2(g) and second order in NO(g). What is the rate law for this reaction?(b) If the rate constant for this reaction at a certain temperature is 7840, what is the reaction rate when [O2(g)] = 0.0162 M and [NO(g)] = 0.0299 M?Rate = _____ M/s.(c) What is the reaction rate when the concentration of O2(g) is doubled, to 0.0324 M while the concentration of NO(g) is 0.0299 M?Rate = _____ M/s