2H₂ NO H₂O 2 H₂0 Consider the following proposed reaction mechanism: N₂0 H₂ 2 N₂0₂ 2N₂ N₂0₂ Step 1: NO + NO N202 Step 2: N202 + H2 - N2O + H2O The reactants in the overall reaction are (include their correct coefficients): 2 NO 2 N₂0 Step 3: N2O + H2-N2 + H20 The second step is the slow (rate-determining) step. Answer the following questions: What is the correct rate law for the overall reaction? O rate= K[NO]²[H₂1² O rate = K[NO]²[H₂] Orate = K[N₂0₂][H₂] O rate = K[N₂0₂]²[H₂] The products in the overall reaction are (include their correct coefficients): N₂ U O NO 2 H₂0 H₂ 2 H₂ 2 N₂0 N₂0₂ 2 NO N₂0 H₂0 2 N₂0₂ 2N₂ The intermediates in the mechanism are: 00 O N₂0 H₂O NO N₂ N₂0₂ H₂

2H₂ NO H₂O 2 H₂0 Consider the following proposed reaction mechanism: N₂0 H₂ 2 N₂0₂ 2N₂ N₂0₂ Step 1: NO + NO N202 Step 2: N202 + H2 - N2O + H2O The reactants in the overall reaction are (include their correct coefficients): 2 NO 2 N₂0 Step 3: N2O + H2-N2 + H20 The second step is the slow (rate-determining) step. Answer the following questions: What is the correct rate law for the overall reaction? O rate= K[NO]²[H₂1² O rate = K[NO]²[H₂] Orate = K[N₂0₂][H₂] O rate = K[N₂0₂]²[H₂] The products in the overall reaction are (include their correct coefficients): N₂ U O NO 2 H₂0 H₂ 2 H₂ 2 N₂0 N₂0₂ 2 NO N₂0 H₂0 2 N₂0₂ 2N₂ The intermediates in the mechanism are: 00 O N₂0 H₂O NO N₂ N₂0₂ H₂

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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Consider the following two-step mechanism for a reaction: NO₂(g) + Cl₂(g) →CINO₂(g) + Cl(g) Slow NO₂(g) + Cl(g) →CINO₂ (g) Fast Part A What is the overall reaction? Express your answer as a chemical equation. Identify all of the phases in your answer. 0 12 Submit Part B ΑΣΦ A chemical reaction does not occur for this question. Request Answer Identify the intermediates in the mechanism. Check all that apply. ✔ NO₂ (g) CINO₂(g) Cl(g) ✔ Cl₂ (g) Submit www ? Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining
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The following data were obtained for the reaction below at 25.0 °C. 2 NO(g) + O2(g) → 2 NO2(g) Trial 1 2 3 Initial Reactant Concentration (M) [NO] 0.030 0.030 0.060 [0₂] 0.0055 0.0110 0.0055 Initial Rate (M/s) 8.55 x 10-3 1.71 x 10-² 3.42 x 10-² Using the rate law you determined previously, calculate the initial rate for an experiment in which the initial concentration of NO is 0.100 M and O₂ is 0.050 M. Round your answer to 2 sig figs and include your units in your answer.
10 Chlorine gas reacts with aqueous hydrogen sulfide (also known as hydrosulfuric acid) to form elemental sulfur and hydrochloric acid. Cl2(g) + H2S(aq) → S(s) + 2HCl(aq) A proposed mechanism for this reaction is Step 1 Cl2 + H2S → Cl+ + HCl + HS- Step 2 Cl + HS¯ → HCl + S (slow) (fast) Sketch a potential energy diagram for this reaction, with labels to identify activation energy, transition state, rate-determining step, and any reaction intermediate.
Some measurements of the initial rate of a certain reaction are given in the table below. [H2] [12] initial rate of reaction 2.42M 1.68 M 0.0836M/s 2.42M 3.71 M 0.185 M/s 0.848 M 1.68 M 0.0293 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k☐ k = = 0 x10 ☐ □·□
Analyze the following reaction mechanism: 1. H₂O2 → H₂O + O 2. O + CF₂Cl2 → CIO + CF₂CI 3. CIO + O3 → CI + 20₂2 4. CI+ CF₂CI → CF₂Cl2 Identify the reaction intermediates in this reaction. A) O, CIO, CI B) CI, CF₂CI, CF₂Cl2 C) O, CIO, O, H₂O D) O, CIO, CI, CF₂CI E) O, CIO, CI, CF₂Cl2 ULL
Calculate the average reaction rate for each time interval in moles of NO2 produced per liter per minute. 0-100 s 500-600 s 1100-1200 s
The following data were collected for the reaction between hydrogen and nitric oxide at 700°C. 2 H2(g) + 2 NO(g) - 2 H20(g) + N2(g) Experiment [H2]/M [NO]/M Initial rate/M-s-1 0.012 0.031 4.5x10-6 0.0060 0.031 2.2x10-6 3 0.012 0.0155 1.1x10-6 (a) What is the rate law for the reaction? (Rate expressions take the general form: rate = k. [A]ª . [B]b.) chemPad Help Greek - (b) Calculate the rate constant for the reaction. 4.0 (c) Suggest a plausible reaction mechanism that is consistent with the rate law. (Hint: Assume that the oxygen atom is the intermediate. Omit states-of-matter from your answer.) First step: chemPad Help Greek - Second step: chemPad Help Greek
Consider the mechanism. step 1: A + B, АB + B, → AB + B step 2: — В, + А 2В, — в, + В overall: Which species is an intermediate? Which species is a catalyst? O B2 B2 B, O АВ about us privacy policy terms of use contact us help careers 耳

A mechanism for a reaction is shown below. Step 1 2 NO(g) ⇄ N2O2(g) (fast) Step 2 N2O2(g) + O2(g) → 2 NO2(g) (slow) a) What is the overall reaction that this mechanism describes? b) Assuming this mechanism is plausible, what is the rate law for the overall reaction? c) Identify any catalysts or intermediates in the mechanism.