**Title: Understanding the Mechanism and Rate Law of a Complex Reaction****Introduction:**In chemical kinetics, understanding the mechanism of a reaction and determining its rate law is essential. Here, we analyze the reaction involving chloride ions (Cl⁻), chlorate ions (ClO₃⁻), and hydrogen ions (H⁺), which leads to the formation of chlorine gas (Cl₂) and water (H₂O).**Reaction:**\[ 5 \, \text{Cl}^-(\text{aq}) + \text{ClO}_3^-(\text{aq}) + 6 \, \text{H}^+(\text{aq}) \rightarrow 3 \, \text{Cl}_2(\text{g}) + 3 \, \text{H}_2\text{O}(\text{l}) \]**Mechanism:**The reaction mechanism, which the overall reaction is expected to follow, involves several steps with varying rates:1. \(\text{ClO}_3^-(\text{aq}) + \text{H}^+(\text{aq}) \leftrightarrow \text{HClO}_3(\text{aq}) \) (Fast equilibrium, \(k_1\))2. \(\text{HClO}_3(\text{aq}) + \text{H}^+(\text{aq}) \leftrightarrow \text{H}_2\text{ClO}_3^+(\text{aq}) \) (Fast equilibrium, \(k_{-1}\))3. \(\text{Cl}^-(\text{aq}) + \text{H}_2\text{ClO}_3^+(\text{aq}) \rightarrow (\text{ClClO2})(\text{aq}) + \text{H}_2\text{O}(\text{l}) \) (Slow, \(k_2\))4. \((\text{Cl-ClO2})(\text{aq}) + 4 \, \text{H}^+(\text{aq}) + 4 \, \text{Cl}^-(\text{aq}) \rightarrow \text{products} \) (Fast)**Rate Law Determination:**From the mechanism, we can derive the rate law based on the rate

The slowest step of the reaction decides the rate of the reaction. So it is also called rate…

The reaction 5 CI (aq) + CIO3(aq) + 6 H*(aq) → 3 Cl₂(g) + 3 H₂O(l) is expected to obey the following mechanism: CIO3(aq) + H+ (aq) = www HCIO3(aq) HCIO3(aq) + H+ (aq) = - H₂CIO3(aq) CIT(aq) + H₂CIO3+ (aq) ₁ (CI-CIO₂)(aq) + H₂O(1) (CI-CIO₂) (aq) + 4 H*(aq) + 4 CI (aq) →→→ products What is the rate law for this reaction? 1. ratek [CI]² [CIO31]² [H+]² 2. rate = k [CI] [CIO3]² [H+]² 3. rate = k [CI]2 [CIO31² [H*] 4. rate = k [CI] [CIO3] [H+]² 5. rate = k [CI]2 [CIO3] [H*] O 4. rate = k [CI-] [CIO3-] [H+]2 O 2. rate = k [CI-] [CIO3-]2 [H+]2 O 1. rate= k [CI-]2 [CIO3-12 [H+]2 O 5. ratek [CI-]2 [CIO3-] [H+] O 3. rate = k [CI-12 [CIO3-]2 [H+] Fast equilibrium Fast equilibrium Slow Fast

The reaction 5 CI (aq) + CIO3(aq) + 6 H(aq) → 3 Cl₂(g) + 3 H₂O(l) is expected to obey the following mechanism: CIO3(aq) + H+ (aq) = www HCIO3(aq) HCIO3(aq) + H+ (aq) = - H₂CIO3(aq) CIT(aq) + H₂CIO3+ (aq) ₁ (CI-CIO₂)(aq) + H₂O(1) (CI-CIO₂) (aq) + 4 H(aq) + 4 CI (aq) →→→ products What is the rate law for this reaction? 1. ratek [CI]² [CIO31]² [H+]² 2. rate = k [CI] [CIO3]² [H+]² 3. rate = k [CI]2 [CIO31² [H] 4. rate = k [CI] [CIO3] [H+]² 5. rate = k [CI]2 [CIO3] [H] O 4. rate = k [CI-] [CIO3-] [H+]2 O 2. rate = k [CI-] [CIO3-]2 [H+]2 O 1. rate= k [CI-]2 [CIO3-12 [H+]2 O 5. ratek [CI-]2 [CIO3-] [H+] O 3. rate = k [CI-12 [CIO3-]2 [H+] Fast equilibrium Fast equilibrium Slow Fast

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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