Textbook Question
Ozone in the upper atmosphere can be destroyed by the following two-step mechanism: Cl1g2 + O31g2¡ClO1g2 + O21g2 ClO1g2 + O1g2¡Cl1g2 + O21g2 (b) What is the catalyst in the reaction?
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Ch.14 - Chemical Kinetics
Chapter 14, Problem 110
The following mechanism has been proposed for the gasphase reaction of chloroform 1CHCl32 and chlorine: Step 1: Cl21g2 Δ k1 k - 1 2 Cl1g2 1fast2 Step 2: Cl1g2 + CHCl31g2 ¡k2 HCl1g2 + CCl31g2 1slow2 Step 3: Cl1g2 + CCl31g2 ¡k3 CCl4 1fast2 (a) What is the overall reaction?
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Reaction Mechanism
A reaction mechanism is a step-by-step description of the pathway through which reactants are converted into products. It outlines individual elementary steps, including the sequence of bond-breaking and bond-forming events. Understanding the mechanism helps in predicting the rate of reaction and the overall stoichiometry of the process.
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03:06
Reaction Mechanism Overview
Rate-Determining Step
The rate-determining step (RDS) is the slowest step in a reaction mechanism that controls the overall reaction rate. In the provided mechanism, the second step is identified as slow, indicating that it is the RDS. Recognizing the RDS is crucial for understanding how changes in conditions can affect the reaction rate.
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01:15Rate Law Determination
Overall Reaction Equation
The overall reaction equation summarizes the net change from reactants to products, combining all elementary steps while canceling out intermediates. To derive the overall reaction from the mechanism, one must add the individual steps and eliminate any species that appear on both sides of the equation, leading to a balanced representation of the chemical transformation.
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07:02Overall Reaction Equilibrium Constant
Related Practice
Textbook Question
The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.
Step 1: O3(g) ⇌ O2(g) + O(g) (fast)
Step 2: O(g) + O3(g) → 2 O2 (slow)
(b) Derive the rate law that is consistent with this mechanism. (Hint: The product appears in the rate law.)
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Textbook Question
The gas-phase decomposition of ozone is thought to occur by the following two-step mechanism.
Step 1: O3(g) ⇌ O2(g) + O(g) (fast)
Step 2: O(g) + O3(g) → 2 O2 (slow)
(d) If instead the reaction occurred in a single step, would the rate law change? If so, what would it be?
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Textbook Question
In a hydrocarbon solution, the gold compound (CH3)3AuPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AuPH3. The following mechanism has been proposed for the decomposition of (CH3)3AuPH3:
Step 1: (CH3)3AuPH3 k1 k -1 (CH3)3Au + PH3 (fast)
Step 2: (CH3)3Au k2 C2H6 + (CH3)Au (slow)
Step 3: (CH3)Au + PH3 ¡k3 1(CH3)AuPH3 (fast)
(c) What is the molecularity of each of the elementary steps?
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Textbook Question
In a hydrocarbon solution, the gold compound (CH3)3AuPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AuPH3. The following mechanism has been proposed for the decomposition of (CH3)3AuPH3:
Step 1: (CH3)3AuPH3 k1 k -1 (CH3)3Au + PH3 (fast)
Step 2: (CH3)3Au k2 C2H6 + (CH3)Au (slow)
Step 3: (CH3)Au + PH3 ¡k3 1(CH3)AuPH3 (fast)
(e) What is the rate law predicted by this mechanism?
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Textbook Question
In a hydrocarbon solution, the gold compound (CH3)3AuPH3 decomposes into ethane (C2H6) and a different gold compound, (CH3)AuPH3. The following mechanism has been proposed for the decomposition of (CH3)3AuPH3:
Step 1: (CH3)3AuPH3 k1 k -1 (CH3)3Au + PH3 (fast)
Step 2: (CH3)3Au k2 C2H6 + (CH3)Au (slow)
Step 3: (CH3)Au + PH3 ¡k3 1(CH3)AuPH3 (fast)
(f) What would be the effect on the reaction rate of adding PH3 to the solution of (CH3)3AuPH3?
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