7.A valid mechanism for a reaction is given below.Step 1: NO (g) + Cl2 (g) → NOCI2 (g)Step 2: NOCI2 (g) + NO (g) -→ 2 NOCI (g)What is the overall reaction?Identify any reactive intermediate

The overall chemical reaction can be obtained by the given elementary steps. The overall chemical…

Answered: 7. A valid mechanism for a reaction is…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter16: Reaction Rates

Section: Chapter Questions

Problem 79A

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A proposed mechanism for the reaction of NO2 and CO is Step 1: Slow, endothermic 2 NO2(g) NO(g) + NO3(g) Step 2: Fast, exothermic NO3(g) + CO(g) NO2(g) + CO2(g) Overall Reaction: Exothermic NO2(g) + CO(g) NO(g) + CO2(g) (a) Identify each of the following as a reactant, product, or intermediate: NO2(g), CO(g), NO3(g), CO2(g), NO(g). (b) Draw a reaction coordinate diagram for this reaction. Indicate on this drawing the activation energy for each step and the overall enthalpy change.
The plot below shows the number of collisions with a particular energy for two different temperatures. a. Which is greater, T2 or T1? How can you tell? b. What does this plot tell us about the temperature of the rate of a chemical reaction? Explain your answer.
The reaction of NO2(g) and CO(g) is thought to occur in two steps to give NO and CO2: Step 1: Slow NO2(g) + NO2(g) NO(g) + NO3(g) Step 2: Fast NO3(g) + CO(g) NO2(g) + CO2(g) (a) Show that the elementary steps add up to give the overall, stoichiometric equation. (b) What is the molecularity of each step? (c) For this mechanism to be consistent with kinetic data, what must be the experimental rate equation? (d) Identify any intermediates in tins reaction.
What is the difference between average rate, initial rate, and instantaneous rate?
11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed mechanism is HBr + O2 -* HOOBr (slow) HOOBr + HBr — 2 HOBr (fast) HOBr + HBr — H2O + Bn (fast) Show that this mechanism can account for the correct stoichiometry. Identify all intermediates in this mechanism. What is the molecularity of each elementary’ step? Write the rate expression for each elementary' step. Identify the rate-determining step.
The mechanism for the reaction of CH3OH and HBr is believed to involve two steps. The overall reaction is exothermic. Step 1: Fast, endothermic CH3OH + H+ CH3OH2+ Step 2: Slow CH3OH2+ + Br CH3Br + H2O (a) Write an equation for the overall reaction. (b) Draw a reaction coordinate diagram for this reaction. (c) Show that the rate law for this reaction is Rate = k[CH3OH][H+][Br].
Why does a catalyst increase the rate of a reaction? What is the difference between a homogeneous catalyst and a heterogeneous catalyst? Would a given reaction necessarily have the same rate law for both a catalyzed and an uncatalyzed pathway? Explain.
The following mechanism is proposed for a reaction: NO + Br2 —* NOBr2 (slow) NOBr2 + NO —»2 NOBr (fast) Write the overall equation for the reaction. What is the rate-determining step? WTiat is the intermediate in this reaction? What is the molecularity of each step of the reaction? Write the rate expression for each step.
There are two molecules with the formula C3H6 Propane, CH3CH = CH2, is the monomer of the polymer polypropylene, which is used for indoor-outdoor carpets. Cyclopropane is used as an anesthetic: When heated to 499 C, cyclopropane rearranges (isomerizes) and forms propane with a rate constant of 5.95104s1. What is the half-life of this reaction? What fraction of the cyclopropane remains after 0.75 h at 499 C?
Tertiary butyl chloride reacts in basic solution according to the equation (CH3)3CCl+OH(CH3)3COH+Cl The accepted mechanism for this reaction is (CH3)3CCl(CH3)3C++Cl(slow)(CH3)3C++OH(CH3)3COH(fast) What should be the rate law for this reaction?
From the given data, use a graphical method to determine the order and rate constant of the following reaction: 2XY+Z Time (s) 5.0 10.0 15.0 20.0 25.0 30.0 35.0 40.0 [X](M) 0.0990 0.0497 0.0332 0.0249 0.0200 0.0166 0.0143 0.0125
In experiments on the decomposition of azomethane. CH3NHCH3(g)C2H6(g)+N2(g) the following data were obtained: Initial Concentration of Azomethane Initial Rate Exp. 1 1.13 102 M 2.8 106 M/s Exp. 2 2.26 102 M 5.6 106 M/s What is the rate law? What is the value of the rate constant?

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7. A valid mechanism for a reaction is given below. Step 1: NO (g) + Cl2 (g) → NOCI2 (g) Step 2: NOCI2 (g) + NO (g) -→ 2 NOCI (g) What is the overall reaction? Identify any reactive intermediate