Chemistry: Atoms First
Chemistry: Atoms First
3rd Edition
ISBN: 9781259638138
Author: Julia Burdge, Jason Overby Professor
Publisher: McGraw-Hill Education
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Textbook Question
Chapter 19, Problem 19.85QP

The bromination of acetone is acid-catalyzed.

Chapter 19, Problem 19.85QP, The bromination of acetone is acid-catalyzed. The rate of disappearance of bromine was measured for , example  1

The rate of disappearance of bromine was measured for several different concentrations of acetone, bromine, and H+ ions at a certain temperature.

Chapter 19, Problem 19.85QP, The bromination of acetone is acid-catalyzed. The rate of disappearance of bromine was measured for , example  2

(a) What is the rate law for the reaction? (b) Determine the rate constant. (c) The following mechanism has been proposed for the reaction.

Chapter 19, Problem 19.85QP, The bromination of acetone is acid-catalyzed. The rate of disappearance of bromine was measured for , example  3

 (a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The following from the given information has to be determined.

  1. (a) The rate law for the given reaction

Concept introduction:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of reactants consumed and how much concentration of product formed in a unit of time is said to be rate of reaction.

  • Rate of reaction depends on time, temperature, pressure, concentration, and pH of the reaction.

Rate law: It is an equation that related to the rate of reaction to the concentrations or pressures of substrates (reactants).  It is also said to be as rate equation.

To determine the rate law for the given reaction

Answer to Problem 19.85QP

The following from the given information has to be determined.

  1. (a) The rate law for the given reaction is rate = k[CH3COCH3][H+]

Explanation of Solution

The given reaction is

CH3COCH3+Br2Catlyst   H+CH3COCH2Br + H++Br-

The rate law for the above reaction in general is

rate = k[CH3COCH3]x[Br2]y[H+]z

In the above equation we need to find out the exponents of the reactant concentrations, which can be determined by comparing the information given in the table.

The exponents for CH3COCH3 , let’s compare the experiments 1 and 5 then find out as first order in CH3COCH3

The exponents for Br2 , let’s compare the experiments 1 and 2 then find out as zero order in Br2

The exponents for H+ , let’s compare the experiments 1 and 3 then find out as first order in H+

Substituting these orders in the above reaction and we get rate law for the given reaction as

rate = k[CH3COCH3][H+]

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The following from the given information has to be determined.

  1. (b) The rate constant for the given reaction

Concept introduction:

Rateof a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of reactants consumed and how much concentration of product formed in a unit of time is said to be rate of reaction.

  • Rate of reaction depends on time, temperature, pressure, concentration, and pH of the reaction.

Rate law: It is an equation that related to the rate of reaction to the concentrationsor pressures of substrates (reactants).  It is also said to be as rate equation.

To determine the rate constant for the given reaction

Answer to Problem 19.85QP

The following from the given information has to be determined.

  1. (b) The rate constant for the given reaction is k=3.8×103/M.s

Explanation of Solution

In order to calculate the rate constant for the given reaction, modify the rate law as follows

 k= rate[CH3COCH3][H+]

 k = 5.7×105M/s(0.30M)(0.050M)=3.8×103/M.sk=3.8×103/M.s

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation:

The following from the given information has to be determined.

(c) The rate law deduced from the mechanism is consistent with that shown in part (a) has to be shown.

Concept introduction:

Rate of a reaction: It represents the speed at which a chemical reaction runs.  How much concentration of reactants consumed and how much concentration of product formed in a unit of time is said to be rate of reaction.

  • Rate of reaction depends on time, temperature, pressure, concentration, and pH of the reaction.

Rate law: It is an equation that related to the rate of reaction to the concentrationsor pressures of substrates (reactants).  It is also said to be as rate equation.

Answer to Problem 19.85QP

The following from the given information has to be determined.

  1. (c) The rate law deduced from the mechanism is consistent with that shown in part (a) is shown.

Explanation of Solution

Assume that k2 as rate constant for the slow step

rate = k2[CH3COCH3][H3O+]

Now, k1andk1 are the rate constants for the forward and reverse steps in the equilibrium

k1[CH3COCH3][H3O+] = k-1[CH3COCH3][H3O+]

rate = k1k2k-1[CH3COCH3][H3O+

And which is same as rate = k1k2k-1

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Chapter 19 Solutions

Chemistry: Atoms First

Ch. 19.4 - The gas-phase reaction of nitric oxide with...Ch. 19.5 - Calculate the rate constant for the first-order...Ch. 19.5 - Prob. 19.7WECh. 19.5 - The reaction 2A B is second order in A with a rate...Ch. 19.5 - Prob. 7PPBCh. 19.5 - Prob. 19.5.4SRCh. 19.7 - Prob. 19.11WECh. 19.7 - Prob. 11PPACh. 19.7 - Prob. 11PPBCh. 19.7 - Consider the gas-phase reaction of nitric oxide...Ch. 19.7 - Prob. 12PPBCh. 19 - The rate of a reaction in which the reactant...Ch. 19 - The rate of a reaction in which the reactant...Ch. 19 - The rate of a reaction in which the reactant...Ch. 19 - Increasing the temperature of a reaction increases...Ch. 19 - Define activation energy. What role does...Ch. 19 - Sketch a potential energy versus reaction progress...Ch. 19 - The reaction H + H2 H2 + H has been studied for...Ch. 19 - What is meant by the rate of a chemical reaction?...Ch. 19 - Distinguish between average rate and instantaneous...Ch. 19 - What are the advantages of measuring the initial...Ch. 19 - Prob. 19.7QPCh. 19 - Consider the reaction N2(g)+3H2(g)2NH3(g) Suppose...Ch. 19 - Prob. 19.9QPCh. 19 - Prob. 19.10QPCh. 19 - Prob. 19.11QPCh. 19 - Prob. 19.12QPCh. 19 - Prob. 19.13QPCh. 19 - What are the units for the rate constants of...Ch. 19 - Consider the zeroth-order reaction: A product....Ch. 19 - Prob. 19.16QPCh. 19 - Prob. 19.17QPCh. 19 - Prob. 19.18QPCh. 19 - Prob. 19.19QPCh. 19 - Prob. 19.20QPCh. 19 - Prob. 19.21QPCh. 19 - Prob. 19.22QPCh. 19 - Prob. 19.23QPCh. 19 - Prob. 19.24QPCh. 19 - Prob. 19.25QPCh. 19 - Prob. 19.26QPCh. 19 - Prob. 19.27QPCh. 19 - Prob. 19.28QPCh. 19 - Prob. 19.29QPCh. 19 - Prob. 19.30QPCh. 19 - Prob. 19.31QPCh. 19 - The rate constant for the second-order reaction...Ch. 19 - Prob. 19.33QPCh. 19 - Consider the first-order reaction X Y shown here,...Ch. 19 - Prob. 19.35QPCh. 19 - Consider the first-order reaction A B in which A...Ch. 19 - Prob. 19.37QPCh. 19 - Prob. 19.38QPCh. 19 - Prob. 19.39QPCh. 19 - Prob. 19.40QPCh. 19 - Prob. 19.41QPCh. 19 - Prob. 19.42QPCh. 19 - Prob. 19.43QPCh. 19 - Prob. 19.44QPCh. 19 - Prob. 19.45QPCh. 19 - The rate at which tree crickets chirp is 2.0 102...Ch. 19 - Prob. 19.47QPCh. 19 - The activation energy for the denaturation of a...Ch. 19 - Variation of the rate constant with temperature...Ch. 19 - Prob. 19.50QPCh. 19 - Prob. 19.51QPCh. 19 - Prob. 19.52QPCh. 19 - Prob. 19.53QPCh. 19 - What is an elementary step? What is the...Ch. 19 - Prob. 19.55QPCh. 19 - Determine the molecularity, and write the rate law...Ch. 19 - What is the rate-determining step of a reaction?...Ch. 19 - Prob. 19.58QPCh. 19 - Prob. 19.59QPCh. 19 - Classify each of the following elementary steps as...Ch. 19 - Prob. 19.61QPCh. 19 - Prob. 19.62QPCh. 19 - Prob. 19.63QPCh. 19 - Prob. 19.64QPCh. 19 - Prob. 19.65QPCh. 19 - What are the characteristics of a catalyst?Ch. 19 - Prob. 19.67QPCh. 19 - Prob. 19.68QPCh. 19 - The concentrations of enzymes in cells are usually...Ch. 19 - Prob. 19.70QPCh. 19 - Prob. 19.71QPCh. 19 - Prob. 19.72QPCh. 19 - Prob. 19.73QPCh. 19 - Prob. 19.74QPCh. 19 - Prob. 19.75QPCh. 19 - In a certain industrial process involving a...Ch. 19 - Prob. 19.77QPCh. 19 - Prob. 19.78QPCh. 19 - Explain why most metals used in catalysis arc...Ch. 19 - Prob. 19.80QPCh. 19 - Prob. 19.81QPCh. 19 - Prob. 19.82QPCh. 19 - Prob. 19.83QPCh. 19 - Prob. 19.84QPCh. 19 - The bromination of acetone is acid-catalyzed. The...Ch. 19 - The decomposition of N2O to N2 and O2 is a...Ch. 19 - Prob. 19.87QPCh. 19 - Prob. 19.88QPCh. 19 - The integrated rate law for the zeroth-order...Ch. 19 - Prob. 19.90QPCh. 19 - Prob. 19.91QPCh. 19 - Prob. 19.92QPCh. 19 - The reaction of G2 with E2 to form 2EG is...Ch. 19 - Prob. 19.94QPCh. 19 - Prob. 19.95QPCh. 19 - Prob. 19.96QPCh. 19 - Strictly speaking, the rate law derived for the...Ch. 19 - Prob. 19.98QPCh. 19 - The decomposition of dinitrogen pentoxide has been...Ch. 19 - Prob. 19.100QPCh. 19 - Prob. 19.101QPCh. 19 - Prob. 19.102QPCh. 19 - To prevent brain damage, a standard procedure is...Ch. 19 - Prob. 19.104QPCh. 19 - Prob. 19.105QPCh. 19 - Prob. 19.106QPCh. 19 - Prob. 19.107QPCh. 19 - Prob. 19.108QPCh. 19 - Prob. 19.109QPCh. 19 - Prob. 19.110QPCh. 19 - (a) What can you deduce about the activation...Ch. 19 - Prob. 19.112QPCh. 19 - Prob. 19.113QPCh. 19 - Prob. 19.114QPCh. 19 - Prob. 19.115QPCh. 19 - Prob. 19.116QPCh. 19 - Prob. 19.117QPCh. 19 - Prob. 19.118QPCh. 19 - Prob. 19.119QPCh. 19 - Prob. 19.120QPCh. 19 - Prob. 19.121QPCh. 19 - Prob. 19.122QPCh. 19 - Consider the following potential energy profile...Ch. 19 - Prob. 19.124QPCh. 19 - Prob. 19.125QPCh. 19 - Prob. 19.126QPCh. 19 - Prob. 19.127QPCh. 19 - Prob. 19.128QPCh. 19 - The following expression shows the dependence of...Ch. 19 - Prob. 19.130QPCh. 19 - The rale constant for the gaseous reaction H2(g) +...Ch. 19 - Prob. 19.132QPCh. 19 - Prob. 19.133QPCh. 19 - At a certain elevated temperature, ammonia...Ch. 19 - Prob. 19.135QPCh. 19 - The rate of a reaction was followed by the...Ch. 19 - Prob. 19.137QPCh. 19 - Prob. 19.138QP
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