Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
bartleby

Concept explainers

bartleby

Videos

Question
Book Icon
Chapter 11, Problem 112CP

(a)

Interpretation Introduction

Interpretation: The order of the reaction is to be specified with respect to the reactants. The values of the rate constants are to be calculated. The reason corresponds to the fact that two-term dependence of the rate on the concentration of H+ ion is to be stated.

Concept introduction: The order of a reaction is the number or the index raise to the concentration term with respect to each component

The rate law or rate equation is a mathematical representation that relates the rate of the reaction with the concentration or pressure.

Rate constant is a proportionality coefficient that relates the rate of chemical reaction at a specific temperature to the concentration of the reactant or the product.

To determine: The order of the reaction with respect to [H2O2] and [I].

(a)

Expert Solution
Check Mark

Answer to Problem 112CP

The order of the reaction with respect to [H2O2] and [I] is zero and first order respectively.

Explanation of Solution

Explanation

The order of the reaction with respect to [H2O2] and [I] is zero and first order respectively.

Given

The given reaction is stated as,

H2O2(aq)+3I(aq)+2H+(aq)I3(aq)+2H2O(l)

The plot of ln[H2O2] Vs time is linear.

The concentration of [H2O2]0=8.00×104M

The rate law for the reaction,

Rate=Δ[H2O2]Δt=(k1+k2[H+])[I]m[H2O2]n

The concentration of [H2O2] is very small which is given above. The concentration of [H+] and [I] is significant. Therefore, the reduced form of rate law is represented as,

d[H2O2]dt=kobserved[H2O2]n

Where,

  • kobserved=(k1+k2[H+])[I]m

The concentration of H2O2 is very small indicates that the reaction is independent of the reactant H2O2

Therefore reaction is zero order with respect to the reactant H2O2.

The order of the reaction with respect to reactant [I] is determined by comparing the values of slopes given in table by the given formula,

Slope(exp1)Slope(exp2)=(k1+k2[H+])[I]m(exp1)(k1+k2[H+])[I]m(exp2)

Where,

  • k1,k2 are the rate constants.
  • Slopes are the experimental determined values.
  • m represents the order of the reaction with respect to reactant I

Substitute the values of slopes, concentration of the reactants form the given data, the value of m is determine as,

Slope(exp1)Slope(exp2)=(k1+k2[H+])[I]m(exp1)(k1+k2[H+])[I]m(exp2)0.3600.120=(k1+k2[0.0400M])[0.3000]m(k1+k2[0.0400M])[0.1000]m3=(0.30000.1000)mm=1

The order of the reaction with respect to [I] is first order.

(b)

Interpretation Introduction

Interpretation: The order of the reaction is to be specified with respect to the reactants. The values of the rate constants are to be calculated. The reason corresponds to the fact that two-term dependence of the rate on the concentration of H+ ion is to be stated.

Concept introduction: The order of a reaction is the number or the index raise to the concentration term with respect to each component

The rate law or rate equation is a mathematical representation that relates the rate of the reaction with the concentration or pressure.

Rate constant is a proportionality coefficient that relates the rate of chemical reaction at a specific temperature to the concentration of the reactant or the product.

To determine: The value of the rate constant k1 and k2 for the given reaction.

(b)

Expert Solution
Check Mark

Answer to Problem 112CP

The value of k1 and k2 are 0.82L/molmin_ and 9.5L2/mol2min_ respectively.

Explanation of Solution

Explanation

The value of k1 and k2 are 0.82L/molmin_ and 9.5L2/mol2min_ respectively.

As proved in step 1 that reaction is first order with respect to one reactant while it is zero order with respect to another reactant. The rate law is given as,

Rate=(k1+k2[H+])[I]

Where,

  • k1,k2 are the rate constant of the given reaction.
  • [H+],[I] represent the concentration of the reactants.

To calculate the value of k1,k2 the slopes of two experiments are considered and then equations are formulated as,

Slope=(k1+k2[H+])[I]

Substitute the values of slopes and concentration of the reactants form the given data of experiment 1.

Slope=(k1+k2[H+])[I]0.120min1=(k1+k2[0.04000M])[0.1000M]1.20min1=k1+k2[0.0400M] (1)

Substitute the values of slopes and concentration of the reactants form the given data of experiment 4.

Slope=(k1+k2[H+])[I]0.0760min1=(k1+k2[0.0200M])[0.0750M]1.01min1=k1+k2[0.0200M] (2)

Subtracts the equation 1 from equation 2,the value of k1,k2 are as follows,

k1=0.82L×mol-1×min-1_k2=0.82L2×mol-2×min-1_

(c)

Interpretation Introduction

Interpretation: The order of the reaction is to be specified with respect to the reactants. The values of the rate constants are to be calculated. The reason corresponds to the fact that two-term dependence of the rate on the concentration of H+ ion is to be stated.

Concept introduction: The order of a reaction is the number or the index raise to the concentration term with respect to each component

The rate law or rate equation is a mathematical representation that relates the rate of the reaction with the concentration or pressure.

Rate constant is a proportionality coefficient that relates the rate of chemical reaction at a specific temperature to the concentration of the reactant or the product.

To determine: The reason for the two-term dependence of the rate on [H+]

(c)

Expert Solution
Check Mark

Answer to Problem 112CP

The reason for the two-term dependence of the rate of the reaction on [H+] is the two rate law expressions.

Explanation of Solution

Explanation

The reason for the two-term dependence of the rate of the reaction on [H+] is the two rate law expressions.

The amount of the acid present in the given reaction is significant. Therefore, the concentration of the given acid takes part in the reaction. The rate law indicates its presence.

On the other hand the given reaction is an acid catalyzed reaction means presence of an acid only enhances the reaction.

The factor which dominates, decide the rate law of the given reaction.

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Chapter 11 Solutions

Chemistry: An Atoms First Approach

Ch. 11 - Why does a catalyst increase the rate of a...Ch. 11 - Prob. 1ALQCh. 11 - Describe at least two experiments you could...Ch. 11 - Prob. 3ALQCh. 11 - Prob. 4ALQCh. 11 - Consider the following statements: In general, the...Ch. 11 - For the reaction A + B C, explain at least two...Ch. 11 - Prob. 7ALQCh. 11 - Prob. 8ALQCh. 11 - Prob. 9ALQCh. 11 - Prob. 10QCh. 11 - Prob. 11QCh. 11 - The plot below shows the number of collisions with...Ch. 11 - For the reaction O2(g)+2NO(g)2NO2(g) the observed...Ch. 11 - Prob. 14QCh. 11 - Prob. 15QCh. 11 - Prob. 16QCh. 11 - Prob. 17QCh. 11 - Prob. 18QCh. 11 - Prob. 19QCh. 11 - Consider the following energy plots for a chemical...Ch. 11 - Prob. 21QCh. 11 - Would the slope of a ln(k) versus 1/T plot (with...Ch. 11 - Prob. 23ECh. 11 - In the Haber process for the production of...Ch. 11 - At 40C, H2O2 (aq) will decompose according to the...Ch. 11 - Consider the general reaction aA+bBcC and the...Ch. 11 - What are the units for each of the following if...Ch. 11 - The rate law for the reaction...Ch. 11 - The reaction 2NO(g)+Cl2(g)2NOCl(g) was studied at...Ch. 11 - The reaction 2I-(aq)+S2O82-(aq)I2(aq)+2SO42-(aq)...Ch. 11 - The decomposition of nitrosyl chloride was...Ch. 11 - The following data were obtained for the gas-phase...Ch. 11 - The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was...Ch. 11 - The reaction 2NO(g)+O2(g)2NO2(g) was studied. and...Ch. 11 - The rote of the reaction between hemoglobin (Hb)...Ch. 11 - The following data were obtained for the reaction...Ch. 11 - The decomposition of hydrogen peroxide was...Ch. 11 - Prob. 38ECh. 11 - The rate of the reaction NO2(g)+CO(g)NO(g)+CO2(g)...Ch. 11 - A certain reaction has the following general form:...Ch. 11 - The decomposition of ethanol (C2H5OH) on an...Ch. 11 - Prob. 42ECh. 11 - The dimerization of butadiene 2C4H6(g)C8H12(g) was...Ch. 11 - The rate of the reaction O(g)+NO2(g)NO(g)+O2(g)...Ch. 11 - Experimental data for the reaction A2B+C have been...Ch. 11 - Prob. 46ECh. 11 - The reaction AB+C is known to be zero order in A...Ch. 11 - The decomposition of hydrogen iodide on finely...Ch. 11 - Prob. 49ECh. 11 - A first-order reaction is 75.0% complete in 320....Ch. 11 - The rate law for the decomposition of phosphine...Ch. 11 - DDT (molar mass = 354.49 g/mol) was a widely used...Ch. 11 - Consider the following initial rate data for the...Ch. 11 - Prob. 54ECh. 11 - Prob. 55ECh. 11 - Prob. 56ECh. 11 - You and a coworker have developed a molecule...Ch. 11 - Consider the hypothetical reaction A+B+2C2D+3E...Ch. 11 - Prob. 59ECh. 11 - A possible mechanism for the decomposition of...Ch. 11 - A proposed mechanism for a reaction is...Ch. 11 - The mechanism for the gas-phase reaction of...Ch. 11 - For the following reaction profile, indicate a....Ch. 11 - Draw a rough sketch of the energy profile for each...Ch. 11 - Prob. 65ECh. 11 - The activation energy for some reaction...Ch. 11 - The rate constant for the gas-phase decomposition...Ch. 11 - The reaction (CH3)3CBr+OH(CH3)3COH+Br in a certain...Ch. 11 - Prob. 69ECh. 11 - A first-order reaction has rate constants of 4.6 ...Ch. 11 - Prob. 71ECh. 11 - Prob. 72ECh. 11 - Which of the following reactions would you expect...Ch. 11 - Prob. 74ECh. 11 - One mechanism for the destruction of ozone in the...Ch. 11 - One of the concerns about the use of Freons is...Ch. 11 - Prob. 77ECh. 11 - The decomposition of NH3 to N2 and H2 was studied...Ch. 11 - The decomposition of many substances on the...Ch. 11 - Prob. 80ECh. 11 - Prob. 81ECh. 11 - Prob. 82ECh. 11 - Consider the following representation of the...Ch. 11 - The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s)...Ch. 11 - Prob. 85AECh. 11 - Sulfuryl chloride (SO2Cl2) decomposes to sulfur...Ch. 11 - For the reaction 2N2O5(g)4NO2(g)+O2(g) the...Ch. 11 - Prob. 88AECh. 11 - Cobra venom helps the snake secure food by binding...Ch. 11 - Iodomethane (CH3I) is a commonly used reagent in...Ch. 11 - Experiments during a recent summer on a number of...Ch. 11 - The activation energy of a certain uncatalyzed...Ch. 11 - Consider the reaction 3A+B+CD+E where the rate law...Ch. 11 - The thiosulfate ion (S2O32) is oxidized by iodine...Ch. 11 - The reaction A(aq)+B(aq)products(aq) was studied,...Ch. 11 - A certain substance, initially present at 0.0800...Ch. 11 - A reaction of the form aAProducts gives a plot of...Ch. 11 - A certain reaction has the form aAProducts At a...Ch. 11 - Which of the following statement(s) is( are) true?...Ch. 11 - Consider the hypothetical reaction A2(g) + B2(g) ...Ch. 11 - Experiments have shown that the average frequency...Ch. 11 - Consider a reaction of the type aA products, in...Ch. 11 - A study was made of the effect of the hydroxide...Ch. 11 - Two isomers (A and B) of a given compound dimerize...Ch. 11 - Prob. 105CPCh. 11 - Most reactions occur by a series of steps. The...Ch. 11 - Prob. 107CPCh. 11 - The decomposition of NO2(g) occurs by the...Ch. 11 - The following data were collected in two studies...Ch. 11 - Prob. 110CPCh. 11 - Prob. 111CPCh. 11 - Prob. 112CPCh. 11 - Sulfuryl chloride undergoes first-order...Ch. 11 - Upon dissolving InCl(s) in HCl, In+(aq) undergoes...Ch. 11 - The decomposition of iodoethane in the gas phase...Ch. 11 - Consider the following reaction: CH3X+YCH3Y+X At...
Knowledge Booster
Background pattern image
Chemistry
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
SEE MORE QUESTIONS
Recommended textbooks for you
  • Text book image
    Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Text book image
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
    Text book image
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
  • Text book image
    Chemistry & Chemical Reactivity
    Chemistry
    ISBN:9781337399074
    Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
    Publisher:Cengage Learning
    Text book image
    Chemistry: The Molecular Science
    Chemistry
    ISBN:9781285199047
    Author:John W. Moore, Conrad L. Stanitski
    Publisher:Cengage Learning
    Text book image
    Chemistry by OpenStax (2015-05-04)
    Chemistry
    ISBN:9781938168390
    Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
    Publisher:OpenStax
Text book image
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Text book image
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry
Chemistry
ISBN:9781133611097
Author:Steven S. Zumdahl
Publisher:Cengage Learning
Text book image
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Text book image
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Text book image
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Photochemistry : Introduction to Basic Theory of Photochemical Process [Part 1]; Author: Dr. Vikrant Palekar;https://www.youtube.com/watch?v=2NDOL11d6no;License: Standard YouTube License, CC-BY
Photochemistry-1; Author: CH-08:ARYABHATT [Mathematics, Physics, Chemistry];https://www.youtube.com/watch?v=DC4J0t1z3e8;License: Standard Youtube License