Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
bartleby

Videos

Textbook Question
Chapter 12, Problem 29E

What are the units for each of the following if the concentrations are expressed in moles per liter and the time in seconds?

a. rate of a chemical reaction

b. rate constant for a zero-order rate law

c. rate constant for a first-order rate law

d. rate constant for a second-order rate law

e. rate constant for a third-order rate law

(a)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The units for each of the given terms are to be calculated taking concentration in terms of moles per liter (mol/L) and time in seconds (s) .

Concept introduction: The rate of a reaction is directly proportional to the concentration of the reactant. For a reaction, XProducts ,

Rate[X]nRate=k[X]n

The constant k in the above expression is the rate constant.

Answer to Problem 29E

The unit of the rate of a chemical reaction is molL1s1 .

Explanation of Solution

Given

Concentration is expressed in moles per liter (mol/L) and time in seconds (s) .

The rate of a reaction is calculated by the formula,

Rateofreaction=ChangeintheconcentrationChangeintime

Substitute the given units of concentration and time in the above expression.

Rateofreaction=mol/Ls=molL1s1

Conclusion

The unit of the rate of a chemical reaction is molL1s1 .

(b)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The units for each of the given terms are to be calculated taking concentration in terms of moles per liter (mol/L) and time in seconds (s) .

Concept introduction: The rate of a reaction is directly proportional to the concentration of the reactant. For a reaction, XProducts ,

Rate[X]nRate=k[X]n

The constant k in the above expression is the rate constant.

Answer to Problem 29E

The unit of the rate constant for a zero order reaction is molL1s1 .

Explanation of Solution

Given

The reaction is a zero order reaction.

Concentration is expressed in moles per liter (mol/L) and time in seconds (s) .

For a reaction, XProducts ,

Rate=k[X]n

Where,

  • k is the rate constant.
  • n is the order of a reaction.
  • [X] is the concentration of the reactant X .

The reaction is of zero order.

Substitute the order and the units in the above expression.

Rate=k[X]nmolL1s1=k[X]0k=molL1s1

Conclusion

The unit of the rate constant for a zero order reaction is molL1s1 .

(c)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The units for each of the given terms are to be calculated taking concentration in terms of moles per liter (mol/L) and time in seconds (s) .

Concept introduction: The rate of a reaction is directly proportional to the concentration of the reactant. For a reaction, XProducts ,

Rate[X]nRate=k[X]n

The constant k in the above expression is the rate constant.

To determine: The unit of the rate constant for a first order reaction.

Answer to Problem 29E

The unit of the rate constant for a first order reaction is s1 .

Given

The reaction is a first order reaction.

Concentration is expressed in moles per liter (mol/L) and time in seconds (s) .

For a reaction, XProducts ,

Rate=k[X]n

Where,

  • k is the rate constant.
  • n is the order of a reaction.
  • [X] is the concentration of the reactant X .

The reaction is of first order.

Substitute the order and the units in the above expression.

Rate=k[X]1molL1s1=k[molL1]1k=s1

Explanation of Solution

Conclusion

The unit of the rate constant for a first order reaction is s1 .

(d)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The units for each of the given terms are to be calculated taking concentration in terms of moles per liter (mol/L) and time in seconds (s) .

Concept introduction: The rate of a reaction is directly proportional to the concentration of the reactant. For a reaction, XProducts ,

Rate[X]nRate=k[X]n

The constant k in the above expression is the rate constant.

Answer to Problem 29E

The unit of the rate constant for a second order reaction is mol1Ls1 .

Explanation of Solution

Given

The reaction is a second order reaction.

Concentration is expressed in moles per liter (mol/L) and time in seconds (s) .

For a reaction, XProducts ,

Rate=k[X]n

Where,

  • k is the rate constant.
  • n is the order of a reaction.
  • [X] is the concentration of the reactant X .

The reaction is of second order.

Substitute the order and the units in the above expression.

Rate=k[X]2molL1s1=k[molL1]2molL1s1=k[mol2L2]

Simplify the above expression.

k=molL1s1[mol2L2]=mol1Ls1

Conclusion

The unit of the rate constant for a second order reaction is mol1Ls1 .

(e)

Expert Solution
Check Mark
Interpretation Introduction

Interpretation: The units for each of the given terms are to be calculated taking concentration in terms of moles per liter (mol/L) and time in seconds (s) .

Concept introduction: The rate of a reaction is directly proportional to the concentration of the reactant. For a reaction, XProducts ,

Rate[X]nRate=k[X]n

The constant k in the above expression is the rate constant.

Answer to Problem 29E

The unit of the rate constant for a third order reaction is mol-2L2s-1 .

To determine: The unit of the rate constant for a third order reaction.

Explanation of Solution

Given:

The reaction is a third order reaction.

Concentration is expressed in moles per liter (mol/L) and time in seconds (s) .

For a reaction, XProducts ,

Rate=k[X]n

Where,

  • k is the rate constant.
  • n is the order of a reaction.
  • [X] is the concentration of the reactant X .

The reaction is of third order.

Substitute the order and the units in the above expression.

Rate=k[X]3molL1s1=k[molL1]3molL1s1=k[mol3L3]

Simplify the above expression.

k=molL1s1[mol3L3]=mol2L2s1

Conclusion

The unit of the rate constant for a third order reaction is mol-2L2s-1 .

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 12 Solutions

Chemistry

Ch. 12 - Why does a catalyst increase the rate of a...Ch. 12 - Define stability from both a kinetic and...Ch. 12 - Describe at least two experiments you could...Ch. 12 - Make a graph of [A] versus time for zero-, first-,...Ch. 12 - How does temperature affect k, the rate constant?...Ch. 12 - Consider the following statements: In general, the...Ch. 12 - For the reaction A+BC, explain at least two ways...Ch. 12 - A friend of yours states, A balanced equation...Ch. 12 - Provide a conceptual rationale for the differences...Ch. 12 - The rate constant (k) depends on which of the...Ch. 12 - Table 11-2 illustrates how the average rate of a...Ch. 12 - The rate law for a reaction can be determined only...Ch. 12 - The plot below shows the number of collisions with...Ch. 12 - For the reaction O2(g)+2NO(g)2NO2(g) the observed...Ch. 12 - Each of the statements given below is false....Ch. 12 - Define what is meant by unimolecular and...Ch. 12 - The type of rate law for a reaction, either the...Ch. 12 - The initial rate of a reaction doubles as the...Ch. 12 - Hydrogen reacts explosively with oxygen. However,...Ch. 12 - The central idea of the collision model is that...Ch. 12 - Consider the following energy plots for a chemical...Ch. 12 - Prob. 21QCh. 12 - Prob. 22QCh. 12 - The combustion of carbohydrates and the combustion...Ch. 12 - Would the slope of a ln(k) versus 1/T plot (with...Ch. 12 - Consider the reaction 4PH3(g)P4(g)+6H2(g) If, in a...Ch. 12 - In the Haber process for the production of...Ch. 12 - At 40C, H2O2 (aq) will decompose according to the...Ch. 12 - Consider the general reaction aA+bBcC and the...Ch. 12 - What are the units for each of the following if...Ch. 12 - The rate law for the reaction...Ch. 12 - The reaction 2NO(g)+Cl2(g)2NOCl(g) was studied at...Ch. 12 - The reaction 2I-(aq)+S2O82-(aq)I2(aq)+2SO42-(aq)...Ch. 12 - The decomposition of nitrosyl chloride was...Ch. 12 - The following data were obtained for the gas-phase...Ch. 12 - The reaction I(aq)+OCl(aq)IO(aq)+Cl(aq) was...Ch. 12 - The reaction 2NO(g)+O2(g)2NO2(g) was studied. and...Ch. 12 - The rote of the reaction between hemoglobin (Hb)...Ch. 12 - The following data were obtained for the reaction...Ch. 12 - The decomposition of hydrogen peroxide was...Ch. 12 - A certain reaction has the following general form:...Ch. 12 - The rate of the reaction NO2(g)+CO(g)NO(g)+CO2(g)...Ch. 12 - A certain reaction has the following general form:...Ch. 12 - The decomposition of ethanol (C2H5OH) on an...Ch. 12 - At 500 K in the presence of a copper surface,...Ch. 12 - The dimerization of butadiene 2C4H6(g)C8H12(g) was...Ch. 12 - The rate of the reaction O(g)+NO2(g)NO(g)+O2(g)...Ch. 12 - Experimental data for the reaction A2B+C have been...Ch. 12 - Prob. 48ECh. 12 - The reaction AB+C is known to be zero order in A...Ch. 12 - The decomposition of hydrogen iodide on finely...Ch. 12 - Prob. 51ECh. 12 - A first-order reaction is 75.0% complete in 320....Ch. 12 - The rate law for the decomposition of phosphine...Ch. 12 - DDT (molar mass = 354.49 g/mol) was a widely used...Ch. 12 - The rate law for the reaction...Ch. 12 - Prob. 57ECh. 12 - Theophylline is a pharmaceutical drug that is...Ch. 12 - You and a coworker have developed a molecule...Ch. 12 - Consider the hypothetical reaction A+B+2C2D+3E...Ch. 12 - Write the rate laws for the following elementary...Ch. 12 - A possible mechanism for the decomposition of...Ch. 12 - A proposed mechanism for a reaction is...Ch. 12 - The mechanism for the gas-phase reaction of...Ch. 12 - Is the mechanism NO+Cl2l1NOCl2NOCl2+NOl22NOCl...Ch. 12 - The reaction 2NO(g) + O2(g) 2NO2(g) exhibits the...Ch. 12 - For the following reaction profile, indicate a....Ch. 12 - Draw a rough sketch of the energy profile for each...Ch. 12 - The activation energy for the reaction...Ch. 12 - The activation energy for some reaction...Ch. 12 - The rate constant for the gas-phase decomposition...Ch. 12 - The reaction (CH3)3CBr+OH(CH3)3COH+Br in a certain...Ch. 12 - The activation energy for the decomposition of...Ch. 12 - A first-order reaction has rate constants of 4.6 ...Ch. 12 - A certain reaction has an activation energy of...Ch. 12 - Prob. 76ECh. 12 - Which of the following reactions would you expect...Ch. 12 - Prob. 78ECh. 12 - One mechanism for the destruction of ozone in the...Ch. 12 - One of the concerns about the use of Freons is...Ch. 12 - Assuming that the mechanism for the hydrogenation...Ch. 12 - The decomposition of NH3 to N2 and H2 was studied...Ch. 12 - The decomposition of many substances on the...Ch. 12 - Prob. 84ECh. 12 - A popular chemical demonstration is the magic...Ch. 12 - Prob. 86ECh. 12 - Consider the following representation of the...Ch. 12 - The reaction H2SeO3(aq) + 6I-(aq) + 4H+(aq) Se(s)...Ch. 12 - Consider two reaction vessels, one containing A...Ch. 12 - Sulfuryl chloride (SO2Cl2) decomposes to sulfur...Ch. 12 - For the reaction 2N2O5(g)4NO2(g)+O2(g) the...Ch. 12 - Experimental values for the temperature dependence...Ch. 12 - At 620. K butadiene dimerizes at a moderate rate....Ch. 12 - For a first order gas phase reaction A products,...Ch. 12 - Cobra venom helps the snake secure food by binding...Ch. 12 - Iodomethane (CH3I) is a commonly used reagent in...Ch. 12 - Experiments during a recent summer on a number of...Ch. 12 - The activation energy of a certain uncatalyzed...Ch. 12 - Consider the following initial rate data for the...Ch. 12 - Consider a hypothetical reaction between A and B:...Ch. 12 - Consider the reaction 3A+B+CD+E where the rate law...Ch. 12 - The thiosulfate ion (S2O32) is oxidized by iodine...Ch. 12 - The reaction A(aq)+B(aq)products(aq) was studied,...Ch. 12 - A certain substance, initially present at 0.0800...Ch. 12 - A reaction of the form aAProducts gives a plot of...Ch. 12 - A certain reaction has the form aAProducts At a...Ch. 12 - Which of the following statement(s) is( are) true?...Ch. 12 - Consider the hypothetical reaction A2(g) + B2(g) ...Ch. 12 - Experiments have shown that the average frequency...Ch. 12 - Consider a reaction of the type aA products, in...Ch. 12 - A study was made of the effect of the hydroxide...Ch. 12 - Two isomers (A and B) of a given compound dimerize...Ch. 12 - The reaction NO(g)+O3NO2(g)+O2(g) was studied by...Ch. 12 - Prob. 114CPCh. 12 - In the gas phase, the production of phosgene from...Ch. 12 - Most reactions occur by a series of steps. The...Ch. 12 - You are studying the kinetics of the reaction...Ch. 12 - The decomposition of NO2(g) occurs by the...Ch. 12 - The following data were collected in two studies...Ch. 12 - Consider the following hypothetical data collected...Ch. 12 - Consider the hypothetical reaction A+B+2C2D+3E In...Ch. 12 - Hydrogen peroxide and the iodide ion react in...Ch. 12 - Sulfuryl chloride undergoes first-order...Ch. 12 - Upon dissolving InCl(s) in HCl, In+(aq) undergoes...Ch. 12 - The decomposition of iodoethane in the gas phase...Ch. 12 - Consider the following reaction: CH3X+YCH3Y+X At...
Knowledge Booster
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
    Recommended textbooks for you
  • Chemistry: Matter and Change
    Chemistry
    ISBN:9780078746376
    Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
    Publisher:Glencoe/McGraw-Hill School Pub Co
    Physical Chemistry
    Chemistry
    ISBN:9781133958437
    Author:Ball, David W. (david Warren), BAER, Tomas
    Publisher:Wadsworth Cengage Learning,
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
  • Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    Introductory Chemistry For Today
    Chemistry
    ISBN:9781285644561
    Author:Seager
    Publisher:Cengage
  • Chemistry: Matter and Change
    Chemistry
    ISBN:9780078746376
    Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
    Publisher:Glencoe/McGraw-Hill School Pub Co
    Physical Chemistry
    Chemistry
    ISBN:9781133958437
    Author:Ball, David W. (david Warren), BAER, Tomas
    Publisher:Wadsworth Cengage Learning,
    Chemistry: An Atoms First Approach
    Chemistry
    ISBN:9781305079243
    Author:Steven S. Zumdahl, Susan A. Zumdahl
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781305957404
    Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
    Publisher:Cengage Learning
    Chemistry
    Chemistry
    ISBN:9781133611097
    Author:Steven S. Zumdahl
    Publisher:Cengage Learning
    Introductory Chemistry For Today
    Chemistry
    ISBN:9781285644561
    Author:Seager
    Publisher:Cengage
    Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32; Author: Crash Course;https://www.youtube.com/watch?v=7qOFtL3VEBc;License: Standard YouTube License, CC-BY