General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
bartleby

Videos

Question
Book Icon
Chapter 14, Problem 14.16QP

(a)

Interpretation Introduction

Interpretation:

From the given data, the order of the reaction has to be determined.

Concept introduction:

Rate law: An expression relating the rate of a reaction to the rate constant and concentrations of the reactants that are involved in the reaction.

For a given type of reaction:

aA+bBcC+dD

The rate law takes the form as:

Rate=k[A]x[B]y

k= Rate constant. It is the constant of proportionality between the rate of a reaction and the concentration of the reactants. Its unit is s-1.

[A]-Concentration of the reactant A in molarity.

[B]-Concentration of the reactant B in molarity.

It is important to note that x and y are not related to a and b.

Rather, they are determined experimentally.

Order of a reaction:  The sum of exponents of the concentrations in the rate law of chemical reaction is known as order of a reaction.

The order of the reaction for the given rate law is:

Rate=k[A]x[B]yRatelawOder=x+y

If the value of the order is 1, then it is known as the 1st order reaction.

If the value of the order is 2, then it is known as the 2ndorder reaction.

If the value of the order is 3, then it is known as the 3rdorder reaction.

If rate of a reaction is independent of [A] and if it is only dependent on [B]. Then the order of such a reaction is known as zero order and hence the corresponding reaction will be known as zero order reaction.

(a)

Expert Solution
Check Mark

Answer to Problem 14.16QP

The order of the reaction is zero order.

Explanation of Solution

The given experiments show that when the concentration of

  • While holding [X] as constant, if [Y] is increased or decreased then the initial rate of disappearance of X changes accordingly. Therefore, the rate of the reaction is directly proportional to the concentration of [Y].
  • While holding [Y] as constant, if [X] is increased or decreased then the initial rate of disappearance of X does not change accordingly. Therefore, the rate of the reaction is not proportional to the concentration of [X].

The experimental observations tell that the rate of the reaction is dependent only on the concentrations of Y and not on the concentration of X.

Hence, form the rate law will be:

rate = k[X]o[Y]

Therefore the order of the reaction is zero order.

Conclusion

The order of the reaction has been found.

(b)

Interpretation Introduction

Interpretation:

From the given data, the initial rate of disappearance of X has to be determined.

Concept introduction:

Rate law: An expression relating the rate of a reaction to the rate constant and concentrations of the reactants that are involved in the reaction.

For a given type of reaction:

aA+bBcC+dD

The rate law takes the form as:

Rate=k[A]x[B]y

k= Rate constant. It is the constant of proportionality between the rate of a reaction and the concentration of the reactants. Its unit is s-1.

[A]-Concentration of the reactant A in molarity.

[B]-Concentration of the reactant B in molarity.

It is important to note that x and y are not related to a and b.

Rather, they are determined experimentally.

(b)

Expert Solution
Check Mark

Answer to Problem 14.16QP

The initial rate of disappearance of X is 0.1176M/s

Explanation of Solution

To determine the initial rate of disappearance of X, the rate constant has to be calculated.

Among the given experiments in the table, data of any one experiment can be considered to calculate the rate constant for the reaction.

Considering the experiment 1:

[X]=0.10M[Y]=0.50MRate=0.147M/s

rate = k[X]o[Y]k=rate[X]o [Y]=0.147M/s1×(0.50M)[X]o=1=0.294s-1

Therefore, the rate constant is k=0.294s-1

Substituting the all the known values in rate law to obtain the rate of the reaction.

Given data:

[X]=0.30M[Y]=0.40M

rate = k[X]o[Y]rate = (0.294s-1)(0.30M)o(0.40M)= (0.294s-1)(1)(0.40M)=0.1176M/s

Therefore, the rate constant is 0.1176M/s

Conclusion

The initial rate of disappearance of X has been calculated.

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 14 Solutions

General Chemistry

Ch. 14.4 - Practice Exercise The first-order rate constant...Ch. 14.4 - Review of Concepts (a) What can you deduce about...Ch. 14.5 - Practice Exercise The reaction between NO2 and CO...Ch. 14.5 - Prob. 1RCCh. 14.6 - Prob. 1RCCh. 14 - Prob. 14.1QPCh. 14 - 15.2 Explain the difference between physical...Ch. 14 - Prob. 14.3QPCh. 14 - Prob. 14.4QPCh. 14 - Prob. 14.5QPCh. 14 - 14.6 Consider the reaction Suppose that at a...Ch. 14 - Prob. 14.7QPCh. 14 - 14.8 What are the units for the rate constants of...Ch. 14 - Prob. 14.9QPCh. 14 - Prob. 14.10QPCh. 14 - Prob. 14.11QPCh. 14 - Prob. 14.13QPCh. 14 - Prob. 14.14QPCh. 14 - Prob. 14.15QPCh. 14 - Prob. 14.16QPCh. 14 - Prob. 14.17QPCh. 14 - Prob. 14.18QPCh. 14 - Prob. 14.19QPCh. 14 - Prob. 14.20QPCh. 14 - 14.21 What is the half-life of a compound if 75...Ch. 14 - 14.22 The thermal decomposition of phosphine (PH3)...Ch. 14 - Prob. 14.23QPCh. 14 - Prob. 14.24QPCh. 14 - 14.25 Consider the first-order reaction A → B...Ch. 14 - Prob. 14.26QPCh. 14 - 14.27 Define activation energy. What role does...Ch. 14 - Prob. 14.28QPCh. 14 - Prob. 14.29QPCh. 14 - 14.30 As we know, methane burns readily in oxygen...Ch. 14 - Prob. 14.31QPCh. 14 - Prob. 14.32QPCh. 14 - Prob. 14.33QPCh. 14 - Prob. 14.34QPCh. 14 - Prob. 14.35QPCh. 14 - Prob. 14.36QPCh. 14 - Prob. 14.37QPCh. 14 - 14.38 The rate at which tree crickets chirp is 2.0...Ch. 14 - 14.39 The diagram here describes the initial state...Ch. 14 - Prob. 14.40QPCh. 14 - Prob. 14.41QPCh. 14 - Prob. 14.42QPCh. 14 - 14.43 Explain why termolecular reactions are...Ch. 14 - 14.44 What is the rate-determining step of a...Ch. 14 - Prob. 14.45QPCh. 14 - Prob. 14.46QPCh. 14 - Prob. 14.47QPCh. 14 - Prob. 14.48QPCh. 14 - Prob. 14.49QPCh. 14 - Prob. 14.50QPCh. 14 - Prob. 14.51QPCh. 14 - Prob. 14.52QPCh. 14 - Prob. 14.53QPCh. 14 - Prob. 14.54QPCh. 14 - Prob. 14.55QPCh. 14 - Prob. 14.56QPCh. 14 - Prob. 14.57QPCh. 14 - Prob. 14.58QPCh. 14 - Prob. 14.59QPCh. 14 - Prob. 14.60QPCh. 14 - Prob. 14.61QPCh. 14 - Prob. 14.62QPCh. 14 - Prob. 14.63QPCh. 14 - Prob. 14.64QPCh. 14 - Prob. 14.65QPCh. 14 - 14.66 The decomposition of N2O to N2 and O2 is a...Ch. 14 - Prob. 14.67QPCh. 14 - Prob. 14.68QPCh. 14 - 14.69 Consider the zero-order reaction a → B....Ch. 14 - Prob. 14.70QPCh. 14 - Prob. 14.72QPCh. 14 - Prob. 14.73QPCh. 14 - Prob. 14.74QPCh. 14 - Prob. 14.75QPCh. 14 - Prob. 14.76QPCh. 14 - Prob. 14.77QPCh. 14 - Prob. 14.78QPCh. 14 - Prob. 14.79QPCh. 14 - Prob. 14.80QPCh. 14 - Prob. 14.81QPCh. 14 - Prob. 14.82QPCh. 14 - 14.83 When a mixture of methane and bromine is...Ch. 14 - 14.84 Consider this elementary step: (a)...Ch. 14 - Prob. 14.85QPCh. 14 - Prob. 14.86QPCh. 14 - 14.87 In recent years ozone in the stratosphere...Ch. 14 - Prob. 14.88QPCh. 14 - Prob. 14.90QPCh. 14 - Prob. 14.91QPCh. 14 - Prob. 14.92QPCh. 14 - Prob. 14.93QPCh. 14 - Prob. 14.94QPCh. 14 - Prob. 14.95QPCh. 14 - Prob. 14.96QPCh. 14 - Prob. 14.97QPCh. 14 - Prob. 14.98QPCh. 14 - Prob. 14.100QPCh. 14 - Prob. 14.101QPCh. 14 - 14.102 Consider the potential energy profiles...Ch. 14 - Prob. 14.103QPCh. 14 - Prob. 14.104QPCh. 14 - 14.105 The activation energy for the...Ch. 14 - Prob. 14.106QPCh. 14 - Prob. 14.107SPCh. 14 - Prob. 14.108SPCh. 14 - Prob. 14.109SPCh. 14 - Prob. 14.110SPCh. 14 - Prob. 14.111SPCh. 14 - Prob. 14.112SPCh. 14 - Prob. 14.113SPCh. 14 - Prob. 14.114SPCh. 14 - Prob. 14.115SPCh. 14 - 14.116 To prevent brain damage, a drastic medical...Ch. 14 - Prob. 14.117SPCh. 14 - Prob. 14.118SP
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.
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
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Text book image
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Text book image
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Text book image
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Text book image
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
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