Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 14.7, Problem 2.1ACP
(a)
Interpretation Introduction
Interpretation: The energy of
(b)
Interpretation Introduction
Interpretation:
The longest
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
a. Use a Haber cycle to show that CaCl has an exothermic enthalpy of formation.
Use Kapustinskii to estimate the lattice energy.
b. Show that CaCl does not exist because the enthalpy for the disproportionation
reaction is favorable:
2CaCl(s) Ca(s) + CaCl2(s)
28. Estimate the enthalpy (change in energy) of reaction for 2 SO(g) + O2(g) →2 SO2(g) using bond
energies. Assume that sulfur in SO2 (g) has an expanded octet.
->
Bond
Energy (kJ/mol)
498
265
a.
498 kJ/mol
c.
-498 kJ/mol
bь.
731 kJ/mol
d.
-32KJ/mol
What makes carbon such a unique element?
a. Elemental carbon comes in two forms, diamond, and graphite.
b. Carbon forms four bonds, although the ground state configuration would predict the formation of fewer bonds.
c. Carbon forms covalent bonds rather than ionic bonds.
d. To a greater extent than any other element, carbon can bond to itself to form straight chains, branched chains and rings
Chapter 14 Solutions
Chemistry & Chemical Reactivity
Ch. 14.1 - Sucrose decomposes to fructose and glucose in acid...Ch. 14.1 - What are the relative rates of appearance or...Ch. 14.3 - The initial rate ( [NO]/ t] of the reaction of...Ch. 14.3 - The rate constant, k, at 25 C is 0.27/h for the...Ch. 14.4 - Sucrose, a sugar, decomposes in acid solution to...Ch. 14.4 - Gaseous azomethane (CH3N2CH3) decomposes to ethane...Ch. 14.4 - Prob. 14.7CYUCh. 14.4 - The catalyzed decomposition of hydrogen peroxide...Ch. 14.4 - Americium is used in smoke detectors and in...Ch. 14.5 - Prob. 14.10CYU
Ch. 14.5 - The colorless gas N2O4, decomposes to the brown...Ch. 14.7 - Nitrogen monoxide is reduced by hydrogen to give...Ch. 14.7 - Prob. 14.13CYUCh. 14.7 - One possible mechanism for the decomposition of...Ch. 14.7 - Prob. 1.1ACPCh. 14.7 - Prob. 1.2ACPCh. 14.7 - Prob. 2.1ACPCh. 14.7 - Prob. 2.2ACPCh. 14.7 - Prob. 2.3ACPCh. 14.7 - Determine the activation energy for the reaction...Ch. 14 - Give the relative rates of disappearance of...Ch. 14 - Give the relative rates of disappearance of...Ch. 14 - In the reaction 2 O3(g) 3 O2(g), the rate of...Ch. 14 - In the synthesis of ammonia, if [H2]/t = 4.5 104...Ch. 14 - Experimental data are listed here for the reaction...Ch. 14 - Phenyl acetate, an ester, reacts with water...Ch. 14 - Using the rate equation Rate = k[A]2[B], define...Ch. 14 - A reaction has the experimental rate equation Rate...Ch. 14 - The reaction between ozone and nitrogen dioxide at...Ch. 14 - Nitrosyl bromide, NOBr, is formed from NO and Br2:...Ch. 14 - The data in the table are for the reaction of NO...Ch. 14 - The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g)...Ch. 14 - Data for the reaction NO(g) + O2(g) NO2(g) are...Ch. 14 - Data for the following reaction are given in the...Ch. 14 - The rate equation for the hydrolysis of sucrose to...Ch. 14 - The decomposition of N2O5 in CCl4 is a first-order...Ch. 14 - The decomposition of SO2Cl2 is a first-order...Ch. 14 - The conversion of cyclopropane to propene (Example...Ch. 14 - Hydrogen peroxide, H2O2(aq), decomposes to H2O()...Ch. 14 - The decomposition of nitrogen dioxide at a high...Ch. 14 - At 573 K, gaseous NO2(g) decomposes, forming NO(g)...Ch. 14 - The dimerization of butadiene, C4H6, to form...Ch. 14 - The decomposition of ammonia on a metal surface to...Ch. 14 - Hydrogen iodide decomposes when heated, forming...Ch. 14 - The rate equation for the decomposition of N2O5...Ch. 14 - Gaseous azomethane, CH3N=NCH3, decomposes in a...Ch. 14 - The decomposition of SO2Cl2 SO2Cl2(g) SO2(g) +...Ch. 14 - The compound Xe(CF3)2 decomposes in a first-order...Ch. 14 - The radioactive isotope 64Cu is used in the form...Ch. 14 - Radioactive gold-198 is used in the diagnosis of...Ch. 14 - Prob. 31PSCh. 14 - Ammonia decomposes when heated according to the...Ch. 14 - Gaseous NO2 decomposes at 573 K. NO2(g) NO(g) + ...Ch. 14 - The decomposition of HOF occurs at 25 C. HOF(g) ...Ch. 14 - Prob. 35PSCh. 14 - Prob. 36PSCh. 14 - Calculate the activation energy, Ea, for the...Ch. 14 - If the rate constant for a reaction triples when...Ch. 14 - When healed lo a high temperature, cyclobutane,...Ch. 14 - When heated, cyclopropane is converted to propene...Ch. 14 - The reaction of H2 molecules with F atoms H2(g) +...Ch. 14 - Prob. 42PSCh. 14 - Compare the lock-and-key and induced-fit models...Ch. 14 - Prob. 44PSCh. 14 - Prob. 45PSCh. 14 - The enzyme carbonic anhydrase catalyzes the...Ch. 14 - What is the rate law for each of the following...Ch. 14 - What is the rate law for each of the following...Ch. 14 - Ozone, O3, in the Earths upper atmosphere...Ch. 14 - The reaction of NO2(g) and CO(g) is thought to...Ch. 14 - A proposed mechanism for the reaction of NO2 and...Ch. 14 - The mechanism for the reaction of CH3OH and HBr is...Ch. 14 - A reaction has the following experimental rate...Ch. 14 - For a first-order reaction, what fraction of...Ch. 14 - Prob. 55GQCh. 14 - Data for the following reaction are given in the...Ch. 14 - Formic acid decomposes at 550 C according to the...Ch. 14 - Isomerization of CH3NC occurs slowly when CH3NC is...Ch. 14 - When heated, tetrafluoroethylene dimerizes to form...Ch. 14 - Data in the table were collected at 540 K for the...Ch. 14 - Ammonium cyanate, NH4NCO, rearranges in water to...Ch. 14 - Prob. 62GQCh. 14 - At temperatures below 500 K, the reaction between...Ch. 14 - Nitryl fluoride can be made by treating nitrogen...Ch. 14 - The decomposition of dinitrogen pentaoxide N2O5(g)...Ch. 14 - The data in the table give the temperature...Ch. 14 - The decomposition of gaseous dimethyl ether at...Ch. 14 - The decomposition of phosphine, PH3, proceeds...Ch. 14 - The thermal decomposition of diacetylene, C4H2,...Ch. 14 - Prob. 70GQCh. 14 - The ozone in the Earths ozone layer decomposes...Ch. 14 - Hundreds of different reactions occur in the...Ch. 14 - Data for the reaction [Mn(CO)5(CH3CN)]+ + NC5H5 ...Ch. 14 - The gas-phase reaction 2 N2O5(g) 4 NO2(g) + O2(g)...Ch. 14 - Prob. 75GQCh. 14 - The decomposition of SO2Cl2 to SO2 and Cl2 is...Ch. 14 - The decomposition of nitrogen dioxide at a high...Ch. 14 - Prob. 78GQCh. 14 - Egg protein albumin is precipitated when an egg is...Ch. 14 - A The compound 1,3-butadiene (C4H6) forms...Ch. 14 - Hypofluorous acid, HOF, is very unstable,...Ch. 14 - We know that the decomposition of SO2Cl2 is...Ch. 14 - Nitramide, NO2NH2, decomposes slowly in aqueous...Ch. 14 - Prob. 84GQCh. 14 - The color change accompanying the reaction of...Ch. 14 - Prob. 87ILCh. 14 - Prob. 88ILCh. 14 - The oxidation of iodide ion by the hypochlorite...Ch. 14 - The acid-catalyzed iodination of acetone...Ch. 14 - Prob. 91SCQCh. 14 - The following statements relate to the reaction...Ch. 14 - Chlorine atoms contribute to the destruction of...Ch. 14 - Prob. 95SCQCh. 14 - Prob. 96SCQCh. 14 - The reaction cyclopropane propene occurs on a...Ch. 14 - Prob. 98SCQCh. 14 - Examine the reaction coordinate diagram given...Ch. 14 - Draw a reaction coordinate diagram for an...Ch. 14 - Consider the reaction of ozone and nitrogen...
Knowledge Booster
Similar questions
- This thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Based of the table (picture): A. What is the lattice enthalpy of MX2? (in kJ/mol) B. What is the enthalpy of formation of MX2? (in kJ/mol) C. Suppose the electron affinity of X were bigger and the heat of sublimation of M were smaller. Would MX2 be more or less stable? Or would it be impossible to tell without more information?arrow_forwardQuestion 8 A) Which of the following substances is paramagnetic? A. KCl B. MgO C. CaCl2 D. Fe2O3 E. CuI B) Analysis of a compound finds it contains 25.0% of species X, by mass, and 75.0% of species Yby mass. The molar mass of species X is 25.0 g/mol, and the molar mass of species Y is 150. g/mol.If the molar mass of the compound is 600. g/mol, what is the molecular formula of the compound? A. X6Y4 B. X4Y5 C. X6Y3 D. X4Y4 E. X2Y5 C) Magnesium metal reacts with hydrochloric acid to produce hydrogen gas and an aqueoussolution of magnesium (II) chloride. What substance is being oxidized. A. H2(g) B. MgCl2(aq) C. HCl(aq) D. Mg(s) E. MgCl(aq)arrow_forwardHow does the electron structure of an isolated atom differ from that of a solid material? Select the most appropriate answer. Select one: O a. The valence electrons of each atom disappear in the bulk material. O b. An isolated atom has an electron band structure. Solid materials have discrete electron energy states. C. An isolated atom has discrete electron energy states. Solid materials have four electron band structures. d. There is no difference in electron structure between an isolated atom and a solid material;arrow_forward
- MCQ 119: When magnesium is burnt on Bunsen burner it gives flame of color A. bright white B. off white C. cream white D. ash whitearrow_forwardElement X has an electron configuration 1s22s22p1. The formula of the choride formed with element X is: a. XCl b. XCl2 c. XCl3 d. X2Cl e. XCl4 f. XCl5arrow_forwardThis thermodynamic cycle describes the formation of an ionic compound MX from a metal element M and nonmetal element X in their standard states. Based of the table (picture): A. What is the lattice enthalpy of MX? (in kJ/mol) B. What is the enthalpy of formation of MX? (in kJ/mol) C. Suppose both the electron affinity of X and the heat of sublimation of M were bigger. Would MX be more or less stable?arrow_forward
- 2. Identify the true statement. a. Polar covalent compounds result from a complete transfer of at least one electron. b. Sodium is unlikely to form a bond with lithium. c. Covalent compounds exist in large lattices. d. The smallest unit of an ionic compound is a molecule. 3. A piece of zinc metal is placed in an aqueous solution of magnesium sulfate. The products of this reaction are a. ZnMg(s) + SO4(aq) b. Mg(s) + ZnSO4(aq) c. MgS(s) + ZnO4(aq) d. ZnO(s) + MgSO4(aq) e. There will be no reaction. 4. The shape of the NC13 molecule is a. linear b. trigonal planar c. tetrahedral d. trigonal pyramidal e. V-shaped Imi 5. Which of the following would have the highest boiling point? a. NH3 b. PH3 c. AsH3 d. They would all have approximately the same boiling point. 20 6. Aqueous solutions of silver nitrate and sodium sulfate are mixed. The products of the reaction are a. Ag2SO4(aq) + 2 NaNO3(aq) b. AgSO4(s) + Na2(NO3)2(aq) c. Ag2SO4(s) + 2 NaNO3(aq) d. AgSO4(aq) + Na2(NO3 e. There will be no…arrow_forwardThis thermodynamic cycle describes the formation of an ionic compound MX2 from a metal element M and nonmetal element X in their standard states. Based of the table (picture): A. What is the lattice enthalpy of MX2 ? (in kJ/mol) B. What is the enthalpy of formation of MX2 ? (in kJ/mol) C. Suppose both the electron affinity of X and the heat of sublimation of M were smaller. Would MX2 be more or less stable?arrow_forwardD. Ascorbic acid, amalgam, salt 5. Which of the following statements explains the structure of a metal? A. The movable valence electrons are highly delocalized that attract all the cations, holding them together. B. The electrons are localized as either shared or unshared pairs, so they are not free to move. C. The ions are held together in a specific position by strong attractive forces. D. Separate particles are not present, instead, strong bands link the atoms together throughout the solidarrow_forward
- Consider the following changes: a. N2(g) →N2(l) b. CO (g) + H2O(g) →H2(g)+CO2(g) c. Ca3P2(s)+6H2O(l) → 3Ca(OH)2(s)+2PH3(g) d. 2CH3OH(l)+3O2(g) →2CO2(g)+4H2O(l) e. I2(s) →I2(g)At constant temperature and pressure, in which of these changes is workdone by the system on the surroundings? By the surroundings on the system? In which of them is no work done?arrow_forward3. In this experiment, you will be studying the oxidation strength of the halogens. a. What is the color of each of the halogens that you will be working with in this experiment? b. Write Lewis dot structures for each of the halogen molecules: F2, Cl2, Br2, and I2. c. On the basis of periodic trends, which of the halogen molecules do you expect to have the shortest bond? Explain why.arrow_forwardThe sun is a giant nuclear reactor, which emits light (electromagnetic radiation) at a range of frequencies. We human can only see visible light (400 – 700 nm), because its absorption results in a conformational change in the retinal molecule, which triggers a neural signal. a. What is the frequency of a 500 nm visible photon? b. How much energy in J does a 500 nm visible photon carry? A typical chemical bond has an energy of 5x10-19 J. Would a visible photon at 500 nm be С. sufficient to break a chemical bond? d. How about a UV (200 nm) photon? Indeed, UV light can damage DNA, the genetic material in our body, leading to mutations and possibly cancer.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning