Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Question
Chapter 16, Problem 2ALQ
Interpretation Introduction
Interpretation: The quantity, among
Concept introduction: The randomness of a molecule of a substance in gaseous form is comparatively more than that of a substance in a liquid or the solid state.
To determine: The quantity, among
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
8. What is the symbol for energy/heat flow in the field of thermochemistry?
O Hf
E
H
15. What is Hess's Law? How is it used? Why is it important in chemistry? Explain your ideas and provide
at least one relevant example to support your answer.
Given these reactions, where X represents a generic metal or metalloid
1) H, (g) + 0,(g) → H,0(g)
AH1 = -241.8 kJ
2) X(s) + 2 Cl,(g) → XCl,(s)
AH2 = +475.9 kJ
3) H,(g) + CL,(g)
HCl(g)
АНз 3 —92.3 kJ
→
4) X(s) + O,(g) –→ XO,(s)
AH4 = -748.7 kJ
5) Н, О(2) — н,00)
AH5 = -44.0 kJ
what is the enthalpy, AH, for this reaction?
XCI, (8) + 2H,О() — ХО,(8) + 4 HCI(g)
Chapter 16 Solutions
Chemistry: An Atoms First Approach
Ch. 16 - Define the following: a. spontaneous process b....Ch. 16 - What is the second law of thermodynamics? For any...Ch. 16 - Prob. 3RQCh. 16 - Prob. 4RQCh. 16 - Prob. 5RQCh. 16 - What is the standard free energy change, G, for a...Ch. 16 - If you calculate a value for G for a reaction...Ch. 16 - Consider the equation G = G + RT ln(Q). What is...Ch. 16 - Even if G is negative, the reaction may not occur....Ch. 16 - Prob. 10RQ
Ch. 16 - For the process A(l) A(g), which direction is...Ch. 16 - Prob. 2ALQCh. 16 - Gas A2 reacts with gas B2 to form gas AB at a...Ch. 16 - Prob. 4ALQCh. 16 - Prob. 5ALQCh. 16 - Prob. 6ALQCh. 16 - Predict the sign of S for each of the following...Ch. 16 - Is Ssurr favorable or unfavorable for exothermic...Ch. 16 - At 1 atm, liquid water is heated above 100C. For...Ch. 16 - Prob. 10ALQCh. 16 - The synthesis of glucose directly from CO2 and H2O...Ch. 16 - When the environment is contaminated by a toxic or...Ch. 16 - Entropy has been described as times arrow....Ch. 16 - Prob. 14QCh. 16 - A mixture of hydrogen gas and chlorine gas remains...Ch. 16 - Consider the following potential energy plots: a....Ch. 16 - Prob. 17QCh. 16 - Given the following illustration, what can be said...Ch. 16 - The third law of thermodynamics states that the...Ch. 16 - Prob. 20QCh. 16 - Prob. 21QCh. 16 - Prob. 22QCh. 16 - Monochloroethane (C2H5Cl) can be produced by the...Ch. 16 - Prob. 24QCh. 16 - Which of the following processes are spontaneous?...Ch. 16 - Which of the following processes are spontaneous?...Ch. 16 - Prob. 27ECh. 16 - Consider the following illustration of six...Ch. 16 - Consider the following energy levels, each capable...Ch. 16 - Prob. 30ECh. 16 - Choose the substance with the larger positional...Ch. 16 - Which of the following involve an increase in the...Ch. 16 - Predict the sign of Ssurr for the following...Ch. 16 - Prob. 34ECh. 16 - Given the values of H and S, which of the...Ch. 16 - At what temperatures will the following processes...Ch. 16 - Ethanethiol (C2H5SH; also called ethyl mercaptan)...Ch. 16 - For mercury, the enthalpy of vaporization is 58.51...Ch. 16 - For ammonia (NH3), the enthalpy of fusion is 5.65...Ch. 16 - The enthalpy of vaporization of ethanol is 38.7...Ch. 16 - Predict the sign of S for each of the following...Ch. 16 - Prob. 42ECh. 16 - Prob. 43ECh. 16 - For each of the following pairs, which substance...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Predict the sign of S and then calculate S for...Ch. 16 - Prob. 47ECh. 16 - Prob. 48ECh. 16 - Prob. 49ECh. 16 - Two crystalline forms of white phosphorus are...Ch. 16 - Consider the reaction 2O(g)O2(g) a. Predict the...Ch. 16 - Prob. 52ECh. 16 - Prob. 53ECh. 16 - The major industrial use of hydrogen is in the...Ch. 16 - Prob. 55ECh. 16 - At 100C and 1.00 atm, H = 40.6 kJ/mol for the...Ch. 16 - Prob. 57ECh. 16 - Prob. 58ECh. 16 - Prob. 59ECh. 16 - Prob. 60ECh. 16 - Consider the reaction...Ch. 16 - Consider the reaction 2POCl3(g)2PCl3(g)+O2(g) a....Ch. 16 - Prob. 63ECh. 16 - Consider two reactions for the production of...Ch. 16 - Prob. 65ECh. 16 - Prob. 66ECh. 16 - Consider the reaction 2NO2(g)N2O4(g) For each of...Ch. 16 - Prob. 68ECh. 16 - One of the reactions that destroys ozone in the...Ch. 16 - Hydrogen sulfide can be removed from natural gas...Ch. 16 - Consider the following reaction at 25.0C:...Ch. 16 - The standard free energies of formation and the...Ch. 16 - Calculate G forH2O(g)+12O2(g)H2O2(g) at 600. K,...Ch. 16 - The Ostwald process for the commercial production...Ch. 16 - Cells use the hydrolysis of adenosine...Ch. 16 - One reaction that occurs in human metabolism is...Ch. 16 - Prob. 77ECh. 16 - Consider the following reaction at 298 K:...Ch. 16 - Prob. 79ECh. 16 - The equilibrium constant K for the reaction...Ch. 16 - Prob. 81AECh. 16 - Some water is placed in a coffee-cup calorimeter....Ch. 16 - Consider the following system at equilibrium at...Ch. 16 - Calculate the entropy change for the vaporization...Ch. 16 - As O2(l) is cooled at 1 atm, it freezes at 54.5 K...Ch. 16 - Prob. 86AECh. 16 - Using the following data, calculate the value of...Ch. 16 - Prob. 88AECh. 16 - Carbon monoxide is toxic because it bonds much...Ch. 16 - Prob. 90AECh. 16 - Prob. 91AECh. 16 - Use the equation in Exercise 79 to determine H and...Ch. 16 - Consider the reaction...Ch. 16 - Consider the following diagram of free energy (G)...Ch. 16 - Prob. 95CWPCh. 16 - For rubidium Hvapo=69.0KJ/mol at 686C, its boiling...Ch. 16 - Given the thermodynamic data below, calculate S...Ch. 16 - Prob. 98CWPCh. 16 - Prob. 99CWPCh. 16 - Consider the dissociation of a weak acid HA (Ka =...Ch. 16 - Prob. 101CWPCh. 16 - The equilibrium constant for a certain reaction...Ch. 16 - For the following reactions at constant pressure,...Ch. 16 - The standard enthalpy of formation of H2O(l) at...Ch. 16 - Prob. 105CPCh. 16 - Liquid water at 25C is introduced into an...Ch. 16 - Using data from Appendix 4, calculate H, G, and K...Ch. 16 - Prob. 108CPCh. 16 - Prob. 109CPCh. 16 - Prob. 110CPCh. 16 - Prob. 111CPCh. 16 - Prob. 112CPCh. 16 - If wet silver carbonate is dried in a stream of...Ch. 16 - Carbon tetrachloride (CCl4) and benzene (C6H6)...Ch. 16 - Sodium chloride is added to water (at 25C) until...Ch. 16 - Prob. 116CPCh. 16 - Prob. 117CPCh. 16 - Prob. 118IPCh. 16 - Prob. 119IPCh. 16 - Prob. 120IPCh. 16 - Consider a sample containing 5.00 moles of a...Ch. 16 - Impure nickel, refined by smelting sulfide ores in...
Knowledge Booster
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
- 9.34 A copper nail and an iron nail of the same mass and initially at the same room temperature are both put into a vessel containing boiling water. Which one would you expect to reach 100°C first? Why?arrow_forwardDefine the following terms: potential energy, kinetic energy, path-dependent function, state function, system, surroundings.arrow_forwardThe diagram below shows a system that is made up of 3 molecules (labeled A, B, and C) that contains a total of 4 units of energy. Assuming that no molecule can have 0 energy associated with it, and that only integral amounts of units of energy are allowed (energy = 1 or energy = 2 is allowed, but energy = 1.5 is not). In the left-most diagram, one possible way of distributing the four units of energy among these three molecules is presented. This distribution is represented as: (1, 1, 2). %3D 6 SEE 6 5 4 4 4 3 3 3 2 2 1 1 1 A B C AB C АВС (1, 1, 2) a. Show explicitly that a total of 4 units of energy are present in the left-most diagram. b. Explain why (1, 3, 0) is not an allowed distribution for this system. Show the other two allowed distributions of energy for this system using the two blank diagrams, and write the corresponding representation below each diagram. С.arrow_forward
- Dulong and Petit’s law states that specific heat capacity x atomic mass = 3R. If the specific heat capacity of an element is 0.93 J/goC, identify the element.arrow_forwardConsider the following data. 2 H₂0 (1) 2 H₂(g) + O₂(g) 2 HNO3(1) = N₂05(9) + H₂O(1) 2 HNO30 (1) ⇒ N₂(g) + 3 O₂(g) + H₂(g) Use Hess's law to calculate AH for the reaction below. ΔΗ= |1083.8 AH = +571.7 kJ AH = +92.0 kJ AH = +348.2 kJ x kJ 2 N₂05(9) 2 N₂(g) + 5 O₂(g)arrow_forwardLook up the Born-Haber Cycle and read about it (book or internet). Use the following information and Hess' Law to calculate AH°iatt of NaCl Na(s) → Na(g) Cl2(g) → 2CI(g) Na(g) > Na*(g) + e Cl(g) + e → Cl'(g) Na(s) +Cl2(g) → NaCl(s) AH° = -411 kJ AH° = 109 kJ AH° = 243 kJ AH° = 496 kJ AH° = -349 kJ %3Darrow_forward
- what is meant by term state function?arrow_forwardCalculate how much energy would be needed for 64.8 g titanium at 19.4 oC to reach 582 degrees Celcius.arrow_forwardUse the following enthalpy data and apply Hess's Law to calculate the formation of NH4Cl(s). 1/2 N2(g) + 3/2 H2 (g) ---> NH3(g) .......................... -45.77 kJ/mol H2(g) + Cl(g) ---> 2HCl (g) ....................................... -184.62 kJ/mol NH3(g) ---> NH3(aq) ............................................... -35.40 kJ/mol HCl(g) ---> HCl(aq) ................................................... -72.84 kJ/mol NH3(aq) + HCl(aq) ---> NH4Cl(aq) ............................ 28.54 kJ/mol NH4Cl(s) ---> NH4Cl(aq) ......................................... -15.38 kJ/mol ΔH for NH4Cl(s): 1/2 N2(g) + 2 H2(g) + 1/2 Cl2(g) ---> NH4Cl(s) The equation above is already balanced, I'm just really confused as to how I use Hess's Law to "add" the other enthalpy reactions to get to this one. Like, I don't know which ones to flip, where to multiple or anything. Any help would be greatly appreciated!arrow_forward
- Please explain the difference between DeltaH and DeltaE in thermochemistry. Thanks!arrow_forwardWhat are the theories or concepts behind the Thermochemistry and explain it.arrow_forward20) Calculate the sublimation enthalpy for Lithium using the following information. Li(s) + ½ F2(g) → LiF(s) -605.6 kJ/mol F2(g) → 2F(g) +158 kJ/mol Li+(g) + F - (g) → LiF(s) -1036 kJ/mol F(g) + e- → F - (g) -328 kJ/mol Li(s) → Li(g) ? Li(g) → Li+(g) + e- +520 kJ/mol A) +238.4 kJ/mol B) +96.2 kJ/mol C) +159.4 kJ/mol D) +80.4 kJ/mol E) -1242.4 kJ/molarrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
- ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / 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
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
The Laws of Thermodynamics, Entropy, and Gibbs Free Energy; Author: Professor Dave Explains;https://www.youtube.com/watch?v=8N1BxHgsoOw;License: Standard YouTube License, CC-BY