Chemistry: The Central Science (13th Edition)
13th Edition
ISBN: 9780321910417
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Textbook Question
Chapter 4, Problem 62E
Which of these statements is true?
- All spontaneous reactions have a negative enthalpy change
- All spontaneous reactions have a positive enthalpy change
- All spontaneous reactions have a positive free-energy change
- All spontaneous reactions have a negetive free-energy change
- All spontaneous reactions have a negative entropy change
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
1. Which of the following is true?
It is possible to convert heat completely into work without wastage.
The enthalpy of the universe is continuously increasing.
The entropy of the universe is continuously increasing.
A reaction is spontaneous if the change in enthalpy is greater than zero and the change in entropy is less than zero.
2. Which of the following is correct? *
The change in free energy is the total free energy of the products added to the total free energy of the reactants.
The change in free energy is the total free energy of the reactants added to the total free energy of the products.
The change in free energy is the total free energy of the products subtracted from the total free energy of the reactants.
The change in free energy is the total free energy of the reactants subtracted from the total free energy of the products.
3. A reaction is an equilibrium if...
The change in the free energy of the system is…
At equilibrium, the free energy of the reactants is equal to the free energy of the products.
true or false
Given the following data:
2 03(g) → 3 0₂(g)
0₂(g) → 2 0(g)
NO(g) + 03(g) → NO₂(g) + O₂(g)
calculate AH for the reaction
NO(g) + O(g) →→ NO₂(g).
KJ
ΔΗ = −286 kJ
ΔΗ = +498 KJ
ΔΗ = – 199 kJ
Chapter 4 Solutions
Chemistry: The Central Science (13th Edition)
Ch. 4.1 - Prob. 4.1.1PECh. 4.1 - How are the boundaries between the regions of the...Ch. 4.2 - Air pollution in the Mexico City metropolitan area...Ch. 4.2 - Prob. 4.2.2PECh. 4.2 - Prob. 4.3.1PECh. 4.2 - Prob. 4.3.2PECh. 4.2 - Prob. 4.4.1PECh. 4.2 - Prob. 4.4.2PECh. 4.3 - Distinguish between photodissociation and...Ch. 4.3 - Prob. 4.5.2PE
Ch. 4.3 - Prob. 4.6.1PECh. 4.3 - Prob. 4.6.2PECh. 4.3 - Do the reactions involved in ozone depletion...Ch. 4.3 - Prob. 4.7.2PECh. 4.4 - Prob. 4.8.1PECh. 4.4 - Prob. 4.8.2PECh. 4.4 - Prob. 4.9.1PECh. 4.4 - Prob. 4.9.2PECh. 4.4 - Prob. 4.10.1PECh. 4.4 - Prob. 4.10.2PECh. 4.5 - Practice Exercise 2 The bond energy in N2 is 941...Ch. 4.5 - Prob. 4.11.2PECh. 4.5 - Prob. 4.12.1PECh. 4.5 - Prob. 4.12.2PECh. 4.5 - Prob. 4.13.1PECh. 4.5 - Prob. 4.13.2PECh. 4.5 - The figure shows the three lowest regions of...Ch. 4.5 - Prob. 4.14.2PECh. 4.6 - Where does the energy come from to evaporate the...Ch. 4.6 - Prob. 4.15.2PECh. 4.6 - Prob. 4.16.1PECh. 4.6 - The first stage of treatment at the reverse...Ch. 4.6 - Prob. 4.17.1PECh. 4.6 - Prob. 4.17.2PECh. 4 - Prob. 1DECh. 4 - Prob. 1ECh. 4 - Prob. 2ECh. 4 - Prob. 3ECh. 4 - Prob. 4ECh. 4 - Prob. 5ECh. 4 - Prob. 6ECh. 4 - Which of the following ions will always be a...Ch. 4 - Prob. 8ECh. 4 - Prob. 9ECh. 4 - Prob. 10ECh. 4 - Prob. 11ECh. 4 - List the common products formed when an organic...Ch. 4 - Prob. 13ECh. 4 - Prob. 14ECh. 4 - Prob. 15ECh. 4 - Prob. 16ECh. 4 - Prob. 17ECh. 4 - Prob. 18ECh. 4 - Prob. 19ECh. 4 - Prob. 20ECh. 4 - Prob. 21ECh. 4 - Prob. 22ECh. 4 - Prob. 23ECh. 4 - Prob. 24ECh. 4 - Prob. 25ECh. 4 - Prob. 26ECh. 4 - Prob. 27ECh. 4 - Prob. 28ECh. 4 - Prob. 29ECh. 4 - Explain, using Le Châtelier’s principle, why the...Ch. 4 - Prob. 31ECh. 4 - Prob. 32ECh. 4 - Prob. 33ECh. 4 - Prob. 34ECh. 4 - Prob. 35ECh. 4 - Prob. 36ECh. 4 - Prob. 37ECh. 4 - Prob. 38ECh. 4 - Prob. 39ECh. 4 - Prob. 40ECh. 4 - Prob. 41ECh. 4 - Prob. 42ECh. 4 - Prob. 43ECh. 4 - Prob. 44ECh. 4 - Prob. 45ECh. 4 - 18.85 The main reason that distillation is a...Ch. 4 - Prob. 47ECh. 4 - Prob. 48ECh. 4 - Prob. 49ECh. 4 - Prob. 50ECh. 4 - Prob. 51ECh. 4 - Prob. 52ECh. 4 - The process of iron being oxidized to make iron...Ch. 4 - At 1 atm pressure, CO2(s) sublimes at 78oC. Is...Ch. 4 - Prob. 55ECh. 4 - Prob. 56ECh. 4 - Prob. 57ECh. 4 - Prob. 58ECh. 4 - Prob. 59ECh. 4 - Prob. 60ECh. 4 - Using the standard molar entropies in Appendix C,...Ch. 4 - Which of these statements is true? All spontaneous...Ch. 4 - Prob. 63ECh. 4 - Prob. 64ECh. 4 - Prob. 65ECh. 4 - Prob. 66ECh. 4 - Prob. 67ECh. 4 - What is the temperature above which the Haber...Ch. 4 - Prob. 69ECh. 4 - Prob. 70ECh. 4 - Prob. 71ECh. 4 - Prob. 72ECh. 4 - Prob. 73ECh. 4 - Prob. 74ECh. 4 - Prob. 75ECh. 4 - Prob. 76ECh. 4 - As shown here, one type of computer keyboard...Ch. 4 - 19.3
a. What are the signs of ΔS and ΔH for the...Ch. 4 - Predict the signs of H and S for this reaction....Ch. 4 - Prob. 80ECh. 4 - The accompanying diagram shows how H (red line)...Ch. 4 - Prob. 82ECh. 4 - Prob. 83ECh. 4 - Prob. 84ECh. 4 - Prob. 85ECh. 4 - Prob. 86ECh. 4 - Prob. 87ECh. 4 - Can endothermic chemical reaction be spontaneous?...Ch. 4 - Prob. 89ECh. 4 - Prob. 90ECh. 4 - Prob. 91AECh. 4 - Prob. 92AECh. 4 - Prob. 93AECh. 4 - Prob. 94AECh. 4 - Prob. 95AECh. 4 - Prob. 96AECh. 4 - Prob. 97AECh. 4 - Prob. 98AECh. 4 - Prob. 99AECh. 4 - Prob. 100AECh. 4 - Prob. 101AECh. 4 - Prob. 102AECh. 4 - Prob. 103AECh. 4 - Alcohol-based fuels for automobiles lead to the...Ch. 4 - Prob. 105IECh. 4 - Prob. 106IECh. 4 - Prob. 107IECh. 4 - Prob. 108IECh. 4 - Prob. 109IECh. 4 - Prob. 110IECh. 4 - Prob. 111IECh. 4 - Prob. 112IECh. 4 - Although there are many ions in seawater, the...Ch. 4 - The Ogallala aquifer described in the Close Look...Ch. 4 - Prob. 115IE
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
- Which of the following circumstances will result in a reaction that is spontaneous only at low temperatures? positive enthalpy change and positive entropy change negative enthalpy change and negative entropy change positive enthalpy change and negative entropy change negative enthalpy change and positive entropy changearrow_forwardThe standard free energy variation, at 25 ºC, for equilibrium: Glucose-6-phosphate (G-6-P) Glucose-1-phosphate (G-1-P) is ΔGº '= + 7280 J / mol. Calculate a) The equilibrium constant of the reaction. b) The real change in free energy when one mole of G-6-P is transformed into G-1-P, both concentrations remaining constant and equal to 10mM and 2 mM respectively.arrow_forward1. Is the Boudouard Reaction exothermic or endothermic? 2. Is the reaction spontaneous at low temperatures? 3. Is the reaction spontaneous at high temperatures? 4. At what temperature the reaction becomes spontaneous? 5. The vant Hoff's equation works if there is no (or very weak) temperature dependence of change of standard enthalpy and standard entropy on temperature. Does your vant Hoff's graph support this assumption?arrow_forward
- Study the reactions for the formation of compounds from their elements. 1. C (s) + 02 (g) → CO2 (g) AH=-394 kJ 2. H2 (9) + 02 (g) → H20 (1) 3. 20 (s) + 3H2 (g) → C2H6 (g) ΔΗ-242 kJ ΔΗ--84 kJ The combustion of C2H6 is shown by the following equation: C2H6 (g) + 02 (9) → 2CO2 (9) + 3H2O (1) AH. = ? -286 kJ -1,430 kJ 286 kJ 1,430 kJarrow_forward5. The change in enthalpy for a certain reaction is a small, positive number. The change in entropy for this reaction is an extremely large positive number. Is this reaction exergonic or endergonic?exergonic endogonicarrow_forwardWhat is AS for the combustion of propane? C3H8(g) +502(g) → 3CO2(g) + 4H₂O(g) Substance C3H8(g) O2(g) CO2(g) H₂O(g) S(J/K mol) 269.9 205.0 213.6 188.7arrow_forward
- oxygen Photosynthesis in plants converts carbon dioxide and water into glucose (C,H,O) and according to the equation below. 6CO₂(g) + 6H₂O() - CH₂O() + 60₂(g) Substance CO(g) H₂O(1) C₂H₁₂O(s) O(g) AHi(kJ/mol) -393.5 -285.8 -1273.3 0 SᵒJ/mol K) 213.6 69.9 209.2 205.0 Calculate the AH, AS, and AG. Is the reaction spontaneous at standard conditions?arrow_forwardConsider a general reaction with the following free energy: Products, AGⓇ' = 5.3 kJ/mol Select all of following that are TRUE about this reaction. Reactants This reaction never occurs. At equilibrium, the reactants are favored. This reaction always occurs. The reactions goes in the forward direction The reaction is non-spontaneous At equilibrium, the products are favored. The reaction is spontaneous The reaction goes in the reverse directionarrow_forwardIndicate which of the four cases below applies to the following four reactions (a through d) by writing 1, 2, 3, or 4 after each letter Spontaneous at all temperatures. Spontaneous above a certain temperature. Spontaneous below a certain temperature. Non-spontaneous at all temperatures. a) PCl3(g) + Cl2(g) ↔ PCl2(g) ΔH° = -87 KJ b) CH4(g) + 2 O2(g) ↔ CO2(g) + 2 H2O(g) ΔH° = +41 KJ c) 2 NH3(g) → N2(g) + 3 H2(g) ΔH° = +160 KJ d) Mg(s) + 2 HCl(aq) → MgCl2(aq) + H2(g) ΔH° = -462 KJ please write which number they classify asarrow_forward
- Given that the reaction of 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 3 H20 (g) ΔΗ - - 906 kJ What would AH for NO (g) + ? H20 (g) → NH3 (g) + O2 (g) be? 2. 906 kJ 226.5 kJ -226.5kJ 453 kJarrow_forwardA certain reaction has negative value of both ∆H and ∆S. Therefore, the reaction must be spontaneous at all temperature cannot be spontaneous at any temperature cannot be spontaneous if the temperature is high enough cannot be spontaneous if the temperature is low enough has a positive free energy at any temperaturearrow_forwardCalculate the standard free energy, ΔGo, for the following equation at 25.0 oC and determine if the reaction is favorable or unfavorable. C2H6(g) + 7Cl2(g) ⟶ 2CCl4(g) + 6HCl(g) Group of answer choices 720.2 kJ/mole, unfavorable -656.2 kJ/mole, favorable 720.2 kJ/mole, favorable -720.2 kJ/mole, unfavorable 19.7 kJ/mole, favorable -656.2 kJ/mole, unfavorable 656.2 kJ/mole, favorable -19.7 kJ/mole, favorable -720.2 kJ/mole, favorable -19.7 kJ/mole, unfavorable 656.2 kJ/mole, unfavorable 19.7 kJ/mole, unfavorablearrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
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