Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 7.19B, Problem 7.36P
The dehydrogenation of butane to trans-but-2-ene has ΔH° = +116kJ/mol( +27.6kcal/mol) and ΔS° = + 117J/Kelvin - mol (+28.0cal/Kelvin — mol).
- a. Compute the value of ΔG° for dehydrogenation at room temperature (25 °C or 298 °K). Is dehydrogenation favored or disfavored?
- b. Compute the value of ΔG for dehydrogenation at 1000 °C, assuming that ΔS and ΔH are constant. Is dehydrogenation favored or disfavored?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of the reactants and products.Compound ΔGof (kJmol)ΔGfo(kJmol)
The equation H2O(l) → H2O(g)
ΔGoΔGokJ
C2H2(g)209.9 CO2(g)-394.4 H2O(g)-228.6 H2O(l)-237.1 N2(g)0 NO(g)87.6 O2(g)0
Which expression below could be used to calculate the free energy change for a chemical reaction at any temperature? Choose one:
1. ΔG°rxn = ΔH°rxn – TΔS°rxn
2. ΔG°rxn = Σ(ΔG°f,Reactants) – Σ(ΔG°f,Products)
3. ΔG°rxn = ΔH°rxn + TΔS°rxn
4. ΔG°rxn = Σ(ΔG°f,Products) – Σ(ΔG°f,Reactants)
3. A reaction has a standard free energy change (G⁰) of -21.6 kJ/mol at 25 ⁰C.a. Is this reaction spontaneous or non-spontaneous at 25 ⁰C? b. Given the value of G⁰ above (-21.6 kJ/mol), what is the value of the equilibrium constant (K or Keq)for this reaction at 25 ⁰C?
Chapter 7 Solutions
Organic Chemistry (9th Edition)
Ch. 7.3A - Prob. 7.1PCh. 7.3A - Prob. 7.2PCh. 7.3B - Draw five more compounds of formula C4H6NOC1.Ch. 7.3B - For each of the following molecular formulas,...Ch. 7.4 - Give the systematic (IUPAC) names of the following...Ch. 7.5B - The following names are all incorrect. Draw the...Ch. 7.5B - Prob. 7.8PCh. 7.5B - a. How many stereogcmc double bonds are in...Ch. 7.6 - Teflon-coated frying pans routinely endure...Ch. 7.7B - Prob. 7.11P
Ch. 7.8B - Use the data in Table7-2 to predict the energy...Ch. 7.8C - Prob. 7.13PCh. 7.8E - Explain why each of the following alkenes is...Ch. 7.8F - Prob. 7.15PCh. 7.10 - Prob. 7.16PCh. 7.10A - SN1 substitution and E1 elimination frequently...Ch. 7.10C - Prob. 7.18PCh. 7.10C - Prob. 7.19PCh. 7.10C - Prob. 7.20PCh. 7.11 - Prob. 7.21PCh. 7.11 - Prob. 7.22PCh. 7.12 - Prob. 7.23PCh. 7.12 - Prob. 7.24PCh. 7.13 - Prob. 7.25PCh. 7.14B - Prob. 7.26PCh. 7.14B - Make models of the blowing compounds, and predict...Ch. 7.15 - Prob. 7.28PCh. 7.15 - Prob. 7.29PCh. 7.15 - Prob. 7.30PCh. 7.15 - Prob. 7.31PCh. 7.16 - Predict the major and minor elimination products...Ch. 7.17B - Predict the products and mechanisms of the...Ch. 7.18 - Propose mechanisms for the following reactions.Ch. 7.18 - Prob. 7.35PCh. 7.19B - The dehydrogenation of butane to trans-but-2-ene...Ch. 7.19B - Prob. 7.37PCh. 7.19B - Prob. 7.38PCh. 7.19B - Prob. 7.39PCh. 7 - Prob. 7.40SPCh. 7 - Prob. 7.41SPCh. 7 - Prob. 7.42SPCh. 7 - Prob. 7.43SPCh. 7 - Prob. 7.44SPCh. 7 - Prob. 7.45SPCh. 7 - Prob. 7.46SPCh. 7 - The energy difference between cis- and...Ch. 7 - Prob. 7.48SPCh. 7 - Prob. 7.49SPCh. 7 - Prob. 7.50SPCh. 7 - What halides would undergo E2 dehydrohalogenation...Ch. 7 - Prob. 7.52SPCh. 7 - Prob. 7.53SPCh. 7 - Write a balanced equation for each reaction,...Ch. 7 - Prob. 7.55SPCh. 7 - Using cyclohexane as your starting material, show...Ch. 7 - Show how you would prepare cyclopentene from each...Ch. 7 - Prob. 7.58SPCh. 7 - E1 eliminations of alkyl halides are rarely useful...Ch. 7 - Prob. 7.60SPCh. 7 - Propose mechanisms for the following reactions....Ch. 7 - Prob. 7.62SPCh. 7 - Prob. 7.63SPCh. 7 - Prob. 7.64SPCh. 7 - Prob. 7.65SPCh. 7 - Prob. 7.66SPCh. 7 - Prob. 7.67SPCh. 7 - Prob. 7.68SPCh. 7 - Prob. 7.69SPCh. 7 - Explain the dramatic difference in rotational...Ch. 7 - One of the following dichloronorbornanes undergoes...Ch. 7 - A graduate student wanted to make...Ch. 7 - Prob. 7.73SPCh. 7 - Prob. 7.74SPCh. 7 - Prob. 7.75SPCh. 7 - Prob. 7.76SP
Additional Science Textbook Solutions
Find more solutions based on key concepts
For Practice 1.1
Is each change physical or chemical? Which kind of property (chemical or physical) is demonst...
Principles of Chemistry: A Molecular Approach (3rd Edition)
4. 38 Strontium has four naturally occurring isotopes, with mass numbers 84, 86, 87, arid 88.
a. Write the atom...
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Describe the orbitals used in bonding and the bond angles in the following compounds: a. CH3O b. CO2 c. H2CO d....
Organic Chemistry (8th Edition)
Calculate the lattice energy of CaCl2 using a Born-Haber cycle and data from Appendices F and L and Table 7.5. ...
Chemistry & Chemical Reactivity
The active ingredient in Tylenol and a host of other over-the-counter pain relievers is acetaminophen (C8H9NO2)...
Chemistry: Atoms First
Consider a sample of ideal gas initially in a volume V at temperature T and pressure P. Does the entropy of thi...
General Chemistry: Principles and Modern Applications (11th Edition)
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
- 1. 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_forwardFor the conversion of reactant A to product B, the change in enthalpy is 7.80 kJ·mol-1 and the change in entropy is 44.4 J·K-1·mol-1. Above what temperature, in Kelvin, does the reaction become spontaneous?___ K.arrow_forwardConsider the reaction represented below, which is spontaneous at 298K SO2(g) + 2 NH3(g) → SO(NH2)2 (s) + H2O(l) ΔH° = -205 kJ 1. For the reaction, how is the value of the standard free energy change, ΔG°, affected by an decrease in temperature? Explain. 2. When SO2 and NH3 are combined at 298 K no measurable amount of product appears after 1 hour. Explain this observation.arrow_forward
- Consider the following reaction at 25 °C: 3 Ni(s) + N₂(g) + 3 H₂O(g) → 3 NiO(s) + 2 NH₃(g) If ∆H° = -85.7 kJ/mol and ∆S° = -348.3 J/mol•K, determine the standard free energy for the reaction at 25 °C.arrow_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_forwardConsider the balanced reaction: 2Cr3+(aq)+3PbO2(s)+6H2O(l)→2CrO42-(aq)+3Pb2+(aq)+4H3O+ (aq) d.How many valence electrons are in the CrO42- ion? e. How many moles of electrons, ne, are transferred per mole of this reaction? f. At a certain point the measured free energy is ∆G. Adding more PbO2 will cause the free energy change of the reaction, ∆G, to choose...(Increase, Stay the same, Decrease)arrow_forward
- Calculate ΔG0 for the combustion of 1 mol ethanol, C2H5OH. C2H5OH(l) + 3O2(g). 2CO2(g) + 3H2O(g) The standard free energies of formation are: ΔG0fof C2H5OH.=-174.8 kJ , ΔG0fof O2(g) = 0,ΔG0fof CO2(g) = -394.4 kJ, ΔG0f of H2O(g) = -228.6 kJarrow_forwarda) Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH₃(g) → 3 Ni(s) + N₂(g) + 3 H₂O(g) Given the information in the table, calculate ∆S° for the reaction. b) Determine the standard free energy for the reaction at 25 °C. c) Determine the value of the equilibrium constant at 25 °C. d) Estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature. e) Determine the value of ∆G assuming that a mixture contains 57.6 g of NiO, 182.3 g of Ni, 0.24 atm of NH₃, 8.54 atm of N₂ and 10.07 atm of H₂O.arrow_forward1. Find DHrxn, DSrxn, and DGrxn, using the tables at the end of your textbook for the phase change of water from liquid to gas at 25.0°C. H2O (l) <---> H2O (g) 2. Is this phase change spontaneous at 25.0°C? Give the reason for your answer. 3. Find the temperature at which this phase change becomes spontaneous. Give in both K and ℃. 4. Is this what you expect, and why? (Is the answer to question #3 what you expect)arrow_forward
- 5. Consider the combustion reaction of octane (C8H18, mol. wt. = 114.23 g/mol, density = 0.703 g/mL). a. Write out the balanced chemical equation for this reaction. All products are in the gas phase. 2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O b. Calculate the standard free energy (in kJ/mol) released in this reaction. ∆Hfo (kJ/mol) Sfo (J/K mol) Octane(l) ─208.4 463.7 H2O(g) ─242 189 02 0 205 CO2(g) ─393.5 214 c. Making the approximation that gasoline consists of 100% octane, how much energy would 1.00 gallon of gasoline release? (1 quart = 946 mL, 1 gallon = 4 quarts)arrow_forwardA spontaneous reaction always has: A. a positive enthalpy change and a negative entropy change. B. a positive Gibbs free energy change. C. a negative Gibbs free energy change. D. a standard enthalpy of formation equal to zero for one of the reactants. E. a standard free energy of formation equal to zero for one of the reactants.arrow_forwardWhich of the following reaction is a spontaneous? 2SO2(g) + O2(g) → 2SO3(g) 2C(s) + O2(g) → 2CO2(g) H2O(l) → H2O(s) CaO(s) + CO2(g) → CaCO3(g)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 Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
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