ORGANIC CHEMISTRY
5th Edition
ISBN: 9781259977596
Author: SMITH
Publisher: MCG
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 6, Problem 6.12P
The equilibrium constant for the conversion of the axial to the equatorial conformation of methoxycyclohexane is
a. Given these data, which conformation is present in the larger amount at equilibrium?
b. Is
c. From the values in Table
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
Given the following data:
4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l)
ΔH°=-480.0 kJ
CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l)
ΔH°=-492.0 kJ
2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l)
ΔH°=-278.0 kJ
H2(g) + 1/2O2(g) → H2O(l)
ΔH°=-286.0 kJ
calculate ΔH° for the reaction:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)
Given the following data:
2 C6H6(l) + 15 O2(g) → 12 CO2(g) + 6 H2O(l) ΔG0= -6399 kJ
C(s) + O2(g) → CO2(g) ΔG0= -394 kJ
H2(g) + ½O2(g) → H2O(l) ΔG0= -237 kJ
Calculate the ΔG0rxn for the reaction
6 C(s) + 3 H2(g) → C6H6(l)
Difluoroacetylene (C2F2) gas has a ΔHf° = 241.2 kJ/mole and a a ΔGf° = 191.2 kJ/mole. Hexafluorobenzene(C6F6) gas has a ΔHf° = 132.8 kJ/mole and a a ΔGf° = 78.2 kJ/mole. For the following reaction:
C6F6(g) ⇌ 3C2F2(g)
Calculate:a) The ΔS for the reaction at 25 °Cb) The equilibrium constant K at 25 °Cc) The equilibrium constant K at 2700 °C (assuming there is no temperature dependance on ΔH and ΔS)
Chapter 6 Solutions
ORGANIC CHEMISTRY
Ch. 6 - Problem 6.1 Classify each transformation as...Ch. 6 - Prob. 6.2PCh. 6 - Problem 6.3 By taking into account...Ch. 6 - Problem 6.4 Use curved arrows to show the movement...Ch. 6 - Problem 6.5 Follow the curved arrows and draw the...Ch. 6 - Prob. 6.6PCh. 6 - Problem 6.7 Use the values in Table 6.2 to...Ch. 6 - Prob. 6.8PCh. 6 - aWhich Keq corresponds to a negative value of G,...Ch. 6 - Given each of the following values, is the...
Ch. 6 - Given each of the following values, is the...Ch. 6 - The equilibrium constant for the conversion of the...Ch. 6 - Prob. 6.13PCh. 6 - For a reaction with H=40kJ/mol, decide which of...Ch. 6 - For a reaction with H=20kJ/mol, decide which of...Ch. 6 - Draw an energy diagram for a reaction in which the...Ch. 6 - Prob. 6.17PCh. 6 - Prob. 6.18PCh. 6 - Problem 6.19 Consider the following energy...Ch. 6 - Draw an energy diagram for a two-step reaction,...Ch. 6 - Which value if any corresponds to a faster...Ch. 6 - Prob. 6.22PCh. 6 - Problem 6.23 For each rate equation, what effect...Ch. 6 - Prob. 6.24PCh. 6 - Identify the catalyst in each equation. a....Ch. 6 - Draw the products of homolysis or heterolysis of...Ch. 6 - Explain why the bond dissociation energy for bond...Ch. 6 - Classify each transformation as substitution,...Ch. 6 - Prob. 6.29PCh. 6 - 6.30 Draw the products of each reaction by...Ch. 6 - 6.31 (a) Add curved arrows for each step to show...Ch. 6 - Prob. 6.32PCh. 6 - Prob. 6.33PCh. 6 - Prob. 6.34PCh. 6 - Calculate H for each reaction. a HO+CH4CH3+H2O b...Ch. 6 - Homolysis of the indicated CH bond in propene...Ch. 6 - Prob. 6.37PCh. 6 - Prob. 6.38PCh. 6 - 6.39. a. Which value corresponds to a negative...Ch. 6 - Prob. 6.40PCh. 6 - For which of the following reaction is S a...Ch. 6 - Prob. 6.42PCh. 6 - Prob. 6.43PCh. 6 - 6.44 Consider the following reaction: .
Use curved...Ch. 6 - Prob. 6.45PCh. 6 - Draw an energy diagram for the Bronsted-Lowry...Ch. 6 - Prob. 6.47PCh. 6 - Indicate which factors affect the rate of a...Ch. 6 - Prob. 6.49PCh. 6 - 6.50 The conversion of acetyl chloride to methyl...Ch. 6 - Prob. 6.51PCh. 6 - Prob. 6.52PCh. 6 - The conversion of (CH3)3Cl to (CH3)2C=CH2 can...Ch. 6 - 6.54 Explain why is more acidic than , even...Ch. 6 - Prob. 6.55PCh. 6 - Prob. 6.56PCh. 6 - Prob. 6.57PCh. 6 - Although Keq of equation 1 in problem 6.57 does...Ch. 6 - Prob. 6.59P
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
- For the complete combustion of 1.000 mole of propane gas at 298 K and 1 atm pressure, ∆H° = -2220 kJ/mol. What will be the heat released when 4.13 g of propane is combusted under these conditions? The chemical formula for propane is C3H8.arrow_forwardConsider these hydrocarbons: Butane, Hexane, Methane, Propane First look up the formulas, and write them down. Then put them in order from least entropy to most entropy. (Assume the temperature is hot enough that all are in gaseous form.)arrow_forward21. CH3CH=CH2 – CH3CH2CH3 What reactants (and catalysts) are needed to make the reaction above occur? a. heat, pressure Ob. HCI с. Н20, Н2SO4 Od. H2, Ptarrow_forward
- Calculate ΔG° for the reaction of benzene with hydrogen gas to give cyclohexane using the following data: ?6?6 + 3H2 → ?6?12 ΔG∘f (benzene) = 124.5 kJ/mol ΔG∘f (cyclohexane) = 217.3 kJ/mol. Is the reaction spontaneous as written?arrow_forwardTwo 3-carbon molecules are shown here. Both molecules can be completely broken down to CO2 in a process that releases free energy. Which molecule has more free energy to release(left or right)? Explain why.arrow_forwardAcetylene burns in air according to the following equation. C2H2(g) + 5/2 02(g) → 2 CO2(g) + H20(g) AH°, rxn = -1255.8 k) Given that AHO of CO2(g) = -393.5 kJ/mol and AH°; of H20(g) = -241.8 kJ/mol, what is AHO, of C2H2(g)? 4.0 Your response differs from the correct answer by more than 10%. Double check your calculations. kJ/mol Submit Answerarrow_forward
- For an addition reaction, why does free energy, ΔG, becomes more negative with decreasing temperature? a. The negative enthalpy dominates at low temperature. b. The negative entropy dominates at low temperature. c. The positive entropy dominates at low temperature. d. The positive enthalpy dominates at low temperature.arrow_forwardConsider the following reaction: 2CH₂OH(g)→2CH₂(g) + O₂(g), AH- +252.8 kJarrow_forwardAssume that the complete combustion of one mole of glucose, a monosaccharide, to carbon dioxide and water liberates 2870 kJ of energy (AG°¹ = −2870 kJ/mol). If the energy generated by the combustion of glucose is entirely converted to the synthesis of a hypothetical compound X, calculate the number of moles of the compound that could theoretically be generated. Use the value AGo' compound X = -54.9 kJ/mol. Round your answer to two significant figures. moles: =arrow_forward
- Running a mile in ten minutes burns between 100 and 120 calories for a 150-pound person. For the same run, a 200-pound person needs about 135-155 calories. In grams, how much ATP is required for this workout? ATP has a molecular mass of 507 g/mol. ATP's g-phosphate group hydrolysis has a free energy of -32 kJ/mol. One calorie is equal to 1000 calories, and one calorie is equal to 4.184 kilojoules (kJ). How much glucose do you need to fuel this run, both aerobically and anaerobically? Assume that one glucose molecule yields 30 ATP when processed aerobically. Molality of glucose is 180g/mol.arrow_forwardA reaction occurs where ethane, C2H6 is prepared by the reaction of C with H2. Given the following data: C (gr) + 02 (g) → CO2 (g) AH° = -393.5 kJ Please note that C (gr) means carbon in the form of graphite. H2 (g) + 1/2 02 (g) → H20 (1) AH° = -285.8 kJ 2 C2H6 (g) + 7 O2 (g) → 4 CO2 (g) + 6 H2O (1) AH° = -3119.6 kJ Determine AH for the reaction: 2 C (s) + 3 H2 (g) → C2H6 (g) 308.9 kJ -478.1 kJ 1475.2 kJ -84.6 kJ 201.2 kJarrow_forward2) The equilibrium constant Ke for the reaction A B is 1 x 105 at room temperature (25°C). a) You make a solution containing compound A at a concentration of 1 M and compound B at a concentration of 1 mM of B, and let the reaction proceed to equilibrium. What are the equilibrium concentrations of A and B? b) Calculate the standard free-energy change (AG) for this reaction. c) What is the standard free-energy change (AG) for the inverse reaction (BA)?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY
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