Use average bond energies to compare the stabilities of allyl alcohol, CH2CHCH2OH, and acetone, (CH3)2CO, both of which have thesame formula, C3H6O.What is the difference in stabilities of the two compounds? Give the absolute value of the difference (positive value).kJeTextbook and MediaSelect all that apply to the stability of allyl alcohol and acetone.O Allyl alcohol is more stable than acetone.Acetone is more stable than allyl alcohol.Allyl alcohol is more stable due to difference in stabilities.O Acetone is more stable due to difference in stabilities.

Answered: Image /qna-images/answer/8ed283fd-f1cc-4270-a239-a462606295cb.jpg

Jse average bond energies to compare the stabilities of allyl alcohol, CH2CHCH2OH, and acetone, (CH3)2CO, both of ame formula, C3H6O. What is the difference in stabilities of the two compounds? Give the absolute value of the difference (positive value) i kJ eTextbook and Media Select all that apply to the stability of allyl alcohol and acetone. O Allyl alcohol is more stable than acetone. O Acetone is more stable than allyl alcohol. O Allyl alcohol is more stable due to difference in stabilities. O Acetone is more stable due to difference in stabilities.

Jse average bond energies to compare the stabilities of allyl alcohol, CH2CHCH2OH, and acetone, (CH3)2CO, both of ame formula, C3H6O. What is the difference in stabilities of the two compounds? Give the absolute value of the difference (positive value) i kJ eTextbook and Media Select all that apply to the stability of allyl alcohol and acetone. O Allyl alcohol is more stable than acetone. O Acetone is more stable than allyl alcohol. O Allyl alcohol is more stable due to difference in stabilities. O Acetone is more stable due to difference in stabilities.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 98QRT

See similar textbooks

Similar questions

9.10 The kinetic energy of molecules is often used to induce chemical reactions. The bond energy in an O1 molecule is 8.221019J . Can an O2 molecule traveling at 780 m/s provide enough energy to break the O = O bond? What is the minimum velocity of an O2 molecule that would give a kinetic energy capable of breaking the bond if it is converted with 100% efficiency?
The molecular structure shown is of one form of glucose, C6H12O6 Glucose can be oxidized to carbon dioxide and water according to the equation C6H12O6(S) + 6 O2(g)6 CO2(g) + 6 H2O(g) (a) Using the method described in Section 6-6a for estimating enthalpy changes from bond energies, estimate rH for the oxidation of this form of glucose. Make a list of all bonds broken and all bonds formed in this process. (b) Compare your result with the experimental value of 2816 kJ/mol for combustion of glucose. Why might there be a difference between this value and the one you calculated in part (a)?
H2 has equilibrium bond length of 0.751 Å and bond dissociation energy of 432 kJ mol21, whereas F2 has equilibrium bond length of 1.417 Å and bond dissociation energyof 155 kJ mol21. On the same graph show qualitativesketches of the effective potential energy curve Veff for anH2 and an F2 molecule. In your solution, show the conversion from kJ mol21to the energy of a single molecule.1
Calculate the bond energy of C-F given that the heat of atominzation of CHFClBr is 1502 kj/mol, and that the bond energies of C--H, C--Br, and C-Cl are 413, 276 and 328 kj/mol, respectively. show the calculations
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation C2H4 (g) + HBr (g) --> C2H5Br(g) Average molar bond enthalpies. (?bond) Bond ??⋅???−1 Bond ??⋅???−1 O−H 464 C≡N 890 O−O 142 N−H 390 C−O 351 N−N 159 O=O 502 N=N 418 C=O 730 N≡N 945 C−C 347 F−F 155 C=C 615 Cl−Cl 243 C≡C 811 Br−Br 192 C−H 414 H−H 435 C−F 439 H−F 565 C−Cl 331 H−Cl 431 C−Br 276 H−Br 368 C−N 293 H−S 364 C=N 615 S−S 225
In trichlorofluoromethane refrigerant (CCl3F, also known as Freon-11, R-11, or CFC-11), there are 3 C-Cl bonds. When these are photochemically broken by solar radiation in the stratosphere, free Cl atoms produced can catalytically destroy ozone, O3. If the C-Cl bond energy is 331 kJ/mol, calculate the energy in J to break one C-Cl bond, the frequency of light that corresponds to this photon energy, and the wavelength in nm of this light. What do we call light in this wavelength region? (visible, UV, IR, etc)
Use average bond enthalpies to calculate the enthalpy change for the following gas-phase reaction. CH3OH(g) + HI(g) --> CH3I(g) + H2O(g) ΔHreaction = ?
Use the data found in Thermodynamic Properties to determine the values for the O-Cl and the O-F bond energies. (heats of formation of OF2 and OCl2 are 24.7 and 80.37 kJ/mol, respectively). Please see https://youtu.be/-OKWJ0LYdNc for assistance. DO-F kJ/mol DO-Cl kJ/mol
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxn for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔ⁢Hrxn° for the equation NH3(g)+2O2(g)⟶HNO3(g)+H2O(g)NH3⁢(g)+2⁢O2⁡(g)⟶HNO3⁢(g)+H2O(g) The bonding in the molecules is shown.
Calculate the H for equation 2C(s) + H2(g) → C2H2(g)
Use the molar bond enthalpy data in the table to estimate the value of Δ?∘rxnΔHrxn° for the equation C2H4 (g) + HBr (g) --> C2H5Br (g) Average molar bond enthalpies. (?bond)(Hbond) Bond ??⋅???−1kJ⋅mol−1 Bond ??⋅???−1kJ⋅mol−1 O−HO−H 464464 C≡NC≡N 890890 O−OO−O 142142 N−HN−H 390390 C−OC−O 351351 N−NN−N 159159 O=OO=O 502502 N=NN=N 418418 C=OC=O 730730 N≡NN≡N 945945 C−CC−C 347347 F−FF−F 155155 C=CC=C 615615 Cl−ClCl−Cl 243243 C≡CC≡C 811811 Br−BrBr−Br 192192 C−HC−H 414414 H−HH−H 435435 C−FC−F 439439 H−FH−F 565565 C−ClC−Cl 331331 H−ClH−Cl 431431 C−BrC−Br 276276 H−BrH−Br 368368 C−NC−N 293293 H−SH−S 364364 C=NC=N 615615 S−SS−S 225225