51-04ec-4333-b719-ddf77f305a4cJoin: 368359Answered-Correct!U6HW Question 20Homework Answered Due Today, 11:59 PMBondC-HkJ/mo! 413Consider the combustion of ethanol (C₂H5OH) to form carbon dioxide and water. The unbalanced chemical reaction is shownusing Lewis structures in the image below. Balance this reaction and then use the AHRXN and the table of bond energies todetermine the energy of the C-O bond in CO₂. Enter your answer as a number without any units.ннH-C-C-0-H + 10 =01 ) 0=c=0 +11HHType your numeric answer and submit392✓20/20 answeredAHRNX = -1372kJ/molC-C346C-O358♥ LELCHLOC=OO-H46362°FAResubmitImportant0=0498€ Consider the combustion of etha X-04ec-4333-b719-ddf77f305a4cJoin: 368359 -Answered-Correct!U6HW Question 20Homework Answered Due Today, 11:59 PMHHH-C-C-0-H + 10 =01BondkJ/molConsider the combustion of ethanol (C₂H5OH) to form carbon dioxide and water. The unbalanced chemical reaction is shownusing Lewis structures in the image below. Balance this reaction and then use the AHRXN and the table of bond energies todetermine the energy of the C-O bond in CO₂. Enter your answer as a number without any units.C-H413Type your numeric answer and submit4392H2 has nonpolar covalent bonds xC-C34620/20 answered20101AHRNX = -1372kJ/molC-O358+0=c=0 +C=OO-H463Resubm62°FImportant0=0498

Answered: Image /qna-images/answer/a6faf131-0536-4d78-b5d8-908e3bd2d6b9.jpg

U6HW Question 20 Homework Answered Due Today, 11:59 PM Consider the combustion of ethanol (C₂H5OH) to form carbon dioxide and water. The unbalanced chemical reaction is shown using Lewis structures in the image below. Balance this reaction and then use the AHRXN and the table of bond energies to determine the energy of the C-O bond in CO₂. Enter your answer as a number without any units. HH H-C-C-0-H +10=01 11 HH Bond kJ/mol -392 C-H 413 Type your numeric answer and submit C-C 7 AHRNX = -1372kJ/mol 346 C-O =c=O + 358 C=O Important O-H 463 H-8TH 0=0 498

U6HW Question 20 Homework Answered Due Today, 11:59 PM Consider the combustion of ethanol (C₂H5OH) to form carbon dioxide and water. The unbalanced chemical reaction is shown using Lewis structures in the image below. Balance this reaction and then use the AHRXN and the table of bond energies to determine the energy of the C-O bond in CO₂. Enter your answer as a number without any units. HH H-C-C-0-H +10=01 11 HH Bond kJ/mol -392 C-H 413 Type your numeric answer and submit C-C 7 AHRNX = -1372kJ/mol 346 C-O =c=O + 358 C=O Important O-H 463 H-8TH 0=0 498

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter9: Energy And Chemistry

Section: Chapter Questions

Problem 9.99PAE: 9.99 The chemical reaction BBr3(g)+BCl3(g)BBr2Cl(g)+BCl2Br(g) , has an enthalpy change very close to...

See similar textbooks

Similar questions

Enthalpy changes for the following reactions can be determined experimentally: N2(g) + 3 H2(g) 2 NH3(g) rH = 91.8 kJ/mol-rxn 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) rH = 906.2 kJ/mol-rxn H2(g) + O2(g) H2O(g) rH = 241.8 kl/mol-rxn Use these values to determine the enthalpy change for the formation of NO(g) from the elements (an enthalpy change that cannot be measured directly because the reaction is reactant-favored). N2(g) + O2(g) NO(g) rH = ?
9.99 The chemical reaction BBr3(g)+BCl3(g)BBr2Cl(g)+BCl2Br(g) , has an enthalpy change very close to zero. Using Lewis structures of the molecules, all of which have a central boron atom, provide a molecular-level description of why H for this reaction might be very small.
A commercial process for preparing ethanol (ethyl alcohol), C2H5OH, consists of passing ethylene gas. C2H4, and steam over an acid catalyst (to speed up the reaction). The gas-phase reaction is Use bond enthalpies (Table 9.5) to estimate the enthalpy change for this reaction when 37.0 g of ethyl alcohol is produced.
The bond energy for a CH bond is about 413 kJ/mol in CH4 but 380 kJ/mol in CHBr3. Although these values are relatively close in magnitude, they are different. Explain why they are different. Does the fact that the bond energy is lower in CHBr3, make any sense? Why?
Use a Born-Haber cycle (Sec. 5-13) to calculate the lattice energy of MgF2 using these thermodynamic data. Compare this lattice energy with that of SrF2, −2496 kJ/mol. Explain the difference in the values in structural terms.
The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?
Given the following data: NO2(g) NO(g) + O(g)H = 233 kJ 2O3(g) 3O2(g)H = 427 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate the bond energy for the O2 bond, that is, calculate H for: O2(g) 2O(g)H = ?
Estimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.
In Exercise 89 in Chapter 3, the Lewis structures for benzene (C6H6) were drawn. Using one of the Lewis Structures, estimate Hf for C6H6(g) using bond energies and given that the standard enthalpy of formation of C(g) is 717 kJ/mol. The experimental Hf value for C6H6 (g) is 83 kJ/mol. Explain the discrepancy between the experimental value and the calculated Hf value for C6H6(g).
Acetic acid. CH3CO2H, is made industrially by the reaction of methanol and carbon monoxide. CH3OH () + CO(g) CH3CO2H() rH= 134.6 kJ/mol-rxn What is the enthalpy change for producing 1.00 L of acetic acid (d = 1.044 g/mL) by this reaction?