Use the molar bond enthalpy data in the table to estimate theAverage molar bond enthalpies (Hpond)value of AHixn for the equationBondkJ-mol-BondkJ-mol-CCI,(g) + 2F,(g) –→ CF,(g) + 2Cl,(g)О-Н464C=N8900-0142N-H390The bonding in the molecules is shown.С-О351N-N159CIO=0502N=N418CI-CIF-F+C=0730N=N945Cl-F-FCI-CIС-С347F-F155C=C615Cl-CI243C=C811Br-Br192С-Н414Н-Н435С-F439Н-F565C-CI331Н-СІ431С-Br276Н-Br368С-N293Н-S364C=N615S-S225ΔΗΚkJ-mol-1

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Answered: Use the molar bond enthalpy data in the…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter12: Thermodynamic Processes And Thermochemistry

Section: Chapter Questions

Problem 52P

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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.
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 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?
In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of 25.00C. After dissolution of the salt, the final temperature of the calorimeter contents is 23.34C. Assuming the solution has a heat capacity of 4.18 J/C g and assuming no heat loss to the calorimeter, calculate the enthalpy change for the dissolution of NH4NO3 in units of kJ/mol.
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 = ?
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
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?
Find the enthalpies of the combustion reactions for methane through n-octane. Plot them versus the number of carbon atoms in the molecule, and determine an equation that gives H for the combustion of a given hydrocarbon. Then use the equation to predict the enthalpy of combustion for n-C12H26 and compare it to experimental values.
Fructose, C6H1206(S), consists of 5 C-C single bonds, 7 C-O bonds, 7 C-H bonds, and 5 O-H bonds with average bond energies of 348 kJ/mol, 360 kJ/mol, 412 kJ/mol, and 463 kJ/mol respectively. The bond energy for C=O is 799 kJ/mol and O=O is 498 kJ/mol. The molar mass of fructose is 180.12 g/mol. Estimate the change in enthalpy if 2.56 g of fructose undergoes complete combustion at standard temperature and pressure.
Nitroglycerin is a very unstable explosive that was used extensively in the 19th century. The nitroglycerin molecule is shown on the right and the equation for the explosion reaction is the following. 4 C3H5N3O9(l) -> 12 CO2(g) + 10 H2O(g) + 6 N2(g) + O2(g) a) Determine the enthalpy change of this reaction, by taking into account the following bond energies. O−H: 464 kJ/mol O=O: 502 kJ/mol C−C: 347 kJ/mol C−H: 414 kJ/mol C−O: 351 kJ/mol C=O (in CO2): 799 kJ/mol N−N: 159 kJ/mol N≡N: 945 kJ/mol N−O: 201 kJ/mol N=O: 607 kJ/mol
Use the bond energies listed in the table below to estimate the standard enthalpy of the reaction: CCl3CHCl2(g) + 2HF(g) → CCl3CHF2(g) + 2HCl(g) C – H 412 kJ mol-1 C – C 348 kJ mol-1 C – Cl 338 kJ mol-1 H – Cl 431 kJ mol-1 C – F 484 kJ mol-1 H – F 565 kJ mol-1
Use bond energies from the table to estimate ΔrH for the following reaction. C2H2(g)+H2(g)→C2H4(g) ΔrH=? Express the answer in kJ/mol to three significant figures.

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