Use bond energies to calculate the heat of reaction: :ɑ—C:+ H—H Round your answer to 3 significant figures. 2 H-Cl: Note: Reference the Bond energies table for additional information. kJ ☐ x10 ☑

Use bond energies to calculate the heat of reaction: :ɑ—C:+ H—H Round your answer to 3 significant figures. 2 H-Cl: Note: Reference the Bond energies table for additional information. kJ ☐ x10 ☑

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter8: Bonding: General Concepts

Section: Chapter Questions

Problem 79E: Compare your answers from parts a and b of Exercise 69 with H values calculated for each reaction...

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Question

Use bond energies to calculate the heat of reaction:
:ɑ—C:+ H—H
Round your answer to 3 significant figures.
2 H-Cl:
Note: Reference the Bond energies table for additional information.
kJ
☐ x10
☑

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Calculate the enthalpy of reaction for HCN(g)H(g)+C(g)+N(g) from enthalpies of formation (see Appendix C). Given that the CH bond enthalpy is 411 kJ/mol, obtain a value for the CN bond enthalpy. Compare your result with the value given in Table 9.5.
Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.
In general the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have +1 charged ions even though +4, + 5, and +6 charged ions would have a more favorable lattice energy?
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.
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When a reaction is exothermic, is the sum of bond energies of products or of reactants greater?
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.
Dinitrogen monoxide, N2O, can decompose to nitrogen and oxygen gas: 2 N2O(g) 2 N2(g) + O2(g) Use bond dissociation enthalpies to estimate the enthalpy change for this reaction.
Calculate the standard heat of formation of the compound ICl(g) at 25C. (Hint: Use Table 8.5 and Appendix 4 data.)
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
Hydrogenation reactions, which involve the addition of H2 to a molecule, are widely used in industry to transform one compound into another. For example, 1-butene (C4H8) is converted to butane (C4H10) by addition of H2. Use the bond dissociation enthalpies in Table 8.8 to estimate the enthalpy change for this hydrogenation reaction.
The equation for the combustion of gaseous methanol is 2 CH3OH(g) + 3 O2(g) 2 CO2(g) + 4 H2O(g) (a) Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy change for this reaction. What is the enthalpy of combustion of one mole of gaseous methanol? (b) Compare your answer in part (a) with the value of tHcalculated using enthalpies of formation data.

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