Use the bond energy to estimate the heat of reaction at 25 °C for the reaction below.CH4 (g) + 2 02 (g) → CO2 (g) + 2 H2O(g)Compare your result with that calculated from enthalpies of formation. Average Bond Energies (kJ/mol)Single BondsMultiple BondsH-H432NH391149C=C614H-F565N-N160208C=C839H-CI427N-F272-Br175O=0495H-Br363N-CI200C=0745HI295N-Br243S H347C=01072N-O201SF327N=0607C-H413O-H467S CI253N=N418C-C3470-0146S Br218N=N941C-N305O-F190266C=N891C-O358O-C203C=N615C-F485234Si Si340C-Cl339Si-H393C-Br276F-F154Si-C360240F-Cl253Si-O452C-S259F-Br237C-CI239ClBr218Br-Br193

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Answered: Use the bond energy to estimate the…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter15: Energy And Chemical Change

Section15.4: Calculating Enthalpy Change

Problem 35PP

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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.
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 = ?
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?
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.
How is average bond strength related to relative potential energies of the reactants and the products?
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 = ?
The reaction of quicklime, CaO, with water produces slaked lime, Ca(OH)2, which is widely used in the construction industry to make mortar and plaster. The reaction of quicklime and water is highly exothermic: CaO(s)+H2O(l)Ca(OH)2(s)H=350kJmol1 (a) What is the enthalpy of reaction per gram of quicklime that reacts?. (b) How much heat, in kilojoules, is associated with the production of 1 ton of slaked lime?
The enthalpy change for the following reaction is 393.5 kJ. C(s,graphite)+O2(g)CO2(g) (a) Is energy released from or absorbed by the system in this reaction? (b) What quantities of reactants and products are assumed? (c) Predict the enthalpy change observed when 3.00 g carbon burns in an excess of oxygen.

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Use the bond energy to estimate the heat of reaction at 25 °C for the reaction below. CH4 (g) + 2 02 (g) → CO2 (g) + 2 H2O(g) Compare your result with that calculated from enthalpies of formation.