Ethyl bromide is synthesized by reacting ethylene with hydrogen bromide.HHC=C+ H-Br:HHH:Br:H-C-C-HH HUse bond energies to find the enthalpy change for this reaction. Round your answer to 3 significant figures.Note: Reference the Bond energies table for additional information.kJ☐ x10Х

Step 1: GivenH2C=CH2 + HBr → H3C-CH2-BrBondEnergy (kJ/mol)C-H413C=C602H-Br366C-C370C-Br293 Step 2:…

Answered: Ethyl bromide is synthesized by…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter9: Chemical Bonds

Section: Chapter Questions

Problem 9.89QE

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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.
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.
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.
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)?
Use Equation 6.1 and values from Table 6.2 to estimate the enthalpy change when methane, CH4, and oxygen combine according to the equation: CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)
hat does temperature measure? Are the molecules in a beaker of warm water moving at the same speed as the molecules in a beaker of cold water? Explain? What is heat? Is heat the same as temperature?
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
Bond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?
Ethyl bromide is synthesized by reacting ethylene with hydrogen bromide. H H:Br: C=C X H + H-Br: Н H-C-C-H H H Use bond energies to find the enthalpy change for this reaction. Round your answer to 3 significant figures. Note: Reference the Bond energies table for additional information. KJ ☐ x10 ☑
2-Butanol can be made by the reaction of 1-butene and water: H2 C=CH-CH,–CH3 (g) + H2O(g) → CH; CH(OH)CH2CH3 (g) a Use bond dissociation enthalpies to estimate the enthalpy change in this reaction. Bond AH (kJ/mol) H-O 463 C=C 610 H-C 413 C-C 346 358 Enthalpy change = kJ b Calculate the enthalpy change for this reaction from enthalpies of formation. Substance AƒH (kJ/mol) CH3 CH(OH)CH2 CH3 (g) -293.1 H2O(g) -241.83 H2C=CH-CH2–CH3 (g) -0.1300 Enthalpy change = kJ
Use the given bond dissociation energies to approximate the enthalpy change for the reaction of methane with molecular chlorine as shown in the reaction below. CH4(g) + 3Cl2₂(g) → CHCl3(g) + 3HCl(g) I BDE: C-H = 410 kJ/mol C-CI 330 kJ/mol a) -227 kJ b) -327 kJ c) -457 kJ d) +227 kJ e) + 327 kJ CI-CI = 243 kJ/mol H-CI = 432 kJ/mol H-H = 436 kJ/mol C-C= 350 kJ/mol
Using the bond energies provided, calculate the enthalpy of the reaction (∆Hrxn, in kJ) for the combustion of methanol shown below. CH3OH(l) +3/2 O2 (g) → CO2 (g) + 2 H2O(g)

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