Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for bond (b).(b)AH° = 356 kJ/molAH° = 385 kJ/mol

The energy required to break one mole of bond is termed as the bond dissociation energy. it depends…

Answered: Explain why the bond dissociation…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter19: The Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 68QRT

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Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for bond (b).
A major short-lived, neutral species in flames is OH.(a) What is unusual about the electronic structure of OH?(b) Use the standard heat of formation of OH(g) (39.0 kJ/mol)and bond energies to calculate the O-H bond energy in OH(g).(c) From the average value for the O-H bond energy in Table and your value for the O-H bond energy in OH(g) find the energy needed to break the first O-H bond in water.
a) The following reaction occurs in an open beaker: C2H5OH (g) ---> C2H4(g) + H2O (g) {Bond Energy (kJ/mol): C-H = 415 ; C-C = 345 ; C-O = 350 ; O-H = 464 ; C=C = 611}i) Calculate the ΔH0rxn for this reaction from the given bond energies. kJ ii) Is this reaction an open, closed or isolated system? iii) Would you feel hot or cold if you were near this reaction when it occurred? This is because (choose from I - V) I. the reaction is exothermic and absorbs energy from the surroundings. II. the reaction is exothemic and releases energy to the surroundings. III. the reaction is endothermic and absorbs thermal energy from the surroundings. IV. the reaction is endothermic and loses heat to the surroundings. V. the reaction produces steam which contains a lot of heat.
Which is the strongest bond energy? Cl(g) ΔH°f, = +121.3 kJ mol–1 CCl4(g) ΔH°f, = –95.98 kJ mol–1 HCl(g) ΔH°f, = –92.3 kJ mol–1 Question 8 options: Cl–Cl in Cl2 H–Cl in HCl C–Cl in CCl4
The species is the simplest polyatomic ion. The geometry of the ion is that of an equilateral triangle. (a) Draw three resonance structures to represent the ion. (b) Given the following information 2 H+ + H+ ---> ∆H° = - 849 kJ/mol and H2 ---> 2H ∆H° = -436.4 kJ/mol calculate ∆H° for the reaction H+ + H2 --->
(a) Compare the bond enthalpies (Table 8.3) of the carbon–carbon single, double, and triple bonds to deduce an averageπ -bond contribution to the enthalpy. What fraction ofa single bond does this quantity represent? (b) Make a similarcomparison of nitrogen–nitrogen bonds. What do youobserve? (c) Write Lewis structures of N2H4, N2H2, and N2,and determine the hybridization around nitrogen in eachcase. (d) Propose a reason for the large difference in yourobservations of parts (a) and (b).
. The bond lengths of carbon-carbon, carbon-nitrogen, carbon-oxygen, and nitrogen-nitrogen single, double, and triple bonds are listed in Table 8.4. Plot bond enthalpy versus bond length listed in Table 8.5 for these bonds. (a) Is this statement true: "The longer the bond, the stronger the bond"? (b) Based on your chart, order the relative strengths of C-C, C-N, C-O, and N-N bonds from weakest to strongest.
42. Given that (1) A,H°of NO is 82 kJ mol-1 (ii) Bond energies of N N, N=N, O=O and N O are 946, 418, 498 and 607 kJ mol- respectively. The resonance energy of NO is (a)-88kJ (b)-66kJ (c)-62 kJ (d)-44kJ JEE Main Online 2013]
22.) Estimate the enthalpy of reaction of the given reaction using the following data: C3H6 (g) + Hz (g) → C3H8 (g) Bond С-Н H-H С-С C=C Bond Energy (kJ/mol) 614 413 432 347 a.) -220 kJ/mol b.) -286 kJ/mol c.) -127 kJ/mol d.) 286 kJ/mol 23.) Calculate the standard enthalpy of combustion of aniline from the following standard enthalpies of formations. C6H5NH2 (1) + 31/4 02 (g) –→ 6 CO2 (g) + ½ N2 (g) + 7/2 H2O (1) H20 (1) CO2 (g) -393.51 C6H5NH2 (1) -285.83 A:H° (kJ/mol) +31.1 c.) -3123 kJ/mol d.) -4107 kJ/mol a.) -3393 kJ/mol b.) -3330 kJ/mol
iii) What is Bond Energy Term? iv) Given the following bond energy terms; C=C: +835KJmol-1, C-C : +346KJmol-1, C-H: +413KJmol-1, H-H: +436KJmol-1. Determine the enthalpy change for the reaction: 2H2 (g) + C2H2 (g) → CH3CH3 (g)
5. For the reaction H2(g) + C2H4(g) C2H6(g) (a) Estimate the enthalpy of reaction, using the bond enthalpy values. (b) Calculate the enthalpy of reaction, using standard enthalpies of formation. (AH? for H2, C2H4, and C2H6 are 0 kJ/mol, 52.3 kJ/mol, and -84.7 kJ/mol, respectively.)
(b) Explain why the following reaction is endothermic based on your knowledge of both bond enthalpy and endothermic reaction profile. Draw the endothermic reaction profile to help. 2NaHCO3 Na,CO3 positive à H,0 CO2 DH = + +

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Explain why the bond dissociation energy for bond (a) is lower than the bond dissociation energy for bond (b). (b) AH° = 356 kJ/mol AH° = 385 kJ/mol