Bundle: Chemistry: The Molecular Science, 5th, Loose-Leaf + OWLv2 with Quick Prep 24-Months Printed Access Card
5th Edition
ISBN: 9781305367487
Author: John W. Moore, Conrad L. Stanitski
Publisher: Cengage Learning
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Textbook Question
Chapter 6, Problem 33QRT
Which bond requires more energy to break: the carbon-oxygen bond in formaldehyde, H2CO, or the carbon-oxygen bond in carbon monoxide, CO?
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Students have asked these similar questions
Acetylene gas (ethyne; HC≡CH) burns with oxygen in an oxyacetylene torch to produce carbon dioxide, water vapor, and the heat needed to weld metals. The heat of combustion for acetylene is −1259 kJ/mol. Calculate the C≡C bond energy.
The average bond energies (kJ/mol)
C―H
413
C―C
347
C═C
620
H―H
436
O―O
142
O═O
498
H―O
467
C―O
351
C═O
799
How many grams of CO2 are produced when C3H8 is combusted in oxygen and 507.0 kJ of heat are released? Estimate ΔHrxn using bond enthalpies from the table above in order to solve this problem.
Bond
Bond Energy (kJ/mol)
Bond
Bond Energy (kJ/mol)
C-C
347
C=O (in CO2)
799
C=C
614
C=O
745
C≡C
839
C≡O
1070
C-H
413
O=O
498
O-H
467
N-H
391
H-H
432
N≡N
945
C-O
358
N-Cl
200
C-N
305
N-O
201
C-Cl
339
C≡N
891
If the following reaction is given:
C2H5F + Cl2
|| AHran
If the bond energy for C-H is 414 kJ/ mole, the bond energy for C-C is 347 kJ/mole, the
bond energy for C-Cl is 377 kJ/ mole, the bond energy for Cl-Cl is 243 kJ/ mole, the
bond energy for C-F is 450 kJ/ mole and the done energy for H-Cl is 431 kJ/ mole,
determine the bond energy for the H-F bond in kJ/mole.
C2H4Cl2 + HF
151kJ
mole
Give your answer as a positive value as all energies for bond values should be written in
terms of a positive value (the energy needed to break the bond = endothermic)
Chapter 6 Solutions
Bundle: Chemistry: The Molecular Science, 5th, Loose-Leaf + OWLv2 with Quick Prep 24-Months Printed Access Card
Ch. 6.2 - Write Lewis structures for (a) NF3, (b) N2H4, and...Ch. 6.3 - Prob. 6.1ECh. 6.3 - Prob. 6.2PSPCh. 6.4 - Prob. 6.2CECh. 6.4 - Write Lewis structures for (a) nitrosyl ion, NO+;...Ch. 6.5 - Prob. 6.4CECh. 6.5 - Prob. 6.5CECh. 6.5 - Prob. 6.4PSPCh. 6.6 - Prob. 6.5PSPCh. 6.6 - Use Equation 6.1 and values from Table 6.2 to...
Ch. 6.6 - Prob. 6.6CECh. 6.7 - Prob. 6.7PSPCh. 6.7 - Prob. 6.7CECh. 6.8 - Prob. 6.8PSPCh. 6.9 - Prob. 6.9PSPCh. 6.9 - Prob. 6.9CECh. 6.10 - Prob. 6.10PSPCh. 6.11 - Prob. 6.10ECh. 6.11 - Prob. 6.11ECh. 6.11 - Prob. 1CECh. 6.11 - Prob. 2CECh. 6.12 - Repeat Problem-Solving Example 6.11, but use N2...Ch. 6.12 - Use MO theory to predict the bond order and the...Ch. 6 - Prob. 1QRTCh. 6 - Prob. 2QRTCh. 6 - Prob. 3QRTCh. 6 - Prob. 4QRTCh. 6 - Prob. 5QRTCh. 6 - Prob. 6QRTCh. 6 - Which of these molecules have an odd number of...Ch. 6 - Prob. 8QRTCh. 6 - Prob. 9QRTCh. 6 - Prob. 10QRTCh. 6 - Prob. 11QRTCh. 6 - Prob. 12QRTCh. 6 - Explain in your own words why the energy of two H...Ch. 6 - Prob. 14QRTCh. 6 - Prob. 15QRTCh. 6 - Prob. 16QRTCh. 6 - Prob. 17QRTCh. 6 - Prob. 18QRTCh. 6 - Prob. 19QRTCh. 6 -
Write Lewis structures for
tetracyanoethene,...Ch. 6 - Prob. 21QRTCh. 6 - Prob. 22QRTCh. 6 - Prob. 23QRTCh. 6 - Prob. 24QRTCh. 6 - Prob. 25QRTCh. 6 - Prob. 26QRTCh. 6 - Prob. 27QRTCh. 6 - Prob. 28QRTCh. 6 - Prob. 29QRTCh. 6 - For each pair of bonds, predict which is the...Ch. 6 - Prob. 31QRTCh. 6 - Prob. 32QRTCh. 6 - Which bond requires more energy to break: the...Ch. 6 -
Estimate ΔrH° for forming 2 mol ammonia from...Ch. 6 - Prob. 35QRTCh. 6 - Light of appropriate wavelength can break chemical...Ch. 6 - Prob. 37QRTCh. 6 - Prob. 38QRTCh. 6 - Prob. 39QRTCh. 6 - Acrolein is the starting material for certain...Ch. 6 - Prob. 41QRTCh. 6 - Prob. 42QRTCh. 6 - Write the correct Lewis structure and assign a...Ch. 6 - Prob. 44QRTCh. 6 - Prob. 45QRTCh. 6 - Two Lewis structures can be written for nitrosyl...Ch. 6 - Prob. 47QRTCh. 6 - Prob. 48QRTCh. 6 - Prob. 49QRTCh. 6 - Prob. 50QRTCh. 6 - Several Lewis structures can be written for...Ch. 6 - Prob. 52QRTCh. 6 - Prob. 53QRTCh. 6 - Prob. 54QRTCh. 6 - Prob. 55QRTCh. 6 - Draw resonance structures for each of these ions:...Ch. 6 - Three known isomers exist of N2CO, with the atoms...Ch. 6 - Write the Lewis structure for (a) BrF5 (b) IF5 (c)...Ch. 6 - Write the Lewis structure for
BrF3
XeF4
Ch. 6 - Prob. 60QRTCh. 6 - Prob. 61QRTCh. 6 - Prob. 62QRTCh. 6 - All carbon-to-carbon bond lengths are identical in...Ch. 6 - Prob. 64QRTCh. 6 - Prob. 65QRTCh. 6 - Prob. 66QRTCh. 6 - Prob. 67QRTCh. 6 - Prob. 68QRTCh. 6 - Prob. 69QRTCh. 6 - Prob. 70QRTCh. 6 - Using just a periodic table (not a table of...Ch. 6 - The CBr bond length in CBr4 is 191 pm; the BrBr...Ch. 6 - Prob. 73QRTCh. 6 -
Acrylonitrile is the building block of the...Ch. 6 - Prob. 75QRTCh. 6 - Write Lewis structures for (a) SCl2 (b) Cl3+ (c)...Ch. 6 - Prob. 77QRTCh. 6 - Prob. 78QRTCh. 6 - A student drew this incorrect Lewis structure for...Ch. 6 - This Lewis structure for SF5+ is drawn...Ch. 6 - Tribromide, Br3, and triiodide, I3, ions are often...Ch. 6 - Explain why nonmetal atoms in Period 3 and beyond...Ch. 6 - Prob. 83QRTCh. 6 - Prob. 84QRTCh. 6 - Prob. 85QRTCh. 6 - Prob. 86QRTCh. 6 - Which of these molecules is least likely to exist:...Ch. 6 - Write the Lewis structure for nitrosyl fluoride,...Ch. 6 - Prob. 91QRTCh. 6 - Methylcyanoacrylate is the active ingredient in...Ch. 6 - Aspirin is made from salicylic acid, which has...Ch. 6 - Prob. 94QRTCh. 6 - Prob. 95QRTCh. 6 - Prob. 96QRTCh. 6 - Prob. 97QRTCh. 6 - Prob. 98QRTCh. 6 - Nitrosyl azide, N4O, is a pale yellow solid first...Ch. 6 - Write the Lewis structures for (a) (Cl2PN)3 (b)...Ch. 6 - Nitrous oxide, N2O, is a linear molecule that has...Ch. 6 - The azide ion, N3, has three resonance hybrid...Ch. 6 - Hydrazoic acid, HN3, has three resonance hybrid...Ch. 6 - Prob. 104QRTCh. 6 - Experimental evidence indicates the existence of...Ch. 6 - Prob. 106QRTCh. 6 - Prob. 107QRTCh. 6 - Pipeline, the active ingredient in black pepper,...Ch. 6 - Sulfur and oxygen form a series of 2 anions...Ch. 6 - Prob. 110QRTCh. 6 - Prob. 111QRTCh. 6 - Prob. 112QRTCh. 6 - Prob. 113QRTCh. 6 - Prob. 114QRTCh. 6 - Prob. 115QRTCh. 6 - Prob. 116QRTCh. 6 - Prob. 117QRTCh. 6 - Prob. 118QRTCh. 6 - Prob. 6.ACPCh. 6 - Prob. 6.BCPCh. 6 - Prob. 6.CCP
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- Write all resonance structures of chlorobenzene, C6H5Cl, a molecule with the same cyclic structure as benzene. In all structures, keep the CCl bond as a single bond. Which resonance structures are the most important?arrow_forwardIs this system endothermic or exothermic, and why? * H2 + CO2 CH202 Reactant bond energies: H-H is 432 kJ/mol, C=O is 799 kJ/mol Product bond energies: C-H is 413 kJ/mol, C=0 is 745 kJ/mol, C-O is 358 kJ/mol, O-H is 467 kJ/mol It is exothermic because more energy is given off by the products versus the amount needed to break up the reactants. It is exothermic because more energy is needed to break up the reactants versus the amount given off by the products. It is endothermic because more energy is needed to break up the reactants versus the amount given off by the products. It is endothermic because more energy is given off by the products versus the amount needed to break up the reactants.arrow_forward13) The average C−C bond dissociation energy (D) is 350 kJ/mol and the average C=C bond dissociation energy is 728 kJ/mol. Based on these values, which is stronger: a σ or a π bond?arrow_forward
- The conversion of graphite into diamond is an endothermic reaction (AH = +3 kJ mol-1). C(graphite) → C(diamond) 1 The enthalpy change of atomisation of diamond is smaller than that of graphite. The bond energy of the C-C bonds in graphite is greater than that in diamond. 2 The enthalpy change of combustion of diamond is greater than that of graphite. 3 Which statements are correct? A 1, 2 and 3 B 1 and 2 only C 2 and 3 only D 1 onlyarrow_forwardOctane (C8H18) is combusted with oxygen to give carbon dioxide and water vapor. Calculate the enthalpy of reaction using the bond energies given. Is the combustion of octane an endothermic or exothermic reaction? The reaction below is not balanced. pleaseanswer neatly so i can see how to do it Bond: C=O O=O C–H O–H C–C Bond energy (kJ/mol): 799 498 414 464 347arrow_forwardBased on the bond energies for the reaction below, what is the enthalpy of the reaction? HC≡CH (g) + 5/2 O₂ (g) → 2 CO₂ (g) + H₂O (g)arrow_forward
- Calculate the enthalpy change for the reaction shown below between ammonia and phosgene to produce urea and HCI. Use the bond-dissociation energies listed in the table. Bond H-CI H-N C-CI C-N CI + 2 NH3 AHBDE (kJ/mol) 432 339 397 748 AHrxn = +444 kJ/mol AHrxn= -888 kJ/mol AHrxn= -444 kJ/mol AHrxn= +888 kJ/mol .C. HẠN-“NH, * 2 H-CIarrow_forwardWhen gaseous sulfur trioxide is dissolved in concentratedsulfuric acid, disulfuric acid forms:SO₃(g)+ H₂SO₄(l) →H₂S₂O₇(l) Use bond energies Table to determine ΔH°ᵣₓₙ. (The S atoms in H₂S₂O₇ are bonded through an O atom. Assume Lewis structures with zero formal charges; BE of SNO is 552 kJ/mol.)arrow_forwardThe enthalpy change for the following reaction is -121 kJ. Using bond energies, estimate the C-H bond energy in CH4(9). CH4(9) + Cl₂(g) →→→CH3CI(g) + HCl(g) kJ/molarrow_forward
- Use bond energies to determine ΔHrxn for the reaction between ethanol and hydrogen chloride. CH3CH2OH(g)+HCl(g)→CH3CH2Cl(g)+H2O(g) Average Bond Energies Bond Bond Energy (kJ/mol) H−C 414 H−O 464 H−F 565 H−Cl 431 H−Br 364 C−Cl 339 C−O 360 Cl−F 253 Cl−Cl 243 Br−Cl 218arrow_forwardEstimate the enthalpy change for the reaction: 2CO + O2 ⟶2CO2 given the following bond energies. BE(C O) = 1074 kJ/mol BE(O=O) = 499 kJ/mol BE(C=O) = 802 kJ/mol Hint: You need to draw the Lewis Structures of the compounds to know the bonds present. Group of answer choices +2380 kJ/mol -561 kJ/mol +744 kJ/mol +1949 kJ/mol -744 kJ/molarrow_forwardHydrazine, N2H4, burns in oxygen as follows: N2H4 + O2 → N2 + 2H2O [The bond energies in kJ/mol are: N-H = 388; N-N 163; N≡N 944; O-H 463; O=O 496] Draw the chemical structures of the reactants and products and give the formula to calculate enthalpy change in a reaction, ΔH.arrow_forward
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