Organic Chemistry (9th Edition)
9th Edition
ISBN: 9780321971371
Author: Leroy G. Wade, Jan W. Simek
Publisher: PEARSON
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Question
Chapter 4, Problem 4.41SP
(a)
Interpretation Introduction
To determine: The value of
Interpretation: The value of
Concept introduction: The value of
(b)
Interpretation Introduction
To determine: The value of
Interpretation: The value of
Concept introduction: The value of
(c)
Interpretation Introduction
To determine: The value of
Interpretation: The value of
Concept introduction: The value of
(d)
Interpretation Introduction
To determine: The value of
Interpretation: The value of
Concept introduction: The value of
(e)
Interpretation Introduction
To determine: The value of
Interpretation: The value of
Concept introduction: The value of
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Students have asked these similar questions
Calculate ΔH° for the reaction using the given bond dissociation energies.
CH4(g)+2O2(g)⟶CO2(g)+2H2O(g)
Bond
ΔH° (kJ/mol)
O–OO–O
142
H–OH–O
459
C−HC−H
411
C=OC=O
799
O=OO=O
498
C–OC–O
358
What type of reaction is this?
Using bond energies from the table, estimate ΔH for the reaction below. The OH group on the product side is attached to a carbon.CH2=CH2(g) + H2O(g) ↔ CH3CH2OH(g)
Bond Energies, kJ/mol
Single Bonds
H
C
N
O
S
F
Cl
Br
I
H
432
C
411
346
N
386
305
167
O
459
358
201
142
S
363
272
---
---
286
F
565
485
283
190
284
155
Cl
428
327
313
218
255
249
240
Br
362
285
243
201
217
249
216
190
I
295
213
---
201
---
278
208
175
149
Multiple Bonds
C=C
602
C=N
615
C=O
799
CºC
835
CºN
887
CºO
1072
N=N
418
N=O
607
S=O (in SO2)
532
NºN
942
O2
494
S=O (in SO3)
469
We want to find the enthalpy change (ΔHΔH) for the reaction:
2CH4->C2H6+H2
Given the following reactions:
H2+1/2O2→H2O (Given ΔH=−285.8 kJ
CH4→2O2->CO2+2H2O (Given ΔH=−890.3 kJ
C2H6+7/2O2→2CO2+3H2O (Given ΔH=−1559.9 kJ
Chapter 4 Solutions
Organic Chemistry (9th Edition)
Ch. 4.3A - Draw Lewis structures for the following free...Ch. 4.3B - a. Write the propagation steps leading to the...Ch. 4.3C - Prob. 4.3PCh. 4.3C - Prob. 4.4PCh. 4.4 - The following reaction has a value of G =...Ch. 4.4 - Under base-catalyzed conditions two molecules of...Ch. 4.5B - When ethene is mixed with hydrogen in the presence...Ch. 4.5B - For each reaction, estimate whether S for the...Ch. 4.7 - a. Propose a mechanism for the free radical...Ch. 4.7 - a. Using bond-dissociation enthalpies from...
Ch. 4.8 - The reaction of tert-butyl chloride with methanol...Ch. 4.8 - Under certain conditions, the bromination of...Ch. 4.8 - When a small piece of plat num is added to a...Ch. 4.10 - Prob. 4.14PCh. 4.10 - Prob. 4.15PCh. 4.12 - The bromination of methane proceeds through the...Ch. 4.12 - a. Using me BDEs in Table4-2 (page 167 ), compute...Ch. 4.13A - What would be the product ratio in the...Ch. 4.13A - Classify each hydrogen atom in the following...Ch. 4.13B - Use the bond-dissociation enthalpies in Tabte4-2...Ch. 4.13B - Prob. 4.21PCh. 4.13B - Prob. 4.22PCh. 4.14 - a. Compute the heats of reaction for abstraction...Ch. 4.14 - 2,3-Dimethylbutane reacts with bromine in the...Ch. 4.14 - Prob. 4.25PCh. 4.15 - Prob. 4.26PCh. 4.15 - Prob. 4.27PCh. 4.16A - Prob. 4.28PCh. 4.16A - Prob. 4.29PCh. 4.16B - Prob. 4.30PCh. 4.16C - Prob. 4.31PCh. 4.16C - Acetonitrile (CH3C N) is deprotonated by very...Ch. 4.16D - Prob. 4.33PCh. 4 - The following reaction is a common synthesis used...Ch. 4 - Consider the following reaction-energy diagram. a....Ch. 4 - Draw a reaction-energy diagram for a one-step...Ch. 4 - Draw a reaction-energy diagram for a two-step...Ch. 4 - Prob. 4.38SPCh. 4 - Treatment of tert-butyl alcohol with concentrated...Ch. 4 - Label each hydrogen atom in the following...Ch. 4 - Prob. 4.41SPCh. 4 - Prob. 4.42SPCh. 4 - Prob. 4.43SPCh. 4 - Prob. 4.44SPCh. 4 - Prob. 4.45SPCh. 4 - Prob. 4.46SPCh. 4 - For each compound, predict the major product of...Ch. 4 - When exactly 1 mole of methane is mixed with...Ch. 4 - Prob. 4.49SPCh. 4 - Prob. 4.50SPCh. 4 - Prob. 4.51SPCh. 4 - When dichloromethane is treated with strong NaOH,...Ch. 4 - Prob. 4.53SPCh. 4 - When a small amount of iodine is added to a...Ch. 4 - Prob. 4.55SPCh. 4 - When healthy, Earths stratosphere contains a low...Ch. 4 - Prob. 4.57SPCh. 4 - lodination of alkanes using iodine (I2) is usually...
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Similar questions
- C2H6 (1) O2 (g) -> CO2 (g) H:O (1) O2 (g) CO2 (g) H:O (1) CH4 (1) -> CHs (1) O2 (g) -> CO2 (g) H2O (1) NO:(g) O2 (g) N2O5 (g) heatarrow_forwardGiven the following data: 4C(s) + 3H2(g) + 1/2O2(g) → HCOC(CH2)(CH3)(l) ΔH°=-139.0 kJ CH3CH2OH(l) + 1/2O2(g) → CH3CHO(l) + H2O(l) ΔH°=-204.0 kJ 2C(s) + 3H2(g) + 1/2O2(g) → CH3CH2OH(l) ΔH°=-278.0 kJ H2(g) + 1/2O2(g) → H2O(l) ΔH°=-286.0 kJ Calculate ΔH° for the reaction:2CH3CHO(l) → HCOC(CH2)(CH3)(l) + H2O(l)arrow_forwardUsing the table of average bond energies below, the AH for the reaction is kJ. ethanol → ethene + water нн нн Н—С—с—0—н → Ć=Ċ + H-0-H Bond сСС-СО-НС-Н СО AH (kJ/mol) 611 348 464 413 360 -6168 6168 -306 63 46 217arrow_forward
- Given that ∆H° for the reaction is -42 kcal/mol and the bond dissociation enthalpies for the C - H, C - Cl, and O - H bonds are 101, 85, and 105 kcal/mol respectively, calculate the bond dissociation enthalpy of the O - Cl bond.arrow_forwardUse bond-dissociation enthalpies to calculate the AH° for each of the following reactions. CH3CH2CH3+H2 → CH3CH3+CH4 CH3CH2CL+HI → CH3CH2I+HCIarrow_forwardA) Given the standard enthalpy changes for the following two reactions:(1) 2C(s) + H2(g)C2H2(g)...... ΔH° = 226.7 kJ(2) 2C(s) + 2H2(g)C2H4(g)......ΔH° = 52.3 kJwhat is the standard enthalpy change for the reaction:(3) C2H2(g) + H2(g)C2H4(g)......ΔH° = ?------- kJ B) Given the standard enthalpy changes for the following two reactions:(1) 2Pb(s) + O2(g)2PbO(s)...... ΔH° = -434.6 kJ(2) Pb(s) + Cl2(g)PbCl2(s)......ΔH° = -359.4 kJwhat is the standard enthalpy change for the reaction:(3) 2PbCl2(s) + O2(g)2PbO(s) + 2Cl2(g)......ΔH° = ?------ kJarrow_forward
- Now consider the following reaction: C2H5OH + 3O2→2CO2+ 3H2O ,ΔH=−1370 kJ/mol What is the enthalpy for the reaction reversed? reaction 1 reversed: 2CO2 + 3H2O→C2H5OH + 3O2arrow_forwardUse the given bond energy values to estimate ΔH for the following gas-phase reaction. (Simple energy units required for the answer.) D-values in kJ/mol DH-H = 432 DH-Br = 363 DH-C = 413 DH-N = 391 DH-O = 467 DC-C = 347 DC=C = 614 DC≡C = 839 DC-N = 305 DC=N = 615 DC≡N = 891 DC-O = 358 DC=O = 745 DC=O (CO2) = 799 DC≡O=1072 DC-Br = 276 DN-N = 160. DN=N = 418 DN≡N = 941 DO-O = 146 DO=O = 495 DN-O = 201 DN=O = 607 DBr-Br = 193 DC-Cl = 339 DH-Cl = 427 DCl-Cl = 239arrow_forwardCalculate the enthalpy change for the reaction below. Compound Нeat Value -> 3NO(s) ,0,ls) AH +174 k (belONH2 -(aloH (2Fo+ ('N AH -183 k AH =-128 k) 2NO(g) O-137 kJ O-128 kJ -174kJ 270KJarrow_forward
- When ethene is mixed with hydrogen in the presence of a platinum catalyst, hydrogen adds across the double bond to form ethane. At room temperature, the reaction goes to completion. Predict the signs of ∆H° and ∆S° for this reaction. Explain these signs in terms of bonding and freedom of motion.arrow_forwardUsing bond dissociation energies predict the energy given off in the following reaction: C2H4 + O2 → CO2 + H2O A 444 kJ B 634 kJ C 246 kJ D 906 kJarrow_forward7. Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis structure for each molecule. CH, (g) + 20, (g) ·CO, (g) + H,O (g) Bond Bond Enthalpy (kJ/mol) C-O 351 C=0 799 CEO 1070 O-O 142 O=0 498 C-H 414 O-H 460arrow_forward
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