ORGANIC CHEMISTRY MASTERINGCHEM ACCESS
9th Edition
ISBN: 9780137249442
Author: Wade
Publisher: INTER PEAR
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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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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
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)
heat
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?
Chapter 4 Solutions
ORGANIC CHEMISTRY MASTERINGCHEM ACCESS
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
- 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 kJarrow_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
- Find the AHn for the following reaction: B2 He (g) + 6 Cl2(9) → 2 RC13(9) + 6 HC(g) given the following reactions and subsequent AH° values $$ BC13 (9) + 3 H2O(1) → H3 BO3(g) + 3 HCl(g) AH° = -113.1 kJ B2 H6 + 6 H2O(l) → 2 H3 BO3(9) + 6 H2 (9) AH° = -496 kJ 1 1 H2 (g) + Cl,(g) 2 HC(g) AH° = -95.5 kJ 2 $$arrow_forwardGiven 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_forward
- A) 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_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
- 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_forwardThe reaction of liquid methyl chloride (CH3Cl) with water produces methanol and hydrogen chloride gas at room temperature, despite the fact that ΔHo rxn = 28.3 kJ/mol. Using thermodynamic arguments, propose an explanation as to why methanol forms. CH3Cl (l) + H2O (l) → CH3OH (l) + HCl (g)arrow_forwardWhen 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_forward
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