A [Review Topics] [References] cyclopropane 115 27.5 cyclobutane 110 26.3 cyclopentane 26.0 6.2 cycloheptane 26.2 6.3 40.5 9.7 cyclooctane ⚫ (Calculate your answer to the nearest 0.1 energy unit, and be sure to specify units, kJ/mol or kcal/mol. The answer is case sensitive.) H H. 9 H. H eq eq M Preq Strain energy = H ball & stick + labels Submit Answer Retry Entire Group 8 more group attempts remaining F4 4 $ % 5 Cengage Learning Cengage Technical Support F5 F6 96 PrtScnF8 Home End PgUp. PgDn F9 F10 27 & ) 8 9 R T Y U I O P F G H J K L

A [Review Topics] [References] cyclopropane 115 27.5 cyclobutane 110 26.3 cyclopentane 26.0 6.2 cycloheptane 26.2 6.3 40.5 9.7 cyclooctane ⚫ (Calculate your answer to the nearest 0.1 energy unit, and be sure to specify units, kJ/mol or kcal/mol. The answer is case sensitive.) H H. 9 H. H eq eq M Preq Strain energy = H ball & stick + labels Submit Answer Retry Entire Group 8 more group attempts remaining F4 4 $ % 5 Cengage Learning Cengage Technical Support F5 F6 96 PrtScnF8 Home End PgUp. PgDn F9 F10 27 & ) 8 9 R T Y U I O P F G H J K L

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 2E: Prepare a table identifying several energy transitions that take place during the typical operation...

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For each organic compound in the table below, name the highlighted side chain. Note for advanced students: don't include the locant of the side chain. compound H-C=0 name of highlighted side chain - - CH₂ — CH₂ — CH₂ — CH₂ — CH₂— CH₂· - CH G H C 0 H C 0 CH3 CH - CH2-CH₂ CH2 | H C 0 CH₂ CH₂2 I CH₂ CH₂ O HOC CH - CH2CH2 CH₂ — CH₂ CH=CH2 ☑ ☐
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Benzene is one of the compounds used as octane enhancers in unleaded gasoline. It is manufactured by the catalytic conversion of acetylene to benzene: 3C2 H2(g) ⟶ C6 H6(g). Which value of Kc would make thisreaction most useful commercially? Kc ≈ 0.01, Kc ≈ 1, or Kc ≈ 10. Explain your answer.
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.
Use and modify some/all the reactions provided to form the indicated overall reaction according to Hess' Law. • If a reaction is not used in your Hess' Law process, include that indication by multiplying the reaction by "0" • If no modification is needed and the reaction is applied as written below, include that indication by multiplying the reaction by "1" • Use whole numbers and simple fractions (such as "2" or "1/2", not 0.5) and negative signs (such as "-2") where needed Then calculate and report the enthalpy change (in kJ) for the overall reaction in the indicated blank, including units with your written value and rounded to 1 decimal place. Overall Reaction: CS2(1) + 302(g) → CO2(g) + 2SO2(g) Rxn # Reaction ΔΗ° (kJ) 1 C(s) → C(g) 716.67 2 C(s) + O2(g) → CO2(g) -393.5 3 3Fe(s) +202(g) → Fe3O4(s) -1118 4 C(s) + 2S(s) → CS2(1) 87.9 5 CH4(g) + O2(g) → CO₂(g) + H₂O(g) -882.0 6 S(s) + O2(g) → SO2(g) -296.8 N2(g) + 4H2(g) + Cl2(g) → 2NH4Cl(g) -629.1 7
Consider the combustion of methane, CH4, shown below: CH4 (g) + 2 O2 (g) ⇋⇋ 2 H2O (g) + CO2 (g) What is the Kc expression? Select one: a. Kc=[CO2][H2O]2[CH4][O2]2Kc=[CO2][H2O]2[CH4][O2]2 b. Kc=[CO2]∗2∗[H2O][CH4]∗2∗[O2]Kc=[CO2]∗2∗[H2O][CH4]∗2∗[O2] c. Kc=[CH4][O2]2[CO2][H2O]2Kc=[CH4][O2]2[CO2][H2O]2 d. Kc=[CO2][H2O][CH4][O2]Kc=[CO2][H2O][CH4][O2] e. Kc=[CO2]2[H2O]4[CH4]2[O2]4
NUMBER 63 and 64 and 65
Name these organic compounds: Η H H H | | | Η· C C C C C=H | | | | | H H H H H — H Η structure — — H H - C C 1 1 Η - Η - - Η - H | H — C - Η | H name
Given the following data: 4C(s) + 4H2(g) + O2(g) → CH3CH2OCOCH3(l) ΔH°=-480.0 kJ CH3CH2OH(l) + O2(g) → CH3COOH(l) + H2O(l) ΔH°=-492.0 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:CH3COOH(l) + CH3CH2OH(l) → CH3CH2OCOCH3(l) + H2O(l)
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CH3 О А OB ос D H3C H3C A C Brz CH₂Cl₂ .Br H/I!! Н ? H3C H3C, B 1114 D H "/Br H "//Br
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