parts b and c please Polyvinyl chloride (PVC) is one of the most commercially important polymers. PVCis made by addition polymerization of vinyl chloride (C2H3 Cl). Vinyl chloride issynthesized from ethylene (C2 H4) in a two-step process involving the followingequilibria:Selected bond dissociation enthalpies are given inthis table.Dissociation enthalpyBondEquilibrium 1: C2H4(g) + Cl2 (g) = C2H¾C12 (g)Equilibrium 2: C2H4 Cl2 (g) = C2H3 Cl(g) + HC1(g)(kJ/mol)C-C348C=C614C=C839Part AC-C1328C-H413What are the C-C bond orders in C2H4C12 and C2H3 Cl, respectively?Cl-Cl242Express your answers numerically separated by commas.Н-Н436• View Available Hint(s)Н-СІ431 Part BUse bond energies to estimate the enthalpy change for Equilibrium 1.Express your answer numerically in kilojoules.• View Available Hint(s)?ΔΗΧ348kJSubmitPrevious AnswersX Incorrect; Try Again; 5 attempts remainingYour answer is the energy change associated with breaking a carbon-carbon single bond. There are several bonds broken and formed in Equilibrium 1 that youmust account for.Part CUse bond energies to estimate the enthalpy change, AHrxn, for Equilibrium 2.Express your answer numerically in kilojoules.• View Available Hint(s)AHrxnkJSubmit

Answered: Image /qna-images/answer/c61dc7e9-03e2-4265-9312-434e6a4dba0e.jpg

Part B Use bond energies to estimate the enthalpy change for Equilibrium 1. Express your answer numerically in kilojoules. • View Available Hint(s) ? AHrxn = 348 kJ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Your answer is the energy change associated with breaking a carbon-carbon single bond. There are several bonds broken and formed in Equilibrium 1 that you must account for. Part C Use bond energies to estimate the enthalpy change, AHrxn, for Equilibrium 2. Express your answer numerically in kilojoules. • View Available Hint(s) AHrxn = kJ Submit

Part B Use bond energies to estimate the enthalpy change for Equilibrium 1. Express your answer numerically in kilojoules. • View Available Hint(s) ? AHrxn = 348 kJ Submit Previous Answers X Incorrect; Try Again; 5 attempts remaining Your answer is the energy change associated with breaking a carbon-carbon single bond. There are several bonds broken and formed in Equilibrium 1 that you must account for. Part C Use bond energies to estimate the enthalpy change, AHrxn, for Equilibrium 2. Express your answer numerically in kilojoules. • View Available Hint(s) AHrxn = kJ Submit

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 78QAP

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Combustion of glucose ( C6H12O6 ) is the main source of energy for animal cells: C6H12O6 ( s ) + 6O2 ( g ) → 6CO2 ( g ) + 6H2O ( l ) =ΔGrxn37°C−2872.kJ This energy is generally stored as ATP (adenosine triphosphate) molecules, which can release it when convenient by hydrolysis ("water-assisted decomposition") into ADP (adenosine diphosphate) molecules and a phosphate anion, often given the symbol Pi in biochemistry: ATP ( aq ) → ADP ( aq ) + Pi ( aq ) =ΔGrxn−35 to 70kJ The actual amount of free energy released by the hydrolysis of ATP varies, depending on the exact conditions inside the cell. Suppose under certain conditions hydrolysis of ATP actually releases −51.3/kJmol . Calculate the maximum number of ATP s that could be created from ADPs and Pi by the combustion of a molecule of glucose. Your answer must be a whole number.
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ in the combustion of ethane in the presence of excess oxygen yields carbon dioxide and water: 2C2H2(g) + 7O2(g) → 4CO2(g) + 6H2O(l) in J/K?
Use the standard reaction energies given below to determine DeltaG^°rxn for the following reaction: 2XO2(g) —> 2XO(g) + O2(g) From the standard reaction energy of X2(g) + O2 —> 2XO(g) DG^°= 155.52 Kjxmol-1 X2(g) + 2O2 —> 2XO2(g) DG^°= 168.55 Kjxmol-1 Given answer in Kj/mol. Give answer to two decimal places.
Use the table below to answer the questions that follow.Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C)Substance ΔH°f (kJ/mol) ΔG°f (kJ/mol) S (J/K-mol) Substance S° (J/K-mol) CO2 (g) 213.6 C2H2 (g) 200.8 O2 (g) 205.0 H2O (l) 69.91 Calculate the value of ΔS° (J/K ∙ mol ) for the catalytic hydrogenation of acetylene to ethane,C2H2 (g) + 2H2 (g) → C2H6 (g)
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 6. What is the ∆S⁰ of the combustion of acetylene in the presence of excess oxygen yields carbon dioxide and water: 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) in J/K?
Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ in the combustion of ethene in the presence of excess oxygen yields carbon dioxide and water: C2H2(g) + 3O2(g) → 2CO2(g) + 2H2O(l) in J/K?
in a particular solution at 30 degrees celcius the ratio of beta-d-glucose to linear glucose is 320:1. Calculate gibbs free energy at standard state for conversion of linear to beta-d-glucose. (R=8.3145 J mol-1 K-1)
consider attached reaction- glucose-6-phosphate -------glucose + phosphatekeq= 126.70a. the standard gibbs free energy for this reaction is _____ kj/mol b. if the concentration of glucose-6-phosphate is adjusted to 1.5M and that of glucose and phosphate is adjusted to 0.50M, the actaul free energy change is equal to ______kj/mol
Describe why it is easier to use Gto determine the spontaneity of a process rather than S u
Calculate the standard free-energy changes for the following reactions at 25°C. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 2MgO(s) → 2Mg(s) + O2(g) Inorganic Substances Substance ΔHo (kJ/mol) f ΔGo (kJ/mol) f So (J/K·mol) CO(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 H2(g) 0 0 131.0 H2O(l) -285.8 -237.2 69.9 O2(g) 0 0 205.0 Organic Substances CH4(g) -74.85 -50.8 186.2 Mg(s) 0 0 32.5 MgO(s) -601.8 569.6 26.78 Table 1. Selected Thermodynamic Data at 1 atm and 25°C* *The ΔHof, ΔGof and S° values for ions are based on the reference states ΔHof (H+) = 0, ΔGof (H+) = 0, and S°(H+) = 0.
Calculate the standard free-energy changes for the following reactions at 25°C. CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) 2MgO(s) → 2Mg(s) + O2(g) Inorganic Substances Substance ΔHo (kJ/mol) f ΔGo (kJ/mol) f So (J/K·mol) CO(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 H2(g) 0 0 131.0 H2O(l) -285.8 -237.2 69.9 O2(g) 0 0 205.0 Organic Substances CH4(g) -74.85 -50.8 186.2 Mg(s) 0 0 32.5 MgO(s) -601.8 569.6 26.78
Calculate the standard free-energy changes for the following reactions at 25°C. 2MgO(s) → 2Mg(s) + O2(g) Inorganic Substances Substance ΔHo (kJ/mol) f ΔGo (kJ/mol) f So (J/K·mol) CO(g) -110.5 -137.3 197.9 CO2(g) -393.5 -394.4 213.6 H2(g) 0 0 131.0 H2O(l) -285.8 -237.2 69.9 O2(g) 0 0 205.0 Organic Substances CH4(g) -74.85 -50.8 186.2 Mg(s) 0 0 32.5 MgO(s) -601.8 569.6 26.78 Table 1. Selected Thermodynamic Data at 1 atm and 25°C* *The ΔHof, ΔGof and S° values for ions are based on the reference states ΔHof (H+) = 0, ΔGof (H+) = 0, and S°(H+) = 0.