CO Со, -4.94876985 x 103 kJ/mol н -3.94506117 x 10' kJ/mol 0.39305376802 kJ/mol/K 0.4111337849 kJ/mol/K S G ? -4.94999564 x 10' kJ/mol -3.94623306 x 105 kJ/mol The enthalpy, entropy, and free energy of CO can be computed as follows. First, we define the geometry at the equilibrium geometry, computed in the Enthalpy lesson mol_CO [["C", 0, 0, 0], ["O", 0, 0, 1.13485718]]; mol_CO [["C", 0, 0, 0]. ["O", 0, 0, 1.13485718]] (2.2) Finally, we compute a table of thermodynamic properties for CO including the enthalpy, entropy, and free energy. By default, the command uses a temperature of 298 K > thermo_CO= Thermodynamics(mol_CO, 'DensityFunctional', basis = "cc-pvdz"); J entropy=389.04949897 energy= -2.97355647 108 mol mol pe13100.56264564 mol thermo COtable , heat capacity= 20.81 00 12 14 ,electronic_energy= -2.97388047 108 J (2.3) mol K mol K J enthalpy= -2.97353168 108 J -2.74504846 K, free_energy= -2.97469163 10° mol 0 2.74504846 K mol в (a) What is the computed enthalpy of CO in kJ/mol? (b) What is the computed entropy of CO in kJ/mol/K? (c) What is the computed free energy of CO in kJmol? We can convert the enthalpy, entropy, and free energy from J to kJ using Maple's convert command kJ >H[CO] comnvertthermo_CO[ enthalpy],'unts'.- mol kJ Hco=-297353.16764385 mol (2.4) kJ SICO] convertthermo_CO[entropy],'units', mol K kJ =0.38904950 Sco (2.5) mol K convert > G[CO] thermo_CO[ free_energy],'units','- mol kJ Gco=-297469.16275 197 mol (2.6) Similarly, answer the following questions: (e) Using the entropy of CO in (b) and the precomputed entropy values in Table 1, calculate the change in entropy in the combustion of l mol of CO Using the free energy of CO in (c) and the precomputed free energy values in Table 1, calculate the change in free energy in the combustion of 1 mol of CO. (g) Using the change in enthalpies and entropies and the Gibbs free energy equation, compute the change in free energy in the combustion of 1 mol of CO (h) Do you results for the free energy change in (f) and (g) agree? i Using the change in enthalpies and entropies and the Gibbs free energy equation, estimate the temperature below which the reaction is spontaneous.
CO Со, -4.94876985 x 103 kJ/mol н -3.94506117 x 10' kJ/mol 0.39305376802 kJ/mol/K 0.4111337849 kJ/mol/K S G ? -4.94999564 x 10' kJ/mol -3.94623306 x 105 kJ/mol The enthalpy, entropy, and free energy of CO can be computed as follows. First, we define the geometry at the equilibrium geometry, computed in the Enthalpy lesson mol_CO [["C", 0, 0, 0], ["O", 0, 0, 1.13485718]]; mol_CO [["C", 0, 0, 0]. ["O", 0, 0, 1.13485718]] (2.2) Finally, we compute a table of thermodynamic properties for CO including the enthalpy, entropy, and free energy. By default, the command uses a temperature of 298 K > thermo_CO= Thermodynamics(mol_CO, 'DensityFunctional', basis = "cc-pvdz"); J entropy=389.04949897 energy= -2.97355647 108 mol mol pe13100.56264564 mol thermo COtable , heat capacity= 20.81 00 12 14 ,electronic_energy= -2.97388047 108 J (2.3) mol K mol K J enthalpy= -2.97353168 108 J -2.74504846 K, free_energy= -2.97469163 10° mol 0 2.74504846 K mol в (a) What is the computed enthalpy of CO in kJ/mol? (b) What is the computed entropy of CO in kJ/mol/K? (c) What is the computed free energy of CO in kJmol? We can convert the enthalpy, entropy, and free energy from J to kJ using Maple's convert command kJ >H[CO] comnvertthermo_CO[ enthalpy],'unts'.- mol kJ Hco=-297353.16764385 mol (2.4) kJ SICO] convertthermo_CO[entropy],'units', mol K kJ =0.38904950 Sco (2.5) mol K convert > G[CO] thermo_CO[ free_energy],'units','- mol kJ Gco=-297469.16275 197 mol (2.6) Similarly, answer the following questions: (e) Using the entropy of CO in (b) and the precomputed entropy values in Table 1, calculate the change in entropy in the combustion of l mol of CO Using the free energy of CO in (c) and the precomputed free energy values in Table 1, calculate the change in free energy in the combustion of 1 mol of CO. (g) Using the change in enthalpies and entropies and the Gibbs free energy equation, compute the change in free energy in the combustion of 1 mol of CO (h) Do you results for the free energy change in (f) and (g) agree? i Using the change in enthalpies and entropies and the Gibbs free energy equation, estimate the temperature below which the reaction is spontaneous.
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter12: Thermodynamic Processes And Thermochemistry
Section: Chapter Questions
Problem 29P
Related questions
Question
Table one is the chart at the top of image 1. Subquestions A-C and their answers are also in that image in Blue. I need help with E-H.
The Equation is
CO(g) + 1/2O2 = CO2 (g)
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Step 1
VIEWTrending now
This is a popular solution!
Step by step
Solved in 1 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning