Hi I need help with these practice problems thank you! In KeaAG°= - RT In Keq andAGRTor Keg= 6AG°/RT[1] Given: CH4(g) + H2O(g) → CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol.Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reversereaction?AG =[b] What does the sign of the free energy have to be such that a reaction is spontaneous?AS =[c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous?[ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous?AH =ДН 3AS =[d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a hightemperature or a low temperature?[e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a lowtemperature be more likely to lead to a spontaneous reaction?[3] For the reaction C,H2(g) + 2H2(g) ) → C2H(g), AG°:(C¿H2) = +209.2kJ/mol and AG°:(C,H6) = -32.89 kJ/mol at25.0°C. What is Keg for this reaction?[4] Calculate the solubility of Ag,CrO4 in pure water if the solubility product constant for silver chromate is 1.1 x 1012.Calculate the solubility of barium sulfate in a 0.020 M sodium sulfate solution. The[5]solubility product constant for barium sulfate is 1.1 x 10*1º.

Answered: Image /qna-images/answer/19c3c09d-e0ec-4a51-8156-6246296b0e9c.jpg

[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol, Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.

[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol, Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter10: Entropy And The Second Law Of Thermodynamics

Section: Chapter Questions

Problem 10.50PAE: For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then...

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Question

Hi I need help with these practice problems thank you!

In Kea
AG°= - RT In Keq and
AG
RT
or Keg
= 6AG°/RT
[1] Given: CH4(g) + H2O(g) → CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol.
Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
[2] [a] The forward reaction is spontaneous for a particular reversible reaction. What can you conclude about the reverse
reaction?
AG =
[b] What does the sign of the free energy have to be such that a reaction is spontaneous?
AS =
[c] [i] Under what conditions of enthalpy and entropy change is a reaction always spontaneous?
[ii] Under what conditions of enthalpy and entropy change is a reaction never spontaneous?
AH =
ДН 3
AS =
[d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high
temperature or a low temperature?
[e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low
temperature be more likely to lead to a spontaneous reaction?
[3] For the reaction C,H2(g) + 2H2(g) ) → C2H(g), AG°:(C¿H2) = +209.2kJ/mol and AG°:(C,H6) = -32.89 kJ/mol at
25.0°C. What is Keg for this reaction?
[4] Calculate the solubility of Ag,CrO4 in pure water if the solubility product constant for silver chromate is 1.1 x 1012.
Calculate the solubility of barium sulfate in a 0.020 M sodium sulfate solution. The
[5]
solubility product constant for barium sulfate is 1.1 x 10*1º.

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