[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
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60cf892a-bc21-4928-b8d7-b5b696620db4%2F7ad0833a-f130-4c35-b4b7-3cf14dc88ec9%2Fn2ddb6a_processed.jpeg&w=3840&q=75)
Transcribed Image Text: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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