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[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.

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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.
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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