A certain reaction has a AG° = 419.0 kJ at 298 K. The value of AS° for this reaction is 188.0 J/K. Above what temperature (in units of K) does this reaction become spontaneous? Assume that AH° and AS° do not depend on temperature.

17. For the reaction: A + B C AH°= +45 kJ/mol and AS° = +60 J/K.mol. At what temperature will this reaction be spontaneous? * O The reaction is nonspontaneous at all temperatures. O At a temperature greater than 477 °C. O The reaction is spontaneous at all temperatures. O At a temperature greater than 750 °C. O At a temperature lower than 477 °C.

Delta H degrees and Delta S degrees for a reaction are –11.7 kJ/mol and –105 J/mol K, respectively. At what temperatures (in K) will this reaction be spontaneous under standard conditions?

For a given reaction, dH = 32 kJ/mol and dS = 117 J/mol. At approximately what temperature would this reaction become spontaneous?

For the reaction Fe3O4 (s) + 4H2(g) → 3Fe(s) + 4H₂O(g) AH° = 151 kJ and AS° = 169 J/K The equilibrium constant for this reaction at 342.0 K is Assume that AH° and AS are independent of temperature.

Use the data to calculate the standard entropy change for the following reaction: 5. S°[Mt(s)] 43.2 J/K mol Mt(s) + ½ O2(g) → MtO(s) S°[O2(g)] = 305.1 J/K-mol S°[MtO(s)] 62.6 J/K mol a) -133.2 J/K b) -285.7 J/K c) 285.7 J/K d) 133.2 J/K

A reaction has AH°= 100 kJ/mol and AS°= 250 J/mol.K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?

A reaction has a ΔH of -87.36 kJ and a ΔS of -175.3 J/K. At what temperature (in K) does the reaction become spontaneous?     626.4 K     This reaction is always spontaneous     498.3 K     434.6 K     This reaction is never spontaneous

alculate ΔS per mole for the melting of H2O at  0.°C,  ΔHfus = 6.0 kJ/mol.   J/mol·K