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it doesn't always favor the reverse reaction. When enthalpy is positive and entropy is negative, then the reaction favors the reverse. However when enthalpy is positive and entropy is also positive, the sign of Delta G depends on the temperature. You would use the equation "DeltaG= DeltaH - T(DeltaS)" to figure out whether the temp makes Delta G positive or negative.
Endothermic would not be favorable because positive entropy is favorable (since more disorder is generally created) and as a result, if you want free energy to be negative and entropy is positive, enthalpy would have to be negative at a high temperature to guarantee a spontaneous reaction (negative free energy). Hope that made sense!
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