Whether a reaction is product-favored, that is, whether the reactants are converted to products under standard-state conditions, is reflected in the sign of its Δ r G° . This equation Δ r G° =  Δ r H° − T Δ r S° shows that the sign of Δ r G°  depends on the signs of Δ r H°  and Δ r S° , and, in some cases, the absolute temperature (which can only have positive values). Four possibilities exist: Both Δ r H°  and Δ r S°  are positive —an endothermic process with an increase in system entropy. Δ r G°  is negative if  T Δ r S° >  Δ r H° , and positive if  T Δ r S°  < Δ r H° . Such a process is  product-favored at high temperatures and reactant-favored at low temperatures. Both Δ r H°  and Δ r S°  are negative —an exothermic process with a decrease in system entropy. Δ r G°  is negative if | T Δ r S °| < |Δ r H °| and positive if | T Δ r S °| > |Δ r H °|. Such a process is  product-favored at low temperatures and reactant-favored at high temperatures.  (Remember that | T Δ r S