1. The problem statement, all variables and given/known data For a particular reversible reaction, the forward process is exothermic and the reverse process is endothermic. Which of the following statements must be true about this reaction? (A) The forward reaction will be spontaneous under standard conditions (B) The reverse reaction will be spontaneous under standard conditions (C) The activation energy will be greater for the forward reaction than for the reverse reaction (D) The activation energy will be greater for the reverse reaction than for the forward reaction. 2. Relevant equations NA 3. The attempt at a solution I eliminated B because if the reverse is endothermic, this will not be spontaneous. I chose the right answer (D) but I wanted to be sure my logic is on the right track. So, I assumed D must be correct because endothermic reactions require much more energy to force a reaction, whereas the forward exothermic reaction would require less.