Posted by Ginger on Monday, March 31, 2008 at 7:45pm.
When we burn benzoic acid (for example in a calorimeter to calibrate the calorimeter), the calorimeter temperature rises; therefore, heat must be given off. That means the reaction is exothermic if I'm not on the wrong track here. And that means a isn't right. If delta S = 0, then Tdelta S = 0 and delta G = delta H. If delta H is exothermic, that makes delta H negative and that makes delta G negative. I would go with answer B. One may ask why benzoic is stable at room temperature instead of spontaneously combusting; I would answer that the activation energy had to be overcome to get the reaction started.
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