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Is there a difference between using kJ vs. kJ/mol when labelling Gibbs Free Energy? I've run across a few problems where you must multiply each molecule's standard value of formation by its number of moles in the reaction, but sometimes the units for the free energy of the reaction are written differently. I would think if you are multiplying everything by the number of moles, you would be cancelling those out in each individual calculation and be left with just kJ (Like in problem #8 on the 2015 midterm). In other cases, they leave the units as kJ/mol. Are both units correct for the Gibbs free energy of the reaction?
Dr. Lavelle said he would be relatively lenient on accepting either kJ or kJ/mol. This is because, given a particular reaction, the delta G is generally the delta G for the reaction as a whole, as written. This could be said as "per mole equivalent" of the reaction.
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