I realize that this is a chem prob, but I'm stuck with what I thought was a straightforward problem while studying for my physical chemistry exam. 1. The problem statement, all variables and given/known data The standard molar enthalpy of combustion of solid phenol (C6H5OH) is -3054 kJ/mol at 298k and it's standard molar entropy is 144.0 J/(K*mol). Calculate the standard free energy of formation of phentol at 298k. 2. Relevant equations G = H - TS 3. The attempt at a solution G = (-3054.0 * 10^3 J/mol) - (298 K) (144.0 J/k/mol) From what I know about the determination of G, I simply plugged in those numbers but my solution was way off. The solution should be -50.42 kJ/mol but help with deriving it from first principle is what I'm after.