Usually the melting point of pure compound should be higher than the impure one, because the impurities messes up of the crystalline lattice by blocking their formation and creates irregularities. Thus the intermolecular bonds become weaker, resulting lower heat energy required to break the bond, making the melting points become lower. But why is it different in benzoic acid?
nvm. figured it out. The melting point of impure benzoic acid is higher than the pure one because the melting point of the impurities exist in the compound have a higher melting point than the benzoic acid. but if anyone have another answer, let me know. thanks
I also think that benzoic acid is in a state of azeotrope with another body considered as an impurity. otherwise, and outside the azeotrope, the impurities taken as solutes, are used to separate molecules of bensoique acid. in this case the stability of the molecule provided by the intermolecular force is weakened by the breakage thereof, which leads to the lowering of the boiling point of which is proportional. So depending on the concentration of impurity, a quantity of molecules folds against it by only satisfying of intramolecular hydrogen bonds. the general rule of the dispersion of the body A by the body B, or soluté- solvent or finally, the impurity notion in the body A (when the content is low). Two factors influence the boiling point are the intermolecular hydrogen bonds and polarity of molecules. Here, it may be the question of the intermolecular Foces causing a hexagonal cyclic stability.
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