First of all, thanks for replying.
Well, all the information that you posted looks very similar to what I got from wikipedia. That's the reason why I posted this question here, because in wikipedia they don't really compare and contrast both of them. I wish you could explain it to me excluding the jargon, I think that's what throws me off. This is what I got so far,
Enthalpy, heat content, refers to the amount of heat a certain reaction can release or absorb. Let's stick with an exothermic reaction for now. As far as I know, the enthalpy in an exothermic reaction would be the heat given off when the reaction takes place. Now, this heat is also energy, and energy can be used to do "work" on a different system.
Gibbs free energy, using the last example, refers to the work that can be done with that heat or that energy from the exothermic reaction. However, in Gibbs free energy you take the enthalpy from that exothermic reaction, but you subtract the entropy. That's why, when entropy is neglected because it is too small, Enthalpy nearly equals Gibbs free energy.
I wish you could explain it to me using your words and using examples if it's not too much trouble.