Olfaction

Like know you these plastic packs you crack and they get cold? I read that it is often this spontaneous endothermic reaction taking place. NH4NO3 (s) –> NH4+ (aq) + NO3- (aq) So, with well-suited electrochemical chamber, I should be able to create current until the reaction reaches equilibrium? Oh wait, because of ΔG° = ΔH° - TΔS° , this reaction will only be spontaneous at high temperatures. So isn’t it simply, that if we create a cold spot in a warmer environment, there is going to be a flow of molecule to fill the hole and therefore kinetic energy?

Oh thanks, that’s the kind of answer I was expecting. That would explain why the Nernst-Equation allows me to convert redox potential into Gibbs Energy and not into Enthalpy… ΔG = -z F ΔE Where G ist the molar Gibbs Free Energy, z the number of exchanged electrons and E ist the standard redox potential…

But why is it called Gibb's free energy, if there is no way to use it? Is there maybe a way to create some gradient and do some diffusion that could be harnessed into work, altough no heat is being produced?

Hello, could someone please help me with this? Some reactions are spontaneous (with dG < 0) although they are endothermic (dH > 0). My question is: Is it possible to extract work from such a reaction? The process I understand to produce work is to heat something in a contained space and transfer the heat pressure into kinetic energy with a turbine. (Sorry I know this is not very formal). For example, this reaction is a spontaneous endothermic reaction. NH4NO3 (s) –> NH4+ (aq) + NO3- (aq) Is there a way I can get my turbine to work with this reaction? Is the Gibbs Free Energy that comes from the raise in Entropy of any use? And how so, if I get not heat? Thank you for you help. I am quite confused.