So a few days ago in class my professor mixed two solids together and it became cold, mushy/liquid and smelled bad.
here is the reaction: Ba(OH)2*8H2O(s) + 2NH4Cl(s) = BaCl2(aq) + 2NH3(g) + 10H2O(l)
What i am having problems with understanding are the terms entropy (not so much, i think i pretty much know this), enthalpy, and free energy relating to this reaction.
So for the entropy, this is what i think: this reaction changed from an ordered state to an disordered state. solid being ordered and gas,liquid being disordered. because this reaction became more disordered change in entropy (S) will have a positive sign.
For enthalpy: i am not quite sure. I think since the container that the reaction took place in became cold, the reaction absorbed heat? so the change in enthalpy (H) will have a positive sign, endothermic reaction. I think it was cold, i didnt get to feel it and i think i remember some in class saying the container was cold.
For free energy: according to this formula ( i dont know how to do the delta triangle symbol) G = H - TS. If H is positive and S is positive then free energy can have a sign of either positive or negative, this is with out doing any kind of calculations. So free energy is the energy left to do work?