1. Calculate ΔG for the dilution of aqueous HCl from 0.89 M to 0.253 M at 25°C. data 2. The process you are considering is: H+(aq) + Cl-(aq)® H+(aq) + Cl-(aq) (for which ΔG°=0 i.e. standard states all round--both sides are the same). Now use ΔG=ΔG° + RTln(Q). (Use the actual concentrations to determine Q). Does this agree with what you intuitively know about the spontaneity of diffusion? 3. DeltaG = (8.314)(298.15)(ln (0.253)) - (8.314)(298.15)(ln(0.89)) = -3117.9 J/mol but this is wrong??