Calculate ΔG for the dilution of aqueous HCl from 0.89 M to 0.253 M at 25°C. THis was a question I had to do some time earlier for one of my assignments. I got some help from a classmate and he said THE FOLLOWING: "H+ and Cl- are equimolar so you have to put them to the power of two.... so the equation reads Deltag = RTln Q delta g = 8.314472J/K/mol*298.15K * 1kJ/1000J *ln (second molarity^2/first molarity^2)" WHEN he says EQUIMOLAR how do i find this out like i have no idea how he figured that out. If i did this question i would just do products over reactions to find the value of Q. But he says put them to power of 2. WHY?? Can someone explain?