Calculate ΔG for the dilution of aqueous HCl from 0.89 M to 0.253 M at 25°C.(adsbygoogle = window.adsbygoogle || []).push({});

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 ofQ.

But he says put them to power of 2. WHY?? Can someone explain?

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# Free Energy of Dilution

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