(adsbygoogle = window.adsbygoogle || []).push({}); 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??

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# Homework Help: Delta G of Dilution

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