We did a lab in chemistry and determined the Gibbs free energy of a titration done at different temperatures. When I graphed free energy vs. temperature, the trend was positive. The lab report outline tells me to explain why my trend is positive, but I'm not sure why it does. Anyone know?
Answer:
DG = DH - TDS
So if your reaction has a positive DS, then DG will become more negative at higher temperatures.
If your reaction has a negative DS, then DG will become more positive at higher temperatures.
Why you would see this in a titration is not immediately obvious to me.
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