Question
I'm confused about the difference between the q in q=mc(Tf-Ti) and (Delta)H, or enthalpy. What exactly does enthalpy mean and how is that different than q?
(I'm also confused about what Gibbs Free Energy actually means; I know that if it's negative, the reaction is spontaneous, but I don't understand why.)
(I'm also confused about what Gibbs Free Energy actually means; I know that if it's negative, the reaction is spontaneous, but I don't understand why.)
Answers
delta H is defined as the change in heat content of a process at constant pressure. Then q<sub>p</sub> = delta H.
In fact, you will see some problems in which a solid is added to water in a calorimeter and the change in T is noted; the question than asks for delta H of the reaction.
In fact, you will see some problems in which a solid is added to water in a calorimeter and the change in T is noted; the question than asks for delta H of the reaction.
So q=mc(Tf-Ti) could be written as Delta H=mc(Tf-Ti) assuming the pressure is constant?
Yes, and for some problems it is written that way.
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