CH302H - Principles of Chemistry II: Honors
Spring 2016, Unique 49420

Lecture Summary, 21 January 2016

Thermochemistry:  We then went on and discussed the topic of thermochemistry, the science of the flow of heat due to chemical transformations:

   Reactant --> Product +/- heat

In chemical thermodynamics we almost always are interested in energies at constant pressure, therefore in reaction enthalpies of a system.  Because enthalpy is a state function, by defining a standard state of P = 1 bar and T = 298 K, we can tabulate enthalpies of formation for any substance under that standard, then use that information to calculate a reaction enthalpy under any set of circumstances, even those far away from the standard state. 
Second Law of Thermodynamics: We have spent quite a bit of time developing the first law of thermodynamics, which we have expressed as energy = heat + work.  We have found that we can find heat, work, internal energies, and enthalpies for a variety of different systems and different paths.  But clearly we are missing something.  For example, we know of simple examples in which a reaction occurs spontaneously even if it requires energy from the surroundings, such as the cold pack I passed around in class. 

We are clearly missing a kind of energy that will provide a driving force for spontaneous events to occur even with no change in internal energy.  We developed a state function, called entropy, S, which defines the direction of spontaneous change (deltaS > 0), and which will quantify this driving force:

      deltaS >= q/T.

Thermochemistry problem 1