State the first law of thermodynamics and the sign conventions used for
heat, q , and work , w.
Calculate the value of one of the following from known values of the other
two: [Delta]E, q, and w.
Explain the purpose served by the thermodynamic property of enthalpy (H),
describe how [Delta]H is related to [Delta]E, and calculate one from the
other for reactions involving gases.
Explain the meaning of the term "spontaneous change" as it applies to
chemical reactions.
Explain why entropy is important and how entropy is related to the disorder
of the system.
Predict whether entropy increases or decreases for certain processes.
Explain why entropy alone is not used to predict a spontaneous change and
why free energy is needed.
Qualitatively predict whether reactions are spontaneous or nonspontaneous
based on their [Delta]H and [Delta]S values.
Determine [Delta]Go from tabulated data, both tables of
[Delta]Gof and those of [Delta]Hof and
So.
Use [Delta]Go =[Delta]Ho -
T[Delta]So, the Gibbs-Helmholtz equation, to determine
[Delta]Go at various temperatures.
Know that [Delta]Gtr = 0 at equilibrium. For phase changes, use
[Delta]Str =[Delta]Htr/Ttr = the molar entropy of
transition.
Write thermodynamic equilibrium constant expressions Keq for
reactions and relate these to Kp and Kc.
Compute values of Keq from tabulated data and [Delta]Go
= -RT ln Keq.
Explain how absolute entropies of substances can be determined with the
third law of thermodynamics.
Relate the equilibrium constant to the standard molar enthalpy of reaction,
[Delta]Ho and to Kelvin temperature, both graphically and
algebraically.