Journal Entry:

What can you do to make a thermodynamically unfavorable (non spontaneous) reaction favorable (spontaneous)?

Learning Intentions

• We will learn how to use representations and models to predict the sign and relative magnitude of the free energy change associated with chemical or physical processes.

• We will learn how to predict whether or not a physical or chemical process is thermodynamically favored (spontaneous) by determination of the signs of both ΔH and ΔS in relation to free energy (ΔG) or direct calculation of ΔG.

• We will learn how to answer FRQs using the appropriate energy equations and supporting your answers with the proper work and explanation.

• We will learn what can be used to make non spontaneous process spontaneous.

Closing Task:

You can calculate Gibb's free energy in a variety of conditions, determine if the reaction is spontaneous or not.

You can determine sign of ΔH, ΔS and ΔG based on conditions of reaction.

Content Standards being covered:

Some physical or chemical processes involve both a decrease in the internal energy of the components under consideration and an increase in the entropy of those components. These processes are necessarily "thermodynamically favored". (E.K. 5.E.2)

If a chemical or physical process is not driven by both entropy and enthalpy changes, then the Gibbs free energy  change can be used to determine whether the process is thermodynamically favored. (E.K. 5.3.E)

External sources of energy can be used to drive change in cases where the Gibbs free energy change is positive. (E.K. 5.E.4)