SCH4U - Gibbs Free Energy and Reaction Spontaneity Assignment

Assignment Task

Introduction: 

Reactions in chemistry are described as either being spontaneous, non-spontaneous, or at equilibrium.  This classification depends on a reaction’s change in enthalpy (∆H), change in entropy (∆S) and temperature (T).  These three variables determine Gibbs energy (∆G), ultimately, the free energy of the system.  Gibbs free energy gives us an idea of the total amount of free energy or work that can be obtained from a reaction but does not tell us the speed at which that work can be obtained. When reactions involve reduction and oxidation this free work and overall spontaneity can be determined by looking at potential differences (Ecell).

For electrochemical reactions differences in standard reduction potential and the conditions in which the reaction is done will dictate the overall cell potential and overall spontaneity. These values can be related to the reaction’s thermodynamics.

When examining the speed of a reaction we need to explore its kinetics. In kinetics we learn that reactions are governed by rate laws. These rate laws correspond to the rate determining step of a more complex reaction mechanism. Up to now we have only been concerned with the net chemical change of a reaction; The starting materials (reactants) and the final product(s) of a reaction.  Although it is only the net chemical change that is directly observable, most chemical reactions, are believed to occur in a series of steps.

In this project you will choose a unique reaction that falls into either one of five reaction categories. It will be your responsibility to understand the thermodynamics, kinetics and possibly electrochemical potential of the reaction.  You will communicate your findings in a recorded video which will be posted to brightspace.  

Description of project:

Presentation

• Your lesson (power point/slides etc). 6-8 minutes.  A recorded presentation.
• A visual aid (model(s) or animations etc) helping your group understand the underlying principles of your reaction). This can be a separate video you prepare and embed in your slides. There must be text or voice over explaining this process.  Note: this is an authentic production and not a video retrieved from the internet.

Portfolio

• Recording of your presentation (lesson). Visual aid (this may be incorporated in your lesson)
• Appendix (communicating the following calculations/equations)
  • ∆⁰H_rxn, ∆⁰S_rxn, ∆⁰G_rxn * ⁰ = (SATP)
  • ∆G_rxn at STP and RTP (20⁰C). Is there a Teq.
  • Potential energy diagram (drawn by you with as much detail as possible. labels and scale)
  • Rate law equation with its description
  • E⁰ and Nernst Equations* only for electrolytic cells. Cell notation wet cell diagrams or dry cell diagram
• References (APA)

Evaluation

Part 1: Prensentation

• Your lesson effectively explains/teaches your reaction’s spontaneity and reaction mechanism illustrating electron movement and the fashion in which bonds break.
• Your presentation of the thermochemistry, kinetics and possibly electric potential differences of your reaction is comprehensive, clear and concise.
• Attention must be made to electron movement through the use of curly arrows and bond type.
• Use of SOA and SRA along with overall potential differences and conditions must be considered for electrochemical reactions.*for electrolytic cells only
• Lesson includes all the relevant chemical language and uses proper IUPAC nomenclature.

Part 2:  Presentation, Visual Aid

• Your presentation of the thermochemistry, kinetics and possibly electric potential differences of your reaction is comprehensive, clear and concise.
• Your visual aid enhances the understanding of your audience
• Your presentation reaches beyond the structure of the exemplars and strives for depth and creativity.

Reaction mechanisms are theoretical.  They suggest plausible pathways and involve reactionary intermediates that are supported by experimental evidence.  Each individual step is called an elementary step and describes how a reaction is believed to occur. The speed of each step will vary and ultimately the slowest step is what limits the overall rate of your reaction.

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