Electrochemistry and Electrolysis
Chapter 19: 5-8 Homework
Textbook assignment: Read Kotz and Triechel, Chemistry and Chemical Reactivity Chapter 18: Sections 5 to 8.
||wmax = nFE
||E: cell potential
nF: amount of electric charge transfered
||E: actual potential at temperature T
E°: potential at STP
n: number of moles of electrons transfered
F: total charge per mole electrons
R: gas constant
T: Temperature (K)
Q: reaction quotient
|Nernst at STP (298.15K)
||Constants R, T, F calculated
|Free Energy (STP)
||ΔrG° = -nFE°
||G°: Gibbs free energy for reduction half-reaction
E°: electric potential change for reduction half-reaction
|Free Energy and Nernst at Equilibrium
||E = 0 at equilibrium
||i: current (Amps)
Read the following weblecture before chat: Electrochemistry and Thermodynamics
Videos for Chapter 19: Principles of Chemical Reactivity: Entropy and Free Energy
Review the Videos at Thinkwell Video Lessons.
- Under "ELECTROCHEMISTRY"
- Galvanic Cells
- The Nernst Equation
- Electrochemical Determinants of Equilibria
- Electrolysis and Electrolytic Cells
- Electrolytic Cells
- The Stoichiometry of Electrolysis
Use the Electrolysis Experiment simulation to run a virtual electrolysis experiment.
- Read the Overview and Learning Outcomes, then click on "Experiment".
- Select the option to run the Experiment.
- Choose your own metals for the positive and negative terminals. Record thee masses of the electrodes.
- Choose a solution from the dropdown menu.
- Set the current to 1.00 amp.
- Set the timer to 5:00 minutes (300 seconds).
- Turn the ammeter on to run the experiment.
- Which metal is the anode? Which is the cathode?
- What is the initial mass of the anode? Of the cathode?
- What are the final masses of each electrode?
- Which increased in mass? Which decreased in mass?
- Which way do the electrons flow?
- Click the rerun button on the ammeter to repeat the experiment with these electrodes at least three more times
- 2.00 amps and 5 minutes
- 3.00 amps and 5 minutes
- 2.00 amps and 10 minutes
- For each run
- Record the starting masses of the anodes for each run.
- Record the final masses of the anodes for each run.
- How does changing the time affect the mass change?
- How does changing the current affect the mass change?
- Repeat the experiment with different electrodes.
Chat Preparation Activities
- Essay question: The Moodle forum for the session will assign a specific study question for you to prepare for chat. You need to read this question and post your answer before chat starts for this session.
- Mastery Exercise: The Moodle Mastery exercise for the chapter will contain sections related to our chat topic. Try to complete these before the chat starts, so that you can ask questions.
- Required: Complete the Mastery exercise with a passing score of 85% or better.
- Go to the Moodle and take the quiz for this chapter.
(Aligns to) AP LAB #16 GUIDED INQUIRY — — Building an Electrochemical cell — Phase III
Use your batteries (or commercial batteries) to observe the results of electrolysis on common molecules and rank results. Write and post your formal report.
- AP2009 20 Determination of Electrochemical Series
- AP2009 21 Measurements using electrochemical cells and electroplating
- IGHCE Lab 16.1 OR HSCKM X-1 Produce Hydrogen and Oxygen by Electrolysis of Water
- IGHCE Lab 16.2 OR HSCKM X-2 Observe the Electrochemical Oxidation of Iron
IGHCE Lab 16.3 OR HSCKM X-3 Measure Electrode Potentials
- IGHCE Lab 16.4 Observe Energy Transformation
- IGHCE Lab 16.5 OR HSCKM X-4 Build a Voltaic Cell
- IGHCE Lab 16.6 Build a Battery
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