Use the formula E(cell) = E (cathode) - E(anode). Determine that when the total is positive, the reaction is product favored. Use table 19.1 to demonstrate that the more positive the E total, the better the oxidizing ability. The more negative the value of reduction potential, the less likely the 1/2 reaction will occur.

Measurement depends on half cell and net reaction, the concentration of reactants and products, and the pressure and temperature of gaseous reactants. Determination of standard potential, Ecell, is performed under standard conditions. The standard hydrogen electrode (SHE) is the favored reaction. The reduction of hydrogen at the electrode and the oxidation of zinc at the anode are listed as half reactions. The potential energy of this reaction produces a reading of 0.76 volts as standard.

Demonstrate in the lab the electrolysis of water, which is the reverse of how a battery works. Electrolysis uses electricity to produce chemical energy. Introduce electromotive force, EMF, as the difference in potential energy of electrons at the electrodes. Define it as the force needed to move the electrons between the electrodes. Define the units as volts. Define what one volt as 1 joule/ coulomb.

Label, define and describe the make up of the voltaic cell diagram, Write Both half cell formulas and then the net formula, Discuss the importance of the salt bridge. Have Joshua sketch a second voltaic cell using a different chemical formulation, label and describe each cell part. Introduce commercial voltaic cells (batteries). Use sketches of dry cells and describe the anode and cathode reactions, along the the paste needed transfer the electrons.

Joshua read Chapter 33 in the Conceptual Physics

Define voltaic cells. Discuss that they all use product favored redox reactions to convert chemical energy into electrical energy. Use a diagram of a typical voltaic cell to label and explain the chemical process which will occur in each half cell.

Use a series of equilibrium reactions to determine the reaction quotient and equilibrium expression. Compare both numbers. Analyze Which reactions have reached equilibrium and why. Determine in which direction the reaction must proceed in order to obtain equilibrium. List and discuss the effect of changing conditions on the equilibrium system. Use examples for each one.

Review and outline what is not included in the equilibrium expression. Use chemical reaction examples. Write the equilibrium expression for some examples of reactions. Analyze the reactions when the Keq is large, equals 1, or is small. Introduce the reaction quotient formula and compare it to the equilibrium formula.

Discuss the equilibrium constant and the rate quotient . Use the formula to determine the equilibrium constant for a given reaction given the initial concentrations and the change in concentration over time. Write the equilibrium expression for a generalized reaction at equilibrium. Discuss reactions which deviate from the normal equilibrium constant expression. These would include reactions which involve a solid and reactions which involve water as the solvent

Display and discuss a reaction in which a precipitate is formed and a gas is released into the atmosphere. Have Joshua write and balance the equation, and note the reactants and products. Describe the reverse reaction. Discuss the reaction which would happen in a closed container. List and discuss the results in the closed container. Define the reaction occurring until equilibrium is reached. Note no change occurs after equilibrium. List and discuss the 4 generalizations which occur with this reaction.Write, define and analyze th equilibrium constant for a given reaction