In this lecture you will learn about Electrochemical Cells and Half-Cell Potentials. First you will cover Electricity from Chemical Reactions by looking at Galvani Volta's concept of Current Electricity, the Voltaic Pile or Battery, and the Potato Clock. Next you will examine the Daniell Cell with its Oxidation of Zinc and Reduction of Copper, and the introduction of concepts such as Spontaneous Overall Reaction, Anode, and Cathode. After that, you will learn about Current Electricity Fundamentals such as the Electric Charge of a Coulomb, Electric Current of an Ampere, Volt, and Ohm's Law. Then you will learn about the Galvanic Cell and its use of the Salt Bridge before looking at Cell Potential and Work which bring back Joules and Coulombs. After, you will look at the Hydrogen Electrode, Half-Cell Potentials and the Electrochemical Series. Lastly you will investigate the Nernst Equation and its applications on the pH Meter and Ion Concentrations.
half-reactions can be made into half-cell electrodes
half-cells gives galvanic or electrochemical cells; chemical
reactions give electric current
a salt-bridge to conduct ions and balance charges
of half-cell potentials is standard hydrogen electrode, SHE
is half-cell potentials are for reduction half reactions
of half-cell potentials is electrochemical series; shows good
oxidizing and reducing agents
= 0.0592VlogK/n n=no. of electrons transferred
equation for non-standard conditions: E = E0
0.0592VlogQ/n; Q = reaction quotient
meter shows use of Nernst equation
ion electrodes for measuring ion concentrations ia Nernst equation
Electrochemical Cells, Half-Cell Potentials
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