Electrolytic Cells Notes. Source or use of electricity. Electrode. Cell. –. Molten or aqueous chemicals. +. –. +. –. +. Overview. In “electrolytic cells”, electricity is used to force chemicals to undergo a redox reaction
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Molten or aqueous chemicals
“Cells” are containers of liquid with electrodes:
The stoichiometry of electrolysis processes can quantify “how much chemical change occurs with the flow of a given current for a specific time”.
A coulomb is the amount of charge that passes a
given point when a current of one ampere (A) flows for one second.
1 ampere (amp) = 1 coulomb/second
1 faraday = 6.022 * 1023 electrons
1 faraday = 1 mole electrons
1.0 mole electrons = 96,485Coulombs
Example: Calculate the mass of palladium produced by the reduction of palladium (II) ions during the passage of 3.20 amperes of current through a solution of palladium (II) sulfate for 30.0 minutes.
Ch 17: 77ab, 79 ab, 81*
Electrochemistry Review Packet (with some more thermochemistry)