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Electrochemistry

TermDefinition
Oxidation Loss of electrons
Reduction Gain of electrons
Oxidizing agent Species that causes other species to be oxidized, or the species that is reduced
Reducing agent Species that causes the other species to be reduced, or the species that is oxidized
Anode The species in a galvanic cell that is oxidized
Cathode The species in a galvanic cell that is reduced
In a galvanic cell, electrons flow from ___ to ___. anode to cathode
In a galvanic cell with a salt bridge, ___ ions flow to the anode and ___ ions flow to the cathode negative ions (anions) to anode, positive ions (cations) to cathode
In a galvanic cell with a porous disc, ___ ions flow to the anode. negative ions (anions)
A spontaneous reaction must have a ____ sign on the cell potential positive
The Faraday Constant 96,485 C/mol e-
The equation for finding the free energy of an electrochemical reaction deltaG = - n * F * E where n is the number of moles of electrons transferred, F is the Faraday constant, and E is the total cell potential
Order of steps when balancing a simple redox reaction 1. Write half-reactions 2. Balance atoms 3. Balance charges by adding electrons 4. Multiply equations to have same number of electrons on either side 5. Cancel electrons 6. Add half-reactions together
Order of steps when balancing a complex redox reaction in acidic solution 1. Write half-reactions 2. Balance atoms 3. Balance oxygens by adding H2O 4. Balance hydrogens by adding H+ 5. Balance charges by adding e- 6. Multiply equations to have same number of electrons on either side 7. Cancel e- 8. Add half-reactions
Order of steps when balancing a complex redox reaction in basic solution 1. Write half-rxns 2. Balance atoms 3. Balance Os by adding H2O and Hs by adding H+ 5. Balance charges by adding e- 6. Multiply to have same # of e- on each side 7. Cancel e- 8. Add half-rxns 9. Add OH- to each side matching # of H+ 10. Cancel H2O
Created by: shudonmiller
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