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Questions: https://docs.google.com/document/d/1KnkO62NCCHOnkUzL5LABgGxtGpfl5IEwJs8NdjJgkVA/edit?usp=sharing

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Pay attention to the base of all logarithms used to solve for cell potential, and ensure they correspond with the constants given.

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The Universal Gas Constant must be expressed in Joules per mole per Kelvin to be utilized in the Nernst Equation

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Standard Reduction potentials are only applicable at standard conditions.

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A chemistry cell is different from a cell in biology class.

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The cathode is the metal with the higher reduction potential in a galvanic cell, but is the metal with the lower reduction potential in a electrolytic cell.

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Reduction occurs at the cathode

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Electrons always flow from anode to cathode.

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Cell potential depends on concentration

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△G°= -nFE

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Units:

E: cell potential (V or J/C)

E°: standard cell potential ( V or J/C)

w: work (VC or J)

q: charge (C)

R: Universal Gas Constant (8.314 J/molK)

K: equilibrium constant

T: temperature

Q: reaction quotient

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Line Notation
Anode | Anode Solution || Cathode Solution | Cathode

| = phase boundary

|| = salt bridge

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Steps to Balancing Redox Reactions:

1. write the two half-reactions

2. balance elements except for O and H

3. balance O by adding water to other side

4. balance H by adding H⁺ to other side

5. balance charges by adding electrons

6. add two half-reactions and cancel like terms (if the reaction is in basic solution)

7. convert H⁺ to water by adding OH⁻

8. put together/cancel water

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Use half-reactions to balance redox reactions

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E = -w/q

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Battery - galvanic cells where potentials of individual cells give total battery potential

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Electroplating - using electrolysis to deposit neutral metal on an electrode by reducing metal ions in solution

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Electrolysis - electrical energy added and forces a non-spontaneous reaction to occur

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Nernst Equation:

Ecell = E°cell - RT/nF * ln(Q)

Ecell = E°cell - .0257/n * ln(Q)

Ecell = E°cell - .0591/n * log(Q)

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Concentration Cells - galvanic cell with electrode and solutions but different concentrations

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E°cell = E°cathode - E°anode

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Standard Reduction Potential (E°) - E° values corresponding to reduction half-reactions with solutes at 1M and all gases at 1atm

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Cell Potential (E) - driving force aka emf

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Anode - oxidized metal
cathode - reduced metal
Oxidation - loss of electrons
Reduction - gain of electrons
Salt Bridge - closes circuit by connecting half cells

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Galvanic/Voltaic Cell - electrochemical cells where spontaneous redox reactions produce electricity

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Oxidation Number - charge an atom would possess if it were ionic

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Redox Reaction - transfer of electrons between two species