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| 5854466042 | Electrochemistry | the study of the interchange of chemical and electrical energy | 0 | |
| 5854466043 | OIL RIG | oxidation is loss, reduction is gain (of electrons) | 1 | |
| 5854475630 | Salt bridge | Bridge between cells; provide ions to balance the charge |  | 2 |
| 5854476636 | Faraday's Law: | The amount of a substance being oxidized or reduced at each electrode during electrolysis is directly proportional to the amount of electricity that passes through the cell. | 3 | |
| 5854477109 | Reduction | the gain of electrons reduction of charge | 4 | |
| 5854478751 | Oxidation number | the assigned charge on an atom | 5 | |
| 5854479515 | Oxidizing agent (OA) | the species that is reduced and thus causes oxidation | 6 | |
| 5854486816 | n in the Nernst equation | n = the # of electrons exchanged in the balanced redox equation Got it? | 7 | |
| 5854488209 | Q in the Nernst equation | Q = reaction quotient (Use the coefficients) [products] / [reactants] (I don't actually know what this means) | 8 | |
| 5854492816 | F in the Nernst equation | Faraday constant - i'm sure it's on detail somewhere | 9 | |
| 5854495760 | R in Nernst equation | 9.315 J/K x mol Gas constant | 10 | |
| 5854477892 | Nernst Equation | E = E cell - (RT/nF ) lnQ Fun fact! When the cell is not at standard conditions, use this equation | 11 | |
| 5854480183 | Reducing agent (RA) | the species that is oxidized and thus causes reduction | 12 | |
| 5854488778 | inert electrodes | used when a gas is involved OR ion to ion involved such as Fe3+ being reduced to FE2+ rather than Fe0. Made of Pt or graphite | 13 | |
| 5854494338 | electron flow | always from anode to cathode (through the wire) | 14 | |
| 5854498651 | voltmeter | measures the cell potential (emf) usually is measured in volts | 15 | |
| 5854494921 | standard cell notation (line notation) | anode/solution//cathode solution/cathode ex. Zn/Zn2+(1.0M)//Cu2+(1.0M)/Cu | 16 | |
| 5854491485 | salt bridge | a device used to maintain electrical neutrality in a galvanic cell. may be filled with agar which contains a neutral salt or it may be replaced with a porous cup. | 17 | |
| 5854482465 | Galvanic (voltaic) cells | spontaneous chemical reactions (battery) | 18 | |
| 5854486934 | cathode | the anode where reduction occurs may become larger over time as ions from the solution plates onto it | 19 | |
| 5854492653 | number of coulombs | amp ( I ) x time | 20 | |
| 5854488833 | Formula weight | grams/mole | 21 | |
| 5854483844 | Electrolytic cells | non-spontaneous require external electron source (DC power source) | 22 | |
| 5854503620 | 23 | |||
| 5854484900 | anode | the electrode where oxidation occurs may become smaller over time as it falls into solution | 24 | |
| 5854487262 | Balanced redox equations | number of moles of electrons/mole of substance | 25 | |
| 5854476363 | Lead- storage batteries | Pb anode, PbO2 cathode, H2SO4 electrolyte | 26 | |
| 5854489107 | electroplating | one type of application of electrolytic cells; it applies a thin layer of an expensive metal to a less expensive one | 27 | |
| 5854476356 | Oxidation | the loss of electrons increase in charge | 28 | |
| 5854491820 | Electrons in a voltaic/galvanic cell always flow from __________ to _____________ | Anode to Cathode | 29 | |
| 5854489438 | Reduction occurs at the... | Cathod (RED CAT) - mass increase | 30 | |
| 5854487556 | Oxidation occurs at the... | Anode (AN OX) - mass decrease | 31 | |
| 5854484341 | Faraday | 96,500 Coulombs/mole of electrons | 32 | |
| 5854482987 | 1 Amp | 1 Coulomb/second | 33 | |
| 5854502080 | Voltmeter | - measures electrical potential, some energy is lost as heat which keeps the voltmeter reading a tad lower than the actual or calculated voltage. |  | 34 |
| 5854480362 | 1 Volt | 1 Joule/Coulomb | 35 | |
| 5854495918 | Cell potential (Ecell, Emf) | It is a measure of the electromotive force or the "pull" of the electrons as they travel from the anode to the cathode | 36 | |
| 5854486602 | Batteries | cells connected in series; potentials add together to give a total voltage | 37 | |
| 5854488151 | Faraday | 96500 Coulombs/mole of electrons | 38 | |
| 5854487354 | 1 amp | 1 Coulomb/second | 39 | |
| 5854478986 | dry cell batteries | acid versions: Zn anode, C cathode; MnO2 and NH4Cl paste alkaline versions: some type of basic paste, ex. KOH Nickel - Cadmium - anode and cathode can be recharged | 40 | |
| 5854492203 | Porous disk or cup | allows both cells to remain neutral by allowing ions to flow | 41 | |
| 5854486838 | 1 volt | 1 Joule/Coulomb | 42 | |
| 5854482818 | Fuel cells | reactants continuously supplied (spacecraft - hydrogen and oxygen) | 43 | |
| 5854485143 | Faraday's law | the amount of a substance being oxidized or reduced at each electrode during electrolysis is directly proportional to the amount of electricity that passes through the cell | 44 | |
| 5854490677 | corrosion | process of returning metals tot heir natural state, the ores | 45 |
