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WGU-Organic Chem 5
Electrochemistry
| Question | Answer |
|---|---|
| reducing agent | the substance that is losing electrons in a redox reaction by supplying another substance with electrons to reduce the other substance |
| oxidizing agent | the substance that is gaining electrons in a redox reaction by taking electrons from another substance undergoing oxidation |
| electrode | a conducting substance that allows electrons to be transferred between an aqueous phase and an external circuit either active or passive |
| anode | electrode within an electrochemical cell where oxidation occurs |
| cathode | electrode within an electrochemical cell where reduction occurs |
| galvanic cell | electrochemical cell that contains components of a spontaneous reaction, whose electron flow can be used as an energy source (e.g. a battery) |
| cell potential | The standard reduction potential of the cathode minus the standard reduction potential of the anode |
| pH meter | instrument that uses differences in standard cell potentials to determine the concentration of hydronium ion in a given solution |
| oxidation | loss of electrons |
| reduction | gain of electrons |
| oxidation number | charge that an atom would have if 100% ionic bonding were assumed |
| standard reduction potential | measure of the tendency that a substance has to undergo reduction under standard conditions(1 M, 1 atm, 25 degrees Celsius) |
| equation for calculation standard potential for a galvanic cell | E(cell)=E(oxidized anode)-E(reduced cathode) |
| equation for calculating the quantity of chemical change given the electrical charge, time, and Faraday constant | W=(IxtxA)/(nxF) where F is Faradays constant 96,485.309 coulombs/equivalent |
| equation for determining pH value of a sample given the electrode potential | electrode cell potential/.0592 |
| why does oxidation and reduction always occur together? | because electrons flow from one to the other and matter can not be destroyed but transferred |
| why must ions be present in an aqueous phase of a galvanic cell? | to attract or repel electron flow |
| describe how to identify oxidizing agents | oxidizing agents are reduced or gain electrons |
| describe how to identify reducing agents | reducting agents are oxidized or lose electrons |
| describe how to calculate the quantity of chemical change given charge and time | weight of plated metal(grams)equals current(coulombs per second or ampere)* time(seconds) *atomic weight(grams per mole)/ moles / Faradays constant(96,485.309 coulombs) |
| RED CAT | mnemonic to remember reduction occurs at the cathode (+) gains electrons |
| AN OX | mnemonic to remember oxidation occurs at the anode (-) loses electrons |
Created by:
elainero
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