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WGU-Organic Chem 5

Electrochemistry

QuestionAnswer
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