Busy. Please wait.
or

show password
Forgot Password?

Don't have an account?  Sign up 
or

Username is available taken
show password

why


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.


Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.

Remove ads
Don't know
Know
remaining cards
Save
0:01
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
Retries:
restart all cards




share
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

ch 20 vocab

TermDefinition
electrochemistry the branch of chemistry that deals with the relationships between electricity and chemical reactions
reducing agent (reductant) the substance that is oxidized and thereby causes the reduction of some other substance in an oxidation reduction reaction
oxidizing agent (oxidant) the substance that is reduced and thereby causes the oxidation of some other substance in an oxidation reduction reaction
half-reactions an equation for either a oxidation or a reduction that explicitly shows the electrons involved
voltaic (galvanic) cell a device in which a spontaneous oxidation-reduction reaction occurs with the passage of electrons through an external circuit
anode an electrode at which oxidation occurs
cathode an electrode at which reduction occurs
electromotive force (emf) a measure of the driving force, or electrical pressure, for the completion of an electrochemical reaction. also called the cell potential
cell potential (E sub cell) a measure of the driving force, or electrical pressure, for an electrochemical reaction. also called electromotive force
standard emf (standard cell potential, E knot sub cell) the emf of a cell when all reagents are at standard conditions
standard reduction potential (E knot sub red) the potential of a reduction half-reaction under standard conditions, measured relative to the standard hydrogen electrode. also called standard electrode potential
standard hydrogen electrode (she) an electrode based on the half-reaction 2H+(1M) + 2e- --> H2(1atm). the standard electrode potential of the standard hydrogen electrode is defended as 0V
faraday a unit of charge that equals the total charge of one mole of electrons: 1F = 96,500C
nernst equation an equation that relates the cell emf, E, to the standard emf, E knot, and the reaction quotient
concentration cell a voltaic cell containing the same electrolyte and the same electrode materials in both the anode and cathode compartments. the emf of the cell is derived form a difference in the concentrations of the same electrolyte solutions in the comportments
battery a self-contained electrochemical power source that contains one or more voltaic cells
fuel cell a voltaic cell the utilizes the oxidation of a conventional fuel
corrosion the process by which a metal is oxidized by a sharing of electrons
cathodic protection a means of protecting a metal against corrosion by making it the cathode in a voltaic cell.
electrolysis reaction a reaction in which a non spontaneous redox reaction is brought about by the passage of current under a sufficient external electrical potential. the devices in which electrolysis reactions occur are called electrolytic cells
electrolytic cell a device in which a non spontaneous oxidation-reduction reaction is caused to occur by passage of current under a sufficient external electrical potential
watt a unit of power 1W = 1 J/s
Created by: agloskowski