Electrochemical Cells

Question 1

Anode

Answer 1

Electrode of a voltaic or electrolytic cell where oxidation (loss of electrons) occurs.

Question 2

Cathode

Answer 2

Electrode of a voltaic or electrolytic cell where reduction (gain of electrons) occurs.

Question 3

Cathodic Protection

Answer 3

Effective method of preventing corrosion of iron in which the iron is forced to become the cathode by using either impressed current or a sacrificial anode.

Question 4

Corrosion

Answer 4

Electrochemical process in which a metal reacts with substances in the environment, returning the metal to an ore-like state (metal becomes an oxide- is oxidized).

Question 5

Electrical Current (I)

Answer 5

A measure of the rate of fow or charge past of point in an electrical circuit; measured by an ammeter in amperes (A).

Question 6

Electric Potential Difference (V)

Answer 6

The energy difference, per unit charge, between any two points in an electrical circuit; measured in volts (V); also called voltage.

Question 7

Electrode

Answer 7

A solid electrical conductor.

Question 8

Electrolysis

Answer 8

The process of supplying electrical energy to force a non-spontaneous redox reaction to occur.

Question 9

Electrolyte

Answer 9

A substance that conducts electricity in aqueous solution; also a liquid such as a molten solid that conducts electricity.

Question 10

Electrolytic Cell

Answer 10

A cell in which a non-spontaneous redox reaction is forced to occur; a combination of two electrodes, an electrolyte, and an external power source.

Question 11

Faraday Constant (F)

Answer 11

The quantity of charge transferred for every mole of electrons that flows in the cell; 9.65 x 10^4 C/mol

Question 12

Faraday’s Law

Answer 12

The statement: the mass of an element produced or consumed at an electrode is directly proportional to the time the cell operates, as long as the current is constant or vice versa.

Question 13

Fuel Cell

Answer 13

An electric cell that produces electricity by the reaction of a fuel that is continuously supplied to keep the cell operating.

Question 14

Half-cell

Answer 14

An electrode-electrolyte combination forming one-half of a complete cell.

Question 15

Inert Electrode

Answer 15

An unreactive solid conductor in a cell that provides a location to connect a wire and a surface on which a half-reaction can occur.

Question 16

Porous Boundary

Answer 16

A physical barrier separating two electrolytes while still permitting ions to move between the two solutions through tiny openings.

Question 17

Primary Cell

Answer 17

A cell that cannot be recharged, usually due to irreversible side reactions.

Question 18

Reference Half-Cell

Answer 18

A half-cell that is chosen as a reference and is arbitrarily assigned an electrode potential of exactly zero volts; a standard hydrogen electrode.

Question 19

Secondary Cell

Answer 19

A rechargeable cell.

Question 20

Standard Cell

Answer 20

A voltaic cell in which each half-cell contains all entities in the half-reaction equation at SATP conditions, with a concentration of 1.0 mol/L for the aqueous solutions

Question 21

Standard Cell Potential

Answer 21

The maximum electrical potential difference (voltage) of the cell operating under standard conditions; the energy difference (per unit of charge) between the cathode and the anode.

Question 22

Standard Reduction Potential

Answer 22

The ability of a standard half-cell to attract/gain electrons under standard conditions.

Question 23

Voltaic Cell

Answer 23

An arrangement of two half-cells, separated by a porous boundary, that spontaneously produces energy.