Electrochemistry

Question 1

Is a device that can generate electrical energy from the chemical reactions occurring in it. Also called galvanic cells or Voltaic cells.

Answer 1

electrochemical cell

Question 2

It is defined as a chemical reaction involving the transfer of electrons between two electrodes in an electrochemical cell

Answer 2

electrochemical process

Question 3

Late 18th century, he discovered the bimetallic driving force

Answer 3

Luigi Galvani

Question 4

In 1800, he invented first electrical cell, or battery: a series of metal disks of two kinds, separated by cardboard disks soaked with acid or salt solutions.

Answer 4

Alessandro Volta

Question 5

Early 19th century- He engineered into the useful protection of metallic structures.

Answer 5

Sir Humphry Davy

Question 6

It is the tendency for an electrode to lose or gain electrons when dipped in the solution of its ions.

Answer 6

electrode potential

Question 7

A device used in an electrochemical cell for connecting its oxidation and reduction half cells wherein an inert electrolyte is used

Answer 7

salt bridge

Question 8

It is a medium that provides the ion transport mechanism between the cathode and anode of a cell.

Answer 8

electrolyte

Question 9

Type of electrochemical cell which involve different types of metals/ nonmetal composition coming into contact, leading to electron transfer between them.

Answer 9

dissimilar electrode cell

Question 10

Type of electrochemical cell with two identical electrodes, each in contact with a solution of different composition

Answer 10

salt concentration cell

Question 11

Type of electrochemical cell when two identical electrodes are immersed in same electrolyte, but the electrodes are immersed into solution of two different temperatures.

Answer 11

differential temperature cell

Question 12

A list that describes the arrangement of elements in the order of their increasing electrode potential values.

Answer 12

electrochemical series

Question 13

An orderly arrangement of the standard potentials for all metals

Answer 13

electromotive force series/ galvanic series

Question 14

It is use in the standard hydrogen electrode since it is relatively inert, has catalytic qualities, surface can be platinized, and improve reaction kinetics.

Answer 14

platinum

Question 15

Pure mercury is placed at the bottom of the tube, which is covered with a paste of mercury-mercurous chloride. Pure mercury covers a platinum wire sealed through the bottom of a glass tube.

Answer 15

calomel reference electrode

Question 16

It is composed of a silver wire, sometimes coated with a layer of solid silver chloride

Answer 16

silver-silver chloride reference electrode

Question 17

It consists of a metallic copper immersed in saturated copper sulfate. It is use where the electrode must be resistant to shock.

Answer 17

saturated copper-copper sulfate reference electrode

Question 18

Relate the current of an electrochemical reaction to the number of moles of the element being reacted and the number of moles of electrons involved.

Answer 18

Faraday’s law of electrolysis

Question 19

If Sc/Sa is > 1

Answer 19

amplifying factor

Question 20

If Sc/Sa is < 1

Answer 20

stifling factor

Question 21

____ occurs when the electrolyte resistance is so high that the resultant current is not sufficient to polarize anodes or cathodes

Answer 21

resistance control

Question 22

The _____ can be calculated from the corrosion potential and the thermodynamic potential

Answer 22

corrosion current

Question 23

If the metal is polarized slightly beyond the open-circuit potential of the anode, the corrosion rate remains ____.

Answer 23

zero