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ANACHEM > ANACHEM QUIZ (MODULE 11) > Flashcards

ANACHEM QUIZ (MODULE 11) Flashcards

1
Q

Relationship between chemical reaction and electricity.

A

electrochemistry

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2
Q

Measurement of current or voltage generated by the activity of an ion.

A

electrochemistry

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3
Q

techniques under Electrochemistry Analyses

A

Redox titration/titrimetry
Potentiometry
Amperometry
Polarography
Electrogravimetry
Voltammetry

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4
Q

Pair of electrodes in contact with an electrolyte solution.

A

electrochemical cell

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5
Q

one direction of flow of e-

A

direct current

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6
Q

Spontaneously produces current (or
energy) when the electrodes are
connected externally by a conducting
wire.

A

galvanic

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7
Q

tore electrical energy

A

galvanic

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8
Q

Current is forced by a battery or some
other external source of energy for
operation.

A

electrolytic cells

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9
Q

Consume electricity

A

electrolytic cells

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10
Q

Batteries are usually made from several
such cells connected in series to produce higher voltages than a single cell can produce.

A

galvanic

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11
Q

Oxidation or reduction reaction occurring at an electrode.

A

half cell reactions

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12
Q

The electrode at which oxidation occurs

A

anode

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13
Q

the electrode at which reduction occurs.

A

cathode

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14
Q

One in which the half-cell reactions are reversed by reversing the current flow; such a cell is said to be in thermodynamic equilibrium.

A

reversible cell

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15
Q

this consists of a platinum electrode coated with platinum black to catalyze the electrode reaction and over the surface of which hydrogen at 760 mm of mercury is passed.

A

standard hydrogen electrode

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16
Q

he potential of an electrode measured relative to a standard, usually the SHE.

A

electrode potential e

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17
Q

It is a measure of the driving force of the electrode reaction and is temperature and activity dependent.

A

electrode potential e

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18
Q

electrode potential measured in solutions where all reactants and products are at unit activity.

A

standard electrode potential

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19
Q

termed as “Redox Potential” which is one way of measuring how easily a substance loses e-

A

standard electrode potential

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20
Q

the algebraic sum of the individual electrode potentials of an electrochemical cell at zero
current.

A

theoretical cell potential

21
Q

When current flows in a cell or a liquid junction is present (vide infra) and for certain electrode systems or reactions, the cell potential departs from the theoretical value.

A

theoretical cell potential

22
Q

potential developed across a boundary
between electrolytes differing in concentration or chemical composition

A

liquid-junction potential

23
Q

A potential developed when a current/flows in an electro-chemical cell.

A

ohmic drop, ir

24
Q

the amount of potential that is lost on the way from the reference electrode to the working electrodes.

A

ohmic drop, ir

25
Q

t is always subtracted from the theoretical cell potential and therefore reduced that of a galvanic cell and increases the potential required to operate an electrolysis cell.

A

ohmic drop, ir

26
Q

the additional potential required to cause some electrode reaction to proceed at an appreciate rate.

A

activation overpotential

27
Q

The result of an ‘energy barrier’ to the electrode reaction concerned, it is substantial for gas evolution and for electrodes made of soft metals
(ex. Hg, Pb, Sn, Zn)

A

activation overpotential

28
Q

the additional voltage that is needed to carry out electrolysis in addition to the standard cell potential.

A

CONCENTRATION OVERPOTENTIAL

29
Q

to maintain a current flowing in a cell when the concentration of the electroactive species at the electrode surface is less than that in the bulk solution.

A

CONCENTRATION OVERPOTENTIAL

30
Q

In an oxidation/reduction electrons are
transferred from one reactant to another.

A

reduction on reaction

31
Q

electron donor.

A

reducing agent

32
Q

species that donate the electron.

A

reducing agent

33
Q

electron acceptor

A

oxidizing agent

34
Q

Substance that has strong affinity of electron

A

oxidizing agent

35
Q

something that permit something to happen.

A

agent

36
Q

species having charges

A

ions

37
Q

neutral charge

A

atoms

38
Q

isolates the reactants but
maintains electrical contact between the two halves of the cell.

A

salt bridge

39
Q

an electrolyte where reduction
occurs.

A

cathode

40
Q

an electrolyte where oxidation
occurs.

A

anode

41
Q

Types of Electrochemical Cells

A

galvanic cells
electrolytic cells

42
Q

used to sense the
presence or change in concentration of the oxidized and reduced forms of a redox couple.

A

indicator electrode

43
Q

has a stable and well-known electrode potential.

A

reference electrode

44
Q

2 types of electrodes

A

indicator electrodes
reference electrode

45
Q

the electrode consists of two concentric glass tubes, the inner one of which contains mercury in contact with a paste of mercury, mercury(I)
chloride (calomel), and potassium chloride.

A

calomel electrode

46
Q

This is in contact with a solution of potassium chloride in the outer tube which itself contacts the sample solution via a porous frit, fiber, or
ground-glass sleeve.

A

calomel electrode

47
Q

consist of a silver wire, coated with silver chloride and in contact with a solution of potassium chloride saturated with silver chloride.

A

silver silver chloride electrode

48
Q

The solution is contained in a tube, the end of which is sealed with a porous plug or disc to facilitate contact with the sample solution.

A

silver silver chloride electrode

ANACHEM (6 decks)

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