Ch 18 Introduction to Electrochemistry Flashcards

1
Q

electrons are transferred from one reactant to
another.

A

oxidation/reduction reaction e

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2
Q

A substance that has a strong affinity for electrons

A

oxidizing agent,

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3
Q

Species that donates electrons to another species.

A

Reducing agent

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4
Q

the reaction is carried out in an ____________ in which the reactants do not come in direct contact with one another.

A

electrochemical cell

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5
Q

are widely used in electrochemistry to prevent
mixing of the contents of the two electrolyte solutions making up electrochemical cells.

A

Salt bridges

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6
Q

A unique aspect of oxidation/reduction reactions is that the transfer of
electrons, and thus an identical net reaction, can often be brought about in an ____________ in which the oxidizing agent and the reducing agent are physically separated from one another

A

electrochemical cell

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7
Q

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

A

salt bridge

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8
Q

When a voltmeter of high internal resistance is connected as
shown or the electrodes are not connected externally, the cell is said to be at _________ and delivers the full cell potential

A

open circuit

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9
Q

A circuit where no net reaction
occurs in the cell, although we shall show that the cell has the potential for doing
work.

A

open circuit

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10
Q

The voltmeter measures the potential difference, or _________, between the two
electrodes at any instant.

A

voltage

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11
Q

is a measure of the tendency of the cell reaction to proceed toward equilibrium.

A

voltage

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12
Q

In a salt bridge, the two ends of the bridge are
fitted with ____________ to prevent liquid from siphoning from one part of the cell to
the other.

A

sintered glass disks/ porous materials

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13
Q

The equilibrium-constant
expression

A

Keq = oxidized/ reduced

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14
Q

As the reaction goes on in an electrochemical cell, the cell potential, when the circuit is open, _________ and approaches ____________
as the overall reaction approaches equilibrium.

A

decreases continuously , zero

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15
Q

The electrodes in some cells share a
common electrolyte; these are known
as

A

cells without liquid junction

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16
Q

An electrochemical cell consists of two conductors

A

electrodes

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17
Q

is an electrode where
reduction occurs.

A

cathode

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18
Q

is an electrode where oxidation occurs.

A

anode

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19
Q

Types of Electrochemical Cells

A

galvanic or electrolytic cells

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20
Q

The cell that store electrical energy

A

Galvanic cells

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21
Q

The cell that consume electricity

A

electrolytic cells

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22
Q

are usually made from galvanic cells connected in series to produce higher voltages than a single cell can produce

23
Q

Galvanic cells operate spontaneously, and the net reaction during discharge is called the

A

spontaneous cell reaction.

24
Q

in contrast to a voltaic cell, requires an external source of
electrical energy for operation.

A

electrolytic cell

25
reversing the current reverses the cell reaction.
reversible cell
26
reversing the current causes a different half-reaction to occur at one or both of the electrodes.
irreversible cell
27
was one of the earliest galvanic cells to find widespread practical application. It was used in the mid-1800s to power telegraphic communication systems.
Daniell Gravity Cell
28
In the shorthand notation to describe electrochemical cells, a single vertical line indicates a _________ at which a potential develops
phase boundary
29
In the shorthand notation to describe electrochemical cells, the double vertical lines represent _____, one at each end of the salt bridge
two-phase boundaries
30
The junction potential results from differences in the rates at which the ions in the cell compartments and the salt bridge migrate across the interfaces.
liquid-junction potential
31
A liquid-junction potential can amount to as much as several hundredths of a volt but can be negligibly small if the electrolyte in the salt bridge has an anion and a cation that migrate at nearly the same rate. A saturated solution of _____________is the electrolyte that is most widely used.
potassium chloride, KCl
32
___________ carry the charge within the electrodes as well as the external conductor. Notice that by convention, __________, which is normally indicated by the symbol I, is opposite in direction to electron flow
Electrons, current
33
are the charge carriers within the cell
Anions and cations
34
The phase boundary between an electrode and its solution is called an .
interface
35
Equation than relates the cell potential, Ecell, to the free energy of the reaction, to the equilibrium constant
△G = -nFEcell = -RT ln Keq
36
The ____ of a substance is a reference state that allows us to obtain relative values of such thermodynamic quantities as free energy, activity, enthalpy, and entropy
standard state
37
If the reactants and products are in their standard states, the resulting cell potential is called the
standard cell potential
38
This rule implies that we always measure the cell potential by connecting the positive lead of the voltmeter to the right-hand electrode in the schematic or cell drawing
plus right rule.
39
The leads of voltmeters are color coded. The__________ is red, and the _________ is black.
positive lead, common lead
40
The reaction is not spontaneous cell reaction when Ecell is _________, and △G is thus _______.
negative, positive
41
This generally agreed-upon reference half-cell against which all others are compared. Such an electrode must be easy to construct, reversible, and highly reproducible in its behavior. The universal reference electrode
standard hydrogen electrode (SHE)
42
The standard hydrogen electrode is sometimes called the
normal hydrogen electrode (NHE).
43
The metal conductor is a piece of platinum that has been coated, or ______________, with finely divided platinum (platinum black) to increase its specific surface area.
platinized
44
______ is a layer of finely divided platinum that is formed on the surface of a smooth platinum electrode by electrolytic deposition of the metal from a solution of chloroplatinic acid, H2PtCl6. It provides a large specific surface area of platinum
Platinum black
45
The assigned value for the potential of standard hydrogen electrode (SHE) at all temperatures
0.000 V
46
is defined as the potential of a cell in which the electrode in question is the right-hand electrode and the standard hydrogen electrode is the left-hand electrode
electrode potential
47
of a half-reaction is defined as its electrode potential when the activities of the reactants and products are all unity
standard electrode potential, E^0
48
A metal ion/metal half-cell is sometimes called a .
couple
49
An ___________is by definition a reduction potential or the half-reactions written as reductions
relative electrode potential
50
An_______________is a measure of the extent to which the concentrations of the species in a half-cell differ from their equilibrium values
electrode potential
51
The _______________for a half-reaction, E^0, is defined as the electrode potential when all reactants and products of a half-reaction are at unit activity.
standard electrode potential
52
A ______________is the electrode potential when the ratio of analytical concentrations of reactants and products of a half-reaction are exactly 1.00 and the molar concentrations of any other solutes are specified. To distinguish the formal potential from the standard electrode potential a prime symbol is added to E^0' .
formal potential
53
are empirical potentials that compensate for the types of activity and competing equilibria effects that we have just described.
formal potential