Chapter 16: Introduction to Electrochemistry

Question 1

sometimes called redox reactions

Answer 1

oxidation/ reduction reactions

Question 2

is an electron donor

Answer 2

reducing agent

Question 3

is an electron acceptor

Answer 3

oxidizing agents

Question 4

A substance that has a strong affinity for electrons

Answer 4

oxidizing agent

Question 5

donates electrons to another species

Answer 5

reducing agent

Question 6

Oxidation/reduction reactions can be viewed in a way that is analogous to the

Answer 6

Bronsted Lowry concept

Question 7

TRUE or FALSE
When an acid donates a proton, it becomes a conjugate base that is capable of accepting a proton

Answer 7

TRUE

Question 8

TRUE or FALSE
when a reducing agent donates an electron, it becomes an oxidizing agent
that can then accept an electron.

Answer 8

TRUE

Question 9

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

Answer 9

electrochemical cell

Question 10

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

Answer 10

salt bridge

Question 11

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

Answer 11

open circuit

Question 12

When the circuit is open, no net reaction occurs in the cell, although we shall show that the cell has the ________ for doing work

Answer 12

potential

Question 13

voltmeter measures what

Answer 13

potential difference or voltage, between two electrodes ar any instant

Question 14

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

Answer 14

voltage

Question 15

TRUE or FALSE
A cell with zero voltage does not
perform work, as anyone who has found a “dead” battery in a flashlight or in a laptop
computer can attest.

Answer 15

TRUE

Question 16

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

Answer 16

cells without liquid junction

Question 17

is an electrode where
reduction occurs

Answer 17

cathode

Question 18

electrode where oxidation occurs

Answer 18

anode

Question 19

An electrochemical cell consists of two conductors called

Answer 19

electrodes

Question 20

TRUE or FALSE
The most common way of avoiding mixing is to insert a salt bridge, between solutions

Answer 20

TRUE

Question 21

stores electrical energy or also known as voltaic cells

Answer 21

galvanic cells

Question 22

consume electricity

Answer 22

electrolytic cells

Question 23

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

Answer 23

batteries

Question 24

TRUE or FALSE
There is a liquid junction potential at each interface of cell notation

Answer 24

TRUE

Question 25

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

Answer 25

spontaneous cell reaction

Question 26

In this cell, reversing the current reverses the cell
reaction when the direction of flo is changed

Answer 26

reversible cell

Question 27

In this cell, reversing the current causes a
different half-reaction to occur at one or both of the electrodes.

Answer 27

irreversible cell

Question 28

was one of the earliest galvanic cells to find widespread practical application

Answer 28

Daneill gravity cell

Question 29

The phase boundary between an
electrode and its solution is called an

Answer 29

interface

Question 30

If the reactants and products are in their standard states, the resulting cell potential is called the

Answer 30

standard cell potential

Question 31

is a reference state that allows
to obtain relative values of such
thermodynamic quantities as free
energy, activity, enthalpy, and
entropy. All substances

Answer 31

standard state

Question 32

formula of delta G

Answer 32

delta G= -nFEcell =-RTln Keq

Question 33

requires an external source of electrical energy for operation

Answer 33

electrolytic cell

Question 34

meets specifications such as an electrode must be easy to construct, reversible, and highly reproducible in its behavior, which has been used throughout the world for many years as a universal reference electrode and is a typical gas electrode

Answer 34

standard hydrogen electrode

Question 35

The standard hydrogen electrode
is sometimes called the

Answer 35

normal hydrogen electrode

Question 36

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,

Answer 36

platinum black

Question 37

TRUE or FALSE
By convention, the potential of
the standard hydrogen electrode is assigned a value of 0.000 V at all temperatures

Answer 37

TRUE

Question 38

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.

Answer 38

electrode potential

Question 39

is defined as its electrode potential when the activities of the reactants and products are all unity

Answer 39

standard electrode potential

Question 40

A metal ion/metal half-cell is
sometimes called a

Answer 40

couple

Question 41

is by
definition a reduction potential

Answer 41

electrode potential

Question 42

is the
potential for the half-reaction written
in the opposite way. The sign of an
oxidation potential is, therefore,
opposite that for a reduction
potential, but the magnitude is
the same.

Answer 42

oxidation potential

Question 43

TRUE or FALSE
The standard electrode potential for a half-reaction is temperature dependent

Answer 43

TRUE

Question 44

The following further complicate application of standard electrode potential data to
many systems of interest in analytical chemistry:

Answer 44

association
dissociation
complex formation
solvolysis equilibria

Question 45

are empirical potentials that compensate for the types of activity and competing equilibria effects that we have just described.

Answer 45

formal potential

Question 46

is the electrode
potential when the ratio of analytical
concentrations of reactants and
products of a half-reaction is exactly
1.00 and the molar concentrations
of any other solutes are specified

Answer 46

formal potential

Question 47

is the potential of the half-cell with respect to the standard hydrogen
electrode measured under conditions such that the ratio of analytical concentrations
of reactants and products as they appear in the Nernst equation is exactly unity and
the concentrations of other species in the system are all carefully specified

Answer 47

formal potential

Question 48

this rule implies that one should always measure the cell potential by connecting the positive lead of the voltmeter to the right-hand electrode in the schematic or cell drawing and the common, or ground, lead of the voltmeter to the left-hand electrode

Answer 48

plus right rule

Question 49

potential of hydrogen electrode depends on

Answer 49

temperature
activities of hydrogen ion
molecular hydorgen in the solution