reduction reaction
Download
Report
Transcript reduction reaction
CHAPTER 2
CORROSION PRINCIPLES
Chapter Outlines
2.1
2.2
2.3
2.4
2.5
4/12/2015
Oxidation and Reduction Reactions
Standard Electrode Half- Cell Potentials
Standard EMF Series
Galvanic Cells With 1 Molar Electrolytes
Galvanic Cells Not 1Molar Electrolytes
1
2.1 Oxidation and Reduction Reactions
In metal, corrosion process is normally
electrochemical @ electrochemistry
(a chemical reaction in which there is transfer
of electrons from one chemical species to
another)
2 reactions that occur during corrosion process:
i. Oxidation reaction
ii. Reduction reaction
4/12/2015
Asyadi
2
i.
Oxidation reaction @ anodic reaction
Definition:
the removal of one or more electrons from an
atom, ion or molecule
Equation:
M
Mn+
+
ne-
(in which M becomes an n+ positively charged ion and in the
process loses its n valence electrons; e- is used to symbolize
an electron)
Zn Zn2 2e
Example:
Anode is the side at which oxidation takes place.
4/12/2015
Asyadi
3
ii.
Reduction reaction
Definition:
the addition of one or more electrons to an atom, ion or
molecule (because the electrons generated from each metal
atom that is oxidized must be transferred to and become a part
of another chemical species = reduction reaction)
Equation:
M+ + e-
M(n-1)+
(some metals undergo corrosion in acid solutions, which have a high
concentration of hydrogen (H+) and hydrogen gas (H2) is evolved)
Cathode is the side at which reduction occurs
4/12/2015
Asyadi
4
There are 3 possibilities of reaction that can occur at
cathode (reduction):
First possibilities
Cathodic half- cell reaction
Condition
Reaction
: 2H 2e H2 (gas )
: if the electrolyte is an acid
solution
: hydrogen ions in the acid solution
will be reduced to hydrogen atom to
form diatomic hydrogen gas
Second possibilities
Cathodic half- cell reaction
Condition
Reaction
4/12/2015
O
4H
4e
2H2O
:
2
: if the electrolyte also contain
oxidizing agent
: oxygen will combine with hydrogen
ions to form water molecules
Asyadi
5
Third possibilities
O
2H
O
4e
4(OH)
Cathodic half- cell reaction : 2
2
Condition
: if the electrolyte is basic or
neutral and oxygen is
present
Reaction
: oxygen and water molecules
will react to form hydroxyl
ions
4/12/2015
6
iii.
Overall Electrochemical Reaction
Consist of at least one oxidation (half reaction) and
one reduction (half reaction), and will be the sum of
them
Example:
(Zinc metal immersed in an acid solution)
At some regions on the metal
surface, zinc will experience
Asyadi
oxidation or corrosion
4/12/2015
7
Oxidation half reaction:
Zn Zn2 2e
Since Zn is a metal and good electrical conductor, these electrons
may be transferred to an adjacent region at which the H+ ions are
reduced.
Reduction half reaction:
2H 2e H2 (gas )
Total electrochemical reaction:
Zn Zn2 2e
2H 2e H2 (gas )
4/12/2015
Zn + 2H+Asyadi Zn2+ + H2 (gas)
8
Zinc metal
Chemical reaction:
Zn + 2HCl
ZnCl2 + H2
Ionic form:
Zn + 2H+
Zn2+ + H2
Half- cell reaction:
Zn
Zn2+ + 2e- (oxidation)
2H+ + 2eH2 (reduction)
hydrochloric acid
Fig. Reaction of hydrochloric acid with zinc to produce hydrogen gas
4/12/2015
Asyadi
9
2.2 Standard Electrode Half- Cell Potentials
Every metal has a different tendency to corrode in a
particular environment
E.g. ‘zinc is chemically attacked or corroded by dilute
hydrochloric acid, whereas gold is not’
Method for comparing the tendency for metals to form
ions in aqueous solution is to compare their half- cell
oxidation or reduction potentials (voltages) to a
standard hydrogen- hydrogen ion half- cell potential.
4/12/2015
Asyadi
10
Experimental Setup for the Determination of
Half- cell Standard Electrode Potentials
Experimental setup for the determination of the standard emf of zinc. In a beaker a
Zn Electrode is placed in a solution of 1 M Zn2+ ions. In the other there is a
4/12/2015
Asyadi
11
standard hydrogen reference electrode
consisting of a platinum electrode
immersed in a solution of 1 MH+ ions which contains H2 gas at 1 atm.
Standard Hydrogen Electrode
Represent only differences in electrical potential and thus it is
convenient to establish a reference point/ reference cell to which
other cell halves may be compared.
It consist of an inert platinum electrode in a 1M solution of
H+ ions, saturated with hydrogen gas that is bubbled through
the solution at a pressure of 1 atm and temperature of 25°C.
The platinum itself does not take part in the electrochemical
reaction: it acts only as a surface on which hydrogen atoms
may be oxidized or hydrogen ions may be reduced.
4/12/2015
Asyadi
12
4/12/2015
Asyadi
13
2.2 Standard EMF Series
Electromotive force (EMF) series:
is generated by coupling to the standard
hydrogen electrode, std half- cells for
various metals and ranking them according to
measured voltage.
Table 17.1- show the list of the standard halfcell potentials of some selected metals which
represents the corrosion tendencies for the
several metals
4/12/2015
Asyadi
14
Increasingly inert
(cathodic)
Increasingly active
(anodic)
4/12/2015
Asyadi
15
those metals at the top (Au & Pt) --- are noble or
chemically inert
Moving down --- metals become increasingly more
active (more susceptible to oxidation) (sodium &
potassium)
The voltages --- are for the half- reactions
oxidation reaction: electron on the right hand side
M1
Mn+
+ ne-
V1º
reduction reaction: electron on the left hand side
(sign of the voltage changed)
M+ + e4/12/2015
M(n-1)+
Asyadi
V2º
16
Overall cell potential ΔV° is:
ΔVcell° = V°
4/12/2015
1
Asyadi
+ V°
2
17
GALVANIC CELLS
Galvanic couple:
Two metals electrically connected in a liquid
electrolyte wherein one metal becomes anode and
corrodes, while the other acts as a cathode
4/12/2015
Asyadi
18
2.4 Galvanic Cells With 1 Molar Electrolytes
Can be constructed with two dissimilar metal electrodes each
immersed in a 1M solution of their own ions
The two solutions are separated by a porous wall to prevent
their mechanical mixing, and an external wire in series with a
switch and a voltmeter connects the two electrodes
E.g.:
zinc electrode immersed in a 1 M solution of Zn2+ ions and
another of copper immersed in a 1 M solution of Cu2+ ions with
the solutions at 25°C
4/12/2015
Asyadi
19
A macroscopic galvanic cell with zinc and copper electrodes. When the switch is closed
and the electrons flow, the voltage difference between the zinc and copper electrodes
4/12/2015
Asyadi
is -1.10V. The zinc electrode is the anode of the cell and corrodes.
20
Calculation of electrochemical potential of Zn- Cu galvanic cell
From the Standard emf Series:
Zn
Zn2+ + 2eCu
Cu2+ + 2e Oxidation half- cell reaction:
Zn
(ANODE)
Zn2+ + 2e-
E° = -0.763
Reduction half- cell reaction:
Cu2+ +
2e-
E° = -0.763 V
E° = +0.340 V
Cu
V°1
(CATHODE)
E° = -0.340
V°2
Overall reaction (by adding):
Zn + Cu2+
4/12/2015
Zn2+ + Cu
Asyadi
E°cell = V°1 + V°2
= -0.763 + (-0.340)
= -1.103 V
21
Problem 1:
A galvanic cell consist of an electrode of zinc in a 1M ZnSO4
solution and another of nickel in a 1 M NiSO4 solution. The two
electrodes are separated by a porous wall so that mixing of the
solutions is prevented. An external wire with a switch connects the
two electrodes. When the switch is just closed:
(a)
(b)
(c)
(d)
(e)
(f)
At which electrode does oxidation occur
Which electrode is the anode of the cell?
Which electrode corrodes?
Write the equation for the half- cell reaction at the anode?
Write the equation for the half- cell reaction at the cathode?
What is the emf of this galvanic cell when the switch is just
closed?
4/12/2015
Asyadi
22
Answer:
(a)
(b)
(c)
(d)
(e)
(f)
Oxidation occurs at the zinc electrode since the zinc half- cell
reaction has a more negative E° potential of -0.763 V as
compared to -0.250 V for the nickel half- cell reaction.
The zinc electrode is the anode since oxidation occurs at the
anode
The zinc electrode corrodes since the anode in a galvanic cell
corrodes.
Zn
Zn2+ + 2eE° = -0.763V
Ni2+ + 2eNi
E° =+0.250V
The emf of the cell is obtained by adding the half- cell reactions
together:
Anode reaction:
Cathode reaction:
Zn
Zn2+
Ni2+ + 2e-
Overall reaction:Zn + Ni2+
4/12/2015
+
2eNi
Zn2+ + Ni
Asyadi
E° = -0.763 V
E° = +0.250 V
E°cell = -0.513 V
23
2.5 Galvanic Cells Not 1 Molar Electrolytes
Most electrolytes for real corrosion galvanic cells are
not 1 M, but are usually dilute solutions that are
much lower than 1 M.
If the concentration of the ions in an electrolyte
surrounding an anodic electrode is less than 1 M, the
driving force for the reaction to dissolve or corrode
the anode is greater since there is a lower
concentration of ions to cause the reverse reaction
4/12/2015
Asyadi
24
Nernst equation:
E = E° + 0.0592 log Cion
n
Where: E = new emf of half- cell
E° = standard emf of half- cell
n = number of electrons transferred
(for example, M
Mn+ + ne-)
Cion = molar concentration of ions
4/12/2015
Asyadi
25
Problem 2:
A galvanic cell at 25ºC consist of an electrode of zinc in a 0.10 M
ZnSO4 solution and another of nickel in a 0.05 M NiSO4 solution.
The two electrodes are separated by a porous wall and connected
by an external wire. What is the emf of the cell when a switch
between the two electrodes is just closed?
4/12/2015
Asyadi
26
Answer:
Zn
Ni
Half cell reactions:
Zn2+ + 2eNi2+ + 2e-
E° = -0.763V (ANODE)
E° = -0.250V (CATHODE)
Apply Nernst Equation:
Ecell = E° + 0.0592 log Cion
n
Anode reaction: EA = -0.763 V + 0.0592 log 0.10 = -0.793 V
2
Cathode reaction: Ec = - (- 0.250 V + 0.0592 log 0.05) = +0.289 V
2
4/12/2015
Asyadi
27
Emf of the cell (Ecell) = EA + EC
= -0.793V + 0.289 V
= -0.505 V
4/12/2015
Asyadi
28