Created By :
A A GANI CHEMISTRY DEPARTMENT
JEMBER UNIVERSITY
• What is electrochemistry ? • What basic concept of chemistry use on electrochemistry • What existence of electrochemical in our life
BRANCH OF CHEMISTRY, LEARN INTERELATION BETTWEN ELECTRICITY AND CHEMICAL CHANGE
CHEMICAL CHANGE BY ELECTRICITY
CHEMICAL CHANGE PRODUCED ELECTRICITY
BASIC CONCEPT CHEMICAL CHANGE
ELECTRON RESTRUCTURE OF CHEMICAL BYELECTRONTRANSFER
IONIC BONDING
ELECTRONSHARING
COVALENT BONDING
INTRAMOLECULE BONDING
POLAR BONDING DIFFERENT ELECTRONEGATIVITY OF ATOMS
N O N P OL A R B ON D I NG SAME ELECTRONEGATIVITY OF ATOMS
REDUCING AND OIDI!ING REACTION AS BASIC PROCESS OF ELECTROCHEMISTRY ELECTROCHEMICAL CELLS COMPONENS OF ELECTROCHEMICAL CELLS ELECTRODE
ELECTROLYTE
ETERNAL CIRCUIT ELECTRICITY
ELCTROLYSIS CELLS CHEMICAL CHANGE BY ELECTRICITY
FARADAY LAW # F $ # E%&'a(e) $ *+-- C./(.01 # C $ # A02ere3 Se4.)d
VOLTAIC"GALVANIC CELLS CHEMICAL CHANGE PRODUCED ELECTRICITY
NERNST LAW
E = E0 – RT ln
Oxidizing agent Reducing agent
ELCTROLYSIS CELLS
NEGATIVE ELECTRODE
POSITIVE ELECTRODE
ANODE
CATHODE
OIDATION PROCESS
ELECTRODE
REDUCTION PROCESS
POSITIVE ELECTRODE
NEGATIVE ELECTRODE
VOLTAIC"GALVANIC CELLS
VOLTAIC"GALVANIC CELLS
REVERSIBLE CELLS
POTENTIAL SOURCE
COMMERCIAL CELLS
CURRENT SOURCE
CHEMICAL CELLS
PRIMARY CELLS
D&55er E(e4tr.de Sy6te0
SECONDARY CELLS
CONCENTRATION CELLS
Sa0e E(e4tr.de Sy6te0, D&55er E(e4tr.(yte C.)4e)trat&.)
FUEL CELLS
CELL NOTATION
ANODE M 768
9
SALT BRIDGE
M; 7a<899
ANODE " NEGATIV ELECTRODE
E0CELL =
y;
N
ANODE ELECTROLYTE
CATHODE 7a<8
9
N 768
CATHODE ELECTROLYTE
e Eter)a( C&r4/&t
E0 reduction potential of substance reduced
CATHODE " POSITIVE ELECTRODE
E0 reduction potential of substance oxidazed
THERMODINAMIC OF CELLS G- = ─ )F E-4e((6
G = ─ )F E4e((
a A; 1 B G=
> )FE4e(( = > )FE
&
$sel % $
sel
G
4e((
−
-
4C;dD
(a ! ) c (a ) d ; RT () (a A ) a (a B ) b
; RT ()
R# n"
ln
(a ! ) c
(a ) d
(a A ) a
(a B ) b
(a ! )c
(a ) d
(a A ) a
(a B ) b
e>
V
ANODE " NEGATIVE ELECTRODE
@ATODE " POSITIVE ELECTRODE !)
!)SO?
C/
C/SO?
DANIELL CELLS 7Ce0&4a( Ce((68 !) 768 !);7a<8 7# M8 99 C/; 7a<8 7# M8 9 C/ 768 E - = #,#- '.(t Fe; 7a<8 ; I 7a<8
Fe ; 7a<8 ; I 7a<8
Pt 9 I 7a<8 , I 7a<8 99 Fe; 7a<8 , Fe; 7a<8 9 Pt E - = -,? '.(t
CdSO? 7a<8 6at/rated
CdSO?3 HO 768
CdSO?3 HO 768
HSO? ; H768 Cd ; Cd 7(8
H
WESTON CELLS
E
B
B
C
A
Ce((6 EMF 7S8
S CELL
G
=
Ce((6 EMF 7E8 Ce((6 EMF 7Sta)dard8 Ce((6 EMF 7U)%).)8
R 7AB8 R 7AC8
=
R 7AB8 R 7AB8
MEASUREMENT DIAGRA M OF CELL POTENSIAL
Pt W&re H78
Pt P(ate
H;, 7HC(8
HYDROGEN ELECTRODE
Pt W&re
H 7(8
@C( 7a<8 6at/rated
@C(7S8, HC( 7S8 @C(7S8
H 7(8 S.5t Ca2&((er
CALOMEL ELECTRODE
BENEFIT OF ELECTRODE POTENTIAL •
T. C.02are re(at&'e 6tre)t .5 .&dat&.) a)d red/4t&.)
•
T. Ca(4/(ate EMF 4e((6 !) 768 9 !)B; 7a<8 99 C/B; 7a<8 9 C/ 768
E0cells = E0 7C/B; 9 C/8 E0 7!)B; 9 !)8 •
T. Pred&4t te .44/rred .5 rea4t&.) 1a6e .) 5ree e)ery e4a)e, K E - .r K G - 762.)ta)e&ty rea4t&.)8
CONCENTRATION AND TEMPERATURE INFLUENCE TO ELECTROMOTIVE FORCE 7EMF8 OF CELLS Pt 9 Fe; 7-,# M8, Fe; 7-, M8 99 H ; 7# M8 9 H A).de Rea4t&.)
: 7Fe ;
Fe;; e8
Cat.de Rea4t&.) : H ; ; H e Ce((6 Rea4t&.)
: Fe ; ; H;
E E
-
= > -,# '.(t =
-,* '.(t ;
Fe; ; H E-4e(( = -,-# '.(t
.) .C .r * @ Fe;Q
RT E 4e(( = E-4e((
E 4e(( = -3-# '.(t
)F
()
Fe;Q H;Q
3 #? J @># 0.(>#3 * @
-3 -Q ()
0.(3 *+-- C 0.(>#
-3#-Q #3 --Q
E 4e(( = -3-# '.(t -3- '.(t E 4e(( = -3 --* '.(t
7N. 62.)ta)e./6 4e((8
PRIMARY CELL A).de rea4t&.) 7)eat&'e e(e438
:
!) 768
!); ; e
Cat.de rea4t&.) 7)eat&'e e(e438 : 7#8 NH?; ; e 78 H !) 768 ; NH
; ?
; M)O 768
NH ; H 78
78 ; M)O 768
M)O 78 ; HO
!); ; NH ; M)O 78 ; H O
SECONDARY CELL A44/ 4e(( ).tat&.) : P1 9 HSO? 7 = #, "0L8 9P1O P1SO? 768 ; H; ; e
A).de rea4t&.)
: P1 768 ; HSO ?
Cat.de rea4t&.)
: P1O 768 ; HSO ? ; H; ; e
Ce(( rea4t&.) U6&) rea4t&.)
: P1 768 ; P1O 768 ; HSO? ; H; : P1 768 ; P1O 768 ; HSO? ; H;
Car&) rea4t&.) : P1SO? 768 ; HO
P1SO? 768 ; H O P1SO ? 768 ; HO P1SO? 768 ; H O
P1 768 ; P1O 768 ; HSO? ; H;
FUEL CELLS
V
7
H
8
@OH
78
O
;
A).de
Cat.de
O&dat&.)Rea4t&.)
Red/4t&.)Rea4t&.)
E(e4tr.(yte
REACTION ON ELECTROLYSIS PROCESSES EL EC T R O D E
ELECTROLYTE
INERT ELECTRODE
ELECTROLYTE MOLTEN
D&55&4/(t O&d&&)
W&t./t Water
NON INERT ELECTRODE
ELECTROLYTE SOLUTION
Ea6y O&d&&)
Added Water
ELECTROLYSIS OF •E(e4tr.(yte 6.(/t&.) /6e : 7#8 &)ert e(e4tr.de, 78 ).) &)ert e(e4tr.de •E(e4tr.(yte 0.(te) /6e : 78 &)ert e(e4tr.de, 7?8 ).) &)ert e(e4tr.de
OIDATION REDUCTION PROCESSES ANODE AREA
CATHODE AREA
S0a((e6t E-red/4t&.)
H&e6t E-red/4t&.)
AVAILABLE SUBSTANCE
N.) I)ert E(e4tr.de >
>
>
>
Ha(&de &.) 7F , C( , I , Br 8 Hydr.&de &.) 7OH>8 Water 7HO8 Oter6 a)&.)
Meta( Cat&.)6, ).) a(%a(& a)d eart a(%a(& Hydr.e) &.) Water 7HO8 A(%a(& a)d eart A(%a(& 4at&.)
E(e4tr.(y6&6 .5 NaC( S.(/t&.) /6e &)ert e(e4tr.de 7Pt, A/, C8 A'a&(a1(e 0ater&a( : HO Na; C(> A).de area : HO a)d C(> A).de rea4t&.)
Cat.de area : HO a)d Na;
C( >
:
Cat.de rea4t&.) :
e ; H O
Te )et rea4t&.) : C(> ; HO Na; F&)a( Pr.4e66
: NaC( ; HO
C( ; e H ; OH > C( ; H ; OH > Na; C( ; H ; NaOH
FARADAY LAW IN ELECTROLYSIS
E(e4tr&4&ty
7Te St.&4&.0etr&4 Re(at&.)6&2 &) E(e4tr.(y6&68 Faraday La Ce0&4a(Ca)e '
# A02ere # Se4.)d = # C./(.01
Ma66 :
*+-- C./(.01
W=
: M.(ar Ma66
# Faraday 0atter
E
M.(e E
e 7ra06"e
GALVANIC CELLS
ELECTROLYSIS CELLS
• 2H>0eter
• E(e4tr.2(at&)
• Lead St.rae Battery
• A(/0&)/0, Ma)e6&/0, S.d&/0 Pr.d/4t&.)
• !&)4 Car1.) Dry Ce(( • N&4e( Cad0&/0 St.rae Ce(( • S2e4&a(&ed Battery : Mer4/ry S&('er O&de F/e( Ce(( • Ir.) C.rr.6&.) Pr.te4t&.) /6e A).d&4>Cat.d&4 Sy6te0
• C.22er Re5&)&) • Br&)e E(e4tr.(y6&6 7Hydr.e), C(.r a)d NaOH Pr.d/4t&.)8
HARAPAN : SEMUA GURU KIMIA MAMPU MENDESAIN PEMBELAJARAN ILMU KIMIA DI SEKOLAH SESUAI TUNTUTAN KEHIDUPAN SISWA MASA DATANG
