Standard cell potential
& Batteries
Electrochemical cells
TULIAO, JOS ENZO
MIKHAIL, NOGALES
ZAFE, JONATHAN
MANLOGON, PATRICK
FALCON, JOHN MICHAEL
PAHECO, KINGTIN
VILLANUEVA, CHESTER
BATAAN, RICH
FERNANDEZ, RUSSEL
OÑATE, DARWIN
Reduction Potential
FREDUCTION FPOTENTIAL
The tendency of a species to gain electrons and
The tendency of a species to gain electrons and
undergo reduction. It's measured in volts (V) and
indicatesindicates the ability of a substance to accept
undergo reduction. It's measured in volts (V) and
the ability of
electrons.
electrons.
Oxidation Potential
OXIDATION FPOTENTIAL
The tendency of a species to lose
electrons and undergo oxidation. Like
reduction potential, it's also measured
in volts (V) and indicates the ability of
a substance to lose electrons.
The tendency of a species to lose
electrons and undergo oxidation. Like
reduction potential, it's also measured
in volts (V) and indicates the ability of
a substance to lose electrons.
Cell Potential
CELL FPOTENTIAL
Also known as electromotive force (EMF) or
Also known as electromotive force (EMF) or
voltage, it's the difference in electric potential
between two electrodes of an electrochemical
cell. It's the measure of the cell's ability to produce
an electric current and is the sum of the reduction
potential and the oxidation potential.
substance to accept
The reaction
occurring in
the different
parts of the
cell
voltage, it's the difference in electric potential
between two electrodes of an electrochemical
cell. It's the measure of the cell's ability to produce
an electric current and is the sum of the reduction
potential and the oxidation potential.
“THE STANDARD CELL POTENTIAL
CE-°CELL) IS CALCULATED USING THE
FORMULA:
E°cell =
E°reduction (cathode) - E°oxidation (anode)
Where E°reduction and E°oxidation are the standard
reduction potentials of the cathode and anode half-
reactions, respectively.
Where E°reduction and E°oxidation are the standard
reduction potentials of the cathode and anode half- .H3
reactions, respectively.
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DID YOU KNOW?
Michael Faraday's laws of electrolysis, formulated
in the 1830s, describe the quantitative
relationship between the amount of substance
produced or consumed during electrolysis and
the amount of electric charge passed through
the electrolyte.
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i. amount of _72-.rie char=- — ssed through
alectroly
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CH3
• Krebs Cycle (Citric Acid Cycle
• Electron Transport Chain:
*Krebs Cycle (Citric Acid Cycle
*Electron Transport Chain:
Cytoplasm:
Mitochondria
Nucleus
CYTOPLASM:
*Glycolysis
• Glycolysis
• Protein Synthesis
*Protein Synthesis
MITOCHONDRIA
INUCLEUS
*Transcription:
• Transcription:
• DNA Replication:
*DNA Replication:
The standard cell potential
(E°cell) is calculated using the
formula:
E°cell = E°reduction (cathode) - E°oxidation (anode)
ENDOPLASMIC FRETICULUM
(ER)
Endoplasmic Reticulum (ER)
• Protein Folding
• Lipid Synthesis
* Protein Folding
*Lipid Synthesis
Golgi Apparatus
GOLGI APPARATUS
• Protein Modification
• Vesicle Formation:
*Protein Modification
*Vesicle Formation:
The value of the cell
potential to the feasibility
of using the cell to
generate an electric
current
“T HE WALUE OF THE CELL
POTENTIAL TO THE FEASIBILITY
GENERATEANELECTRIC
If the cell potential is too low, the battery might not
be able to produce enough voltage to power
OFUSINGTHECELLTO
If the cell potential is too low, the battery might not
be able to produce enough voltage to power a
device or generate a sufficient electric current.
If the cell potential is too low, the battery might not
be able to produce enough voltage to power a
device or generate a sufficient electric current.
GROUP 5GROUPS
GENERAL CHEMISTRY
GENERAL CHEMISTRY
device orgeneratea sufficient electric current.
If the cell potential is too low, the battery might not
beable to produce enough voltage to power a
device orgenerate a sufficient electric current.
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QUIZ TIME
It is the the tendency of a
species to gain electrons
and undergo reduction.
A. Cell potential
B. Oxidation potential
C. Reduction potential
It is also know as
coin cell batteries.
A. Lechanche dry cell
B. Fuel cells
C. Button cells
It happens when metals react
with their surroundings or
environment, due to
electrochemical processes.
A. Errosion
B. Correction
C. Corrosion
Sodium hydroxide is
also knows as.
A. Polyvinyl chloride
B. Toothpaste
C. Caustic soda
Calculate the cell
potential of galvanic cells
show below:
Zn2+(aq) + 2e- → Zn(s) E° =
-0.76 V (anode)
Cu2+(aq) + 2e- → Cu(s) E° =
+0.34 V (cathode)
82
the electrochemistry
involved in some
common batteries:
Leclanche dry cell
The Leclanché cell is a type of dry cell
battery invented in the 19th century by
Georges Leclanché. It consists of zinc
anode, manganese dioxide cathode, and
moist electrolyte paste. Its appearance is
one of the earliest forms of portable
batteries.
Button batteries
Button batteries, also known as coin cell
batteries, operate through a similar
electrochemical process. They typically
consist of a zinc anode, a cathode made
of manganese dioxide or silver oxide, and
an electrolyte, often potassium hydroxide.
Fuel cells
A fuel cell is an electrochemical cell that
generates electrical energy from fuel via
an electrochemical reaction.
Types of fuel cells:
The Polymer Electrolyte Membrane
(PEM) Fuel Cell
Solid Acid Fuel Cell
Alkaline Fuel Cell
Solid Oxide Fuel Cell
Molten Carbonate Fuel Cell
Lead storage battery
The lead-acid battery, also known as the
lead storage battery, operates through a
reversible electrochemical reaction
Lead
207.2
between lead dioxide (PbO2) and lead
(Pb) in a sulfuric acid (H2SO4) electrolyte
solution.
reactions in some
commercial
electrolytic
processes
Electrolytic process
of aluminum:
Aluminum is a versatile
metal used in various
industries,
including
construction,
transportation, packaging,
and electronics.
Copper
electrorefining:
Copper is primarily used in
electrical wiring, plumbing,
and electronics due to its
excellent
conductivity,
corrosion resistance, and
malleability
Chlorine production:
Chlorine is an essential
chemical
in
the
manufacturing of PVC
(polyvinyl chloride), which is
widely used in construction
for pipes, window frames,
and siding.
Sodium hydroxide
production:
Sodium hydroxide, also
known as caustic soda, is a
key
ingredient
production
of
in the
soaps,
detergents, paper, textiles,
and various chemicals.
QUIZ TIME
It is the the tendency of a
species to gain electrons
and undergo reduction.
A. Cell potential
B. Oxidation potential
C. Reduction potential
It is also know as
coin cell batteries.
A. Lechanche dry cell
B. Fuel cells
C. Button cells
It happens when metals react
with their surroundings or
environment, due to
electrochemical processes.
A. Errosion
B. Correction
C. Corrosion
Sodium hydroxide is
also knows as.
A. Polyvinyl chloride
B. Toothpaste
C. Caustic soda
Calculate the cell
potential of galvanic cells
show below:
Zn2+(aq) + 2e- → Zn(s) E° =
-0.76 V (anode)
Cu2+(aq) + 2e- → Cu(s) E° =
+0.34 V (cathode)
82
the electrochemistry
involved in some
common batteries:
Leclanche dry cell
The Leclanché cell is a type of dry cell
battery invented in the 19th century by
Georges Leclanché. It consists of zinc
anode, manganese dioxide cathode, and
moist electrolyte paste. Its appearance is
one of the earliest forms of portable
batteries.
Button batteries
Button batteries, also known as coin cell
batteries, operate through a similar
electrochemical process. They typically
consist of a zinc anode, a cathode made
of manganese dioxide or silver oxide, and
an electrolyte, often potassium hydroxide.
Fuel cells
A fuel cell is an electrochemical cell that
generates electrical energy from fuel via
an electrochemical reaction.
Types of fuel cells:
The Polymer Electrolyte Membrane
(PEM) Fuel Cell
Solid Acid Fuel Cell
Alkaline Fuel Cell
Solid Oxide Fuel Cell
Molten Carbonate Fuel Cell
Lead storage battery
The lead-acid battery, also known as the
lead storage battery, operates through a
reversible electrochemical reaction
Lead
207.2
between lead dioxide (PbO2) and lead
(Pb) in a sulfuric acid (H2SO4) electrolyte
solution.
reactions in some
commercial
electrolytic
processes
Electrolytic process
of aluminum:
Aluminum is a versatile
metal used in various
industries,
including
construction,
transportation, packaging,
and electronics.
Copper
electrorefining:
Copper is primarily used in
electrical wiring, plumbing,
and electronics due to its
excellent
conductivity,
corrosion resistance, and
malleability
Chlorine production:
Chlorine is an essential
chemical
in
the
manufacturing of PVC
(polyvinyl chloride), which is
widely used in construction
for pipes, window frames,
and siding.
Sodium hydroxide
production:
Sodium hydroxide, also
known as caustic soda, is a
key
ingredient
production
of
in the
soaps,
detergents, paper, textiles,
and various chemicals.
Standard cell potential
& Batteries
Electrochemical cells
TULIAO, JOS ENZO
MIKHAIL, NOGALES
ZAFE, JONATHAN
MANLOGON, PATRICK
FALCON, JOHN MICHAEL
PAHECO, KINGTIN
VILLANUEVA, CHESTER
BATAAN, RICH
FERNANDEZ, RUSSEL
OÑATE, DARWIN
Reduction Potential
The tendency of a species to gain electrons and
undergo reduction. It's measured in volts (V) and
indicates the ability of a substance to accept
electrons.
Oxidation Potential
The tendency of a species to lose
electrons and undergo oxidation. Like
reduction potential, it's also measured
in volts (V) and indicates the ability of
a substance to lose electrons.
Cell Potential
Also known as electromotive force (EMF) or
voltage, it's the difference in electric potential
between two electrodes of an electrochemical
cell. It's the measure of the cell's ability to produce
an electric current and is the sum of the reduction
potential and the oxidation potential.
The standard cell potential
(E°cell) is calculated using the
formula:
E°cell = E°reduction (cathode) - E°oxidation (anode)
Where E°reduction and E°oxidation are the standard
reduction potentials of the cathode and anode half-
reactions, respectively.
trivia
DID YOU KNOW?
Michael Faraday's laws of electrolysis, formulated
in the 1830s, describe the quantitative
relationship between the amount of substance
produced or consumed during electrolysis and
the amount of electric charge passed through
the electrolyte.
The reaction
occurring in
the different
parts of the
cell
• Krebs Cycle (Citric Acid Cycle
• Electron Transport Chain:
Cytoplasm:
Mitochondria
Nucleus
• Glycolysis
• Protein Synthesis
• Transcription:
• DNA Replication:
Endoplasmic Reticulum (ER)
• Protein Folding
• Lipid Synthesis
Golgi Apparatus
• Protein Modification
• Vesicle Formation:
The value of the cell
potential to the feasibility
of using the cell to
generate an electric
current
If the cell potential is too low, the battery might not
be able to produce enough voltage to power a
device or generate a sufficient electric current.
If the cell potential is too low, the battery might not
be able to produce enough voltage to power a
device or generate a sufficient electric current.
GROUP 5
GENERAL CHEMISTRY