Applications of Electrochemistry and Bioelectricity
2. Industrial Electrochemistry
Learning outcomes
- I can identify industrial processes that use electrochemistry.
- I can explain how electrolysis is used in manufacturing.
- I can describe electrochemical methods of metal extraction and purification.
- I can evaluate the economic importance of industrial electrochemistry.
- I can analyze the benefits and challenges of electrochemical technologies.
What Is Industrial Electrochemistry?
Industrial electrochemistry is the large-scale use of chemical reactions involving the transfer of electrons to manufacture useful materials, extract and purify metals, produce chemicals, protect surfaces, and store or convert energy.
Electrochemistry connects:
chemical reactions ↔ electrical energy
Some electrochemical processes produce electrical energy from chemical reactions.
Others use electrical energy to force chemical reactions to occur.
Industrial electrochemistry is used to produce enormous quantities of materials that modern society depends on.
Important applications include:
- aluminum production
- chlorine production
- sodium hydroxide production
- hydrogen production
- metal purification
- electroplating
- battery manufacturing
- fuel cells
- metal recovery
- corrosion protection
Two Major Types of Electrochemical Cells
Industrial electrochemistry uses two important types of cells.
convert:
chemical energy → electrical energy
Batteries are an important example.
Electrolytic cells
convert:
electrical energy → chemical energy
Industrial electrolysis is an important example.
Both involve:
oxidation and reduction reactions.
Oxidation and Reduction
All electrochemical processes involve the transfer of:
electrons.
Oxidation means:
loss of electrons.
Reduction means:
gain of electrons.
Remember:
OIL RIG
Oxidation Is Loss
Reduction Is Gain
At the:
anode → oxidation
At the:
cathode → reduction
These definitions apply to both galvanic and electrolytic cells.
Industrial Electrolysis
Electrolysis uses electrical energy to drive a chemical reaction that would not occur spontaneously under the operating conditions.
Industrial electrolysis can be used to:
- extract metals
- purify metals
- produce gases
- manufacture chemicals
- coat surfaces
- produce hydrogen
- recover valuable materials
Industrial electrolytic cells may operate continuously and process very large quantities of:
materials.
Metal Extraction
Many metals occur naturally as:
compounds in ores.
To obtain the metal, its positive ions must be:
reduced.
For example:
Al³⁺ + 3e⁻ → Al
Some metals can be extracted chemically using reducing agents such as carbon.
However, highly reactive metals form very stable compounds and are difficult to extract this way.
Electrolysis is therefore particularly important for extracting metals such as:
- aluminum
- sodium
- magnesium
Why Electrolysis Can Extract Metals
Metal ions are positively charged.
During electrolysis, they move toward the:
cathode.
At the cathode they gain electrons:
Mⁿ⁺ + ne⁻ → M
The metal ions are therefore:
reduced to metal atoms.
This provides a general method for producing reactive metals.
Aluminum Production
One of the most important examples of industrial electrochemistry is the production of:
aluminum.
Aluminum is used in:
- aircraft
- vehicles
- buildings
- electrical cables
- packaging
- electronics
- machinery
Its combination of low density, corrosion resistance, and useful mechanical properties makes it an important:
engineering material.
The Hall-Héroult Process
Aluminum is produced industrially using the:
Hall-Héroult process.
Aluminum oxide is obtained from aluminum-containing ores such as bauxite and dissolved in a molten cryolite-based electrolyte.
The electrolyte is kept at a high temperature so that ions can:
move freely.
A large electric current passes through the cell.
Aluminum at the Cathode
Aluminum ions move toward the cathode.
They gain electrons:
Al³⁺ + 3e⁻ → Al
This is:
reduction.
Molten aluminum forms and collects in the lower part of the cell.
It can then be:
removed for processing.
The Anode in Aluminum Production
The Hall-Héroult process commonly uses:
carbon anodes.
At the anode, oxide-containing species are oxidized.
The oxygen produced reacts with the carbon anode, producing mainly:
carbon dioxide.
As a result, the carbon anodes are gradually:
consumed.
They must therefore be replaced periodically.
Why Cryolite Is Important
Pure aluminum oxide has a very high melting point.
Operating with pure molten aluminum oxide would require:
extremely high temperatures.
Dissolving aluminum oxide in a molten cryolite-based electrolyte allows the cell to operate at a substantially lower temperature.
This helps reduce:
energy requirements and operating difficulties.
Energy Use in Aluminum Production
Primary aluminum production requires a large amount of:
electrical energy.
Electricity is therefore a major factor in:
- production cost
- location of smelters
- environmental impact
Aluminum smelters are often located where large supplies of reliable electricity are available.
Recycling Aluminum
Recycling aluminum requires much less energy than producing primary aluminum from ore.
Recycling also reduces:
- demand for mining
- processing of new ore
- waste
- some associated environmental impacts
This makes aluminum recycling economically and environmentally:
important.
Sodium Production
Sodium is a highly reactive metal.
It cannot be produced from aqueous sodium chloride because water would be reduced instead.
Industrial sodium can be produced by electrolysis of:
molten sodium chloride.
At the cathode:
Na⁺ + e⁻ → Na
At the anode:
2Cl⁻ → Cl₂ + 2e⁻
The products are:
sodium and chlorine.
Magnesium Production
Magnesium can also be produced using electrolysis.
Molten magnesium chloride contains:
Mg²⁺ and Cl⁻ ions.
At the cathode:
Mg²⁺ + 2e⁻ → Mg
At the anode:
2Cl⁻ → Cl₂ + 2e⁻
Magnesium is valued because it is:
lightweight.
It is used in alloys and specialized engineering applications.
The Chlor-Alkali Industry
One of the world's major electrochemical manufacturing processes is the electrolysis of concentrated sodium chloride solution:
brine.
This process is called the:
chlor-alkali process.
It produces three important chemicals:
chlorine
hydrogen
and:
sodium hydroxide.
Reactions in the Chlor-Alkali Process
At the cathode, water is reduced:
2H₂O + 2e⁻ → H₂ + 2OH⁻
Hydrogen gas is produced.
At the anode:
2Cl⁻ → Cl₂ + 2e⁻
Chlorine gas is produced.
Na⁺ ions remain in solution with OH⁻ ions, producing:
sodium hydroxide solution.
Why Chlorine Is Important
Chlorine is an important industrial chemical.
It is used in:
- water treatment
- disinfectant manufacture
- production of many chemicals
- manufacture of some plastics
- chemical synthesis
The large-scale production of chlorine therefore supports many other:
industries.
Why Sodium Hydroxide Is Important
Sodium hydroxide is also an important industrial chemical.
It is used in:
- paper production
- soap and detergent manufacturing
- chemical processing
- textile processing
- cleaning
- petroleum processing
It is sometimes called:
caustic soda.
Hydrogen from the Chlor-Alkali Process
Hydrogen is another useful product.
It can be used in:
- chemical manufacturing
- fuel applications
- hydrogenation reactions
- production of other industrial chemicals
Rather than treating hydrogen as waste, industrial facilities can use or sell it as a:
valuable co-product.
Membrane Cells
Modern chlor-alkali plants commonly use:
membrane cells.
A specialized membrane allows selected ions to pass while helping keep products:
separated.
This is important because chlorine, hydrogen, and sodium hydroxide must not simply mix together.
Separation improves:
- product purity
- efficiency
- safety
Metal Purification
Electrochemistry can also be used to:
purify metals.
This process is called:
electrorefining.
Copper is one of the most important examples.
High-purity copper is essential for:
- electrical wiring
- electronics
- motors
- generators
- transformers
- telecommunications
Copper Electrorefining
In copper electrorefining:
Impure copper → anode
Pure copper sheet → cathode
The electrolyte contains:
Cu²⁺ ions.
At the anode:
Cu → Cu²⁺ + 2e⁻
Copper atoms enter the electrolyte.
At the cathode:
Cu²⁺ + 2e⁻ → Cu
Pure copper is deposited.
What Happens to the Impurities?
Not all impurities behave like copper.
Some may remain in solution.
Others can collect below the anode as:
anode sludge or anode slime.
This material can contain valuable metals such as:
- silver
- gold
- other precious or valuable elements
These materials may be recovered and processed separately.
Therefore electrorefining can produce both:
high-purity copper and valuable by-products.
Why Copper Must Be Pure
Electrical applications require copper with very high:
electrical conductivity.
Impurities can reduce its performance.
Electrorefining produces copper suitable for demanding applications such as:
electrical wiring and electronics.
Electroplating
Another major industrial electrochemical process is:
electroplating.
Electroplating uses electrolysis to deposit a thin metal coating onto an object.
The object being coated is normally the:
cathode.
Metal ions gain electrons and form a solid coating:
Mⁿ⁺ + ne⁻ → M
Industrial Uses of Electroplating
Electroplating can improve:
- appearance
- corrosion resistance
- wear resistance
- electrical conductivity
- surface hardness
- contact reliability
It is used in:
- automotive manufacturing
- electronics
- jewelry
- aerospace
- tools
- machinery
Electrowinning
Electrowinning is an electrochemical process used to recover metals from solutions containing metal ions.
Metal ions are reduced at the cathode:
Mⁿ⁺ + ne⁻ → M
The solid metal can then be collected.
Electrowinning is used in the production or recovery of metals such as:
- copper
- zinc
- nickel
- cobalt
Electrorefining vs Electrowinning
These processes are related but have different purposes.
Electrorefining
starts with an impure metal and uses electrochemistry to produce a:
purer metal.
Electrowinning
starts with metal ions in a solution and uses electrochemistry to recover:
solid metal.
Both rely on reduction at the:
cathode.
Hydrogen Production by Electrolysis
Water electrolysis can produce:
hydrogen gas.
At the cathode, hydrogen-containing species are reduced.
At the anode, oxygen is produced.
Overall:
2H₂O → 2H₂ + O₂
Electrical energy is converted into:
chemical energy stored in hydrogen.
Hydrogen and Renewable Electricity
Hydrogen production by electrolysis can be combined with electricity generated from:
- solar power
- wind power
- hydroelectric power
- other low-carbon sources
The hydrogen can then be:
- stored
- transported
- used in chemical production
- used as a fuel
- converted back into electricity in a fuel cell
This creates a connection between electrochemistry and:
energy storage.
What Is "Green Hydrogen"?
The term green hydrogen is commonly used for hydrogen produced by water electrolysis using electricity from:
renewable energy sources.
The electrolysis itself does not release carbon dioxide as a direct product.
However, the overall environmental impact depends on factors such as:
- electricity source
- equipment manufacture
- water supply
- compression
- storage
- transportation
Therefore the full production system must be considered when evaluating:
environmental impact.
Batteries as Industrial Electrochemistry
Battery production is another major electrochemical industry.
Batteries convert:
chemical energy → electrical energy
during discharge.
Rechargeable batteries can also convert electrical energy back into:
stored chemical energy.
Examples include:
- lead-acid batteries
- nickel-metal hydride batteries
- lithium-ion batteries
- sodium-ion batteries
Lithium-Ion Batteries
Lithium-ion batteries are widely used in:
- smartphones
- laptops
- electric vehicles
- power tools
- grid energy storage
During operation, lithium ions move through the electrolyte while electrons move through the:
external circuit.
Large-scale battery manufacturing therefore depends heavily on:
electrochemical science and engineering.
Fuel Cells
Fuel cells convert chemical energy directly into:
electrical energy.
Unlike a battery that stores reactants internally, a fuel cell can continue operating while fuel and oxidant are continuously:
supplied.
Hydrogen fuel cells are one example.
They produce electricity through electrochemical reactions involving:
hydrogen and oxygen.
Electrochemical Corrosion Protection
Electrochemical principles can also be used to prevent:
corrosion.
One technique is:
cathodic protection.
The metal structure being protected is forced to behave as the:
cathode.
This reduces its tendency to oxidize.
Sacrificial Protection
A more reactive metal can be attached to a structure.
The more reactive metal oxidizes preferentially.
It is called the:
sacrificial anode.
Metals such as:
- zinc
- magnesium
- aluminum alloys
can be used in suitable applications.
This technique can protect:
- pipelines
- ships
- storage tanks
- offshore structures
Electrochemical Manufacturing
Electrochemical methods can sometimes replace manufacturing processes that require large quantities of chemical reagents.
Instead of adding a chemical oxidizing or reducing agent, an industrial process may use:
electrical current.
Electrons effectively become a controllable:
chemical reagent.
This can offer important manufacturing advantages.
Precise Control
Electrochemical processes can often be controlled by adjusting:
- voltage
- current
- current density
- temperature
- electrolyte concentration
- electrode area
- reaction time
- electrode material
This gives engineers precise control over:
reaction rates and product formation.
Faraday's Laws in Industry
The amount of material produced during electrolysis is related to the quantity of:
electric charge.
Charge is calculated using:
Q = It
where:
Q = charge in coulombs
I = current in amperes
t = time in seconds
This allows manufacturers to calculate how much electrical charge is needed to produce a particular amount of:
material.
Example: Industrial Charge
An electrolytic cell operates at:
5000 A
for:
1 hour.
Convert time:
1 hour = 3600 s
Use:
Q = It
Q = 5000 × 3600
Q = 18,000,000 C
A huge quantity of electrical charge passes through the cell.
This illustrates why industrial electrolysis commonly uses:
very large electric currents.
Why Industrial Electrochemistry Is Economically Important
Industrial electrochemistry provides materials needed throughout modern economies.
It supports industries such as:
- construction
- transportation
- electronics
- energy
- telecommunications
- chemical manufacturing
- mining
- medicine
- consumer products
Many products depend directly or indirectly on:
electrochemical manufacturing.
High-Purity Materials
One major advantage of electrochemical processing is the ability to produce:
high-purity materials.
Electrorefining can separate metals from many impurities.
This is particularly important when the material will be used in:
- electronics
- electrical systems
- specialized alloys
- advanced manufacturing
Valuable Co-Products
Industrial electrochemical processes can produce several useful products simultaneously.
The chlor-alkali process produces:
- chlorine
- hydrogen
- sodium hydroxide
Copper electrorefining can also allow recovery of valuable metals from:
anode residues.
Using and selling co-products can improve the economics of an:
industrial process.
Energy Costs
A major challenge of industrial electrochemistry is:
electricity consumption.
Processes such as aluminum production require very large amounts of electrical energy.
Electricity prices can therefore strongly affect:
production costs.
Improving electrical efficiency can have major economic benefits.
Energy Efficiency
Not all electrical energy supplied to an industrial cell becomes useful chemical energy.
Energy can be lost through:
- electrical resistance
- heating
- unwanted reactions
- overpotential
- equipment inefficiencies
Engineers try to minimize these losses to improve:
energy efficiency.
Current Efficiency
Another important concept is:
current efficiency.
Ideally, all electrical charge would produce the desired chemical reaction.
In reality, some charge may drive:
side reactions.
Higher current efficiency means a greater fraction of the supplied charge produces the:
desired product.
Raw Material Costs
Industrial electrochemical processes also require:
- ores
- electrolytes
- electrodes
- water
- membranes
- catalysts
- replacement components
The cost and availability of these materials influence the:
economics of production.
Electrode Consumption
Some industrial electrodes are consumed during operation.
For example, carbon anodes in conventional aluminum production gradually react and must be:
replaced.
This increases:
- material costs
- maintenance requirements
- waste
- associated emissions
Developing more durable electrode technologies is therefore an important area of:
research.
Environmental Challenges
Industrial electrochemistry can create environmental impacts through:
- electricity generation
- mining
- chemical waste
- wastewater
- greenhouse gas emissions
- hazardous substances
- spent electrodes
- end-of-life equipment
The scale of the impact depends strongly on the:
specific process and energy source.
Electricity Source Matters
Two electrolysis plants performing the same reaction can have different overall environmental impacts if their electricity comes from different:
energy sources.
Electricity generated mainly from fossil fuels may have greater associated greenhouse gas emissions than electricity generated from lower-carbon sources.
Therefore evaluating electrolysis requires considering both:
the chemical process and the electricity supply.
Benefits of Industrial Electrochemistry
Industrial electrochemical processes can offer several advantages.
They can:
- produce highly reactive metals
- produce high-purity materials
- allow precise process control
- manufacture important chemicals
- recover valuable metals
- create specialized surface coatings
- support energy storage
- integrate with renewable electricity
- reduce the need for some chemical reducing or oxidizing agents
Challenges of Industrial Electrochemistry
Challenges can include:
- high electricity demand
- high equipment costs
- electrode degradation
- corrosion
- hazardous chemicals
- wastewater management
- raw-material requirements
- side reactions
- heat management
- maintaining product purity
Industrial engineers must balance these factors against the:
value of the products.
Comparing Major Industrial Processes
| Process | Main Purpose | Important Product |
|---|---|---|
| Hall-Héroult process | Metal extraction | Aluminum |
| Chlor-alkali process | Chemical manufacturing | Cl₂, H₂, NaOH |
| Copper electrorefining | Metal purification | High-purity copper |
| Electrowinning | Metal recovery | Cu, Zn, Ni and others |
| Electroplating | Surface modification | Metal coating |
| Water electrolysis | Chemical/energy production | Hydrogen and oxygen |
| Battery manufacturing | Energy storage | Electrochemical cells |
| Cathodic protection | Corrosion control | Protected metal structures |
Evaluating an Industrial Process
When evaluating an electrochemical technology, consider more than whether:
the chemistry works.
Ask:
What does it produce?
How much energy does it require?
How expensive is the electricity?
What raw materials are required?
Are valuable co-products produced?
Does the process create hazardous waste?
Can materials be recycled?
What is the source of the electricity?
How long does the equipment last?
Are there safer or more efficient alternatives?
This provides a more complete evaluation of the:
technology.
Worked Example 1
Why is electrolysis used to extract aluminum?
Aluminum is highly reactive and forms very stable compounds.
Al³⁺ ions can be reduced at the cathode:
Al³⁺ + 3e⁻ → Al
Electrolysis therefore allows aluminum metal to be:
produced industrially.
Worked Example 2
Why is aluminum production expensive?
One major reason is the large amount of:
electrical energy required.
The process also requires high-temperature equipment, raw materials, electrodes, and continuous industrial operation.
Worked Example 3
Why is copper electrorefined?
Many electrical applications require:
very pure copper.
Electrorefining transfers copper from an impure anode to a high-purity cathode.
Worked Example 4
A copper electrorefining cathode gains mass.
Explain why.
Cu²⁺ ions gain electrons:
Cu²⁺ + 2e⁻ → Cu
Solid copper is deposited on the cathode.
Therefore its:
mass increases.
Worked Example 5
Why is the chlor-alkali process economically important?
It produces several widely used industrial chemicals:
chlorine, hydrogen, and sodium hydroxide.
These products are used as inputs in many other manufacturing processes.
Worked Example 6
Why might a hydrogen electrolyzer be located near a renewable electricity source?
Electrolysis requires:
electricity.
Locating production near suitable renewable generation can provide low-carbon electricity and may reduce some transmission or infrastructure requirements.
Worked Example 7
Why can recycling metals reduce energy use?
Producing metals from ores may require:
- mining
- ore processing
- high temperatures
- electrolysis
Recycling can avoid some of these energy-intensive stages.
Worked Example 8
What is the difference between electrorefining and electrowinning?
Electrorefining:
purifies an existing impure metal.
Electrowinning:
recovers metal from ions in solution.
Both deposit metal through reduction at the:
cathode.
Worked Example 9
Why is electroplating economically useful?
A thin coating can provide valuable surface properties without making the entire object from an:
expensive material.
This can reduce material costs while improving product performance.
Worked Example 10
An industrial electrolysis cell uses 20,000 A for 30 minutes.
Calculate the charge transferred.
Convert time:
30 min × 60 = 1800 s
Use:
Q = It
Q = 20,000 × 1800
Q = 36,000,000 C
Therefore:
36 million coulombs
of charge pass through the cell.
Future Industrial Electrochemistry
Electrochemistry is increasingly important in developing technologies related to:
- renewable energy storage
- hydrogen production
- carbon dioxide conversion
- battery recycling
- metal recovery
- low-carbon manufacturing
- advanced batteries
- new electrode materials
The ability to use electricity to drive chemical reactions creates opportunities to connect industrial manufacturing with:
low-carbon electricity.
Common Mistake: Electrochemistry Is Only About Batteries
Batteries are one application.
Industrial electrochemistry also includes:
- metal extraction
- metal purification
- electroplating
- chemical production
- hydrogen production
- corrosion protection
Its industrial applications are:
much broader.
Common Mistake: Electrolysis Only Produces Metals
Electrolysis can produce many different substances.
Examples include:
- metals
- hydrogen
- oxygen
- chlorine
- sodium hydroxide
- specialized chemical products
The products depend on the:
electrolyte and operating conditions.
Common Mistake: The Cheapest Process Uses the Least Electricity
Electricity is only one part of industrial cost.
Manufacturers must also consider:
- raw materials
- labor
- equipment
- maintenance
- product value
- waste treatment
- transport
- co-products
Economic evaluation requires considering the:
whole process.
Common Mistake: Electrolysis Is Automatically Environmentally Friendly
Electrolysis can support lower-carbon technologies, but its environmental impact depends on:
- electricity source
- energy efficiency
- raw materials
- waste
- equipment manufacture
- product handling
The entire system must therefore be:
evaluated.
Check Your Understanding
- Define industrial electrochemistry.
- Give five examples of industrial electrochemical processes.
- What energy transformation occurs during electrolysis?
- What energy transformation occurs in a galvanic cell?
- Where does oxidation occur?
- Where does reduction occur?
- Why is electrolysis useful for extracting reactive metals?
- Write the reduction half-equation for Al³⁺.
- Name the industrial process used to produce aluminum.
- Why is cryolite used in aluminum production?
- What happens to carbon anodes during conventional aluminum production?
- Why does aluminum production require large amounts of electricity?
- Why is recycling aluminum important?
- Write the cathode half-equation for sodium production.
- Write the cathode half-equation for magnesium production.
- What is the chlor-alkali process?
- Name its three major products.
- Write the cathode half-equation for the chlor-alkali process.
- Write the anode half-equation.
- Give two industrial uses of chlorine.
- Give two industrial uses of sodium hydroxide.
- What is electrorefining?
- Describe the arrangement used in copper electrorefining.
- Write the reaction at the copper anode.
- Write the reaction at the copper cathode.
- Why is highly pure copper economically important?
- What can happen to impurities during copper electrorefining?
- What is electrowinning?
- How does electrowinning differ from electrorefining?
- What is electroplating?
- Give three industrial reasons for electroplating.
- Explain how water electrolysis produces hydrogen.
- What is commonly meant by green hydrogen?
- Why does the electricity source matter when evaluating hydrogen production?
- Explain how batteries use electrochemistry.
- What is cathodic protection?
- What is a sacrificial anode?
- Give two structures that can use cathodic protection.
- State the equation Q = It.
- Calculate the charge transferred by a 1000 A current for 600 s.
- Why are large currents often used in industrial electrolysis?
- What is current efficiency?
- Give three causes of energy loss in industrial electrolysis.
- Give three economic benefits of industrial electrochemistry.
- Give three challenges associated with industrial electrochemistry.
- Explain why electroplating can reduce manufacturing costs.
- Explain why electrorefining can increase the economic value of a metal.
- Explain why renewable electricity could affect the environmental impact of electrolysis.
- Compare the purposes of metal extraction, electrorefining, and electrowinning.
- Evaluate one industrial electrochemical process by considering its products, benefits, energy requirements, costs, and environmental impacts.
Key Terms
Industrial electrochemistry: Large-scale application of electrochemical reactions to manufacturing, energy, metal processing, and other industrial processes.
Electrolysis: Use of electrical energy to drive a non-spontaneous chemical reaction.
Electrorefining: Electrochemical purification of an impure metal.
Electrowinning: Electrochemical recovery of a metal from ions in solution.
Electroplating: Electrochemical deposition of a metal coating onto an object.
Hall-Héroult process: Industrial electrolytic process used to produce aluminum.
Chlor-alkali process: Electrolysis of brine to produce chlorine, hydrogen, and sodium hydroxide.
Brine: Concentrated sodium chloride solution.
Cathodic protection: Technique that reduces corrosion by making the protected structure act as a cathode.
Sacrificial anode: More reactive metal deliberately oxidized to protect another metal.
Current efficiency: Fraction of electrical charge that produces the desired electrochemical reaction.
Energy efficiency: Fraction of supplied energy converted into useful output.
Co-product: Useful secondary product produced alongside the main product.
Green hydrogen: Common term for hydrogen produced by electrolysis using renewable electricity.
Key Takeaways
- Industrial electrochemistry uses electron-transfer reactions on a large scale.
- Electrolysis converts electrical energy into chemical change.
- Electrochemistry is used for metal extraction, purification, electroplating, chemical manufacture, hydrogen production, batteries, and corrosion protection.
- Highly reactive metals such as aluminum, sodium, and magnesium can be produced using electrolysis.
- Aluminum is produced industrially using the Hall-Héroult process.
- The chlor-alkali process produces chlorine, hydrogen, and sodium hydroxide from brine.
- Electrorefining produces high-purity metals such as copper.
- Electrowinning recovers metals from solutions containing their ions.
- Electroplating modifies surfaces without requiring the entire object to be made from the coating material.
- Water electrolysis can convert electrical energy into chemical energy stored in hydrogen.
- Batteries and fuel cells are also major applications of industrial electrochemistry.
- Electrochemical technologies can provide precise control and high-purity products.
- Major challenges include electricity demand, cost, electrode degradation, waste, raw materials, and environmental impacts.
- The environmental impact of electrolysis depends strongly on the source of the electricity and the efficiency of the process.
- Industrial electrochemistry is economically important because it supplies essential materials and chemicals to many other industries.