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Questions and Answers
What is a battery?
What is a battery?
A device that can store chemical energy and later release it as electrical energy at a constant voltage.
What are the three main types of batteries?
What are the three main types of batteries?
- Primary Batteries
- Secondary Batteries
- Flow Batteries and Fuel Cells
- All of the above (correct)
Primary cells can be recharged.
Primary cells can be recharged.
False (B)
What determines the lifetime of a primary cell?
What determines the lifetime of a primary cell?
The battery "dies" when the reactants have been converted into products.
The battery "dies" when the reactants have been converted into products.
The voltage output of a battery remains constant throughout its lifetime.
The voltage output of a battery remains constant throughout its lifetime.
What is a secondary cell?
What is a secondary cell?
To make a rechargeable battery, we must be able to reverse the redox reaction.
To make a rechargeable battery, we must be able to reverse the redox reaction.
The cell reaction must be endothermic to supply energy.
The cell reaction must be endothermic to supply energy.
An external energy source is always needed to recharge a battery.
An external energy source is always needed to recharge a battery.
A given reaction can always be reversed.
A given reaction can always be reversed.
What is the defining characteristic of primary batteries?
What is the defining characteristic of primary batteries?
What is the defining characteristic of secondary batteries?
What is the defining characteristic of secondary batteries?
What is the defining characteristic of flow batteries and fuel cells?
What is the defining characteristic of flow batteries and fuel cells?
What is the purpose of the anode in a battery?
What is the purpose of the anode in a battery?
What is the purpose of the electrolyte in a battery?
What is the purpose of the electrolyte in a battery?
What is the purpose of the separator in a battery?
What is the purpose of the separator in a battery?
What is voltage/EMF?
What is voltage/EMF?
What is current?
What is current?
What is current capacity?
What is current capacity?
What is power density?
What is power density?
Energy efficiency is applicable for both primary and secondary cells.
Energy efficiency is applicable for both primary and secondary cells.
What is cycle life?
What is cycle life?
What is self-discharge?
What is self-discharge?
Which of the following are differences between primary and secondary batteries?
Which of the following are differences between primary and secondary batteries?
What happens during discharging in a battery?
What happens during discharging in a battery?
What is the most common type of secondary battery in use today?
What is the most common type of secondary battery in use today?
The lead-acid battery was invented in the late 19th century.
The lead-acid battery was invented in the late 19th century.
What are the three main components of a single lead-acid cell?
What are the three main components of a single lead-acid cell?
Why is an insulating separator used in a lead-acid battery?
Why is an insulating separator used in a lead-acid battery?
A single lead-acid cell produces a potential of approximately 12.6V.
A single lead-acid cell produces a potential of approximately 12.6V.
How is a 12.6V lead-acid battery typically constructed?
How is a 12.6V lead-acid battery typically constructed?
The lead-acid battery is the first rechargeable battery ever discovered.
The lead-acid battery is the first rechargeable battery ever discovered.
What is the electrolyte in a lead-acid battery?
What is the electrolyte in a lead-acid battery?
Lead-acid batteries are generally categorized as nontoxic waste.
Lead-acid batteries are generally categorized as nontoxic waste.
What is the anode reaction in a lead-acid battery?
What is the anode reaction in a lead-acid battery?
What is the overall chemical reaction in a lead-acid battery during discharging?
What is the overall chemical reaction in a lead-acid battery during discharging?
What happens to the concentration of H2SO4 during discharging?
What happens to the concentration of H2SO4 during discharging?
The lead-acid battery can be recharged indefinitely.
The lead-acid battery can be recharged indefinitely.
What is the anode reaction in a lead-acid battery during charging?
What is the anode reaction in a lead-acid battery during charging?
What is the most common application of lead-acid batteries?
What is the most common application of lead-acid batteries?
What is a lithium-ion battery?
What is a lithium-ion battery?
What is the anode material in a lithium-ion battery?
What is the anode material in a lithium-ion battery?
Lithium-ion batteries use an aqueous electrolyte.
Lithium-ion batteries use an aqueous electrolyte.
Why is lithium-ion battery technology known for its lightweight and high energy density features?
Why is lithium-ion battery technology known for its lightweight and high energy density features?
Lithium-ion batteries are considered nontoxic waste.
Lithium-ion batteries are considered nontoxic waste.
Overcharging lithium-ion batteries can cause a loss in efficiency.
Overcharging lithium-ion batteries can cause a loss in efficiency.
Dendrites are a potential safety concern in lithium-ion batteries.
Dendrites are a potential safety concern in lithium-ion batteries.
Flashcards
Redox Reaction
Redox Reaction
A chemical reaction involving the transfer of electrons between species.
Oxidation
Oxidation
A process where a substance loses electrons.
Reduction
Reduction
A process where a substance gains electrons.
Battery
Battery
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Primary Battery
Primary Battery
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Secondary Battery
Secondary Battery
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Flow Battery
Flow Battery
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Fuel Cell
Fuel Cell
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Anode
Anode
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Cathode
Cathode
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Electrolyte
Electrolyte
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Separator
Separator
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Cycle Life
Cycle Life
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Shelf Life
Shelf Life
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Self-Discharge
Self-Discharge
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Lead-Acid Battery
Lead-Acid Battery
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Battery Discharging
Battery Discharging
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Battery Charging
Battery Charging
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Battery Failure Point
Battery Failure Point
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Intercalation
Intercalation
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Lithium-ion Battery
Lithium-ion Battery
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Overcharging Effect
Overcharging Effect
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Dendrites
Dendrites
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Rechargeable Nature
Rechargeable Nature
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Cathode
Cathode
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Anode
Anode
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Electrolyte
Electrolyte
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Separator
Separator
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Primary Battery
Primary Battery
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Secondary Battery
Secondary Battery
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Study Notes
Batteries
- Batteries are devices that store chemical energy and release it as electrical energy at a constant voltage.
- Redox reactions, involving electron transfer between species, are fundamental to battery function. Electrons move in generating and delivering electricity, connecting redox reactions to electrical systems.
- If the oxidation and reduction half-reactions are separated, electrons can flow, creating a circuit.
- A galvanic cell generates an electric current. A battery is a commercially significant example of a galvanic cell.
Battery Classification
- Primary Batteries: Electrochemical reactions are irreversible. Once the reactants are used up, no more current can be produced.
- Secondary Batteries: Electrochemical reactions are reversible. These can be recharged and used repeatedly.
- Flow Batteries and Fuel Cells: Materials (reactants, products, electrolyte) flow through the battery. Unlike traditional batteries, these don't store electrical energy but directly convert chemical energy into electrical at need.
Primary Cell Structure and Lifetimes
- The lifetime of a primary battery depends on the amount of reactants.
- A battery "dies" when the reactants run out, halting the reaction.
- In practice, the voltage output of a typical primary battery decreases near the end of its life, usually failing before reactants are completely consumed.
Secondary Cell
- Secondary cells can be recharged, offering a much longer life cycle.
- To be rechargeable, the redox reaction must be fully reversible, converting products back to reactants. The reverse reaction needs an external energy source, like a charger, to overcome this.
Principal Components
- Anode: Electrode where materials oxidize, releasing electrons.
- Cathode: Electrode where materials reduce, accepting electrons.
- Electrolyte: Facilitates ion migration, leading to electrical current production.
- Separator: Prevents product mixing at the electrodes and ensures only ions move through the electrolyte while electrons travel through the circuit.
Battery Characteristics
- Voltage/EMF: Potential difference between battery electrodes.
- Current: Rate of discharge reactions in the cell.
- Current Capacity: Amount of current generated per unit time.
- Power Density: Amount of power output per unit weight of the cell.
- Energy Density: Amount of energy available per unit weight of the cell.
- Energy Efficiency (applicable for secondary cells): Efficiency of converting input energy to electrical output.
- Cycle Life: Repeated number of discharge/charge cycles a battery can handle.
- Shelf Life: Time duration a battery can store charge without use under steady conditions.
- Self-Discharge: Battery loses charge even when not in use due to ongoing chemical reactions.
Lead-Acid Battery
- The lead-acid battery is one of the first commercially available secondary batteries.
- It consists of a lead anode, lead dioxide cathode, and a sulfuric acid electrolyte.
- A single cell produces about 2.05 volts; commonly 6 cells are connected in series to reach roughly 12.1 volts.
Lead-Acid Battery: Discharging and Charging Process
- Discharging involves oxidation at the anode and reduction at the cathode; electrons flow through an external circuit.
- Lead sulfate precipitates on the electrodes.
- Concentration of H2SO4 in the electrolyte decreases during discharging.
- Charging reverses this process. The PbSO4 coating returns to Pb and PbO2, requiring an external energy source (like charging). The H2SO4 concentration increases in the process.
Lead-Acid Battery: Issues
- Overcharging: water electrolysis, hydrogen and oxygen gas generation, increased water loss, and more acid concentration lead to higher electrode corrosion.
- Water evaporation: Increased H2SO4 concentration, increasing electrolyte viscosity, decreasing ionic mobility, requiring water re-addition
- Leaking: New batteries need to have appropriate sealed components and housings; old batteries need proper disposal
Lithium-ion Batteries
- The lithium-ion battery is a popular rechargeable battery, used in laptops, cell phones and electric vehicles.
- It's constructed with an anode (e.g., graphite) and a cathode (e.g., lithium metal oxide, often cobalt oxide).
- An organic solvent based electrolyte is necessary to prevent oxidation. Porous separators facilitate ion flow.
- In discharge, lithium ions move from the anode to the cathode; in charging, lithium moves back to anode.
- Lithium-ion batteries have high energy density, making them useful in lightweight devices but are vulnerable to overcharging leading to dendrite formation, which can cause fires.
Lithium-ion Battery Applications
- Extensively used in consumer electronics.
- Used in many portable electronic devices to improve power.
Summary of Key Differences
| Feature | Primary Battery | Secondary Battery |
|---|---|---|
| Chemical Reactions | Irreversible | Reversible |
| Rechargeability | No | Yes |
| Use | Reusable once reacted, single use | Reusable and rechargable |
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Description
Explore the fascinating world of batteries and how they operate. This quiz covers the fundamental principles of batteries, including redox reactions, types of batteries such as primary and secondary batteries, as well as flow batteries and fuel cells. Test your knowledge on how these energy storage devices function and their significance in electrical systems.
