The document provides information about batteries, including their components and functions. It discusses the basic components of batteries like electrodes, electrolytes and separators. It explains the differences between primary and secondary batteries and provides examples like dry cell and lead acid batteries. It also covers topics like charging, discharging, specific gravity, electrolysis, series and parallel connections. Guidelines are provided for maintenance, safety, ventilation and jump starting batteries.
The document discusses batteries and their components. It describes how batteries work by converting chemical energy into electrical energy through reversible chemical reactions. The two main types are primary batteries that cannot be recharged and secondary batteries that can be recharged by passing a current in the opposite direction of discharge. Key components include electrodes, electrolyte and separators. Safety issues like ventilation and handling of hazardous materials like sulfuric acid and lead are also covered.
The document provides information on batteries, including:
1) Batteries convert chemical energy into electrical energy through reversible chemical reactions and can be recharged by passing current in the opposite direction of discharge.
2) Batteries contain hazardous materials like sulfuric acid and lead that can cause burns, nerve damage, and other health issues if exposed.
3) Primary batteries convert chemical energy directly while secondary batteries must be charged first before use and can be recharged multiple times.
battery presentation on lead acid cycle and chargingvineetnavrang7882
This document provides information about lead-acid batteries, including:
1. It describes the basic components and chemistry of lead-acid batteries, including electrodes, electrolyte, plates, and charging/discharging reactions.
2. It discusses different types of lead-acid batteries like flooded, VRLA, tubular, and flat plate designs.
3. It provides specifications, test procedures, troubleshooting tips, and maintenance guidelines for lead-acid batteries used in railway applications.
The document discusses caring for and testing lead-acid batteries used in railway signaling applications. It describes the classification of primary and secondary cells, the types of lead-acid cells used, their construction, chemical reactions, and how to monitor state of charge through specific gravity measurements. It also provides guidance on initial charging, maintenance, capacity testing, and tips to maximize battery life.
The document discusses caring for and testing lead-acid batteries used in railway signaling applications. It describes the classification of primary and secondary cells, the types of lead-acid cells used, their construction, chemical reactions, and how to monitor state of charge through specific gravity measurements. It also provides guidance on initial charging, maintenance, capacity testing, and tips to maximize battery life.
1. The document provides a historical overview of water electrolysis from its discovery in 1789 to modern developments. Nicholson and Carlisle were the first to develop the technique in 1800, and by 1902 there were over 400 industrial units in operation.
2. It explains the theory behind water electrolysis, including the chemical reactions that produce hydrogen and oxygen, factors that determine minimum voltage requirements, and sources of inefficiency.
3. Various methods for producing hydrogen through water electrolysis are briefly described, including alkaline electrolysis, proton exchange membrane electrolysis, and producing hydrogen as a byproduct of chloralkali production. Advanced alkaline systems and high-pressure designs are highlighted.
The document discusses automotive batteries and their characteristics. It begins by introducing lead-acid batteries and their electrochemical reactions that allow them to store and produce electrical energy. It then discusses (1) the construction of lead-acid batteries, including their lead plates and sulfuric acid electrolyte, (2) how their chemical reactions allow them to convert chemical energy into electrical energy during discharge and vice versa during charging, and (3) common tests used to determine a battery's state of charge such as hydrometer tests and heavy duty discharge tests. The document emphasizes that a battery's rating is determined by how much current it can produce and for how long, with common ratings including amp-hour capacity, reserve capacity, and cold cranking
This document discusses direct energy conversion through photovoltaic cells and fuel cells. It provides details on:
1) How photovoltaic cells convert solar energy into electrical energy through a module of approximately 30 cells producing around 15V and 1.5A of current. Applications include water pumping, commercial and residential power, and consumer electronics.
2) What fuel cells are, how they convert hydrogen and oxygen into water and electricity through electrochemical reactions. Types are classified by temperature and electrolyte used, with hydrogen-oxygen and fossil fuel cells discussed in detail.
3) Advantages of fuel cells include high efficiency and low emissions, while disadvantages include higher costs and difficulties with hydrogen production and storage.
The document discusses batteries and their components. It describes how batteries work by converting chemical energy into electrical energy through reversible chemical reactions. The two main types are primary batteries that cannot be recharged and secondary batteries that can be recharged by passing a current in the opposite direction of discharge. Key components include electrodes, electrolyte and separators. Safety issues like ventilation and handling of hazardous materials like sulfuric acid and lead are also covered.
The document provides information on batteries, including:
1) Batteries convert chemical energy into electrical energy through reversible chemical reactions and can be recharged by passing current in the opposite direction of discharge.
2) Batteries contain hazardous materials like sulfuric acid and lead that can cause burns, nerve damage, and other health issues if exposed.
3) Primary batteries convert chemical energy directly while secondary batteries must be charged first before use and can be recharged multiple times.
battery presentation on lead acid cycle and chargingvineetnavrang7882
This document provides information about lead-acid batteries, including:
1. It describes the basic components and chemistry of lead-acid batteries, including electrodes, electrolyte, plates, and charging/discharging reactions.
2. It discusses different types of lead-acid batteries like flooded, VRLA, tubular, and flat plate designs.
3. It provides specifications, test procedures, troubleshooting tips, and maintenance guidelines for lead-acid batteries used in railway applications.
The document discusses caring for and testing lead-acid batteries used in railway signaling applications. It describes the classification of primary and secondary cells, the types of lead-acid cells used, their construction, chemical reactions, and how to monitor state of charge through specific gravity measurements. It also provides guidance on initial charging, maintenance, capacity testing, and tips to maximize battery life.
The document discusses caring for and testing lead-acid batteries used in railway signaling applications. It describes the classification of primary and secondary cells, the types of lead-acid cells used, their construction, chemical reactions, and how to monitor state of charge through specific gravity measurements. It also provides guidance on initial charging, maintenance, capacity testing, and tips to maximize battery life.
1. The document provides a historical overview of water electrolysis from its discovery in 1789 to modern developments. Nicholson and Carlisle were the first to develop the technique in 1800, and by 1902 there were over 400 industrial units in operation.
2. It explains the theory behind water electrolysis, including the chemical reactions that produce hydrogen and oxygen, factors that determine minimum voltage requirements, and sources of inefficiency.
3. Various methods for producing hydrogen through water electrolysis are briefly described, including alkaline electrolysis, proton exchange membrane electrolysis, and producing hydrogen as a byproduct of chloralkali production. Advanced alkaline systems and high-pressure designs are highlighted.
The document discusses automotive batteries and their characteristics. It begins by introducing lead-acid batteries and their electrochemical reactions that allow them to store and produce electrical energy. It then discusses (1) the construction of lead-acid batteries, including their lead plates and sulfuric acid electrolyte, (2) how their chemical reactions allow them to convert chemical energy into electrical energy during discharge and vice versa during charging, and (3) common tests used to determine a battery's state of charge such as hydrometer tests and heavy duty discharge tests. The document emphasizes that a battery's rating is determined by how much current it can produce and for how long, with common ratings including amp-hour capacity, reserve capacity, and cold cranking
This document discusses direct energy conversion through photovoltaic cells and fuel cells. It provides details on:
1) How photovoltaic cells convert solar energy into electrical energy through a module of approximately 30 cells producing around 15V and 1.5A of current. Applications include water pumping, commercial and residential power, and consumer electronics.
2) What fuel cells are, how they convert hydrogen and oxygen into water and electricity through electrochemical reactions. Types are classified by temperature and electrolyte used, with hydrogen-oxygen and fossil fuel cells discussed in detail.
3) Advantages of fuel cells include high efficiency and low emissions, while disadvantages include higher costs and difficulties with hydrogen production and storage.
Direct energy conversion (PV Cell, Fuel Cell)Ashish Bandewar
Direct Energy Conversion :- Photo voltage cells: Principle, concept of energy conversion, conversion efficiency, power output and performance, storage, Fuel Cells : Principles types of fuel cells, conversion efficiency
Potentiometry is an electroanalytical technique that uses potentiometers to measure electrochemical potential. It involves using reference and indicator electrodes immersed in analyte solutions. The potential difference between the electrodes depends on ion activity/concentration based on the Nernst equation, allowing for quantitative analysis. A salt bridge containing a neutral salt maintains electrical neutrality between electrode half-cells. Common reference electrodes include silver/silver chloride and saturated calomel electrodes. Potentiometry is used for pH measurements and potentiometric titrations.
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Electrochemistry is the study of chemical reactions caused by the passage of an electric current and the production of electrical energy from chemical reactions. It encompasses phenomena like corrosion and devices like batteries and fuel cells. Electrochemical cells are either electrolytic cells, where an external power source drives non-spontaneous reactions, or galvanic/voltaic cells, where spontaneous reactions produce electricity. The kinetics and rates of electrochemical reactions, as well as mass transfer of reactants, influence current production in fuel cells and other devices.
The document provides an overview of traction batteries and chargers. It discusses how lead-acid batteries work by storing chemical energy that is converted to electrical energy. It covers best practices for operations and maintenance of batteries, including proper charging, water levels, and safety procedures. Factors that affect battery life such as charging currents and temperatures are also summarized.
The document discusses the basics of electrochemical cells and batteries. It covers topics like nominal voltage, operating voltage, capacity, self-discharge, depth of discharge, energy density, service life, and shelf life. It also discusses primary cells like Leclanché cells, alkaline cells, and lithium primary cells. Their chemistries and applications are explained. Secondary cells and batteries are defined. The differences between galvanic cells and electrolytic cells are highlighted.
Electrogravimetry involves the electrolytic deposition of an element onto an electrode, which is then weighed before and after deposition to determine the amount deposited. There are two main methods - constant current electrolysis, where current is kept constant and potential varies, and constant potential electrolysis, where potential is kept constant. Electrogravimetry can be used to determine the concentration of elements in solutions and to separate elements electrolytically based on their deposition potentials. It has applications in quantitative analysis, electrosynthesis, separating species in solutions, and purifying reagents.
The document discusses the function, construction, types, inspection, and charging of automotive batteries. It states that a battery provides electricity to vehicle systems when the engine is not running and supplies power to start the engine. It is constructed of six lead plate cells filled with sulfuric acid electrolyte. Battery condition, electrolyte level, specific gravity, and voltage are checked during inspection. Batteries are charged using manual or automatic chargers to reverse the chemical reaction and restore the lost charge.
This document discusses cyclic voltammetry, which is a type of potentiodynamic electrochemical measurement where the current in an electrochemical cell is measured while the cell's potential is varied linearly with time. It describes the components of a voltammetry system, including the working, reference, and counter electrodes, as well as the supporting electrolyte. It also explains the triangular potential waveform used and defines terms like peak current and peak potential. Examples of using cyclic voltammetry to study the redox reaction of hexacyanoferrate ions and biological redox systems like cytochromes are provided.
This document provides an overview of an active learning assignment on fuel cells. It discusses the basic components and workings of a fuel cell, including the electrodes, electrolyte, and catalyst. It also describes the reactions that take place in fuel cells to convert chemical energy to electrical energy. Finally, it outlines the main types of fuel cells, classified based on their electrolyte: alkaline, molten carbonate, phosphoric acid, proton exchange membrane, and solid oxide fuel cells. For each type it provides details on operating temperature, efficiency, applications, and other characteristics.
Basic Fundamental Electronics by D-Sarda PART VIIDinesh Sarda
Alessandro Volta invented the first battery in 1791 by arranging two different metals separated by a brine-soaked material. A cell generates electricity through a chemical reaction between electrodes and an electrolyte. A battery consists of two or more connected cells. Primary batteries produce electricity through an irreversible chemical reaction and cannot be recharged, while secondary batteries use a reversible reaction and can be recharged. The lead-acid battery commonly uses sulfuric acid electrolyte and lead plates; it produces about 2 volts per cell and is widely used in automobiles and backup power systems.
This document provides an overview of electrochemistry concepts including:
1) Galvanic (voltaic) cells which are spontaneous chemical reactions that can be used as batteries. They have an anode, cathode, salt bridge or porous disk, and electron flow from anode to cathode.
2) Electrolytic cells which are non-spontaneous and require an external electron source like a DC power supply.
3) Standard reduction potentials which indicate the tendency of elements to gain or lose electrons. More positive potentials indicate easier reduction. This can be used to determine if a reaction is spontaneous.
4) The Nernst equation relates cell potential to non-standard conditions by accounting for react
Batteries convert chemical energy into electrical energy through reversible chemical reactions. There are two main types - primary batteries that cannot be recharged and secondary batteries that can be recharged. Lead-acid batteries are commonly used for storage in photovoltaic systems due to their low cost and long life, though they require regular maintenance. Proper ventilation is needed when charging batteries to prevent accumulation of explosive hydrogen gas. State of charge, depth of discharge, and other factors must be considered when selecting and sizing batteries.
The document discusses key parameters for energy storage batteries including costs, energy and power densities, life cycles, capacity, charging and discharging rates, and safety. It provides details on lithium-ion battery chemistry, comparing chemistries like LCO, NMC, LFP. Slow versus fast charging rates are outlined based on C-rates. Requirements for batteries like energy, power, life, safety and costs are covered. The document also discusses concepts like state of charge estimation, measuring state of health, and self-discharge in batteries. Battery pack design considerations like thermal management, cell balancing and safety are also summarized.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
The document discusses pH electrodes and their working mechanism. It describes that a pH electrode consists of a glass electrode and a calomel electrode that are dipped in an aqueous solution. The potential difference developed across the thin glass bulb of the electrode depends on the pH of the solution. This potential is recorded using a potentiometer or pH meter calibrated to read pH directly. Important components of a pH meter including the glass electrode, calomel electrode, and electrometer are also explained.
This document provides an overview of various electrochemical techniques used to measure corrosion rates, including polarization resistance (LPR), electrochemical frequency modulation (EFM), and electrochemical impedance spectroscopy (EIS). It explains that corrosion is an electrochemical process involving electron transfer, and electrochemical methods are fast, sensitive techniques that can be used both in the lab and in the field to measure very low corrosion rates. It also discusses important concepts in electrochemistry including potential, current, reference electrodes, and how controlled potential experiments are commonly used to obtain corrosion rate measurements.
Batteries -Introduction – Types of Batteries – discharging and charging of battery - characteristics of battery –battery rating- various tests on battery- – Primary battery: silver button cell- Secondary battery :Ni-Cd battery-modern battery: lithium ion battery-maintenance of batteries-choices of batteries for electric vehicle applications.
Fuel Cells: Introduction- importance and classification of fuel cells - description, principle, components, applications of fuel cells: H2-O2 fuel cell, alkaline fuel cell, molten carbonate fuel cell and direct methanol fuel cells.
Direct energy conversion (PV Cell, Fuel Cell)Ashish Bandewar
Direct Energy Conversion :- Photo voltage cells: Principle, concept of energy conversion, conversion efficiency, power output and performance, storage, Fuel Cells : Principles types of fuel cells, conversion efficiency
Potentiometry is an electroanalytical technique that uses potentiometers to measure electrochemical potential. It involves using reference and indicator electrodes immersed in analyte solutions. The potential difference between the electrodes depends on ion activity/concentration based on the Nernst equation, allowing for quantitative analysis. A salt bridge containing a neutral salt maintains electrical neutrality between electrode half-cells. Common reference electrodes include silver/silver chloride and saturated calomel electrodes. Potentiometry is used for pH measurements and potentiometric titrations.
I Hope You all like it very much. I wish it is beneficial for all of you and you can get enough knowledge from it. Clear and appropriate objectives, in terms of what the audience ought to feel, think, and do as a result of seeing the presentation. Objectives are realistic – and may be intermediate parts of a wider plan.
Electrochemistry is the study of chemical reactions caused by the passage of an electric current and the production of electrical energy from chemical reactions. It encompasses phenomena like corrosion and devices like batteries and fuel cells. Electrochemical cells are either electrolytic cells, where an external power source drives non-spontaneous reactions, or galvanic/voltaic cells, where spontaneous reactions produce electricity. The kinetics and rates of electrochemical reactions, as well as mass transfer of reactants, influence current production in fuel cells and other devices.
The document provides an overview of traction batteries and chargers. It discusses how lead-acid batteries work by storing chemical energy that is converted to electrical energy. It covers best practices for operations and maintenance of batteries, including proper charging, water levels, and safety procedures. Factors that affect battery life such as charging currents and temperatures are also summarized.
The document discusses the basics of electrochemical cells and batteries. It covers topics like nominal voltage, operating voltage, capacity, self-discharge, depth of discharge, energy density, service life, and shelf life. It also discusses primary cells like Leclanché cells, alkaline cells, and lithium primary cells. Their chemistries and applications are explained. Secondary cells and batteries are defined. The differences between galvanic cells and electrolytic cells are highlighted.
Electrogravimetry involves the electrolytic deposition of an element onto an electrode, which is then weighed before and after deposition to determine the amount deposited. There are two main methods - constant current electrolysis, where current is kept constant and potential varies, and constant potential electrolysis, where potential is kept constant. Electrogravimetry can be used to determine the concentration of elements in solutions and to separate elements electrolytically based on their deposition potentials. It has applications in quantitative analysis, electrosynthesis, separating species in solutions, and purifying reagents.
The document discusses the function, construction, types, inspection, and charging of automotive batteries. It states that a battery provides electricity to vehicle systems when the engine is not running and supplies power to start the engine. It is constructed of six lead plate cells filled with sulfuric acid electrolyte. Battery condition, electrolyte level, specific gravity, and voltage are checked during inspection. Batteries are charged using manual or automatic chargers to reverse the chemical reaction and restore the lost charge.
This document discusses cyclic voltammetry, which is a type of potentiodynamic electrochemical measurement where the current in an electrochemical cell is measured while the cell's potential is varied linearly with time. It describes the components of a voltammetry system, including the working, reference, and counter electrodes, as well as the supporting electrolyte. It also explains the triangular potential waveform used and defines terms like peak current and peak potential. Examples of using cyclic voltammetry to study the redox reaction of hexacyanoferrate ions and biological redox systems like cytochromes are provided.
This document provides an overview of an active learning assignment on fuel cells. It discusses the basic components and workings of a fuel cell, including the electrodes, electrolyte, and catalyst. It also describes the reactions that take place in fuel cells to convert chemical energy to electrical energy. Finally, it outlines the main types of fuel cells, classified based on their electrolyte: alkaline, molten carbonate, phosphoric acid, proton exchange membrane, and solid oxide fuel cells. For each type it provides details on operating temperature, efficiency, applications, and other characteristics.
Basic Fundamental Electronics by D-Sarda PART VIIDinesh Sarda
Alessandro Volta invented the first battery in 1791 by arranging two different metals separated by a brine-soaked material. A cell generates electricity through a chemical reaction between electrodes and an electrolyte. A battery consists of two or more connected cells. Primary batteries produce electricity through an irreversible chemical reaction and cannot be recharged, while secondary batteries use a reversible reaction and can be recharged. The lead-acid battery commonly uses sulfuric acid electrolyte and lead plates; it produces about 2 volts per cell and is widely used in automobiles and backup power systems.
This document provides an overview of electrochemistry concepts including:
1) Galvanic (voltaic) cells which are spontaneous chemical reactions that can be used as batteries. They have an anode, cathode, salt bridge or porous disk, and electron flow from anode to cathode.
2) Electrolytic cells which are non-spontaneous and require an external electron source like a DC power supply.
3) Standard reduction potentials which indicate the tendency of elements to gain or lose electrons. More positive potentials indicate easier reduction. This can be used to determine if a reaction is spontaneous.
4) The Nernst equation relates cell potential to non-standard conditions by accounting for react
Batteries convert chemical energy into electrical energy through reversible chemical reactions. There are two main types - primary batteries that cannot be recharged and secondary batteries that can be recharged. Lead-acid batteries are commonly used for storage in photovoltaic systems due to their low cost and long life, though they require regular maintenance. Proper ventilation is needed when charging batteries to prevent accumulation of explosive hydrogen gas. State of charge, depth of discharge, and other factors must be considered when selecting and sizing batteries.
The document discusses key parameters for energy storage batteries including costs, energy and power densities, life cycles, capacity, charging and discharging rates, and safety. It provides details on lithium-ion battery chemistry, comparing chemistries like LCO, NMC, LFP. Slow versus fast charging rates are outlined based on C-rates. Requirements for batteries like energy, power, life, safety and costs are covered. The document also discusses concepts like state of charge estimation, measuring state of health, and self-discharge in batteries. Battery pack design considerations like thermal management, cell balancing and safety are also summarized.
Electrochemistry class 12 ( a continuation of redox reaction of grade 11)ritik
Electrochemistry involves the study of chemical reactions that produce electricity and chemical reactions produced by electricity. A galvanic (voltaic) cell converts the chemical energy of a spontaneous redox reaction into electrical energy. Daniell's cell uses the redox reaction of zinc oxidizing copper ions to produce a cell potential of 1.1 V. An electrolytic cell uses an applied voltage to drive a nonspontaneous redox reaction in the opposite direction of the natural reaction in a galvanic cell. Standard reduction potentials allow prediction of the tendency of half-reactions to occur and their oxidizing or reducing power.
The document discusses pH electrodes and their working mechanism. It describes that a pH electrode consists of a glass electrode and a calomel electrode that are dipped in an aqueous solution. The potential difference developed across the thin glass bulb of the electrode depends on the pH of the solution. This potential is recorded using a potentiometer or pH meter calibrated to read pH directly. Important components of a pH meter including the glass electrode, calomel electrode, and electrometer are also explained.
This document provides an overview of various electrochemical techniques used to measure corrosion rates, including polarization resistance (LPR), electrochemical frequency modulation (EFM), and electrochemical impedance spectroscopy (EIS). It explains that corrosion is an electrochemical process involving electron transfer, and electrochemical methods are fast, sensitive techniques that can be used both in the lab and in the field to measure very low corrosion rates. It also discusses important concepts in electrochemistry including potential, current, reference electrodes, and how controlled potential experiments are commonly used to obtain corrosion rate measurements.
Batteries -Introduction – Types of Batteries – discharging and charging of battery - characteristics of battery –battery rating- various tests on battery- – Primary battery: silver button cell- Secondary battery :Ni-Cd battery-modern battery: lithium ion battery-maintenance of batteries-choices of batteries for electric vehicle applications.
Fuel Cells: Introduction- importance and classification of fuel cells - description, principle, components, applications of fuel cells: H2-O2 fuel cell, alkaline fuel cell, molten carbonate fuel cell and direct methanol fuel cells.
Use PyCharm for remote debugging of WSL on a Windo cf5c162d672e4e58b4dde5d797...shadow0702a
This document serves as a comprehensive step-by-step guide on how to effectively use PyCharm for remote debugging of the Windows Subsystem for Linux (WSL) on a local Windows machine. It meticulously outlines several critical steps in the process, starting with the crucial task of enabling permissions, followed by the installation and configuration of WSL.
The guide then proceeds to explain how to set up the SSH service within the WSL environment, an integral part of the process. Alongside this, it also provides detailed instructions on how to modify the inbound rules of the Windows firewall to facilitate the process, ensuring that there are no connectivity issues that could potentially hinder the debugging process.
The document further emphasizes on the importance of checking the connection between the Windows and WSL environments, providing instructions on how to ensure that the connection is optimal and ready for remote debugging.
It also offers an in-depth guide on how to configure the WSL interpreter and files within the PyCharm environment. This is essential for ensuring that the debugging process is set up correctly and that the program can be run effectively within the WSL terminal.
Additionally, the document provides guidance on how to set up breakpoints for debugging, a fundamental aspect of the debugging process which allows the developer to stop the execution of their code at certain points and inspect their program at those stages.
Finally, the document concludes by providing a link to a reference blog. This blog offers additional information and guidance on configuring the remote Python interpreter in PyCharm, providing the reader with a well-rounded understanding of the process.
Embedded machine learning-based road conditions and driving behavior monitoringIJECEIAES
Car accident rates have increased in recent years, resulting in losses in human lives, properties, and other financial costs. An embedded machine learning-based system is developed to address this critical issue. The system can monitor road conditions, detect driving patterns, and identify aggressive driving behaviors. The system is based on neural networks trained on a comprehensive dataset of driving events, driving styles, and road conditions. The system effectively detects potential risks and helps mitigate the frequency and impact of accidents. The primary goal is to ensure the safety of drivers and vehicles. Collecting data involved gathering information on three key road events: normal street and normal drive, speed bumps, circular yellow speed bumps, and three aggressive driving actions: sudden start, sudden stop, and sudden entry. The gathered data is processed and analyzed using a machine learning system designed for limited power and memory devices. The developed system resulted in 91.9% accuracy, 93.6% precision, and 92% recall. The achieved inference time on an Arduino Nano 33 BLE Sense with a 32-bit CPU running at 64 MHz is 34 ms and requires 2.6 kB peak RAM and 139.9 kB program flash memory, making it suitable for resource-constrained embedded systems.
CHINA’S GEO-ECONOMIC OUTREACH IN CENTRAL ASIAN COUNTRIES AND FUTURE PROSPECTjpsjournal1
The rivalry between prominent international actors for dominance over Central Asia's hydrocarbon
reserves and the ancient silk trade route, along with China's diplomatic endeavours in the area, has been
referred to as the "New Great Game." This research centres on the power struggle, considering
geopolitical, geostrategic, and geoeconomic variables. Topics including trade, political hegemony, oil
politics, and conventional and nontraditional security are all explored and explained by the researcher.
Using Mackinder's Heartland, Spykman Rimland, and Hegemonic Stability theories, examines China's role
in Central Asia. This study adheres to the empirical epistemological method and has taken care of
objectivity. This study analyze primary and secondary research documents critically to elaborate role of
china’s geo economic outreach in central Asian countries and its future prospect. China is thriving in trade,
pipeline politics, and winning states, according to this study, thanks to important instruments like the
Shanghai Cooperation Organisation and the Belt and Road Economic Initiative. According to this study,
China is seeing significant success in commerce, pipeline politics, and gaining influence on other
governments. This success may be attributed to the effective utilisation of key tools such as the Shanghai
Cooperation Organisation and the Belt and Road Economic Initiative.
Discover the latest insights on Data Driven Maintenance with our comprehensive webinar presentation. Learn about traditional maintenance challenges, the right approach to utilizing data, and the benefits of adopting a Data Driven Maintenance strategy. Explore real-world examples, industry best practices, and innovative solutions like FMECA and the D3M model. This presentation, led by expert Jules Oudmans, is essential for asset owners looking to optimize their maintenance processes and leverage digital technologies for improved efficiency and performance. Download now to stay ahead in the evolving maintenance landscape.
2. The Battery
• Main Entry: storage battery
• Function: noun
• Date: 1881
• : a cell or connected group of cells that converts
chemical energy into electrical energy by
reversible chemical reactions and that may be
recharged by passing a current through it in the
direction opposite to that of its discharge -- called
also storage cell.
4. Types of Batteries
The primary battery converts chemical energy
to electrical energy directly, using the chemical
materials within the cell to start the action.
The secondary battery must first be charged
with electrical energy before it can convert
chemical energy to electrical energy.
The secondary battery is frequently called a
storage battery, since it stores the energy that is
supplied to it.
5. DRY CELL
• Uses An electrolytic paste.
• The electrolytic paste
reacts with the electrodes
to produce a negative
charge on one electrode
and a positive charge on
the other.
• The difference of potential
between the two
electrodes is the output
voltage.
6. Lead Acid Battery
• Electrolyte for the
most part distilled
(pure) water, with
some sulfuric acid
mixed with the water.
• Electrodes must be of
dissimilar metals.
• An active electrolyte.
8. The basic primary wet cell
• The metals in a cell are called
the electrodes, and the chemical
solution is called the electrolyte.
• The electrolyte reacts
oppositely with the two
different electrodes
• It causes one electrode to lose
electrons and develop a positive
charge; and it causes one other
electrode to build a surplus of
electrons and develop a
negative charge.
• The difference in potential
between the two electrode
charges is the cell voltage.
9. The Electrolyte
• When charging first started,
electrolysis broke down each
water molecule (H2O) into two
hydrogen ions (H+) and one
oxygen ion (O-2).
• The positive hydrogen ions
attracted negative sulfate ions
(SO4
-2) from each electrode.
• These combinations produce
H2SO4, which is sulfuric acid.
11. Specific Gravity
• Ratio of the weight of
a given volume of a
substance to the
weight of an equal
volume of some
reference substance,
or, equivalently, the
ratio of the masses of
equal volumes of the
two substances.
• Example: It is the
weight of the sulfuric
acid - water mixture
compared to an equal
volume of water. Pure
water has a specific
gravity of 1,000.
13. Hydrometer
The chart below gives state of charge vs.
specific gravity of the electrolyte.
State of Charge Specific
Gravity
• 100% Charged 1.265
• 75% Charged 1.239
• 50% Charged 1.200
• 25% Charged 1.170
• Fully Discharged 1.110
• These readings are correct at 75°F
14. •If you are simply using an accurate voltmeter, along with occasional checks with your hydrometer, this
chart should be helpful in determining your batteries state of charge.
Charge Level Specific Gravity Voltage 2V n Voltage 6V n Voltage 12V n Voltage 24V n
100.00% 1.270 2.13 6.38 12.75 25.50
75.00% 1.224 2.08 6.24 12.48 24.96
50.00% 1.170 2.02 6.06 12.12 24.24
20.00% 1.097 1.94 5.82 11.64 23.28
0.00% 1.045 1.89 5.67 11.34 22.68
n stands for nominal voltage
Voltmeter = Hydrometer
15. Ohm’s Law
• Ohm’s Law can be
expressed by the
equation:
– E = IR
– I = E/R
– R = E/I
16. Ohm’s Law
• Series circuits, the total voltage is equal to
the sum of the individual voltages. The
current is constant.
• Parallel circuits, the voltage is constant.
The current is equal to the sum of the
individual currents.
17. Currents
• If one volt of potential difference across a
device causes on ampere of current to flow,
then the device has a resistance of
1 ohm = 1 = 1V/A
• Most of your electrical resistance is in your
skin and varies from 500 ohms (clean) to
several million ohms (dirty).
18. Currents
Current
Amperes
Physiological
Phenomena
Effect on Man
< 0.001 None Imperceptible
0.001 Perception Threshold Mild Sensation
0.003 Pain Threshold Painful Sensation
0.010 Paralysis Threshold of
Arms and Hands
Person cannot release grip;
if no grip, victim may be
thrown clear. Tighter grip
because of paralysis may
allow more current to flow;
may be fatal.
0.030 Respiratory Paralysis Stoppage of breathing,
frequently fatal.
0.075 Fibrillation Threshold Heart action uncoordinated,
probably fatal.
4.000 Heart Paralysis Threshold Heart stops on current
passage, normally restarts
when current interrupted.
5.000 Tissue Burning Not fatal unless vital organs
are burned
19. Series Connected Batteries
• Positive terminal of one
cell is connected to the
negative terminal of the
next, is called a series
connected battery.
• The voltage of this type of
battery is the sum of a
individual cell voltages.
20. Parallel Connected Batteries
• Connect the negative
terminal from one cell to
the negative of the next
cell
• Connect the positive
terminal to the positive
terminal, is parallel
connected.
• Voltage remains constant
and the current is
cumulative.
22. Capacity Rating System
• The Society of Automotive Engineers
(SAE) has established two ratings for
domestic made batteries:
– Reserve Capacity (RC)
– Cold Cranking Amps (CCA)
23. Reserve Capacity
• Reserve capacity is the time required (in
minutes) for a fully charged battery at 80°F
under a constant 25 amp draw to reach a
voltage of 10.5 volts.
24. Cold Cranking Amps (CCA)
• CCA is an important measurement of
battery capacity.
• This rating measures the discharge lead (in
amps) that a battery can supply for 30
seconds at 0°F (-17°C), while maintaining a
voltage of 1.2 volts per cell (7.2 volts per
battery or higher).
25. Preventive Maintenance
• When the top of a battery is “dirty or looks
damp.
• Give a battery a general cleaning, use hot
water (130° F to 170° F) with a neutralizer /
detergent solution.
26. Charging
• Chemical reaction occur during charging.
• Lead sulfate on both plates is separated into Lead
(Pb).
• Sulfate (SO4) leaves both plates.
• It combines with hydrogen (H) in the electrolyte to
form sulfuric acid (H2SO4).
• Oxygen (O) combines with the lead (Pb) at the
positive plate to form lead oxide (PbO2).
• The negative returns to original form of lead (Pb.
27. Charging
• Clean Battery Terminals.
• Attach clamps to the battery in proper polarity.
• Keep open flames and sparks away from battery.
• Ventilate the battery well while charging.
28. Charging
• The charge a battery receives is equal to the
charge rate in amperes multiplied by the
time in hours.
• Measure the specific gravity of a cell once
per hour during charging to determine full
charge.
29. Overcharging
• Results in warped or broken plates,
damaged separators, severe shedding of the
active materials pasted to the plates, and
excessive loss of water, which cause plates
to dry out.
30. Ventilation Requirements
• The oxygen and hydrogen gases released during
the gassing phase of a typical flooded lead-acid
battery recharge can be dangerous if allowed to
exceed 0.8 % (by volume) or 20 percent of the
lower explosive range. Concentrations of
hydrogen between 4 % and 74% are considered
explosive (40,000 ppm and 740,000 ppm).
31. HYDROGEN
• Chemical Formula: H2
• Specific Gravity: 0.0695
• Color: None Odor: None
• Taste: None
• Origin: Applying water to super hot mine fires, explosions electrolysis of
battery acid.
• Explosive Range: 4.1% - 74%
• Ignition Temp: 1030o - 1130o F
• % Oxygen Needed To Burn or Explode: 5%
• TLV: None
• STEL: None
• Effect on Body:Asphxysiant Due to Displacement of Oxygen.
• How Detected: Electronic Detectors, Squeeze Tube Detectors, Chemical
Analysis.
• NOTE: Hydrogen is the reason a flame safety lamp is not permitted in a battery
32. Ventilation
• All lead acid power batteries give off gases
when recharging and also for a period after
the charge is completed.
– A Concentration of hydrogen in excess of 4%
(by volume). It is suggested that the
concentration be controlled to a maximum of
2% (by volume).
33. Ventilation (cont.)
• A typical lead acid motive power cell will, evolve
approximately .016 cubic feet of hydrogen gas over A.H.
overcharge.
• Since this gas is given off at the maximum rate at the end
of the charging period, the following calculation assumes a
charging current of 5% of the 6 hour A.H. capacity (C6)
during this over charge period. (This charging current is
excessive but has been used to take account of the worst
case.)
• Gas given off per hour per cell = 0.16 x .05 = .0008 C6
cu / ft. / cell / hr.
34. Example:
• Consider a battery of 24 cells, type 75CB-13 (C6 = 450 A.H.).
• From the above formula, the rate of gas evolution during overcharge is
24 x .0008 x 450 A.H. = 8.64 cu. Ft./hr.
• Assume that there are 10 such batteries on charge simultaneously in a
room whose dimensions are 25 ft. x 20ft. x 12 ft. high.
• Volume of charging room = 6,000 cu. Ft.
• Volume of Hydrogen gas given off = 8.64 x 10 = 86.4 cu. Ft./hr.
• In order that the concentration of hydrogen is kept at 2% maximum,
the air must be changer every 6,000 x 60/83 = 86.4 cu. X 60 = 83
minutes.
• Consequently, fans capable of extracting 6,000 x 60/83 = 4337 cu.ft.
per hour should be installed as near the roof as possible.
35. Jump Starting
• Be sure to turn off accessories.
• Connect the red cable to the positive terminal on the good battery while the
engine is running.
• Connect the other end of the red cable to the positive terminal on the dead
battery.
• Then connect one end of the black cable to the negative terminal on the good
battery.
• Connect the other end of the negative cable to a known good ground in the
vehicle with the dead battery.
• After starting the vehicle with the discharged battery, allow the engine to
return to idle speed.
• Remove the negative jumper cable starting with the end that is connected to
the vehicle ground
• Remove the positive cable.