The document discusses phase diagrams and chemical kinetics. It introduces new phase diagrams that account for both temperature and pressure. Key terms like critical point and triple point are defined. Reaction mechanisms are explained using collision theory and activated complexes. The factors that affect reaction rates - nature of reactants, temperature, concentration, and catalysts - are outlined. Reversible reactions and Le Chatelier's principle are also summarized.
The document discusses key concepts in chemical thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
2) Spontaneous processes are those that can occur without outside intervention, while reversible processes can be undone by exactly reversing changes made to the system.
3) The second law of thermodynamics states that the entropy of the universe increases for spontaneous processes. Entropy is a measure of disorder and generally increases when the number of possible molecular arrangements increases.
This document discusses key concepts in chemical thermodynamics including the first, second, and third laws of thermodynamics. It describes how energy, entropy, enthalpy, and Gibbs free energy relate to spontaneous processes and equilibrium. Spontaneous processes are irreversible and result in an increase in entropy of the universe according to the second law. The third law states that the entropy of a pure crystalline substance is 0 at absolute zero. Gibbs free energy can be used to predict spontaneity based on its sign and relationship to the reaction quotient and equilibrium constant.
The document discusses key concepts in chemical thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
2) Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in the reverse direction.
3) Entropy is a measure of the randomness or disorder of a system. It increases for spontaneous processes according to the second law of thermodynamics.
4) The Gibbs free energy, ΔG, can be used to determine whether a process is spontaneous, with a negative ΔG corresponding to a spontaneous process.
The document discusses key concepts in engineering chemistry including:
1) Laws of thermodynamics like entropy change and Gibbs free energy are covered as well as kinetics concepts like activation energy and the Arrhenius equation.
2) Specific topics covered include the three laws of thermodynamics, concepts like enthalpy, heat capacity, and various thermodynamic processes.
3) The Carnot cycle is discussed as a theoretical reversible heat engine cycle used to demonstrate the maximum efficiency possible for a heat engine.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value. If ΔG is negative, the forward reaction is spontaneous.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether a process is spontaneous, with negative ΔG corresponding to spontaneity. ΔG depends on the temperature, enthalpy, and entropy of the system.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether a process is spontaneous, with negative ΔG corresponding to spontaneity. ΔG depends on the temperature, enthalpy, and entropy of the system.
The document discusses key concepts in chemical thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
2) Spontaneous processes are those that can occur without outside intervention, while reversible processes can be undone by exactly reversing changes made to the system.
3) The second law of thermodynamics states that the entropy of the universe increases for spontaneous processes. Entropy is a measure of disorder and generally increases when the number of possible molecular arrangements increases.
This document discusses key concepts in chemical thermodynamics including the first, second, and third laws of thermodynamics. It describes how energy, entropy, enthalpy, and Gibbs free energy relate to spontaneous processes and equilibrium. Spontaneous processes are irreversible and result in an increase in entropy of the universe according to the second law. The third law states that the entropy of a pure crystalline substance is 0 at absolute zero. Gibbs free energy can be used to predict spontaneity based on its sign and relationship to the reaction quotient and equilibrium constant.
The document discusses key concepts in chemical thermodynamics including:
1) The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
2) Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in the reverse direction.
3) Entropy is a measure of the randomness or disorder of a system. It increases for spontaneous processes according to the second law of thermodynamics.
4) The Gibbs free energy, ΔG, can be used to determine whether a process is spontaneous, with a negative ΔG corresponding to a spontaneous process.
The document discusses key concepts in engineering chemistry including:
1) Laws of thermodynamics like entropy change and Gibbs free energy are covered as well as kinetics concepts like activation energy and the Arrhenius equation.
2) Specific topics covered include the three laws of thermodynamics, concepts like enthalpy, heat capacity, and various thermodynamic processes.
3) The Carnot cycle is discussed as a theoretical reversible heat engine cycle used to demonstrate the maximum efficiency possible for a heat engine.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value. If ΔG is negative, the forward reaction is spontaneous.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether a process is spontaneous, with negative ΔG corresponding to spontaneity. ΔG depends on the temperature, enthalpy, and entropy of the system.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether a process is spontaneous, with negative ΔG corresponding to spontaneity. ΔG depends on the temperature, enthalpy, and entropy of the system.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value. If ΔG is negative, the forward reaction is spontaneous.
This document discusses bond enthalpy, bond dissociation enthalpy, and Hess's law of constant heat summation. It provides examples of calculating average bond enthalpy using Hess's law. It also covers spontaneous and non-spontaneous processes, entropy, Gibbs free energy, and the three laws of thermodynamics.
Basic concept and first law of thermodynamics agsmeice
This document provides an introduction to engineering thermodynamics. It defines key terms like heat, power, temperature, and the science of thermodynamics. It describes different types of thermodynamic systems like closed, open, isolated, homogeneous, and heterogeneous systems. The document outlines thermodynamic properties, processes, cycles, and the first law of thermodynamics. It also reviews the laws of perfect gases and examples of thermodynamic processes like isothermal, isobaric, isochoric, reversible, and adiabatic processes.
This document provides an overview of chemical thermodynamics, including:
- The first law of thermodynamics which states that change in internal energy equals heat added plus work done.
- The second law of thermodynamics which states that the entropy of the universe increases for spontaneous processes.
- How changes in entropy and free energy determine whether processes are spontaneous, with spontaneous processes favoring higher entropy and more negative free energy.
This document provides an overview of chemical kinetics and reaction rates. It introduces key concepts such as activation energy, the Arrhenius equation, reaction order, and factors that affect reaction rates such as temperature, concentration, and surface area. It also describes the collision theory of chemical reactions and how an increase in temperature results in more molecules possessing sufficient kinetic energy to overcome the activation energy barrier.
This document provides an introduction to engineering thermodynamics. It defines key concepts like systems, properties, processes, and the first law of thermodynamics. Specific topics covered include the classification of thermodynamic systems as closed or open, homogeneous or heterogeneous. The document also discusses intensive and extensive properties, pressure, temperature, and the gas laws of Boyle, Charles, and Gay-Lussac. Common thermodynamic processes like isothermal, isobaric, isochoric, and adiabatic processes are defined. The first law of thermodynamics relating heat, work, and changes in internal energy is stated.
This document provides an introduction to engineering thermodynamics. It defines key concepts like systems, properties, processes, and the first law of thermodynamics. Specific topics covered include the classification of thermodynamic systems as closed or open, homogeneous or heterogeneous. The document also discusses intensive and extensive properties, pressure, temperature, and the gas laws of Boyle, Charles, and Gay-Lussac. Common thermodynamic processes like isothermal, isobaric, isochoric, and adiabatic processes are defined. The first law of thermodynamics relating heat, work, and changes in internal energy is stated.
This document provides an overview of enzymology and enzymes. It discusses how enzymes are biological catalysts that accelerate chemical reactions in living organisms. Each reaction is catalyzed by one or more specific enzymes, which are proteins that recognize substrate molecules and facilitate their transformation. Enzymes play a key role in coupling exergonic and endergonic reactions to allow biochemical processes to occur under the constraints of thermodynamics. The document covers basics of enzyme kinetics, cofactors, classification, factors influencing enzyme activity such as temperature and pH, inhibition, and measurement of enzymatic activity.
This document provides an outline and overview of key concepts in thermodynamics. It begins with an introduction to thermodynamics laws including zero law, first law, and second law. It then discusses key concepts such as Gibbs free energy, the relationship between free energy and equilibrium constants, and kinetics. Other topics covered include heat energy, relationships between thermodynamics and material properties, spontaneity, and applications of thermodynamic principles in pharmacy.
1. The document discusses concepts from engineering chemistry including the laws of thermodynamics, kinetics, and related topics.
2. It explains key thermodynamic concepts such as state functions, path functions, the four laws of thermodynamics, entropy, enthalpy, and Gibbs free energy.
3. The document also discusses kinetic concepts such as activation energy, the Arrhenius equation, and enzyme catalysis using the Michaelis-Menten mechanism.
The document discusses concepts related to energy and chemical change, covering topics like:
- Energy can exist in different forms including potential and kinetic energy. Chemical potential energy is stored due to a substance's composition.
- Thermochemistry involves measuring heat changes in reactions and processes using instruments like calorimeters. Enthalpy is a measure of heat content.
- Thermochemical equations express heat released or absorbed in chemical reactions. Standard enthalpies of formation allow calculating enthalpy changes.
- Spontaneous processes are those that occur without outside intervention, driven by increases in entropy according to the second law of thermodynamics.
This document provides information on thermodynamics and spontaneity of chemical reactions. It defines key concepts such as the first and second laws of thermodynamics, entropy, free energy, and Gibbs free energy. Equations for calculating entropy, enthalpy, and Gibbs free energy changes in chemical reactions are presented. Examples are provided to demonstrate how to apply these equations and determine if reactions are spontaneous based on the sign and value of their Gibbs free energy changes. The dependence of spontaneity on temperature is also discussed.
i hope, it will helpful to the students and peoples in the search of topics mentioned
it is informative to study to even get passing marks or for revision
The document provides an overview of key concepts in thermochemistry including:
- Defining energy, work, potential energy, kinetic energy, and endothermic and exothermic processes.
- The first law of thermodynamics and how changes in internal energy can be calculated using heat and work.
- How enthalpy changes can be determined using calorimetry and Hess's law.
- How standard enthalpies of formation are used to calculate enthalpy changes in chemical reactions.
The document covers fundamental thermochemistry concepts and calculations in chemistry.
This document provides an overview of key concepts in chemical thermodynamics, including:
1. Systems, surroundings, boundaries, open vs closed vs isolated systems, and extensive vs intensive properties are introduced.
2. The three laws of thermodynamics - first law regarding energy conservation, second law regarding entropy, and third law regarding unattainability of zero kelvin - are briefly outlined.
3. Key thermodynamic processes like isothermal, adiabatic, isobaric, and isochoric processes are defined.
4. Important thermodynamic parameters like internal energy, work, heat, and enthalpy are explained. Sign conventions and the mathematical statement of the first law relating these parameters
Thermodynamics is the study of heat, work, and energy. It describes macroscopic properties of systems in thermal equilibrium. A system is defined along with its surroundings and properties. Systems can be open, closed, or isolated. Thermodynamic properties include extensive properties that depend on system size and intensive properties that do not. The four laws of thermodynamics relate temperature, heat, work, and energy within a system. Heat transfer and phase changes involve latent heat in addition to specific heat.
Energy and the biological systems are joined together and no biological world is almost impossible without ATP. This study material intends to explore the beauty of ATP to drive different biological processes.
Chemistry-Unit 8 Notes HC (Solution Chemistry).pdfrajatrokade185
This document provides information about different ways to determine the composition of solutions, including molarity, molality, mole fraction, and mass percent. It defines key terms like solute, solvent, solution, and discusses how temperature, surface area, and agitation affect the rate at which a solute dissolves in a solvent. Examples are provided for calculating molarity, molality, mole fraction and mass percent. The document also covers dilutions and how to calculate the concentration of a diluted solution using the dilution equation.
This document provides information about the electromagnetic spectrum. It begins by asking questions about how waves in the electromagnetic spectrum differ and how each type is utilized. It then defines key terms like light, electromagnetic spectrum, and the different types of waves. It explains that light is a transverse wave that can travel without a medium. Frequency determines a wave's color/type, with higher frequencies having more energy. The electromagnetic spectrum includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays. Each type of wave is then described in more detail along with common uses. Videos are provided for further explanation of infrared and the full electromagnetic spectrum.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value.
The document discusses key concepts in chemical thermodynamics including:
- The first law of thermodynamics states that energy cannot be created or destroyed, only converted from one form to another.
- Spontaneous processes are those that can proceed without outside intervention. Processes that are spontaneous in one direction are nonspontaneous in reverse.
- Entropy is a measure of disorder or randomness. It increases for spontaneous processes according to the second law of thermodynamics.
- The Gibbs free energy, ΔG, can indicate whether processes are spontaneous or at equilibrium based on its sign and value. If ΔG is negative, the forward reaction is spontaneous.
This document discusses bond enthalpy, bond dissociation enthalpy, and Hess's law of constant heat summation. It provides examples of calculating average bond enthalpy using Hess's law. It also covers spontaneous and non-spontaneous processes, entropy, Gibbs free energy, and the three laws of thermodynamics.
Basic concept and first law of thermodynamics agsmeice
This document provides an introduction to engineering thermodynamics. It defines key terms like heat, power, temperature, and the science of thermodynamics. It describes different types of thermodynamic systems like closed, open, isolated, homogeneous, and heterogeneous systems. The document outlines thermodynamic properties, processes, cycles, and the first law of thermodynamics. It also reviews the laws of perfect gases and examples of thermodynamic processes like isothermal, isobaric, isochoric, reversible, and adiabatic processes.
This document provides an overview of chemical thermodynamics, including:
- The first law of thermodynamics which states that change in internal energy equals heat added plus work done.
- The second law of thermodynamics which states that the entropy of the universe increases for spontaneous processes.
- How changes in entropy and free energy determine whether processes are spontaneous, with spontaneous processes favoring higher entropy and more negative free energy.
This document provides an overview of chemical kinetics and reaction rates. It introduces key concepts such as activation energy, the Arrhenius equation, reaction order, and factors that affect reaction rates such as temperature, concentration, and surface area. It also describes the collision theory of chemical reactions and how an increase in temperature results in more molecules possessing sufficient kinetic energy to overcome the activation energy barrier.
This document provides an introduction to engineering thermodynamics. It defines key concepts like systems, properties, processes, and the first law of thermodynamics. Specific topics covered include the classification of thermodynamic systems as closed or open, homogeneous or heterogeneous. The document also discusses intensive and extensive properties, pressure, temperature, and the gas laws of Boyle, Charles, and Gay-Lussac. Common thermodynamic processes like isothermal, isobaric, isochoric, and adiabatic processes are defined. The first law of thermodynamics relating heat, work, and changes in internal energy is stated.
This document provides an introduction to engineering thermodynamics. It defines key concepts like systems, properties, processes, and the first law of thermodynamics. Specific topics covered include the classification of thermodynamic systems as closed or open, homogeneous or heterogeneous. The document also discusses intensive and extensive properties, pressure, temperature, and the gas laws of Boyle, Charles, and Gay-Lussac. Common thermodynamic processes like isothermal, isobaric, isochoric, and adiabatic processes are defined. The first law of thermodynamics relating heat, work, and changes in internal energy is stated.
This document provides an overview of enzymology and enzymes. It discusses how enzymes are biological catalysts that accelerate chemical reactions in living organisms. Each reaction is catalyzed by one or more specific enzymes, which are proteins that recognize substrate molecules and facilitate their transformation. Enzymes play a key role in coupling exergonic and endergonic reactions to allow biochemical processes to occur under the constraints of thermodynamics. The document covers basics of enzyme kinetics, cofactors, classification, factors influencing enzyme activity such as temperature and pH, inhibition, and measurement of enzymatic activity.
This document provides an outline and overview of key concepts in thermodynamics. It begins with an introduction to thermodynamics laws including zero law, first law, and second law. It then discusses key concepts such as Gibbs free energy, the relationship between free energy and equilibrium constants, and kinetics. Other topics covered include heat energy, relationships between thermodynamics and material properties, spontaneity, and applications of thermodynamic principles in pharmacy.
1. The document discusses concepts from engineering chemistry including the laws of thermodynamics, kinetics, and related topics.
2. It explains key thermodynamic concepts such as state functions, path functions, the four laws of thermodynamics, entropy, enthalpy, and Gibbs free energy.
3. The document also discusses kinetic concepts such as activation energy, the Arrhenius equation, and enzyme catalysis using the Michaelis-Menten mechanism.
The document discusses concepts related to energy and chemical change, covering topics like:
- Energy can exist in different forms including potential and kinetic energy. Chemical potential energy is stored due to a substance's composition.
- Thermochemistry involves measuring heat changes in reactions and processes using instruments like calorimeters. Enthalpy is a measure of heat content.
- Thermochemical equations express heat released or absorbed in chemical reactions. Standard enthalpies of formation allow calculating enthalpy changes.
- Spontaneous processes are those that occur without outside intervention, driven by increases in entropy according to the second law of thermodynamics.
This document provides information on thermodynamics and spontaneity of chemical reactions. It defines key concepts such as the first and second laws of thermodynamics, entropy, free energy, and Gibbs free energy. Equations for calculating entropy, enthalpy, and Gibbs free energy changes in chemical reactions are presented. Examples are provided to demonstrate how to apply these equations and determine if reactions are spontaneous based on the sign and value of their Gibbs free energy changes. The dependence of spontaneity on temperature is also discussed.
i hope, it will helpful to the students and peoples in the search of topics mentioned
it is informative to study to even get passing marks or for revision
The document provides an overview of key concepts in thermochemistry including:
- Defining energy, work, potential energy, kinetic energy, and endothermic and exothermic processes.
- The first law of thermodynamics and how changes in internal energy can be calculated using heat and work.
- How enthalpy changes can be determined using calorimetry and Hess's law.
- How standard enthalpies of formation are used to calculate enthalpy changes in chemical reactions.
The document covers fundamental thermochemistry concepts and calculations in chemistry.
This document provides an overview of key concepts in chemical thermodynamics, including:
1. Systems, surroundings, boundaries, open vs closed vs isolated systems, and extensive vs intensive properties are introduced.
2. The three laws of thermodynamics - first law regarding energy conservation, second law regarding entropy, and third law regarding unattainability of zero kelvin - are briefly outlined.
3. Key thermodynamic processes like isothermal, adiabatic, isobaric, and isochoric processes are defined.
4. Important thermodynamic parameters like internal energy, work, heat, and enthalpy are explained. Sign conventions and the mathematical statement of the first law relating these parameters
Thermodynamics is the study of heat, work, and energy. It describes macroscopic properties of systems in thermal equilibrium. A system is defined along with its surroundings and properties. Systems can be open, closed, or isolated. Thermodynamic properties include extensive properties that depend on system size and intensive properties that do not. The four laws of thermodynamics relate temperature, heat, work, and energy within a system. Heat transfer and phase changes involve latent heat in addition to specific heat.
Energy and the biological systems are joined together and no biological world is almost impossible without ATP. This study material intends to explore the beauty of ATP to drive different biological processes.
Chemistry-Unit 8 Notes HC (Solution Chemistry).pdfrajatrokade185
This document provides information about different ways to determine the composition of solutions, including molarity, molality, mole fraction, and mass percent. It defines key terms like solute, solvent, solution, and discusses how temperature, surface area, and agitation affect the rate at which a solute dissolves in a solvent. Examples are provided for calculating molarity, molality, mole fraction and mass percent. The document also covers dilutions and how to calculate the concentration of a diluted solution using the dilution equation.
This document provides information about the electromagnetic spectrum. It begins by asking questions about how waves in the electromagnetic spectrum differ and how each type is utilized. It then defines key terms like light, electromagnetic spectrum, and the different types of waves. It explains that light is a transverse wave that can travel without a medium. Frequency determines a wave's color/type, with higher frequencies having more energy. The electromagnetic spectrum includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays. Each type of wave is then described in more detail along with common uses. Videos are provided for further explanation of infrared and the full electromagnetic spectrum.
Young's double slit experiment demonstrated the wave nature of light by showing that light passing through two slits will produce an interference pattern of bright and dark fringes on a screen. The experiment showed that light acts as a wave and can interfere with itself. The fringe width of the interference pattern varies with the wavelength of light used in the experiment.
Badminton is played between two players or teams using rackets to hit a shuttlecock back and forth over a net. A match consists of best-of-three games to 21 points, needing a 2-point lead unless the score reaches 29-30. The server alternates sides each point if the score is even or odd, and service passes to the opponent if a rally is lost. Faults result in a point for the opponent if service is incorrect or the shuttle touches outside the court, net, or body.
Atoms are composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus at the center of the atom, while electrons exist in orbitals surrounding the nucleus. The number of protons determines the element and its placement on the periodic table. Electrons farther from the nucleus have more energy and are more easily lost or gained, influencing chemical properties and bonding abilities.
This document summarizes key concepts from a physics chapter on particles and waves:
1) Light and matter exhibit both wave-like and particle-like properties according to the principle of wave-particle duality.
2) Electromagnetic radiation is quantized into particle-like units called photons according to Planck's constant and the photoelectric effect provides evidence that light consists of photons.
3) Heisenberg's uncertainty principle establishes fundamental limits on the precision with which certain pairs of physical properties of a particle, like position and momentum, can be known simultaneously.
This document provides instructions for the key skills in cricket: batting, bowling, catching, and fielding. For batting, it lists the steps to properly hit the ball and be ready to run. For bowling, it outlines the motion to release the ball towards the target. Catching instructions include watching the ball and extending the arms to catch it. Fielding tips are to stand side on, eyes on the target, point and throw towards it as the runner moves.
This document contains slides from a chapter about semiconductor diodes. It discusses the basic operation and characteristics of ideal diodes, including their conduction and non-conduction regions. Real diodes are not ideal due to the influence of majority and minority carriers. The document covers diode testing methods and specifications. It also introduces other types of diodes such as Zener diodes, light emitting diodes, and diode arrays.
Football was invented in 1879 by Walter Camp, who is known as the "Father of football." The document outlines the history and basics of football, including positions on both offense and defense, scoring, equipment used, penalties, and facts such as the average roster size of 53 players per NFL team. The Hall of Fame was created in 1963 to honor outstanding football players, coaches, contributors, and teams.
This document provides an overview of optics concepts including reflection, refraction, Snell's law, total internal reflection, fiber optics, and mirages. Key points covered include:
- Reflection and refraction occur when light changes direction at an interface between two mediums. Snell's law relates the angles of incidence and refraction.
- Total internal reflection occurs when light travels from a higher to lower index of refraction material at an angle greater than the critical angle, causing the light to reflect back into the first medium.
- Fiber optics use total internal reflection to transmit light signals over long distances through thin glass or plastic strands.
- Mirages are optical illusions caused by the ref
The document discusses electromagnetic induction and Faraday's law. It explains Michael Faraday's experiment showing that a changing magnetic field can induce a current in a nearby coil. It defines magnetic flux and explains how a changing flux induces an electromotive force (emf) according to Faraday's law. It also discusses Lenz's law, which describes how the direction of induced current opposes the change that caused it. Examples are given of motional emf induced in a conductor moving through a magnetic field.
Macroeconomics- Movie Location
This will be used as part of your Personal Professional Portfolio once graded.
Objective:
Prepare a presentation or a paper using research, basic comparative analysis, data organization and application of economic information. You will make an informed assessment of an economic climate outside of the United States to accomplish an entertainment industry objective.
Executive Directors Chat Leveraging AI for Diversity, Equity, and InclusionTechSoup
Let’s explore the intersection of technology and equity in the final session of our DEI series. Discover how AI tools, like ChatGPT, can be used to support and enhance your nonprofit's DEI initiatives. Participants will gain insights into practical AI applications and get tips for leveraging technology to advance their DEI goals.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Training: ISO/IEC 27001 Information Security Management System - EN | PECB
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Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
Physiology and chemistry of skin and pigmentation, hairs, scalp, lips and nail, Cleansing cream, Lotions, Face powders, Face packs, Lipsticks, Bath products, soaps and baby product,
Preparation and standardization of the following : Tonic, Bleaches, Dentifrices and Mouth washes & Tooth Pastes, Cosmetics for Nails.
This presentation was provided by Steph Pollock of The American Psychological Association’s Journals Program, and Damita Snow, of The American Society of Civil Engineers (ASCE), for the initial session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session One: 'Setting Expectations: a DEIA Primer,' was held June 6, 2024.
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Exploiting Artificial Intelligence for Empowering Researchers and Faculty, In...Dr. Vinod Kumar Kanvaria
Exploiting Artificial Intelligence for Empowering Researchers and Faculty,
International FDP on Fundamentals of Research in Social Sciences
at Integral University, Lucknow, 06.06.2024
By Dr. Vinod Kumar Kanvaria
This presentation includes basic of PCOS their pathology and treatment and also Ayurveda correlation of PCOS and Ayurvedic line of treatment mentioned in classics.
Thinking of getting a dog? Be aware that breeds like Pit Bulls, Rottweilers, and German Shepherds can be loyal and dangerous. Proper training and socialization are crucial to preventing aggressive behaviors. Ensure safety by understanding their needs and always supervising interactions. Stay safe, and enjoy your furry friends!
2. PHASE DIAGRAMS (N. AND I.)
■New and Improved!
■Phase Change Diagrams only account for
temperature
■New Phase Diagrams account for
Pressure, as well.
■Terms:
■Critical Point
■Triple Point
*This change comes as a result of our study of Gas Laws!
3. PHASE DIAGRAMS
Temperature →
Pressure
→
A
B
C
D
Solid
Liquid
Vapor
The large white dot
(T) represents the
triple point.
The triple point is the
equilibrium* point of
all three phases–
solid, liquid, gas.
Point C – The Critical Point– at temperatures higher than
this, there can only the gas phase
T
4. MORE TRIPLE POINT
■Along any line,
the two phases
represented are at
equilibrium.
Temperature →
Pressure
→
A
B
C
D
Solid
Liquid
Vapor
5. CHEMICAL LINE UP
Temperature →
Pressure
→
A
B
C
D
Solid
Liquid
Vapor
Each Line has a “meaning”:
Tp
-A: Solid-Liquid Eq.
Tp
-B: Solid-Gas Eq.
Tp
-C: Liquid-Solid Eq.
Tp
-D: Supercooled H2O
6. EQUILIBRIUM
■The state in which two or more processes
are occurring at the same time:
■Phase Changes
■As one molecule melts, another freezes
■As one molecule boils, another condenses
■Triple Point:
■ALL of the phase changes occur at the SAME time, at
Equilibrium
7. RELATIONSHIPS (FOR WATER)
■1 atm:
■BP = 100 C
■FP = 0.016 C
(273.16K)
■0.0063 atm:
■BP = 0.0098 C
■FP = 0.0098 C
Temperature →
Pressure
→
A
B
C
D
Solid
Liquid
V
a
p
o
r
1 atm
100
C
0.0063 atm
0.0098
C
0
C
High-Density
Ice
1000 atm
8. SOME IDEAS TO CONSIDER
■Adding pressure causes a shift to the more
dense phase.
■Adding temp. causes a shift to the less
dense phase
■“Gibbs Phase Rule”
9. WATER’S UNIQUE PROPERTY
■What is the most dense phase of water?
Gibbs’ Phase Rule explains why ice skates work the way they do!!!
The blade of a skate provides pressure to the ice, which should be
near 0 C
This causes a shift to the more dense phase.
This provides a film of water which allows the skate to slide!
10. OTHER PHASE CHANGE GRAPHS
■Carbon
Dioxide
■What can this
tell us about
CO2
?
Temperature →
Pressure
→
Solid
Liquid
Vapor
1 atm
0 C
11. THERMODYNAMICS
■The study of heat/energy as it moves
through a system
■Phase changes: Melting = Freezing?
■Yes-- in one, energy is being added (melting); in the other,
it’s being taken away (freezing)
■Calculated using Calorimetry
■Uses masses and temperature changes to
determine energy flow
12. CALORIMETRY
■Energy can be calculated using the
formula:
Q = m x c x ∆T
Where:
Q = energy (joules, kilojoules, or calories)
m = mass in g
c = Specific Heat (more)
∆T = Change in Temperature (K or o
C)
13. SPECIFIC HEAT
■Term given for the amount of energy
needed to raise 1 g of a substance a given
temperature:
■For water, c = 1 cal / g o
C
■Also c = 4.18 j / g o
C
■From which we can deduce:
■1 cal = 4.18 j
14. FOR ICE? STEAM?
■Ice’s Specific Heat:
■2.09 j/g o
C
■Steam’s Specific Heat:
■1.84 j/g o
C
15. ENERGY OF A PHASE CHANGE
■Heat of Fusion: The amount of heat
required to MELT a solid;
■Also, the heat given off by freezing a liquid
■For H2
O: 333 j / g
■Heat of Vaporization: The amount of heat
needed to BOIL a liquid;
■Also, the heat given off by condensing a gas
■For H2
O: 2230 j / g
17. WE KNOW:
■Chemical Bonds form due to electron
movement to a state of lower energy.
■NOW: we begin learning about the forces
that drive reactions.
18. CHEMICAL KINETICS HAS FOUR
PRIMARY PARTS:
■Kinetic Molecular Theory
■Reaction Mechanisms
■Reaction Rates
■Phases and Phase Changes (already started!)
19. KINETIC MOLECULAR THEORY
■Says that all particles are moving at all
times
■Also called collision theory
■“Proven” (sorta) through our studies of
gases.
20. POSTULATES OF KMT
■All molecules are extremely small in mass.
■All molecules are in constant motion.
■There are so many particles, even in a
small sample, that we can use statistics
(mean, median, mode, etc.) to make
generalizations about particle movement.
21. MORE POSTULATES OF KMT
■Collisions are perfectly elastic (all energy
remains kinetic)
■The kinetic energy of the system is directly
related to the temperature (higher temp. =
more E!)
■… So what?
22. WHAT IT MEANS:
■Heat is a function of the energy of
motion of particles
■When something gets hot, its particles are
moving faster than before.
■Everything, whether you like it or not, is
moving (at a molecular level).
■Chemical reactions and interactions
are all a result of chemicals colliding with
one another… which leads us to…
23. REACTION MECHANISMS
■Chemical Kinetic Theory says that NO
reaction can occur without the effective
collision of two or more molecules.
■Contact
■Electron Clouds Must “touch”
■Proper Alignment
■Molecules Must Align correctly in order to react
■High Enough Energy to Begin Reacting
■Activation E!
■This WHOLE concept is called:
COLLISION THEORY
24. REACTION MECHANISMS
■Are defined as the underlying action in a
chemical reaction
■2C8
H18
+ 25 O2
16CO2
+ 18 H2
O
■What are the odds that both Octanes and ALL 25
O2
collide at the same time?
■Problem: this is a highly exothermic reaction,
rapid reaction-- How can this be?
25. ANSWER: ACTIVATED COMPLEXES
■Molecules that exist ONLY DURING a
reaction
■Parts of molecules that have either:
■Broken apart from reactants
■Formed together to make products
■CO and OH (0) exist during this reaction,
among others.
■Act. Complexes Video
26. SO WHAT?
■If we agree that kinetic theory is true,
and…
■Activated Complexes exist, then…
■We can control how fast some chemical
reactions occur.
27. RATE DETERMINING STEP
■Activated Complexes say that reactions
occur in steps.
■Some steps are slower than others, which
limit how fast a reaction can occur.
■Video here
28. REACTION RATES
■Demonstration Reaction:
■Zn + NH4
NO3
ZnO + N2
+ H2
O
■Slow Reaction was Changed to a quick one!
■Reaction Rate can be Affected!
■Slow Rate: Heat given off
■Fast Rate: EXPLOSION!!
■Watch this guy…
29. FACTORS AFFECTING REACTION
RATE
■There are FOUR you need to know:
■Nature of the Reactants
■Temperature of the System
■Concentration of Reactants and/or Products
■Catalysts
30. NATURE OF REACTANTS
■Depends on what types of things are
being reacted.
■Primarily a measure of the reactivity of
the involved chemicals.
■The more reactive each participant, the more
quickly the reaction occurs.
■Reactivity increases as E! increases
■Affects the number of effective collisions
■Includes Phase Differences: More later
31. TEMPERATURE
■In a vast majority of Reactions, a
higher temp. Results in a faster
reaction
■An increase in effective collisions from
having higher E! available
■To effectively deliver temperature:
■Add Heat: Fire, Sun, etc.
■Add H2
O: Has a high Specific Heat
32. CONCENTRATION AND REACTION
RATE
■An increase in the Conc. of Reactants=
Faster Reaction
■An increase in the Conc. of Products=
Slower Reaction
■Think of a Jr. High dance…
33. CONCENTRATION AND REACTION
RATE (CONTINUED)
■Surface Area Increase = An Increase in
Conc.
■More Molecules Available to Collide
■Phases have variable surface area*:
■Liquid-Liquid
■Liquid-Gas (bubbling)
■Gas-Gas
■Liquid-Solid
■Gas-Solid
■Solid-Solid
34. CATALYSTS AND REACTION RATE
■Catalysts always increase reaction
rate.
■Defined:
■Chemicals that act to speed up a reaction
without being used up themselves in the
reaction.
■We do not fully understand the function
of Catalysts
■Catalysts MAY break down during a
reaction-- but will always re-form by the
end of it.
35. REVERSIBLE REACTIONS
■Chemical Reactions that can occur in
either direction in nature.
■Under certain circumstances, reactants
become products
■Under different circumstances, products
turn back into reactants
■Can (and will) achieve Equilibrium
A + B C + D
Vid Here
36. LECHATELIER’S PRINCIPLE
■LeChatelier said that a reversible reaction
can be affected by adding a stress.
■Stresses include:
■Concentration of Chemicals
■Temperature
■Addition of a Catalyst
37. LECHATELIER’S RESULTS
■Concentration of Chemicals
■More reactant added
■Shifts reaction to the products side
■More product added
■Shifts reaction to the reactants side
■Temperature
■Increasing temp causes:
■Exothermic reactions to move toward reactants
■Endothermic reactions to move towards products
38. LAST FOR LECHATELIER
■A Catalyst will ALWAYS move a reaction
towards the products side
■Catalysts always act to speed up reactions
39. CONTROLLING REACTIONS IN THE FIRST
PLACE?
■We can control how fast reactions take place.
■We know that collisions are the root of all
chemical reactions.
■We know that particles are in constant motion.
■Can we make a reaction occur? Stop a reaction
from occurring?
40. CONTROLLING CHEMICAL REACTIONS
■It is possible to prevent reactions from
occurring, and it is possible to make
reactions occur that normally wouldn’t:
■Activation Energy
■Enthalpy and Entropy
41. ACTIVATION ENERGY
■The Energy Required to START a
Chemical Reaction
■E! act (abbr.)
■Examples: Gasoline; Ba(OH)2
+ NH4
Cl
■Can be shown on an potential E! Graph
■Without enough E!, no reaction will
occur.
42. REACTION RATE FORCES
■Additionally, nature controls whether or
not reactions through two forces:
■Enthalpy, or ΔH
■The total amount of energy in an object/chemical
■Entropy, or ΔS
■The amount of disorder in an object or chemical
43. WHAT NATURE WANTS…
■Nature wants:
■Energy to be given off to the universe
■An decrease in ∆H (- ∆H)
■Entropy to increase
■An increase in ∆S (+ ∆S)
44. PREDICTING REACTION OCCURRENCE
■Given the ΔH and ΔS of a system, you can
predict if a reaction will occur.
■If ΔH is negative and:
ΔS is Positive, the reaction will occur
ΔS is Negative, the reaction will occur if:
ΔH has a greater absolute value than ΔS
■If ΔS is positive and:
ΔH is positive, the reaction will occur if:
ΔS has the larger absolute value
45. MORE PREDICITING
■If ΔH is positive and ΔS is negative the
reaction will never occur.
■Although not “the whole story,” phases are
related to ΔH and ΔS.
46. PHASES AND FORCES
■Recall:
Solids: Very Low ΔS, Very Low ΔH
Orderly, low E!
Liquids: Low ΔS, Low H
Semi-Orderly, moderate E!
Gases: High ΔS, High ΔH
Disorderly, high E!
Plasma: Very High ΔS, Very High ΔH
Ridiculous disorder, ridiculous E!
47. INTERMOLECULAR FORCES
■Forces that act between 2 separate
molecules.
■Phases are directly related to the
strength of the Intermolecular Forces in
a system.
■Solids- Strong IMF
■Plasma- Weak IMF
49. REMEMBER THIS?
■To aide in your understanding of IMF,
check out this blast from the past:
0 2
0.9
3
1.8
1
50. LONDON DISPERSION FORCES
■Occur primarily in Non-Polar Covalent Cpds., but
do occur in all substances.
■Caused by the random “dispersion” of electrons
within a compound.
■As e- move, they create weak positive and negative areas
that are therefore attracted to each other.
■A temporary electro-magnetic force
51. DIPOLE FORCES
■Occur in polar molecules and ionic
compounds only.
■The (∂+) or (+) portion is attracted, quite
strongly, to the (∂-) or (-) part.
■*This force is stronger as substances become
more ionic in character.*
■A permanent, though variable (depending on
the differential), electro-magnetic force
52. HYDROGEN BONDS
■Occur only in Polar Molecules that
contain a hydrogen and highly
electronegative element.
■F, O, Cl <in decreasing order>
■A permanent, average strength (because of
the partial differential) electro-magnetic force
H O
H
H
H
O
Hydrogen Bond
53. GRAVITY
■The pull of two massive bodies towards
each other
■For their size, atoms are quite massive
■Extremely weak force in spite of this
■Gravity is directly tied to mass; size, at the atomic level, is
generally irrelevant
54. IMF AFFECT PHYSICAL PROPERTIES
■According to periodic trends, Water
should boil at a much lower temperature:
Atomic Mass →
Temp
●H2S
●H2Se
●H2Te
●(H2Po)
H2O ●H2S
●H2Se
●H2Te
●(H2Po)
● H2O
● H2O boils at 100 C; H2Te boils at -2 C!
Trends Say:
Real Life Proves: