This document provides information about gases and the kinetic molecular theory. It defines 11 common gases, lists their properties and uses. The kinetic molecular theory explains that gases are made of particles that move rapidly in random straight lines and collide elastically. The theory accounts for gas properties like compressibility and the fact that gas density varies with temperature and pressure. Key gas properties like volume, pressure, temperature and amount are also defined.
The document discusses gases and their properties according to the kinetic molecular theory. It defines the key concepts of gases including their state, composition of molecules, and random motion. It also outlines the assumptions of the kinetic molecular theory for ideal gases and describes the variables used in gas laws - temperature, pressure, volume, and moles. Real gases are known to deviate from ideal behavior at high pressures or low temperatures due to intermolecular forces and molecular size.
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.
The document discusses gases and their properties according to the kinetic molecular theory. It defines gases as being composed of particles in constant, random motion that collide elastically. The particles are considered to have negligible volume and no intermolecular forces. It describes the variables used in gas laws - temperature, pressure, volume, and moles - and how they relate to the kinetic molecular theory and behavior of gas particles. It also discusses gas measurement techniques like manometers and the different units used to measure pressure.
The document discusses the gas laws and properties of gases. It begins by describing the composition of Earth's atmosphere, which is primarily nitrogen and oxygen. It then discusses that gases have mass and low densities compared to liquids and solids. The document outlines four variables that describe gases - pressure, volume, temperature, and amount. It explains concepts such as gas compressibility, units of measurement for gases, and the kinetic molecular theory which describes gas particles as being in constant random motion.
States of matter can exist as solids, liquids, or gases. Gases have no definite shape or volume, are highly compressible, and their molecules are far apart with weak intermolecular forces. Liquids have a definite volume but no definite shape, while solids have both a definite shape and volume. The behavior of gases is explained by gas laws such as Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, Graham's law of diffusion, and the ideal gas law. Gases can be liquefied under high pressure and low temperature due to intermolecular attractions that cause real gases to deviate from ideal behavior.
This document discusses gases and the Kinetic Molecular Theory (KMT). It defines important characteristics of gases such as being highly compressible and having low densities. It also lists measurable properties of gases like pressure, volume, and temperature and their units. The KMT makes assumptions about gas particles being in constant random motion, having negligible actual volume, and not attracting or repelling each other. The KMT also assumes elastic collisions and that average kinetic energy is directly proportional to Kelvin temperature. A gas that follows all KMT postulates is considered an ideal gas.
Gases have unique characteristics compared to liquids and solids. They expand to fill their container and are highly compressible with low densities. To describe a gas, its volume, amount, temperature, and pressure must be specified. The behavior of gases is explained by kinetic molecular theory, which describes gases as particles in constant random motion. Real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces. The van der Waals equation accounts for these non-ideal effects.
This document provides information about gases and the kinetic molecular theory. It defines 11 common gases, lists their properties and uses. The kinetic molecular theory explains that gases are made of particles that move rapidly in random straight lines and collide elastically. The theory accounts for gas properties like compressibility and the fact that gas density varies with temperature and pressure. Key gas properties like volume, pressure, temperature and amount are also defined.
The document discusses gases and their properties according to the kinetic molecular theory. It defines the key concepts of gases including their state, composition of molecules, and random motion. It also outlines the assumptions of the kinetic molecular theory for ideal gases and describes the variables used in gas laws - temperature, pressure, volume, and moles. Real gases are known to deviate from ideal behavior at high pressures or low temperatures due to intermolecular forces and molecular size.
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.
The document discusses gases and their properties according to the kinetic molecular theory. It defines gases as being composed of particles in constant, random motion that collide elastically. The particles are considered to have negligible volume and no intermolecular forces. It describes the variables used in gas laws - temperature, pressure, volume, and moles - and how they relate to the kinetic molecular theory and behavior of gas particles. It also discusses gas measurement techniques like manometers and the different units used to measure pressure.
The document discusses the gas laws and properties of gases. It begins by describing the composition of Earth's atmosphere, which is primarily nitrogen and oxygen. It then discusses that gases have mass and low densities compared to liquids and solids. The document outlines four variables that describe gases - pressure, volume, temperature, and amount. It explains concepts such as gas compressibility, units of measurement for gases, and the kinetic molecular theory which describes gas particles as being in constant random motion.
States of matter can exist as solids, liquids, or gases. Gases have no definite shape or volume, are highly compressible, and their molecules are far apart with weak intermolecular forces. Liquids have a definite volume but no definite shape, while solids have both a definite shape and volume. The behavior of gases is explained by gas laws such as Boyle's law, Charles's law, Avogadro's law, Dalton's law of partial pressures, Graham's law of diffusion, and the ideal gas law. Gases can be liquefied under high pressure and low temperature due to intermolecular attractions that cause real gases to deviate from ideal behavior.
This document discusses gases and the Kinetic Molecular Theory (KMT). It defines important characteristics of gases such as being highly compressible and having low densities. It also lists measurable properties of gases like pressure, volume, and temperature and their units. The KMT makes assumptions about gas particles being in constant random motion, having negligible actual volume, and not attracting or repelling each other. The KMT also assumes elastic collisions and that average kinetic energy is directly proportional to Kelvin temperature. A gas that follows all KMT postulates is considered an ideal gas.
Gases have unique characteristics compared to liquids and solids. They expand to fill their container and are highly compressible with low densities. To describe a gas, its volume, amount, temperature, and pressure must be specified. The behavior of gases is explained by kinetic molecular theory, which describes gases as particles in constant random motion. Real gases deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces. The van der Waals equation accounts for these non-ideal effects.
The document discusses the three states of matter - solid, liquid, and gas. It explains the properties of gases and how gas particles are in constant random motion. The gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation are described. It also covers gas pressure, measurement of pressure using barometers and manometers, gas density calculations, and sample problems involving the gas laws.
Chemistry - Chp 14 - The Behavior of Gases - PowerPointMr. Walajtys
1) Gases are easily compressed and expand to fill their container due to the empty space between particles and their ability to move around.
2) The behavior of gases is described by gas laws relating pressure, volume, temperature, and amount of gas. These include Boyle's law, Charles's law, Gay-Lussac's law, Dalton's law of partial pressures, and Graham's law.
3) The ideal gas law combines these relationships and allows for calculations involving gases assuming they behave ideally. Real gases deviate from ideal behavior at high pressures and low temperatures.
Gases are composed of molecules that are widely separated and in constant, rapid motion. This motion causes gases to exert pressure on their container walls and diffuse freely. The state of a gas is defined by its volume, pressure, temperature, and amount. Under normal conditions, gases approximate ideal gas behavior described by the ideal gas law (PV=nRT), though deviations occur at high pressures and low temperatures when molecular interactions are significant. Common gases in the atmosphere and human body include nitrogen, oxygen, carbon dioxide and their behaviors and roles are described.
This document provides an overview of key concepts related to gases, including:
- Characteristics of gases and units of pressure like atmospheres and torr
- Gas laws like Boyle's, Charles', and Avogadro's laws and how they relate to the ideal gas equation
- How to calculate variables like pressure, volume, moles, and temperature using the ideal gas equation
- Kinetic molecular theory and how it explains gas behavior and properties
- Deviations from ideal gas behavior at high pressures or low temperatures
- The van der Waals equation for correcting for non-ideal behavior
Attacking the TEKS: Focus on Gases presented by Jane Smith, ACT2 2010
This session will expose you to the new TEKS and College Readiness Standards. Ideas for sequencing and planning the unit will be shared along with tips for appropriate demos, labs, and assessments. The intended audience is for teachers with 3 or less years of experience or anyone who wants to delve deeper into the new standards.
The document discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It explains how changing variables like pressure, volume, temperature, and moles of gas affects the behavior of gases based on these laws. Examples are provided to demonstrate how to use the gas laws to calculate unknown variable values.
1. The document discusses the different states of matter and summarizes the key differences between gases, liquids, and solids.
2. It then covers various gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
3. The kinetic molecular theory is introduced to explain gas behavior at the molecular level in terms of molecule motion and interactions.
The document discusses several measurable properties of gases, including volume, pressure, and temperature. It defines volume as the space a gas occupies in its container. Pressure is defined as the force exerted by gas molecules divided by the surface area. Common pressure units are provided. Temperature is defined as the average kinetic energy of gas particles. Standard temperature and pressure conditions for gases are outlined, with standard temperature being 0°C and standard pressure being 1 atmosphere. Boyle's law relating the inverse relationship between gas pressure and volume at constant temperature is briefly explained.
Applied Chapter 12.1 : Characteristics of GasesChris Foltz
The document describes the kinetic molecular theory of gases and its relationship to gas properties. It defines key concepts like pressure, temperature, volume, number of particles and diffusion. The kinetic molecular theory proposes that gases are made of particles in continuous, rapid motion that are far apart with no intermolecular forces. This explains gas properties like expansion to fill its container, fluidity, compressibility, and diffusion due to random particle motion. Standard temperature and pressure are also defined.
Kinetic Molecular Theory describes the behavior of gases in terms of particles in motion. It makes several assumptions about the size, motion, and energy of gas particles. Specifically, it assumes that gas particles are small, move randomly in straight lines until colliding elastically, and have a distribution of kinetic energies determined by their masses and velocities. This theory explains the low density, compressibility, and diffusion of gases as well as how temperature and pressure arise from the motion and collisions of gas particles.
Kinetic Gas Theory including Ideal Gas Equation. Temperature, Volume, Applications
Boyle's Law, Charles' Law and Avogadro's Law. Ideal Gas Theory, Dalton's Partial Pressure
This document provides an overview of chemical thermodynamics and ideal and real gases. It discusses key concepts such as:
- Physical chemistry and thermodynamics, which deals with the application of physics to chemical systems and the relationship between heat and other forms of chemical energy.
- Ideal gases, which obey gas laws at all conditions, versus real gases, which deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces and molecular volumes.
- Equations of state, such as the ideal gas law, which relate pressure, volume, temperature and amount of substance for gases. Van der Waals proposed corrections for real gas behavior accounting for excluded molecular volume and attraction forces.
The document discusses the kinetic theory of gases and gas laws. It describes the assumptions of the kinetic theory, including that gas particles are in constant random motion and collisions are elastic. It defines key variables that describe gases like pressure, volume, temperature and number of moles. The document then explains several important gas laws, including Boyle's Law, Charles's Law, Gay-Lussac's Law, Dalton's Law of Partial Pressures, Graham's Law of Effusion, and Avogadro's Law. It provides examples of using the gas laws to solve problems involving changes in pressure, volume and temperature of gas samples.
This document is a report on ideal and real gases submitted by eight students from the Chemical Engineering Department at Koya University. It includes an abstract, introduction, body with sections on what gases are, the two types of gases (ideal and real), differences between them, applications, and deviations from ideal gas behavior. The body contains figures and explanations of concepts. It concludes that ideal gases have theoretical, non-real properties, while real gas equations can be derived from the ideal gas law to account for intermolecular forces and particle volumes at different pressures and temperatures.
1) The document discusses the kinetic molecular theory and gas laws, which describe the behavior of ideal gases.
2) It explains that ideal gases are made of small, hard spheres that move rapidly in random motion and exert pressure through collisions with container walls.
3) The gas laws described are Boyle's law (inverse relationship between pressure and volume at constant temperature), Charles's law (direct relationship between volume and temperature at constant pressure), and Gay-Lussac's law (direct relationship between pressure and temperature at constant volume).
The document discusses the three states of matter - solid, liquid, and gas. It focuses on the gaseous state and properties of gases. Some key points:
- Gases have molecules that are separated by large distances and move freely and independently of each other.
- Many substances can exist as gases under normal conditions, including elements like hydrogen, nitrogen, oxygen as well as compounds like carbon dioxide and ammonia.
- Gases exert pressure uniformly on all surfaces. Gas pressure is measured using instruments like barometers and manometers.
- The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
The document outlines a unit on matter and its interactions. It includes modules on the behavior of gases, chemical reactions, and biomolecules. The gases module covers properties of gases, gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It also discusses the kinetic molecular theory and differences between ideal and real gases.
1. This document summarizes key concepts about gases from Chapter 5 of Zumdahl's chemistry textbook, including gas laws like Boyle's, Charles', and Avogadro's law, as well as concepts like pressure, the ideal gas law, kinetic molecular theory, and the makeup of the atmosphere.
2. It introduces tools for measuring gas properties such as barometers, manometers, and describes gas behavior using the kinetic molecular theory and concepts like effusion and diffusion.
3. It also discusses how real gases deviate from ideal behavior and the van der Waals equation that accounts for intermolecular forces between particles.
The document discusses the three states of matter - solid, liquid, and gas. It explains the properties of gases and how gas particles are in constant random motion. The gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation are described. It also covers gas pressure, measurement of pressure using barometers and manometers, gas density calculations, and sample problems involving the gas laws.
Chemistry - Chp 14 - The Behavior of Gases - PowerPointMr. Walajtys
1) Gases are easily compressed and expand to fill their container due to the empty space between particles and their ability to move around.
2) The behavior of gases is described by gas laws relating pressure, volume, temperature, and amount of gas. These include Boyle's law, Charles's law, Gay-Lussac's law, Dalton's law of partial pressures, and Graham's law.
3) The ideal gas law combines these relationships and allows for calculations involving gases assuming they behave ideally. Real gases deviate from ideal behavior at high pressures and low temperatures.
Gases are composed of molecules that are widely separated and in constant, rapid motion. This motion causes gases to exert pressure on their container walls and diffuse freely. The state of a gas is defined by its volume, pressure, temperature, and amount. Under normal conditions, gases approximate ideal gas behavior described by the ideal gas law (PV=nRT), though deviations occur at high pressures and low temperatures when molecular interactions are significant. Common gases in the atmosphere and human body include nitrogen, oxygen, carbon dioxide and their behaviors and roles are described.
This document provides an overview of key concepts related to gases, including:
- Characteristics of gases and units of pressure like atmospheres and torr
- Gas laws like Boyle's, Charles', and Avogadro's laws and how they relate to the ideal gas equation
- How to calculate variables like pressure, volume, moles, and temperature using the ideal gas equation
- Kinetic molecular theory and how it explains gas behavior and properties
- Deviations from ideal gas behavior at high pressures or low temperatures
- The van der Waals equation for correcting for non-ideal behavior
Attacking the TEKS: Focus on Gases presented by Jane Smith, ACT2 2010
This session will expose you to the new TEKS and College Readiness Standards. Ideas for sequencing and planning the unit will be shared along with tips for appropriate demos, labs, and assessments. The intended audience is for teachers with 3 or less years of experience or anyone who wants to delve deeper into the new standards.
The document discusses various gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It explains how changing variables like pressure, volume, temperature, and moles of gas affects the behavior of gases based on these laws. Examples are provided to demonstrate how to use the gas laws to calculate unknown variable values.
1. The document discusses the different states of matter and summarizes the key differences between gases, liquids, and solids.
2. It then covers various gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
3. The kinetic molecular theory is introduced to explain gas behavior at the molecular level in terms of molecule motion and interactions.
The document discusses several measurable properties of gases, including volume, pressure, and temperature. It defines volume as the space a gas occupies in its container. Pressure is defined as the force exerted by gas molecules divided by the surface area. Common pressure units are provided. Temperature is defined as the average kinetic energy of gas particles. Standard temperature and pressure conditions for gases are outlined, with standard temperature being 0°C and standard pressure being 1 atmosphere. Boyle's law relating the inverse relationship between gas pressure and volume at constant temperature is briefly explained.
Applied Chapter 12.1 : Characteristics of GasesChris Foltz
The document describes the kinetic molecular theory of gases and its relationship to gas properties. It defines key concepts like pressure, temperature, volume, number of particles and diffusion. The kinetic molecular theory proposes that gases are made of particles in continuous, rapid motion that are far apart with no intermolecular forces. This explains gas properties like expansion to fill its container, fluidity, compressibility, and diffusion due to random particle motion. Standard temperature and pressure are also defined.
Kinetic Molecular Theory describes the behavior of gases in terms of particles in motion. It makes several assumptions about the size, motion, and energy of gas particles. Specifically, it assumes that gas particles are small, move randomly in straight lines until colliding elastically, and have a distribution of kinetic energies determined by their masses and velocities. This theory explains the low density, compressibility, and diffusion of gases as well as how temperature and pressure arise from the motion and collisions of gas particles.
Kinetic Gas Theory including Ideal Gas Equation. Temperature, Volume, Applications
Boyle's Law, Charles' Law and Avogadro's Law. Ideal Gas Theory, Dalton's Partial Pressure
This document provides an overview of chemical thermodynamics and ideal and real gases. It discusses key concepts such as:
- Physical chemistry and thermodynamics, which deals with the application of physics to chemical systems and the relationship between heat and other forms of chemical energy.
- Ideal gases, which obey gas laws at all conditions, versus real gases, which deviate from ideal behavior at high pressures and low temperatures due to intermolecular forces and molecular volumes.
- Equations of state, such as the ideal gas law, which relate pressure, volume, temperature and amount of substance for gases. Van der Waals proposed corrections for real gas behavior accounting for excluded molecular volume and attraction forces.
The document discusses the kinetic theory of gases and gas laws. It describes the assumptions of the kinetic theory, including that gas particles are in constant random motion and collisions are elastic. It defines key variables that describe gases like pressure, volume, temperature and number of moles. The document then explains several important gas laws, including Boyle's Law, Charles's Law, Gay-Lussac's Law, Dalton's Law of Partial Pressures, Graham's Law of Effusion, and Avogadro's Law. It provides examples of using the gas laws to solve problems involving changes in pressure, volume and temperature of gas samples.
This document is a report on ideal and real gases submitted by eight students from the Chemical Engineering Department at Koya University. It includes an abstract, introduction, body with sections on what gases are, the two types of gases (ideal and real), differences between them, applications, and deviations from ideal gas behavior. The body contains figures and explanations of concepts. It concludes that ideal gases have theoretical, non-real properties, while real gas equations can be derived from the ideal gas law to account for intermolecular forces and particle volumes at different pressures and temperatures.
1) The document discusses the kinetic molecular theory and gas laws, which describe the behavior of ideal gases.
2) It explains that ideal gases are made of small, hard spheres that move rapidly in random motion and exert pressure through collisions with container walls.
3) The gas laws described are Boyle's law (inverse relationship between pressure and volume at constant temperature), Charles's law (direct relationship between volume and temperature at constant pressure), and Gay-Lussac's law (direct relationship between pressure and temperature at constant volume).
The document discusses the three states of matter - solid, liquid, and gas. It focuses on the gaseous state and properties of gases. Some key points:
- Gases have molecules that are separated by large distances and move freely and independently of each other.
- Many substances can exist as gases under normal conditions, including elements like hydrogen, nitrogen, oxygen as well as compounds like carbon dioxide and ammonia.
- Gases exert pressure uniformly on all surfaces. Gas pressure is measured using instruments like barometers and manometers.
- The behavior of gases is described by gas laws including Boyle's law, Charles' law, Avogadro's law, and the ideal gas equation.
The document outlines a unit on matter and its interactions. It includes modules on the behavior of gases, chemical reactions, and biomolecules. The gases module covers properties of gases, gas laws including Boyle's law, Charles' law, Gay-Lussac's law, the combined gas law, and the ideal gas law. It also discusses the kinetic molecular theory and differences between ideal and real gases.
1. This document summarizes key concepts about gases from Chapter 5 of Zumdahl's chemistry textbook, including gas laws like Boyle's, Charles', and Avogadro's law, as well as concepts like pressure, the ideal gas law, kinetic molecular theory, and the makeup of the atmosphere.
2. It introduces tools for measuring gas properties such as barometers, manometers, and describes gas behavior using the kinetic molecular theory and concepts like effusion and diffusion.
3. It also discusses how real gases deviate from ideal behavior and the van der Waals equation that accounts for intermolecular forces between particles.
Similar to INTRO-GASES.pptx reviewer for 4th quarte (20)
Monitor indicators of genetic diversity from space using Earth Observation dataSpatial Genetics
Genetic diversity within and among populations is essential for species persistence. While targets and indicators for genetic diversity are captured in the Kunming-Montreal Global Biodiversity Framework, assessing genetic diversity across many species at national and regional scales remains challenging. Parties to the Convention on Biological Diversity (CBD) need accessible tools for reliable and efficient monitoring at relevant scales. Here, we describe how Earth Observation satellites (EO) make essential contributions to enable, accelerate, and improve genetic diversity monitoring and preservation. Specifically, we introduce a workflow integrating EO into existing genetic diversity monitoring strategies and present a set of examples where EO data is or can be integrated to improve assessment, monitoring, and conservation. We describe how available EO data can be integrated in innovative ways to support calculation of the genetic diversity indicators of the GBF monitoring framework and to inform management and monitoring decisions, especially in areas with limited research infrastructure or access. We also describe novel, integrative approaches to improve the indicators that can be implemented with the coming generation of EO data, and new capabilities that will provide unprecedented detail to characterize the changes to Earth’s surface and their implications for biodiversity, on a global scale.
There is a tremendous amount of news being disseminated every day online about dangerous forever chemicals called PFAS. In this interview with a global PFAS testing expert, Geraint Williams of ALS, he and York Analytical President Michael Beckerich discuss the hot-button issues for the environmental engineering and consulting industry -- the wider range of PFAS contamination sites, new PFAS that are unregulated, and the compliance challenges ahead.
Widespread PFAS contamination requires stringent sampling and laboratory analyses by certified laboratories only -- whether it is for PFAS in soil, groundwater, wastewater or drinking water.
Contact us at York Analytical Laboratories for expert environmental testing with fast turnaround times and client service. We have 4 state-certified laboratories in Connecticut, New York and New Jersey, and 4 client service centers.
P: 800-306-YORK
E: clientservices@YorkLab.com
W: YorkLab.com
(Q)SAR Assessment Framework: Guidance for Assessing (Q)SAR Models and Predict...hannahthabet
The webinar provided an overview of the new OECD (Q)SAR Assessment Framework for evaluating the scientific validity of (Q)SAR models, predictions, and results from multiple predictions. The QAF provides assessment elements for existing principles for evaluating models, as well as new principles for evaluating predictions and results. In addition to the principles, assessment elements, and guidance for evaluating each element, the QAF includes a checklist for reporting assessments.
This new Framework provides regulators with a consistent and transparent approach for reviewing the use of (Q)SAR predictions in a regulatory context and increases the confidence to accept alternative methods for evaluating chemical hazards. The OECD worked closely together with the Istituto Superiore di Sanità (Italy) and the European Chemicals Agency (ECHA), supported by a variety of international experts to develop a checklist of criteria and guidance for evaluating each criterion. The aim of the QAF is to help establish confidence in the use of (Q)SARs in evaluating chemical safety, and was designed to be applicable irrespective of the modelling technique used to build the model, the predicted endpoint, and the intended regulatory purpose.
The webinar provided an overview of the project and presented the main aspects of the framework for assessing models and results based on individual or multiple predictions.
Trichogramma spp. is an efficient egg parasitoids that potentially assist to manage the insect-pests from the field condition by parasiting the host eggs. To mass culture this egg parasitoids effectively, we need to culture another stored grain pest- Rice Meal Moth (Corcyra Cephalonica). After rearing this pest, the eggs of Corcyra will carry the potential Trichogramma spp., which is an Hymenopteran Wasp. The detailed Methodologies of rearing both Corcyra Cephalonica and Trichogramma spp. have described on this ppt.
Emerging Earth Observation methods for monitoring sustainable food productionCIFOR-ICRAF
Presented by Daniela Requena Suarez, Helmholtz GeoResearch Center Potsdam (GFZ) at "Side event 60th sessions of the UNFCCC Subsidiary Bodies - Sustainable Bites: Innovating Low Emission Food Systems One Country at a Time" on 13 June 2024
2. RECAP…
In your grade 8 chemistry, you learned different properties of Gases.
Identify whether the statement isTRUE or FALSE.
1. Gases have indefinite shape and volume.
2. Gas is the state in which matter expands to occupy the volume and
shape of its container.
3. Gases have low density which contain scattered molecules that are
dispersed across a given volume.
4. Particles of gases move in random motion with little attraction to each
other.
5. Gases are highly compressible.
4. Scientists have observed some activities
involving gases. They found out that the behavior
of gases is determined by the behavior of its
individual particle. In 1870, scientists formulated
the Kinetic Molecular Theory (KMT) using a simple
model of an ideal gas or a theoretical gas. The
particles of an ideal gas behave consistently and in
a predictable manner.
13. PRESSURE
The pressure of a confined gas is the average effect of the
forces of the colliding molecules.
It can be measured in atmosphere (atm), torr, psi, cmHg,
mmHg)
P = F/A where: P=pressure, F=force, A= area
When you open a can or bottle of softdrinks, it fizzes
because of the escaping dissolved carbon dioxide due to
change of pressure.
When the wind blows, it exerts pressure too
14. MASS
The amount of gas or its mass could be
expressed in moles or grams. The mass is
negligible.
Which is heavier, inflated balloon or
deflated balloon?
15. VOLUME
The volume of gas is the amount of space occupied by the gases.
Gases have the tendency to occupy all the spaces of the container that
they are confined.
Gases have weak intermolecular forces of attraction, hence, they are
arranged as far away as possible from each other.
The common units used in expressing the volume of gas are liter (L)
and milliliter (mL).
The basketball is filled with air. So, it bounces while you are dribbling
it.
16. TEMPERATURE
The temperature of a gas is the measure of the hotness or
coldness of an object.
It is proportional to the average kinetic energy of its
molecules.
It can be measured in Celsius and Kelvin.
Kelvin is the absolute scale
17.
18. UNITS BEING USED TO EXPRESS
THE PROPERTIES OF GASES
VARIABLE UNIT
Volume Cubic meter (m3 )
Cubic decimeter (dm3 )
Cubic centimeter (cm3 )
Liter (L)
Milliliter (mL)
Quart (qt)
Gallon (gal)
Pressure Pascal (Pa), kPa
Atmosphere (atm)
Millimeters of mercury (mmHg)
Centimeters of mercury (cmHg)
Torr
Lb/in2 (psi)
Temperature Celcius (⁰C)
Farenheight (⁰F)
19. EQUIVALENTS
Volume units and their equivalents
1 mL = 1 cm3 1 L = 1 dm3 1 m3 = 1000 L
Pressure units and their equivalents
1 atm = 760 mmHg = 76 cmHg = 760 torr = 101325Pa = 101.325kPa=14.6956 psi
Temperature units and their equivalents
0 ⁰C = 273.15 K 0 ⁰C = 32 ⁰F
21. GAS LAWS
GAS LAW SCIENTIST FORMULA CONSTANT RELATIONSHIP
BOYLE’S LAW Robert Boyle P1 V1 = P2 V2 Temperature Inversely
proportional
CHARLES’LAW Jacques Charles V1T2 = V2 T1 Pressure Directly
proportional
GAY-LUSSAC’S
LAW
Joseph Loius Gay-
Lussac
P1T2 = P2 T1 Volume Directly
proportional
COMBINED GAS
LAW
V1P1T2 = V2P2 T1
AVOGADRO’S
LAW
Lorenzo Romano
Amedeo Carlo
Avogadro
V1n2 = V2 n1 Pressure,
Temperature
Directly
proportional
IDEAL GAS LAW PV = nRT
22. WHERE:
V= Volume
T = Temperature
n = amount of gas in moles
R = Universal gas constant
1 = Used as subscript, means initial condition
2 = used as subscript, means final condition