Chapter 4
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This document provides an overview of key concepts related to properties of matter and energy transformations. It defines physical and chemical properties of substances and describes physical and chemical changes. It introduces concepts like conservation of mass and energy, and how energy is involved in chemical reactions through absorption or release. Chemical equations are used to represent reactions where energy is either absorbed or released, in accordance with the law of conservation of energy.
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Applied Chapter 2.1 : Energy
1) Physical and chemical changes in matter involve transfers of energy. Energy can move or change objects and form new compounds. It is always involved in changes of matter.
2) The law of conservation of energy states that energy cannot be created or destroyed, just changed from one form to another. Changes can be endothermic, absorbing energy, or exothermic, releasing energy.
3) Heat is the energy transferred between objects, while temperature is a measure of the average kinetic energy of particles. Heat is involved in both physical and chemical changes, but does not necessarily affect the temperature.
Thermal Properties of Matter
Specific Heat Capacity
Melting and Boiling
Evaporation
Thermal Expansion of Solids, Liquids and Gases
Thermal physics ppt
This document discusses key concepts in thermal physics including heat, temperature, specific heat capacity, and latent heat. It begins by defining heat as a form of energy and temperature as a measurement of how hot or cold something is. It explains that different materials require different amounts of heat to change temperature by the same amount due to differences in specific heat capacity. The document then discusses phase changes and how heat is required for changes of state, like melting and boiling, without a change in temperature due to the absorption of latent heat. It provides examples of calculating specific heat capacity and using the principle of conservation of energy to solve problems involving heat transfer.
Sci 1010 chapter 5
The document discusses different topics relating to temperature and heat transfer. It defines temperature as a measure of the average kinetic energy of molecules. It describes how thermometers work using properties like thermal expansion. Common temperature scales like Celsius, Fahrenheit and Kelvin are presented along with equations to convert between them. The document also discusses concepts such as heat, specific heat, latent heat and the phases of matter. It explains different methods of heat transfer including conduction, convection and radiation.
Energy
This document summarizes key concepts about energy and chemical change from a chapter in a textbook. It defines energy as the ability to do work or produce heat, and distinguishes between potential and kinetic energy. Potential energy depends on an object's composition and arrangement, while kinetic energy is energy of motion. Chemical reactions can convert chemical potential energy into other forms like heat. The law of conservation of energy states that energy cannot be created or destroyed, only changed from one form to another. Heat is a transfer of energy between objects at different temperatures, and can be measured using calories or joules. Specific heat refers to the amount of heat needed to change an object's temperature and differs between substances.
Energy
This document provides information about energy and chemical changes from a chemistry textbook. It defines energy as the ability to do work or produce heat, and discusses the two main forms of energy as potential and kinetic. Potential energy is due to the position or composition of an object, while kinetic energy is energy of motion. It also introduces the law of conservation of energy, which states that energy cannot be created or destroyed, only changed from one form to another. The document provides examples of potential, kinetic, chemical, and heat energy. It defines heat as energy transferred between objects at different temperatures and discusses units used to measure heat. The specific heat of a substance, or amount of heat needed to change its temperature, is also explained. Examples of
NWTC General Chemistry Ch 04
The document is a chapter from an introductory chemistry textbook about properties of matter. It discusses physical and chemical properties, physical and chemical changes, conservation of mass and energy during chemical reactions. It provides examples of physical and chemical changes and properties. It also discusses heat, temperature, specific heat, and the various forms energy takes in chemical and physical processes.
FM 3.pptx
The document discusses fuel types, water treatment processes, and heat transfer calculations. It describes the three main types of fuels as solid, liquid, and gaseous. It also outlines several water treatment steps including removal of suspensions, dissolved salts, minerals, and pathogens. Specific heat capacity and formulas for calculating heat requirements for various processes like heating food or water are provided.
Basic Chemistry-1-.pptx
This document provides an overview of key chemistry concepts including:
- Matter and its classifications including elements, compounds, and mixtures
- The three states of matter and phase changes
- Physical and chemical properties of substances
- Energy, heat, and their relationship to chemical changes and physical processes
- Calorimetry and calculation of energy changes using specific heat
Energy and chemical change - Section 1
Introduction to thermochemistry. It includes a definition for heat and energy. the units of heat. How to calculate the heat absorbed or released. Definition of specific heat.
Specific Heat Ditto
1. The document provides background information on specific heat, which is the measure of heat energy required to increase the temperature of a substance by 1 degree. It takes more energy to raise the temperature of water than air.
2. It includes questions about specific heat values of different substances like water, basalt, granite, and air. An equation is also provided to calculate the heat energy required to change a substance's temperature based on its mass, specific heat, and change in temperature.
3. Sample problems are given applying the specific heat equation to calculate the heat energy needed to change the temperature of various substances by given amounts.
Specific Heat Ditto
1. The document provides background information on specific heat, which is the measure of heat energy required to increase the temperature of a substance by 1 degree. It takes more energy to raise the temperature of water than air.
2. It includes questions about specific heat values of different substances like water, basalt, granite, and air. An equation is also provided to calculate the heat energy required to change a substance's temperature based on its mass, specific heat, and change in temperature.
3. Sample problems are given applying the specific heat equation to calculate the heat energy needed to change the temperature of various substances by given amounts.
17.1 17.2 lecture slides
Thermochemistry is the study of energy changes that occur during chemical reactions and changes in state. Heat is energy that transfers from one object to another due to a temperature difference. In an endothermic process, the system gains heat from its surroundings, while in an exothermic process the system loses heat to its surroundings. Calorimetry allows for the precise measurement of heat flow during chemical and physical processes using an insulated calorimeter. The enthalpy change of a reaction, measured in kilojoules, can be determined from calorimetry experiments and represented in a thermochemical equation.
Chapter 17
1. Thermochemistry examines energy changes that occur during chemical reactions and changes in state.
2. Energy can be transferred as heat or work. Exothermic processes release heat to the surroundings while endothermic processes absorb heat from the surroundings.
3. The specific heat of a substance depends on its mass and chemical composition and determines how much its temperature changes when heat is added or removed. Water has a high specific heat.
Chemistry Unit 2 Part 1
This document discusses different types of properties and changes in matter. It defines extensive and intensive properties, with examples like mass and density. Physical properties can be observed without changing a substance's identity, while chemical properties involve changes in a substance's composition or structure. Physical changes alter a substance's state or form without changing its chemical makeup, like phase changes between solid, liquid and gas. Chemical changes form new substances through chemical reactions. All changes require a transfer of energy.
Thermochemistry ch 16
This document provides an overview of thermochemistry and key concepts related to heat and energy transfers during chemical and physical processes. It defines important terms like heat, temperature, enthalpy, and heat capacity. It also distinguishes between endothermic and exothermic reactions, and describes heat changes associated with phase changes like melting, vaporization, solidification, and condensation. Specific concepts covered include Hess's law of heat summation, standard heats of formation and reaction, and calculating heat changes using thermochemical data.
Production of hydrocarbons
The document summarizes key methods for producing hydrocarbons including alkanes, alkenes, and alkynes. It describes hydrogenation and the Wurth reaction as two methods for preparing alkanes, where hydrogenation involves adding hydrogen across a double bond and the Wurth reaction involves reacting two alkyl halides with sodium. It also explains that alkenes can be prepared through dehydration of alcohols using heat or catalysts, which removes a water molecule. Finally, it states that alkynes can be produced from calcium carbide and water or through pyrolysis of methane at high temperatures.
Chemistry Chapter 1
This document provides an introduction to chemistry, including:
1. Definitions of key terms like elements, compounds, physical and chemical properties and changes.
2. An overview of the major branches of chemistry like organic, inorganic, physical and analytical chemistry.
3. Descriptions of the periodic table, including groups like alkali metals and halogens, and periodic trends.
Energy changes
This is a summary of the topic "Energy changes" in the GCE O levels subject: Chemistry. Students taking either the combined science (chemistry/physics) or pure chemistry will find this useful. These slides are prepared according to the learning outcomes required by the examinations board.
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Chapter 4
- 1. Properties of Matter Chapter 4
- 2. Chapter Outline 4.1 Properties of Substances 4.2 Physical Changes 4.3 Chemical Changes 4.4 Conservation of Mass 4.5 Energy 4.6 Heat: Quantitative Measurement 4.7 Energy in Chemical Changes 4.8 Conservation of Energy
- 11. Â
- 12. Physical Changes
- 14. Chemical Changes
- 15. In a chemical change new substances are formed that have different properties and composition from the original material.
- 16. Formation of Copper(II) Oxide Heating a copper wire in a Bunsen burner causes the copper to lose its original appearance and become a black material. The black material is a new substance called copper(II) oxide. Copper is 100% copper by mass. Copper (II) oxide is: 79.94% copper by mass and 20.1% oxygen by mass. The formation of copper(II) oxide from copper and oxygen is a chemical change. The copper (II) oxide is a new substance with properties that are different from copper.
- 17. Formation of Copper(II) Oxide Copper(II) oxide is made up of Cu 2+ and O 2- Neither Cu nor O 2 contains Cu 2+ or O 2- A chemical change has occurred. 4.2
- 18. Water is decomposed into hydrogen and oxygen by passing electricity through it. Decomposition of Water The composition and physical appearance of hydrogen and oxygen are different from water. The hydrogen explodes with a pop upon the addition of a burning splint. The oxygen causes the flame of a burning splint to intensify. They are both colorless gases. But the burning splint is extinguished when placed into the water sample.
- 20. Water decomposes into hydrogen and oxygen when electrolyzed. reactant products yields
- 21. Chemical symbols can be used to express chemical reactions
- 22. Water decomposes into hydrogen and oxygen when electrolyzed. reactant yields 2H 2 O 2H 2 O 2 products
- 23. Copper plus oxygen yields copper(II) oxide. yield product reactants heat
- 24. Copper plus oxygen yields copper(II) oxide. heat yield product reactants 2Cu O 2 2Cu 2 O
- 25. Â
- 26. Conservation of Mass
- 27. No change is observed in the total mass of the substances involved in a chemical change.
- 28. sodium + sulfur ď‚® sodium sulfide 78.1 g 78.1 g product mass products 78.1 g reactant -> 46.0 g 32.1 g mass reactants =
- 29. Energy
- 30. Energy is the capacity to do work
- 32. Potential Energy Energy that an object possesses due to its relative position.
- 33. The potential energy of the ball increases with increasing height. increasing potential energy 50 ft 20 ft increasing potential energy
- 34. Potential Energy Stored energy.
- 36. Kinetic Energy Energy matter possesses due to its motion.
- 41. Heat: Quantitative Measurement
- 43. Units of Heat Energy
- 45. An Example of the Difference Between Heat and Temperature A form of energy associated with small particles of matter. A measure of the intensity of heat, or of how hot or cold a system is.
- 46. Twice as much heat energy is required to raise the temperature of 200 g of water 10 o C as compared to 100 g of water. 200 g water 20 o C A 100 g water 20 o C B heat beakers temperature rises 10 o C 100 g water 30 o C 200 g water 30 o C 4184 J 8368 J
- 47. Specific Heat
- 48. The specific heat of a substance is the quantity of heat required to change the temperature of 1 g of that substance by 1 o C.
- 49. Â
- 53. Example 1
- 54. Calculate the specific heat of a solid in J/g o C and in cal/ g o C if 1638 J raise the temperature of 125 g of the solid from 25.0 o C to 52.6 o C. (mass of substance)(specific heat of substance) Δ t = heat (g)(specific heat of substance) Δ t = heat heat = 1638 J mass = 125 g Δ t = 52.6 o C – 25.0 o C = 27.6 o C
- 55. Calculate the specific heat of a solid in J/g o C and in cal/ g o C if 1638 J raise the temperature of 125 g of the solid from 25.0 o C to 52.6 o C. Convert joules to calories using 1.000 cal/4.184 J
- 56. Energy in Chemical Changes
- 57. In all chemical changes, matter either absorbs or releases energy .
- 58. Energy Release From Chemical Sources Chemical changes occurring within body cells. Body Combustion of fuels. Heat and Light A lightstick. Fuel combustion. Light Storage batteries Electrical Energy Source Type of Energy
- 59. Chemical Changes Caused by Absorption of Energy Photosynthesis in green plants. Light Electroplating of metals. Decomposition of water into hydrogen and oxygen Electrical Chemical Change Type of Energy
- 62. 4.4 H 2 + O 2 have higher potential energy than H 2 O Electrolysis of Water Burning of Hydrogen in Air energy is given off energy is absorbed higher potential energy lower potential energy
- 63. Law of Conservation of Energy Energy cannot be created or destroyed, it can only change forms.
- 64. The End