Thermodynamics AP Chem
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Thermodynamics
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Kinetics and Equilibrium AP Chem
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Chemistry Chp. 11 Review
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Holt Modern Chemistry Review CHAPTER 11: GASES The following pages contain the bulk (but not all) of the information for the chapter 11 test. Focus on this content, but make sure to review class notes, activities, handouts, questions, etc. If you study this document and NOTHING else, you should at least be able to PASS the test. ***** Test items will be recall, examples, and/or application of this content. ***** OUTCOMES Collaborate with peer(s) to understand chemistry content (C C) Communicate chemistry content to teacher and peer(s) (E C) 11.2: Identify gas laws: Boyle?s, Charles?, Ideal gas law (T & R) 11.3: Apply reaction stoichiometry to solve gas stoichiometry problems (F & PK) 11.1: GASES AND PRESSURE Chapter Highlights
energy_sources
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The University of Hong Kong - Faculty of Engineering L1: Energy Sources Faculty of Engineering CCST9016 Energy: Its Evolution and Environmental Impacts Dr. Match Wai Lun Ko Department of Mechanical Engineering The University of Hong Kong [email protected] 1 The University of Hong Kong - Faculty of Engineering Course objectives 2 Through lectures, technical visit, project and discussion of key energy and environmental issues, students would be able to: 1. Develop a broader perspective and critical understanding of various energy issues. 2. Appreciate various viewpoints and responsibilities as global and local citizens; 3. Develop problem-solving ability on energy issues. The University of Hong Kong - Faculty of Engineering Lecturers
Holt Earth Science Chapter 18, Section 18.1
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Water?s Changes of State Water exists in all 3 states of matter and is made of hydrogen and oxygen atoms. In all 3 stages of matter, these molecules are in constant motion (higher temperature: more movement). Difference between 3 states is the arrangement of the water molecules. A. Ice, Liquid Water, and Water Vapor Ice is made of water molecules held together by mutual molecular attractions.They form a tight, orderly network and don?t move - they vibrate in a fixed position. When ice is heated, the molecules vibrate more, and when the rate of movement increases enough, the bonds between the molecules break, resulting in melting In the liquid state, the molecules are still tightly packed but move fast enough to slide past each other (this causes liquid water to be fluid)
IB Topic 3 problems set
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Topic 3 ? Thermal physics Formative Assessment PROBLEM SET NAME: ________________________________ TEAM:__ THIS IS A PRACTICE ASSESSMENT. Show formulas, substitutions, answers, and units! Topic 3.1 ? Thermal concepts [ NGSS Supplement to Topic 3.1 begins at problem 51... ] The following questions are about internal energy. 1. What are the two forms of internal energy? 2. Suppose a liquid?s starting temperature is 20(C and its ending temperature is 35(C. Explain what happens to each form of internal energy. 3. How can you tell if the internal potential energy of a substance has changed? 4. How can you tell if the internal kinetic energy of a substance has changed? The following questions are about temperature scales.
Chapter 10
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Chapter 10 Gases James F. Kirby Quinnipiac University Hamden, CT Lecture Presentation ? 2015 Pearson Education, Inc. 1 Characteristics of Gases Physical properties of gases are all similar. Composed mainly of nonmetallic elements with simple formulas and low molar masses. Unlike liquids and solids, gases expand to fill their containers. are highly compressible. have extremely low densities. Two or more gases form a homogeneous mixture. Gases ? 2015 Pearson Education, Inc. 2 Properties Which Define the State of a Gas Sample Temperature Pressure Volume Amount of gas, usually expressed as number of moles Having already discussed three of these, we need to define pressure. Gases ? 2015 Pearson Education, Inc. Pressure is the amount of force applied to an area: Pressure
ideal gas law
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IDEAL GAS LAW THE REALTIONSHIP PV=nRT describes THE BEHAVIOR OF AN IDEAL GAS. (PRESSURE*VOLUME=#MOLES*R VALUE*TEMPERATURE)
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Kinetic Molecular Theory
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Kinetic Molecular Theory All matter is composed of small particles. Particles of matter are in constant motion. Particle collisions are elastic. (No transfer of energy/loss of energy in a collision) Gases only: Volume of each gas particle is negligible compared to the volume of the sample. Particles of gases exert no forces of attractions on each other. (This is due to the great distance between molecules.) Ideas of KMT explain ideal gas behavior. Deviations of ideal gas behavior occur among real gases because real gases do have volume and IMF?s. Deviations are minimized under conditions of low pressure and high temperature (PLIGHT) Hydrogen and helium behave most like ideal gases due to their small size and very weak IMFs.
Gas Laws
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Gas Laws -study the relationships that exist between pressure, volume, temperature and amount (moles) of gas. Boyle?s Law Pressure-volume relationship At constant temperature and amount, the pressure and volume of a gas are inversely proportional. As pressure increases, volume decreases. P1V1=P2V2 Charles? Law Temperature-volume relationship At constant pressure and amount, the temperature and volume of a gas are directly proportional. V1/T1=V2/T2 Gay Lussac?s Law Pressure-temperature relationship Under conditions of constant volume and amount, the temperature and pressure of a gas are directly proportional. P1/T1=P2/T2
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