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Gas

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

alg

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Fundamentals of Chemistry What is Chemistry? What is Matter? How does it change? (How do we organize the types of changes? What categories? How do we categorize the types of matter? We can identify the specific types of matter with its ________ (characteristics). Definition: How many Smallest unit Examples Element: Compound: Mixture: What is the table of elements called? Is a compound considered a pure substance? How is a compound different than a mixture? Is a mixture considered a pure substance? How are mixtures classified? Draw sketches: solid liquid gas Macroscopic Microscopic How do the microscopic models explain the macroscopic properties? Property Solid Liquid Gas Fluidity (fixed shape) Why? Compressibity (fixed volume)

IB Topic 3 problems set

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Temperature
Isobaric process

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 1.2 Outline

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Gas
Liquid

Matter Classified by? Physical State (Gas/ Liquid/ Solid) Composition (Element/ Compound/ Mixture) States of Matter Gas (vapor) No fixed volume or shape Uniformly fills its container Can be compressed to occupy a smaller volume Can be expanded to occupy a larger volume Molecules are far apart, move quickly, and often collide with the surrounding container Liquid Distinct volume (independent of container) No fixed shape (assumes shape of occupied container) Can't be compressed Molecules are packed closely but can still move (they flow over each other, reducing viscosity Solid Definite shape and definite volume Can't be compressed Molecules have fixed positions an wiggle only slightly *Temperature and pressure changes lead to phase changes of the substance

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

IDEAL GAS LAW THE REALTIONSHIP PV=nRT describes THE BEHAVIOR OF AN IDEAL GAS. (PRESSURE*VOLUME=#MOLES*R VALUE*TEMPERATURE)
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AP serway notes chp 9

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Solid
Gas
Crystal

Chapter 9 Solids and Fluids States of Matter Solid Liquid Gas Plasma Solids Have definite volume Have definite shape Molecules are held in specific locations By electrical forces Vibrate about equilibrium positions Can be modeled as springs connecting molecules More About Solids External forces can be applied to the solid and compress the material In the model, the springs would be compressed When the force is removed, the solid returns to its original shape and size This property is called elasticity Crystalline Solid Atoms have an ordered structure This example is salt Gray spheres represent Na+ ions Green spheres represent Cl- ions Amorphous Solid Atoms are arranged almost randomly Examples include glass Liquid

Gas Laws

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Joseph Louis Gay-Lussac
Charles's law

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

The atmosphere

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Noble gases
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Argon
Xenon
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The atmosphere Made up of a mixture of gases (mainly N2 and O2) Mole fractions of major gases (nitrogen, oxygen, carbon dioxide, argon) are pretty constant with altitude ?interesting stuff? involves tiny amounts of trace gases ? ozone, oxides of nitrogen and sulfur and some others ~ 100% Breathing!!! Argon, Neon, Xenon ? rare gases often used in ?neon? lights Atmospheric gases can be separated by distillation, since they have different boiling points N2 77 K O2 90 K Ar 87 K Ne 24 K CH4 111 K Pressure profile of atmosphere Pressure drops almost exponentially with increasing altitude ... why?? Trop. Strat. Temperature profile in the atmosphere stratosphere pV = nRT ideal gas law is ?pretty good? (why??)
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