'Avogadro' diaporamas de présentation

Halliday/Resnick/Walker Fundamentals of Physics 8 th edition

Halliday/Resnick/Walker Fundamentals of Physics 8 th edition. Classroom Response System Questions. Chapter 19 The Kinetic Theory of Gases. Reading Quiz Questions.

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Compounds & Moles

Compounds & Moles. Unit 5. Overview. Naming Ionic Covalent Acids Simple Organic The Mole Molar Mass Mole Conversions. Calculations Percent Composition Empirical Formula Molecular Formula. Why do we name compounds?. Think of some common compounds that you know of.

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Chapter 7 Review (Part II)

Chapter 7 Review (Part II). CP Chemistry Mrs. Klingaman. Q :1. What types of atoms are covalent (aka: molecular) compounds made of?. A :1. nonmetals. Q :2. True or False: When naming ionic compounds, roman numerals are used to express the charge of the transition metal ion. A:2. True.

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Mole Problems

Mole Problems. Calculating molar mass. Round all masses to the 10ths place. Calculate the molecular weight of F e 2 O 3. Step One: two atoms of iron and three of oxygen Step Two: Fe = 55.8 amu and O = 16.0 amu Step Three: (2 x 55.8) + (3 x 16.0)

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What Is a Mole?

What Is a Mole?. One mole = 6.022 x 10 23 items. A mole of atoms Or molecules. How Big is a Mole?. N=6.022x10 23 One mole of Marshmallows would cover the entire earth 12 miles high

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Molar Mass/The Mole

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The Mole

The Mole. Chemistry SOL 1.g.14; 4.a.1-6. Chemical Measurements. Atomic Mass The weighted average of the masses of existing isotopes of an element Measured in atomic mass units (amu). Formula Mass The sum of the atomic masses of all atoms in a compound as represented in a chemical formula.

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Chapter 2: Atoms and Molecules

Chapter 2: Atoms and Molecules. Chemistry 140 HCC/TCHS. LEARNING OBJECTIVES/ASSESSMENT. 1. Use symbols for chemical elements to write formulas for chemical compounds. 2. Identify the characteristics of protons, neutrons, and electrons.

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Mass Relationships

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AP Chemistry

AP Chemistry. Chapter 3 Stoichiometry (Part 1). 3.1 Atomic Masses (p. 80) An atomic mass unit ( amu ) is defined such that the mass of 12 C is exactly 12 amu . Atomic mass in the periodic table is the average atomic mass of all stable isotopes of the element.

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Chapter 7 - Review Chemical Quantities

Chapter 7 - Review Chemical Quantities. Milbank High School. Chapter 7 - Review. What SI unit is used to measure the number of representative particles in a substance? How many moles of Tungsten atoms are there in 4.8 x 10 25 atoms of Tungsten?

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Chemistry 1 Notes #5 Chapter 11 Section 1 THE MOLE & particle calculations

Chemistry 1 Notes #5 Chapter 11 Section 1 THE MOLE & particle calculations. Last updated June 10, 2014. MOLEs. Moles Moles Moles Moles Moles Moles Moles. Measuring Matter. What is a mole? The Mole is an SI base unit for the amount of a substance.

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Physical Properties of Matter Intensive Properties : Do not change regardless of quantity.

Physical Properties of Matter Intensive Properties : Do not change regardless of quantity. Examples: Density, color, chemical composition Extensive Properties : Are dependent on quantity. Examples: grams, milliliters, moles

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How many atoms of aluminum are present in 1.423 moles of aluminum?

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III. Ideal Gas Law (p. 334-335, 340-346)

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Amedeo Avogadro

Amedeo Avogadro. In order to state that equal volumes of all gases at the same temperature and pressure contain the same number of molecules, Amedeo Avogadro used the ideas of Gay-Lussac in the year 1811. Avogadro's Principle.

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Weighing gases lab

Weighing gases lab. Results. Gas. Flask. Flask+gas. Mass (g). Density(g/L). H 2. 345.00. 345.08. 0.0835. 0.0835. O 2. 345.00. 346.32. 1.32. 1.32. CO 2. 345.00. 346.82. 1.82. 1.82. Gas. Molar mass (g/mol). Moles (mol). # of molecules. H 2. 2.02. 0.041 3. 2.4 9 x 10 22.

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How Do Gases Behave?

How Do Gases Behave?. The behavior of gases can be described by the kinetic molecular theory of ideal gases. Gases consist of submicroscopic particles moving about randomly with no attractive forces for one another.

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Do NOW

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