Chapter 3(a) Stoichiometry. Copyright © Houghton Mifflin Company. All rights reserved.3a–2 Figure 3.1: (left) A scientist injecting a sample into a mass.

Slides:

Advertisements

Similar presentations

Chapter 3 Stoichiometric

Advertisements

Calculations with Chemical Formulas and Equations 3.1 Molecular/Formula Weights 3.2 The Mole Concept 3.3 Mass Percentages 3.4 Elemental Analysis 3.5 Determining.

Chem 1A Chapter 3 Lecture Outlines

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

Chapter Three: STOICHIOMETRY.

Chemical Reactions Unit

Chapter 3 Stoichiometry.

The Gaseous State Chapter 5 Suggested problems to start: 19, 23-27, 29, 31, 33, 35, 39, 41, 45.

Chapter 3 Stoichiometry. Chapter 3 Table of Contents Copyright © Cengage Learning. All rights reserved Counting by Weighing 3.2 Atomic Masses 3.3.

Section 5: Empirical and Molecular Formulas

Zumdahl • Zumdahl • DeCoste

Copyright © Houghton Mifflin Company. All rights reserved. 8 | 1 Atomic Masses Balanced equations tell us the relative numbers of molecules of reactants.

Chapter 3.1 to 3.5 Student Notes Stoichiometry. Chapter 3 Table of Contents Copyright © Cengage Learning. All rights reserved Counting by Weighin3.1.

NOTES: 10.3 – Empirical and Molecular Formulas What Could It Be?

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chapter 3 Stoichiometric Atomic Masses, Mole concept, and Molar Mass (Average atomic.

Copyright©2004 by Houghton Mifflin Company. All rights reserved. 1 Chemical Composition Chapter 8.

Chapter 3: STOICHIOMETRY Stoichiometry - The study of quantities of materials consumed and produced in chemical reactions.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chapter 3 Stoichiometric Atomic Masses, Mole concept, and Molar Mass (Average atomic.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

Chapter 3 Stoichiometry. Chapter 3 Chemical Stoichiometry  Stoichiometry – The study of quantities of materials consumed and produced in chemical reactions.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 QUESTION.

Lecture #7 - (a) The Mole Concept, (b) Formula of an Unknown Chemistry 142 B James B. Callis, Instructor Autumn Quarter, 2004.

Chapter 3 Stoichiometry Stoichiometry: The study of quantities of materials consumed and produced in chemical reactions Atomic Masses: Are determined by.

William L Masterton Cecile N. Hurley Edward J. Neth University of Connecticut Chapter 3 Mass Relations.

The Mole: A measurement of Matter

You should view this in slideshow mode and make sure to enable active content if asked Copyright © Houghton Mifflin Company. All rights reserved.3–13–1.

Calculations with Chemical Formulas and Equations.

Empirical Formulas. Empirical formula tells the relative number of atoms of each element in a compound Mole concept provides a way of calculating the.

Chemical Formulas and Composition Stoichiometry د. كريم محمد الصاوى استاذ مساعد الكيمياء الفيزيائية قسم الكيمياء - جامعة القصيم.

1. What is the empirical formula of a compound

The Representative Elements: Groups 5A Through 8A

1.5 Infinite Limits. Copyright © Houghton Mifflin Company. All rights reserved Figure 1.25.

Dr. S. M. Condren Chapter 3 Calculations with Chemical Formulas and Equations.

Calculations with Chemical Formulas and Equations Chapter 3.

Chapter 3 Stoichiometric

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemical Stoichiometry Stoichiometry - The study of quantities of materials consumed.

Chapter 19(a) The Representative Elements: Groups 1A Through 4A.

Percentage Percentage means ‘out of 100’

Zumdahl Zumdahl DeCoste CHEMISTRY World of. Topic Properties of Gases.

Stoichiometry & the Mole. The Mole __________ - SI base unit used to measure the amount of a substance. A mole of anything contains __________ representative.

What Could It Be? Empirical Formulas The empirical formula is the simplest whole number ratio of the atoms of each element in a compound. Note: it is.

Chapter 3 Stoichiometric

Chapter 3 Calculations with Chemical Formulas and Equations HSTMr. Watson.

Advanced Chemistry Chapter Three Stoichiometry. 3.1 Counting by Weighing Average Mass = total mass/ number of objects For purposes of counting, objects.

Chapter 3 Stoichiometry. Chapter 3 Copyright © Cengage Learning. All rights reserved 2 Chemical Stoichiometry Stoichiometry – The study of quantities.

Entry Task: Feb 6 th - 7 th Block #2 Write the question down: Provide the percent composition of Gold III chloride You have 5 minutes!

Chapter 2(a) Atoms, Molecules, and Ions. Copyright © Houghton Mifflin Company. All rights reserved.2a–2 Figure 2.7: A cathode-ray tube. The fast- moving.

 Tin IV sulfate  Aluminum hydroxide  Oxygen gas  Iron III nitrate  Iodine.

Percent Composition and Empirical and Molecular Formula.

WHITEBOARD PRACTICE TEST REVIEW. How many molecules of ethane, C 2 H 6 are present in g C 2 H 6 ?

Chapter 1 Ingredients of Change: Functions and Models.

Chapter 5 Accumulating Change: Limits of Sums and the Definite Integral.

Chemical Stoichiometry

Calculations with Chemical Formulas and Equations

Mathematics of Chemical Formulas

Calculations with Chemical Formulas and Equations

Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter

Chapter 3 Stoichiometry.

Chemical Reactions: An Introduction (cont’d)

Covalent Bonding: Orbitals (cont’d)

10.1 What is a Mole? A mole of any substance contains Avogadro’s number of representative particles, or 6.02  1023 representative particles. The term.

Copyright © by Houghton Mifflin Company. All rights reserved.

Mass Spectrometer.

Chapter 3 Stoichiometry.

New Century, New Challenges, 1996 to the Present

What Could It Be? Finding Empirical and Molecular Formulas.

Chemical Stoichiometry

Empirical and Molecular Formulas

Combustion analysis Combustion analysis is a method used in both organic chemistry and analytical chemistry to determine the elemental composition (more.

Presentation transcript:

Chapter 3(a) Stoichiometry

Copyright © Houghton Mifflin Company. All rights reserved.3a–2 Figure 3.1: (left) A scientist injecting a sample into a mass spectrometer. (right) Schematic diagram of a mass spectrometer.

Copyright © Houghton Mifflin Company. All rights reserved.3a–3 Figure 3.2: (a) Neon gas glowing in a discharge tube. (b) "peaks" and (c) a bar graph.

Figure 3.3: Mass spectrum of natural copper.

Copyright © Houghton Mifflin Company. All rights reserved.3a–5 Figure 3.4: Proceeding clockwise from the top samples containing one mole each of copper, aluminum, iron, sulfur, iodine, and (in the center) mercury.

Copyright © Houghton Mifflin Company. All rights reserved.3a–6

Copyright © Houghton Mifflin Company. All rights reserved.3a–7 Pure aluminum.

Copyright © Houghton Mifflin Company. All rights reserved.3a–8 Aluminum alloys are used for many high- quality bicycle components, such as this chain wheel.

Copyright © Houghton Mifflin Company. All rights reserved.3a–9 Figure 3.5: A schematic diagram of the combustion device used to analyze substances for carbon and hydrogen.

Copyright © Houghton Mifflin Company. All rights reserved.3a–10 Figure 3.6: Examples of substances whose empirical and molecular formulas differ. Notice that molecular formula = (empirical formula) n, where n is an integer.

Copyright © Houghton Mifflin Company. All rights reserved.3a–11 Figure 3.7: The two forms of dichloroethane.