Examples: Al2(SO4)3 Al 2 x 27.0 = S 3 x 32.1 = O 12 x 16.0 = NiSO3 6H2O Ni 1 x 58.7 = S 1 x 32.1 = O 3 x 16.0 = H2O 6 x 18.0 =
|
|
- Jodie Hardy
- 5 years ago
- Views:
Transcription
1 Moles Conversion factor: a fraction, equal to one, used to change one unit into another. A conversion factor is formed from an equality! Example: 12 inches = 1 foot 12 in or 1 ft 1 ft 12 in Dimensional Analysis: a problem-solving method using conversion factors also known as factor-label method, picket fence method, or ladder method. Examples: $ nickels $25 4 quarters 5 nickels = 500 nickels $1 1 quarter miles inches 2.5 miles 5280 ft 12 in = in 1 mile 1 ft cm km 125 cm 1 m 1 km = km 100 cm 1000 m m/s miles/hr (mph) 9.76 m 1 km 0.62 miles 60 s 60 min = 21.6 miles s 1000 m 1 km 1 min 1 hr hr Formula Mass: the sum of the average atomic masses of all the atoms present in a chemical formula. There are synonyms based upon the type of compound! Ionic compounds formula mass Molecular compounds molecular mass Elements atomic mass Examples: Al2(SO4)3 Al 2 x 27.0 = S 3 x 32.1 = O 12 x 16.0 = NiSO3 6H2O Ni 1 x 58.7 = S 1 x 32.1 = O 3 x 16.0 = H2O 6 x 18.0 = C6H12O6 C 6 x 12.0 = H 12 x 1.0 = O 6 x 16.0 = amu amu amu Chip Shea 1 3/16/2019
2 Percent composition: the percent, by mass, of each element in a compound. Example: Find the % composition of Al2(SO4)3 (see work for formula mass above!) Al 54.0 amu x 100% = % Al amu S 96.3 amu x 100% = % S amu O amu x 100% = % O amu 100.0% Find the % composition of NiSO3 6H2O (see work for formula mass above!) Ni 58.7 amu x 100% = % Ni amu S 32.1 amu x 100% = % S amu O 48.0 amu x 100% = % O amu H2O amu x 100% = % H2O amu 100.0% Mole conversions Avogadro s Hypothesis: Equal volumes of gases at the same temperature and pressure have equal numbers of particles. Avogadro s number: x This is the number of particles (atoms, molecules, formula units, ions) in one mole of a substance. Mole: the amount of a substance that contains as many particles as are in 12.00g of carbon-12. Molar mass: the mass in grams of one mole of a substance (Equal to the formula mass in grams instead of amu) Molar volume: the volume occupied by one mole of a gas at STP (0 C, 1 atm) = 22.4 L. Conversions with moles: since the mole is a number, it can be used to relate mass (or volume) with the large number of particles that make up that mass (or volume) Particles to moles: particles = moles 6.02 x Example: Convert 4.52 x atoms Au to moles 4.52 x particles Au = moles Au 6.02 x Chip Shea 2 3/16/2019
3 Moles to particles moles 6.02 x = particles Example: Convert 10.5 moles Au to particles 10.5 moles Au 6.02 x = particles Au Grams to moles grams = moles grams Example: Convert 245.7g Au to moles 245.7g Au = moles Au g Au Moles to Grams moles grams = grams Example: Convert moles Au to grams moles Au g g Au s Au Liters to moles liters = moles 22.4 L Example: Convert 495L O2 to liters 495L O2 = moles O2 22.4L O2 Moles to liters moles 22.4 L = liters Example: Convert 10.0 moles O2 to liters 10.0 moles O L = L O2 Particles to grams particles grams = grams 6.02 x Example: Convert 4.52 x particles Au to grams 4.52 x particles g Au = grams Au 6.02 x Chip Shea 3 3/16/2019
4 Grams to particles grams 6.02 x = particles grams Example: Convert 2259g Au to particles 2259g Au 6.02 x = particles Au g Au Determining Empirical and Molecular Formulas Empirical Formula: the simplest formula with the smallest whole number ratio of elements. (Remember: an ionic compound is an empirical formula (f.u.!), but a molecular compound may not be!) Example: CH Molecular formula: the actual formula, often a multiple of the empirical formula. Example: C6H6 (note: NOT an empirical formula!) Calculating Empirical Formulas An empirical formula may be calculated from mass data or percent composition data. Step 1: Convert grams to moles Step 2: Divide each by the smallest number (Step 3: Rationalize to 1 if necessary!) Step 4: Write the empirical formula Examples: Calculate the empirical formula of 2.50g of a compound containing 0.90g Ca and 1.60g Cl. Ca 0.90g Ca = mol Ca 40.1g Ca Cl 1.60g Cl = mol Cl 35.5g Cl Ca mol = Cl mol = CaCl2. No Step 3! Chip Shea 4 3/16/2019
5 Calculate the empirical formula of 13.69g of a compound containing 2.16g of aluminum, 3.85g of sulfur, and 7.68g of oxygen. Al 2.16g Al = mol Al 27.0g Al S 3.85g S = mol S 32.1g S O 7.68g O = mol O 16.0g O Al mol = S mol = Go to Step 3! O mol = Step 3: Gotta do it! Al = x = S = x = O = x = which simplifies to What is the empirical formula of a compound that is 66.0% Ca and 34.0% P? Ca 66.0g Ca = mol Ca 40.1g Ca P 34.0g Cl = mol P 31.0g P Steps 2 and 3: divide each by the smallest number of moles and rationalize Ca mol = x = The empirical formula is P mol = x = Chip Shea 5 3/16/2019
6 Determining Molecular Formulas: A molecular formula may be calculated from an empirical formula and molecular mass. The molecular formula is a whole-number multiple of the empirical formula. Step 1: Convert grams to moles Step 2: Divide each by the smallest number (Step 3: Rationalize to 1 if necessary!) Step 4: Write the empirical formula Step 5: Find the mass of the empirical formula Step 6: Step 7: Divide the molecular mass by the empirical mass Multiply each element in the empirical formula the result of Step 6 Example: Calculate the molecular formula of a compound whose molar mass is 150. g/mol and has a composition of 40.0% C, 6.67% H, and 53.3% O C 40.0g C = 3.33 mol C 12.0 g C H 6.67g H = 6.67 mol H 1.0 g H O 53.3g O = 3.33 mol O 16.0 g O Step 2, 4, and 5: divide each by the smallest number of moles C 3.33 mol = H 6.67 mol = O 3.33 mol = CH2O. The empirical formula mass is 30.0 g/mol. Step 6 and g/mol = g/mol CH2O. The molecular formula is C5H10O5. Chip Shea 6 3/16/2019
7 Determining the Formula of a Hydrate The formula of a hydrated ionic compound may be found using the same basic steps. Example: A g sample of hydrated BaI2 is heated. The anhydrous mass is 9.520g. What is the formula for the hydrate? BaI g BaI2 = mol BaI g BaI2 H2O 0.887g H2O = mol H2O 18.0g H2O BaI mol = 1 The formula for the hydrate is H2O mol = BaI2 2H2O. Example: A sample of hydrated MgSO4 is found to be 48.9% anhydrous salt. What is the formula for the hydrate? MgSO4 48.9g MgSO4 = mol MgSO g MgSO4 H2O 51.1g H2O = mol H2O 18.0g H2O MgSO4 mol = The formula for the hydrate is H2O mol = Chip Shea 7 3/16/2019
CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units
CHAPTER 11 The Mole 11.1 The Mole: Measurement of Matter Matter is measured in one of three ways: (How many?) Mole SI unit that measures the amount of a substance 6.02 x 10 particles of that substance.
More informationChapter 10 CHEMICAL QUANTITIES The MOLE
Chapter 10 CHEMICAL QUANTITIES The MOLE Avogadro s Hypothesis Equal volumes of gases (@ same T and p) have the same # molecules. The number of 12 C atoms in 12.00 grams of carbon is called Avogadro s Number
More informationName Class Date = + 1 S atom 32.1 amu +
Molar Mass 10. What is the atomic mass of an element? 11. Circle the letter of the phrase that completes this sentence correctly. The atomic masses of all elements a. are the same. b. are based on the
More information6.02 x 1023 CHAPTER 10. Mole. Avogadro s Number. Chemical Quantities The Mole: A Measurement of Matter Matter is measured in one of three ways:
Chapter 10 Notes CHAPTER 10 10.1 The Mole: A Measurement of Matter Matter is measured in one of three ways: Chemical Quantities Mole SI unit that measures the amount of a substance A mole of a substance
More informationPart 01 - Notes: The Mole and Its Calculations
Part 01 - Notes: The Mole and Its Calculations Objectives: Identify, define, and explain: mole, Avogadro s number, representative particle, gram atomic mass, gram molecular mass, gram formula mass, molar
More information23 carbon atoms The number is known as Avogadro s d Number.
THE MOLE (a counting unit).again! i A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon
More informationChapter 10 Chemical Quantities
Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter OBJECTIVES: Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance.
More informationChapter 10. How you measure how much? Moles. Representative particles. Conversion factors. Chemical Quantities or
Chapter 10 Chemical Quantities or 1 2 How you measure how much? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters. We count pieces in MOLES.
More informationUnit 6: Chemical Quantities. Understanding The Mole
Unit 6: Chemical Quantities Understanding The Mole 1 How do We Typically Measure Matter? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters.
More informationFinding Formulas. using mass information about a compound to find its formula
Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula
More informationAverage Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom.
Average Atomic Mass Since atoms are so small and the mass of individual atoms is also very small, it is not useful to use the units of grams or kilogram. A new unit called the atomic mass unit (amu) was
More informationMolar Conversions & Calculations
Molar Conversions & Calculations Ch. 11 The Mole 1 A. What is the Mole? A counting number (like a dozen) Avogadro s number (n) 1 mol = 6.02 x 10 23 items A VERY large amount!!!! 2 A. What is the Mole?
More informationHydrates, Percent Composition, and Empirical and Molecular Formulas
Hydrates, Percent Composition, and Empirical and Molecular Formulas Hydrates Hydrates are ionic cmpds (salts) that have water molecules bound to their ions. Examples: CuSO 4 5H 2 O Fe(NO 3 ) 3 9H 2 O CoCl
More information6 atomic # C symbol Carbon name of element atomic mass. o Examples: # 1 mol C = g # 1 mol O = g # 1 mol H = 1.
7.1 AVOGADRO S NUMBER AND MOLAR CONVERSIONS CHEMISTRY NOTES Identify the mole as the unit used to count particles, whether atoms, ions, or molecules. Use Avogadro s number to convert between amount in
More informationWhat is a Representative Particle
Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What
More informationCHAPTER 9 AVOGADRO S NUMBER
CHAPTER 9 AVOGADRO S NUMBER Just like we count in dozens, gross or ream, we count atoms in groups because of their minute sizes. Like in finding the number of atoms in12.01g of C, Experiments have shown
More informationChemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
More informationWorksheet 1: REPRESENTATIVE PARTICLES
Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is
More informationTHE MOLE (a counting unit)
MOLE AND MATH THE MOLE (a counting unit) A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mole eggs = 6.022 x 10 23 eggs 1 dozen
More informationName Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages )
10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate
More information1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq)
1) Write the reaction for Calcium and nitrogen reacting 3) What element on the periodic table is the largest? 3)Name these a) H2S (aq) b) HNO 3 (aq) Stoichiometry: mathematical relationships in formulas
More informationAtoms, Ions and Molecules Calculations
Atoms, Ions and Molecules Calculations 1. How do you calculate the atomic mass of an element? Atomic Mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope2)(mass of isotope 2)
More information90.14 g/mol x g/mol. Molecular formula: molecular formula 2 empirical formula 2 C OH C O H
Whole-number multiple: M x M actual compound C2OH5 90.14 g/mol x 45.07 g/mol 90.14 g/mol x 45.07 g/mol 2 Molecular formula: molecular formula 2 empirical formula 2 C OH 2 5 C O H 4 2 10 Check Your Solution
More informationMOLECULAR FORMULA AND EMPIRICAL FORMULA
MOLECULAR FORMULA AND EMPIRICAL FORMULA Molecular Formula is a formula indicating the actual number of atoms of each element making up a molecule. The molecular formula must accurately state the exact
More informationMeasuring matter 11.1
The Mole Ch 11 Measuring matter 11.1 Review 11.1 Vocabulary o molecule: two or more atoms that covalently bond together to form a unit New mole Avogadro s number Main Idea - Chemists use the mole to count
More informationA TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH Chapter Outline Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly.
More informationChapter 8. The Mole Concept
Chapter 8 The Mole Concept Chapter 9 2 Avogadro s Number Avogadro s number (symbol N) is the number of atoms in 12.01 grams of carbon. Its numerical value is 6.02 10 23. Therefore, a 12.01 g sample of
More informationCHEMISTRY MOLES PACKET 2017 NAME: PER:
CHEMISTRY MOLES PACKET 2017 NAME: PER: We have learned that a mole can be a certain mass of a substance and a certain number of particles. A mole can also be a measure of volume when we are talking about
More informationUNIT 6 STOICHIOMETRY 1
UNIT 6 STOICHIOMETRY 1 There are three ways to measure matter count (number of particles representative particles) mass (grams) volume (Liters) Mole unit for amt of matter relating these quantities 2 Representative
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change Table Of Contents Section.1 Measuring Matter Section.2 Mass and the Mole Section.3 Moles of Compounds Chapter : Section.4 Empirical and Molecular Formulas Section.5 Formulas
More information10.2 Mole-Mass and Mole- Volume Relationships. Chapter 10 Chemical Quantities. Volume Relationships The Mole: A Measurement of Matter
Chapter 10 Chemical Quantities 101 The Mole: A Measurement of Matter 102 Mole-Mass and Mole- 103 Percent Composition and Chemical Formulas 1 http://wwwbrightstormcom/science/chem istry/chemical-reactions/molar-mass/
More informationWhat is a Mole? An Animal or What?
Unit 7: (Chapter 9) Chemical Quantities What is a Mole? An Animal or What? Section 9.1 The Mole: A Measurement of Matter Describe how Avogadro s number is related to a mole of any substance. Calculate
More informationUnit 6 Chemical Analysis. Chapter 8
Unit 6 Chemical Analysis Chapter 8 Objectives 39 Perform calculations using the mole to calculate the molar mass 40 Perform calculations using the mole to convert between grams, number of particles, volume,
More informationUnit 6: Mole Assignment Packet Period:
Unit 6: Mole Assignment Packet Name: Period: A1: Mole Conversions 1. Identify the representative particle in each of the following: (atom, molecule, formula unit) a. CuSO 4 b. H 2 O c. NaCl d. Zn e. Cu
More informationAtoms, Molecules, and the Mole
The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting
More informationChapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
More informationLecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
More informationChemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
More informationChapter 5. Mole Concept. Table of Contents
Mole Concept Table of Contents 1. Mole 2. Avagadro s Number 3. Molar Mass 4. Molar Volume of Gases 5. The Mole Concept Calculations 6. Several Types of Problems Mole Concept Warm up List common units used
More informationFormula Mass. not all compounds are molecular formula mass calculated exactly the same way as molecular mass. Solid structure of NaCl
Molecular Mass Molecular Mass synonymous with molar mass and molecular weight is the sum of the atomic masses of all the atoms in a molecule the mass in grams of one mole of a compound Formula Mass not
More informationB. stoichiometry using balanced chemical equations to obtain info. C. mole-to-r.p. and r.p.-to-mole example problems:
Chem. Ch. 10 ~ THE MOLE NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 10.1 Notes I. Measuring Matter A. SI unit of chemical quantity = the mole (abbreviated
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
More informationChemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9
Chapter 9 Chemical Calculations: The Mole concept and Chemical Formula This material is not included in Midterm 1 1 Law of Definite Proportions (John Dalton) Chapter 9 A given compound always contains
More informationHonors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?
Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula
More informationCHEMISTRY Matter and Change. Chapter 10: The Mole
CHEMISTRY Matter and Change Chapter 10: The Mole CHAPTER 10 Table Of Contents Section 10.1 Measuring Matter Section 10.2 Mass and the Mole Section 10.3 Moles of Compounds Section 10.4 Empirical and Molecular
More informationChapter 7 Chemical Quantities. 7.1 A Mole. Samples of One Mole Quantities. A Mole of Molecules
Chapter 7 Chemical Quantities 7.1 A Mole 7.1 The Mole 7.2 Molar Mass 7.3 Calculations Using Molar Mass 7.4 Percent Composition and Empirical Formulas A mole contains 6.02 x 10 23 particles (atoms, ions,
More informationName Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages )
Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches
More informationNOTES: 10.3 Empirical and Molecular Formulas
NOTES: 10.3 Empirical and Molecular Formulas What Could It Be? Empirical Formulas Indicate the lowest whole number ratio of the atoms in a compound: 1) Determine moles of each element present in the compound
More informationUnit 5. Chemical Composition
Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles
More information9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses
9/14/1 Chemistry Second Edition Julia Burdge Stoichiometry: Ratios of Combination Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Stoichiometry: Ratios
More informationEmpirical Formulas and Molecular Formulas. Ch 3.5
Empirical Formulas and Molecular Formulas Ch 3.5 Empirical Formulas are the simplest (lowest) whole number ratio of atoms in a molecule or ionic compound Molecular Formulas are true formulas. For example:
More informationNotes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl -
Name I. Essential Terminology Notes: The Mole Period Chemistry Pre-AP The smallest particle of an element is the atom. Diatomic elements (like O 2 ) are the main exception to this. We say that diatomic
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationTHE MOLE. Chapter 10 Who is that Little Guy with Squinty Eyes?
THE MOLE Chapter 10 Who is that Little Guy with Squinty Eyes? THE MOLE NO, Not this mole, this guy has nothing to do with Chemistry! THINGS YOU SHOULD KNOW Chapter 10 Section 1 and 2 Know what a mole is.
More informationTest Review Unit 3_1_Amount of substance Mole, molar mass and Avogadro s number test
Test Review Unit 3_1_Amount of substance Mole, molar mass and Avogadro s number test (Information extracted from file FQ3eso_t3_1_Amount of substance ) The Mole Read and then answer the Multiple choice
More informationQ: How long would it take to spend a mole of $1 coins if they were being spent at a rate of 1 billion per second? A:
: The Mole- 6.02 x 10 23 ODE TO A MOLE I find that my heart beat goes out of control Just thinking how useful to man is the mole! So perfectly compact. What could be neater? Only occupying twenty-two and
More informationTHE MOLE (a counting unit).again!
Name: Period: Date: THE MOLE (a counting unit).again! A mole represents a, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon
More informationComposition and formulae. Of moles and men
Composition and formulae Of moles and men Learning objectives Count atoms in formula Define the mole Determine numbers of atoms or molecules in molar quantities Determine molar mass from chemical formula
More informationChemistry I Notes Unit 7: Stoichiometry Notes
Chemistry I Notes Unit 7: Stoichiometry Notes Stoichiometry Relating Mass to Numbers of Atoms The Mole The mole is the SI unit for amount of substance. A mole (abbreviated mol) is the amount of a substance
More informationGeneral Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
More informationRight Side NOTES ONLY
Ch 5.11 & Ch 6 Title and Highlight Right Side NOTES ONLY TN Ch 5.11 Topic: EQ: Date Write Question out (left side of red line) and answer it (Highlight answer) based on from what you read. Write out the
More informationVideos 1. Crash course Partial pressures: YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion:
Videos 1. Crash course Partial pressures: https://youtu.be/jbqtqcunyza?list=pl8dpuualjxtphzz YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion: https://youtu.be/tlrzafu_9kg?list=pl8dpuualjxtph zzyuwy6fyeax9mqq8ogr
More informationChapter 3. Mass Relations in Chemistry; Stoichiometry
Chapter 3 Mass Relations in Chemistry; Stoichiometry Copyright 2001 by Harcourt, Inc. All rights reserved. Requests for permission to make copies of any part of the work should be mailed to the following
More informationMany common quantities have names that are used to describe them: Six of something are a half-dozen, and twelve are a dozen.
THE MOLE THE MOLE Many common quantities have names that are used to describe them: Two of something are called a pair. Three of something are called a trio. Six of something are a half-dozen, and twelve
More informationب 3 18 قسم الكيمياء مصطفي عيد
memxtd@yahoo.com m.moustapha@sau.edu.sa 0115888078 ب 3 18 قسم الكيمياء مصطفي عيد The Atom Nucleus Electron Shell or Orbit The Atom. What are the 3 major parts of an atom? Proton Neutron Electron Stoichiometry
More informationChemical Reactions, Chemical Equations, and Stoichiometry. Brown, LeMay Ch 3 AP Chemistry
Chemical Reactions, Chemical Equations, and Stoichiometry Brown, LeMay Ch 3 AP Chemistry 1 3.: Types of reactions http://web.fuhsd.org/kavita_gupta/july.html 3.3: Atomic, Molecular & Formula Weights Atomic
More informationNotes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas
Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas In Chemistry, a Mole is: the unit that measures the amount of a substance - equals 6.022 x 10 23 particles of
More informationStoichiometry. Please take out your notebooks
Stoichiometry Please take out your notebooks Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.
More informationChapter 11. Molecular Composition of Gases
Chapter 11 Molecular Composition of Gases PART 1 Volume-Mass Relationships of Gases Avogadro s Law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Recall
More informationDetermining Chemical Formulas
SECTION 7.4 Determining Chemical Formulas When scientists discover or produce a new compound, they analyze it to learn its composition. Often what they measure is the percentage composition of the substance.
More informationTopics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas
Composition Stoichiometry Composition Stoichiometry NOTES 1 So far, we ve studied the products of a chemical reaction in terms of their identity. Stoichiometry is a branch of chemistry dealing with quantities.
More informationUNIT 9. Stoichiometry
UNIT 9 Stoichiometry FORMULA MASS Atomic Mass Unit (u): unit of mass for measuring atoms. (1 u = 1/12 th the mass of a carbon 12 atom) FORMULA MASS FORMULA MASS Example 2: Find the mass of one molecule
More informationChapter No. 1 BASIC CONCEPTS Short Question With Answer Q.1 Calculate the grams atoms in 0.4 gm of potassium. Gram atoms of potassium = = = 0.01 grams atoms Q.2 23 grams of sodium and 238 gram of uranium
More informationAP Chemistry. Mole, Molecular Formula Review One Mole = o This is Avogadro s number. Molar Mass: The mass of one mole of a substance in grams.
AP Chemistry Ms Ye Name Date Block Mole, Review One Mole = o This is Avogadro s number Molar Mass: The mass of one mole of a substance in grams Percent Composition: Identifies the elements present in a
More informationMath of Formulas. Chapter 10
Math of Formulas Chapter 10 Macro vs. Micro Chemistry has two worlds: The macroscopic world = what a scien>st can see and weigh The microscopic world = the atomic level, filled with >ny molecules Chemists
More informationDescription Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)
Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular
More informationChapter 8. Chemical Composition
Chapter 8 Chemical Composition Section 8.1 Counting by Weighing Objects do not need to have identical masses to be counted by weighing. All we need to know is the average mass of the objects. To count
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationUnit 5 Percent Composition, Empirical Formulas, and Reactions
Chemistry 1 West Linn High School Unit 5 Packet and Goals Name: Period: Unit 5 Percent Composition, Empirical Formulas, and Reactions Unit Goals: As you work through this unit, you should be able to: 1.
More information4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia
Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate
More informationPercent Composition, Empirical Formula, Molecular Formula, Hydrates
Name: Percent Composition, Empirical Formula, Molecular Formula, Hydrates Essential Questions How can one explain the structure, properties, and interactions of matter? How do substances combine or react
More informationDo Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet
Do Now Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet All the math Molar Mass the mass of one mole of any substance, reported in grams (gram atomic mass)
More information6.02 X Memorize this Number
Honors Chemistry - Unit 6 Chapters 3 & 7 The Mole Math with Chemical Formulas Voc. Assignment Due: Quiz Date(s): TBA Problem Set (UT Quest) Due: Test Date: Unit 6 Packet - Page 1 of 14 **VOCABULARY Assignment**
More informationStoichiometry Dr. M. E. Bridge
Preliminary Chemistry Course Stoichiometry Dr. M. E. Bridge What is stoichiometry? The meaning of the word: The word stoichiometry comes from two Greek words: stoichon(meaning element ) and metron(meaning
More informationUnit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
More informationMolecular vs. Empirical Formula Chemistry H 2 O H 2 O 2. NaCl
Molecular vs Empirical Formula Chemistry Name Block Read the information below and then answer the questions that follow Definitions: Molecular formula the total number of atoms of each element in a compound
More informationTopic 7: The Mole Concept Relating Mass to Numbers of Atoms
Topic 7: The Mole Concept Relating Mass to Numbers of Atoms (Chapter 3 in Modern Chemistry beginning on p.82) In order to understand the quantitative parts of chemistry, there are three very important
More informationJOHN BURKE HIGH SCHOOL
JOHN BURKE HIGH SCHOOL Chemistry 2202 Midterm Examination January, 2013 Instructions: Part I: Multiple Choice: Choose the best answer to each item. Place all answers on the Answer Sheet provided. 40 marks
More informationThe Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
More informationLesson 01: Atomic Masses and Avogadro s Hypothesis. 01 Counting Atoms and Molecules
Chemistry 11, Mole Concept, Unit 04 1 Lesson 01: Atomic Masses and Avogadro s Hypothesis 01 Counting Atoms and Molecules The chemical changes we observe always involve a certain number of atoms that rearrange
More informationContents. Content Guidance. Questions & Answers. Getting the most from this book... 4 About this book... 5
Contents Getting the most from this book... 4 About this book.... 5 Content Guidance Atomic structure......................................... 6 Amount of substance....................................
More informationThe quantities in formulas and in chemical reactions can be counted singly or in groups, such as the mole.
CHEM110 Week 4 Notes Mass relationships in Chemical Formulas Page 1 of 5 Recall the Law of Definite Proportions. All samples of a compound have the same atomic composition (or) all samples have the same
More informationLesson 13: Ionic Equations & Intro to the Mole with Conversions
NOTES Name: Date: Class: Lesson 13: Ionic Equations & Intro to the Mole with Conversions Box 1: Balance: 1. Mg + O2 MgO 2. KClO3 KCl + O2 3. C2H6 + O2 CO2 + H2O Write and balance the equation that represents
More informationCHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet
CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is
More informationAll Roads Lead to the Mole
CHEMICAL QUANTITIES Chemical Quantities Dozen: Baker as Mole: Chemist Measuring doughnuts: o 1 dozen = 1 doughnuts (count) o 1 dozen = 500 g doughnuts (mass) o 1 dozen = 1 box doughnuts (volume) All Roads
More informationGermanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets
Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For
More informationUsing the Mole to Calculate % Composition, Empirical Formulas and Molecular Formulas
Using the Mole to Calculate % Composition, Empirical Formulas and Molecular Formulas Law of Definite Proportions Compounds have constant composition This means that the ratios by mass of the elements chemically
More informationSolutions to the Extra Problems for Chapter 8
Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.
More information