Ch 3. Chemical Reactions and Reaction Stoichiometry
|
|
- Stella Barrett
- 5 years ago
- Views:
Transcription
1 Ch 3 Chemical Reactions and Reaction Stoichiometry
2 { { Chemical Reactions involve the rearrangement of atoms. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Reactant Products s Law of Conservation of Mass states that during a chemical reaction, atoms are neither created or destroyed. They are rearranged. Mass of reactants = Mass of products CH 4 Subscript say how many of atom before the number Coefficient say how many of molecule, atom, or moles 2 O 2
3 A g sample of Mg is completely burned in g of O 2 (g). The only product is MgO. After the reaction the mass of unreacted O 2 (g) is g. What mass of MgO is formed?
4 CH 4 (g) Physical state of substance g = gas l = liquid s = solid aq = aqueous (dissolved in water)
5 Balancing chemical equations Know reactants, products, and physical state Know correct formulas, write as an unbalanced equation Conserve atoms by placing coefficients in front of the chemicals until there is the same number of each kind of atom on opposite sides of
6 C 3 H 8 (g) + O 2 (g) CO 2 (g) + H 2 O (g) (NH 4 ) 2 Cr 2 O 7 (s) Cr 2 O 3 (s) + N 2 (g) + H 2 O (g) Ag 2 O (s) Ag (s) + O 2 (g) NH 3 (g) + O 2 (g) NO (g) + H 2 O (g)
7 Simple Patterns of Chemical Reactivity Combination (synthesis) A + B C Decomposition Combustion C A + B C x H y O z + O 2 CO 2 + H 2 O Single Replacement (single displacement) A + XY X + AY Double Replacement (double displacement) AB + XY AY + XB
8 Formula weight (FW) is the sum of atomic weights in amu of the atoms in the chemical formula. Molecular weight (MW) is the same as the formula weight for molecules. Molar mass is the sum of atomic weights in grams for all atoms in the chemical formula.
9 Mole is the number of atoms in exactly g of carbon. A mole of any substance is the amount that contains the same number of elementary entities as there are in 12 C atoms in exactly g 12 C. That number is Avogadro s Constant = 6.02 x The mass of 1 mole of atoms is the molar mass. It is the number of atoms (6.02 x atoms) and is equal to the mass in amu expressed in grams. A mass of iron is described as being 2.35 mol Fe. How many Fe atoms are present? How many moles of Mg are present in a sample containing 1.00 x Mg atoms? What is the mass of the sample?
10 Potassium 40 K is one of the few naturally occurring radioactive isotopes of low atomic number. It s % abundance is 0.012%. How many 40 K atoms do you ingest drinking one cup of whole milk containing 371 mg K?
11 Gold (Au) occurs in seawater to the extent of 0.15 mg / ton of seawater. How many Au atoms are present in a glassful (300 g) of seawater? (1 ton = 2000 lbs) (1 lb = g)
12 How many ions form when 0.1 mg MgCl 2 dissolves? Halothane, C 2 HBrClF 3, is an anesthetic. What is the amount of F in moles, in 75 ml sample of halothane? (d = g / ml )
13 Chloral hydrate (C 2 H 3 Cl 3 O 2 ), is a drug formerly used as a sedative and hypnotic. It is the compound used to make Mickey Finns in detective stories. a. Calculate u. b. What amount (in moles) of C 2 H 3 Cl 3 O 2 molecules are in 500.0g? c. What is the mass in grams of 2.0 x 10-2 mol? d. What number of Cl atoms are in 5.0 g? e. What mass of C 2 H 3 Cl 3 O 2 would contain 1.0 g Cl? f. What is the mass of exactly 500 molecules?
14 For the compound Ge[S(CH 2 ) 4 CH 3 ] 4 1. Total number of atoms in 1 molecule? 2. Ratio by number of C atoms to H atoms? 3. Ratio by mass of Ge to S? 4. Number of S in 1 mol of compound? 5. Number of C atoms in g of compound?
15 % Composition by element (m) % comp of element by m Total mass of element = ( Mass of compound ( 100 The formula for penicillin is C 14 H 20 N 2 SO 4. Find the % composition for each element.
16 A hydrate compound is one which has water attached to the molecule. An anhydrous compound is one which has no water attached. It is dry.
17 % H 2 O = ( Total mass of water Mass of hydrate compound ( 100 Find the % H 2 O in CuSO 4. 5H 2 O.
18 Formula is the smallest unit of a compound. Empirical formula is the simplest formula you can write with the types and number of atoms reflected in the formula. Molecular formula is the actual molecule formula and is equal to or some multiple of the empirical formula. (formula and molecular formula are basically the same)
19 Steps for establishing formula from % composition. 1. List mass of elements (as a of %, use mass in 100 grams) 2. Convert mass of element to moles 3. Write a tentative formula using mole values as subscripts 4. Attempt to convert subscripts to smallest whole numbers by dividing mole values by the smallest mole value 5. If decimal numbers, multiple by a small whole number to obtain empirical formula 6. To find molecular formula, compare empirical formula mass to molar mass of compound. Multiple subscripts by multiplication factor.
20 Dibutyl Succinate is an insect repellant used against household ants and roaches. It s composition is % C, 9.63 % H, and % O. It s experimentally determined molar mass is 230 u. What is the empirical formula and molecular formula?
21 Caffeine, a stimulant found in coffee, contains 49.5 % C, 5.15 % H, 28.9 % N, and 16.5 % O by mass and has a molar mass of 195 g/ mol. Determine the empirical formula and molecular formula.
22 Adipic acid is an organic compound composed of % C, % O and the rest hydrogen. If the molar mass of adipic acid is g/ mol,what are the empirical and molecular formulas.
23 Monosodium glutamate (MSG), a flavor enhancer in certain foods, contains % C, 4.77 % H, % O, 8.29 % N, and % Na and has a molar mass of 169 g/ mol Determine the empirical formula and the molecular formula.
24 C x H y O z + _ O 2 _ CO 2 + _ H 2 O Combustion analysis is used to find the empirical formula of a CH or CHO molecule. It is allowed to go through combustion to produce CO 2 + H 2 O. Analyze the amount of C + H then compare the mass to the original mass to determine the amount of O that was originally present.
25 Vitamin C is essential for prevention of Scurvy. Combustion analysis of a g sample of this C, H, O compound yields g CO 2, and g H 2 O. What is the empirical formula?
26 Stoichiometry Making mass relations in chemical reactions Balance equation Work in moles Set up mole ratio X mole Y mole X = Y 2 A + B 3 C + 4 D 2 3 Use moles and coefficients of the known to determine moles of the unknown! Use limiting reagent (reactant) to determine the moles of products. This is a chemical that is used up, thus limiting the amount of product that can be made. Convert back to grams if needed moles = grams Molar mass
27 Fire in a jug. Determine the exact amount of ethanol required to combust with the amount of oxygen in the jug. C 2 H 6 O (g) + O 2 (g) CO 2 (g) + H 2 O (g) Knowns: 20 L jug Density of air 1.15 g / L Air is ~ 20% O 2 Density of C 2 H 6 O 0.80 g / ml
28 Determine the mass of sodium bicarbonate needed to react exactly with 1 g of citric acid, and the mass of CO 2 (g) released. + NaHCO 3 C 6 H 5 O 7 Na 3 + H 2 CO 3? grams citric acid H 2 CO 3 H 2 O + CO m 1 gram? grams
29 An alloy used in fabricating aircraft structures consists of 93.7 % Al and 6.3 % Cu by mass. The alloy has a density of 2.85 g / cm 3. A cm 3 piece of alloy reacts with an excess of HCl. If one assumes that all of the Al reacts, but none of the Cu reacts, what mass of H 2 (g) is obtained?
30 Solid LiOH is used in space vehicles to remove exhaled CO 2 (g) from the living environment. What mass of CO 2 (g) can be removed by 1.00 Kg of LiOH?
31 How many moles of H 2 O (g) are produced by burning 2.72 mole of H 2 (g) in an excess of O 2 (g)?
32 Limiting Reagent is the reactant which is completely consumed during a chemical reaction, therefore limits the amount of product formed. What mass of PCl 3 (L) is formed when 125 g of P 4 (L) reacts with 325 g Cl 2 (g)? P 4 (L) + Cl 2 (g) PCl 3 (L)
33 NaHCO 3 (s) + HC 2 H 3 O 2 (aq) NaC 2 H 3 O 2 (aq) + CO 2 (g) + H 2 O (L) Stoichiometry Balloon Race Flask Amount of 2M HC 2 H 3 O 2 10 ml 10 ml 10 ml 10 ml 10 ml 10 ml Moles of HC 2 H 3 O 2 Mass of NaHCO g 1.00 g 1.50 g 2.00 g 2.50 g 3.00 g Moles of NaHCO 3 Moles of CO 2 Limiting reactant
34 Theoretical Yield is the amount of product formed when all of the limiting reactant is used up. Actual Yield is the amount of product actually formed. Rarely does a reaction go to completion. Percent Yield = ( Actual Yield ) 100 Theoretical Yield Billions of pounds of urea CO(NH 2 ) 2 are produced annually for fertilizer. 1 mol 2 NH 3 + CO 2 CO(NH 2 ) 2 + H 2 O If 47.7 g urea forms per mol of CO 2 that reacts, what is the theoretical yield, actual yield, and percent yield?
35 Parts per million (ppm) Measured in mg / L
Chapter 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 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 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 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 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 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 informationChapter 3 Stoichiometry
Chapter 3 Sep 22 1:45 PM Average atomic mass: The weighted average of all isotopes of a specific element. Takes into consideration abundance of each isotope. (% x M 1 ) + (% x M 2 ) +... Sep 22 1:45 PM
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 informatione) How many atoms of nitrogen are in 1.2 g aspartame? #11 HC 4 of 4
Ch. 3 Honors Chem HW #11 HC 1 of 4 A2) An element is a mixture of two isotopes. One isotope of the element has an atomic mass of 34.96885 amu and has a relative abundance of 75.53%. The other isotope has
More informationBalancing Chemical Reactions. CHAPTER 3: Quantitative Relationships in Chemical Reactions. Zn + HCl ZnCl 2 + H 2. reactant atoms product atoms
CHAPTER 3: Quantitative Relationships in Chemical Reactions Stoichiometry: Greek for measure elements Stoichiometry involves calculations based on chemical formulas and chemical equations (reactions) quantitative.
More informationMass Relationship in Chemical Reaction
CHEMISTRY - DMCU 1233 Fakulti Kejuruteraan Mekanikal, UTeM Lecturer: IMRAN SYAKIR BIN MOHAMAD MOHD HAIZAL BIN MOHD HUSIN NONA MERRY MERPATI MITAN Mass Relationship in Chemical Reaction Chapter 3 1 Atomic
More informationChapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
More informationCHEM 120: Introduction to Inorganic Chemistry. Chapters Covered and Test dates. The mole concept and atoms. Avogadro s number
CHEM 120: Introduction to Inorganic Chemistry Instructor: Upali Siriwardane (Ph.D., Ohio State University) CTH 311, Tele: 257-4941, e-mail: upali@chem.latech.edu Office hours: 10:00 to 12:00 Tu & Th ;
More informationStoichiometry Ratios of Combination
Chapter 3 Stoichiometry Ratios of Combination Dr. A. Al-Saadi 1 Preview Concepts of atomic mass, molecular mass, mole, molar mass, and percent compositions. Balancing chemical equations. Stoichiometric
More informationAP Chemistry Chapter 3. Stoichiometry
AP Chemistry Chapter 3 Stoichiometry Stoichiometry Is the study of the quantities of substances consumed and produced in chemical reactions Derived from the Greek words stoicheion meaning element and metron
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationFormulas and Models 1
Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in
More informationCHAPTER 3: PART 2 8/9/2015. A chemical change (a chemical reaction) converts one substance into another.
8/9/015 A chemical change (a chemical reaction) converts one substance into another. CHAPTER 3: PART Chemical Equations and Stoichiometry Chemical reactions involve: 1. Breaking bonds in the reactants.
More informationClass XI Chapter 1 Some Basic Concepts of Chemistry Chemistry
Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
More informationChapter 3. Chemical Equations & Reaction Stoichiometry. Symbolic representation of a chemical reaction
Chapter 3 Chemical Equations & Reaction Stoichiometry I) Chemical Equations Symbolic representation of a chemical reaction potassium + water v potassium hydroxide + hydrogen 2 K(s) + 2 H 2 O(R)! 2 KOH(aq)
More informationNotes: Unit 7 Moles & Stoichiometry
Regents Chemistry: Notes: Unit 7 Moles & Stoichiometry 1 KEY IDEAS A compound is a substance composed of two or more different elements that are chemically combined in a fixed proportion. A chemical compound
More informationA chemical reaction shows the process in which a substance (or substances) is changed into one or more new substances
A chemical reaction shows the process in which a substance (or substances) is changed into one or more new substances Chang, R. 2002. Chemistry 7 th ed. Singapore: McGraw-Hill. A chemical equation uses
More informationChemistry B11 Chapter 5 Chemical reactions
Chapter 5 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl A + BC AC +
More informationQuestion 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
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 informationMoles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
More informationStoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)
Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number
More informationAP Chemistry A Review of Analytical Chemistry
AP Chemistry A Review of Analytical Chemistry AP Chemistry Ch 1 (Prentice Hall) What Temperature Do You Read? A measurement always has some amount of uncertainty To indicate the uncertainty of a single
More informationHL First-Year Chemistry
1. Atomic Structure and Stoichiometry Solutions to further problems: 1. (a) 55 86 6 Fe (b) Rb (c) 1 1 7 81 Tl (d) Cr HL First-Year Chemistry. Introduction of the source, vaporization of the sample, ionization,
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry
Chapter 3 : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2
More informationChapter 3: Phenomena. Chapter 3: Stoichiometry. Mass of A. Mass of C. Mass of A. Mass of D. Mass of B. Mass of B. Mass of C
Chapter 3: Phenomena Phenomena: When some substances are mixed together other substances form. Below is data for the reaction A(s) + 2B(aq) C(aq) + D(aq). Look at the data below and identify any patterns
More information(Q5) How many moles of cobalt (Co) atoms are there in 6.00 x 10 9 (6 billion) Co atoms? 9.96 x mol Co
(Q1) The atomic masses of Cl (75.53 percent) and Cl (24.47 percent) are 34.968 amu and 36.956 amu, respectively. Calculate the average atomic mass of chlorine. The percentages in parentheses denote the
More informationChapter 3. Stoichiometry:
Chapter 3. Stoichiometry: Watch Bozeman Videos & other videos on my website for additional help: Big Idea 1: Chemical Analysis Conservation of Atoms Balancing Equations Symbolic Representation Mole Big
More informationStoichiometry. Chapter 3
Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry: The study of quantities of materials consumed and produced in chemical reactions. In macroworld, we can count objects by weighing assuming
More informationChapter 3 Stoichiometry. Ratios of combination
Chapter 3 Stoichiometry Ratios of combination Topics Molecular and formula masses Percent composition of compounds Chemical equations Mole and molar mass Combustion analysis (Determining the formula of
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 informationChemical Equations. Law of Conservation of Mass. Anatomy of a Chemical Equation CH4(g) + 2O2(g) Chapter 3
Chemical Equations Chemical equations are concise representations of chemical reactions. Chapter 3 : Calculations with Chemical Formulas and Equations Law of Conservation of Mass Anatomy of a Chemical
More informationAP CHEMISTRY CHAPTER 3 STOICHIOMETRY. Avg. atomic mass- weighted avg. based on isotopic composition This is determined using a mass spectrometer.
AP CHEMISTRY CHAPTER 3 STOICHIOMETRY Avg. atomic mass- weighted avg. based on isotopic composition This is determined using a mass spectrometer. To calculate : % Isotope A (mass of A) + % Isotope B (mass
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 informationBasic Concepts of Chemistry and Chemical Calculations. The ratio of the average mass factor to one twelfth of the mass of an atom of carbon-12
Basic Concepts of Chemistry and Chemical Calculations Relative Atomic mass: The relative atomic mass is defined as the ratio of the average atomic mass factor to the unified atomic mass unit. (Or) The
More informationNotes: Unit 7 Moles & Stoichiometry
Regents Chemistry: Notes: Unit 7 Moles & Stoichiometry 1 KEY IDEAS In all chemical reactions there is a conservation of mass, energy, and charge. (3.3a) A balanced chemical equation represents conservation
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Lecture Outline 3.1 Chemical Equations The quantitative nature of chemical formulas and reactions is called stoichiometry. Lavoisier
More informationChemistry (www.tiwariacademy.com)
() Question 1.1: Calculate the molecular mass of the following: (i) H2O (ii) CO2 (iii) CH4 Answer 1.1: (i) H2O: The molecular mass of water, H2O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen)
More informationStoichiometry ( ) ( )
Stoichiometry Outline 1. Molar Calculations 2. Limiting Reactants 3. Empirical and Molecular Formula Calculations Review 1. Molar Calculations ( ) ( ) ( ) 6.02 x 10 23 particles (atoms or molecules) /
More informationUnit 1 SOME BASIC CONCEPTS OF CHEMISTRY I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings of mass which are given
More informationChapter 3. Stoichiometry
Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average
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 informationReactants and products. Indications of state. Mass balance: coefficients vs. subscripts
1 of 9 I. Chemical equations Chemical equations - shorthand representations of chemical reactions The reaction of aqueous silver (I) nitrate and aqueous ammonium chloride results in the formation of solid
More informationChapter 3 Stoichiometry
Chapter 3: Phenomena Phenomena: When some substances are mixed together other substances form. Below is data for the reaction A(s) + 2B(aq) C(aq) + D(aq). Look at the data below and identify any patterns
More informationLecture outline: Section 3. Law of conservation of mass: atoms are not created or. reactions. They simply rearrange. Mass before = mass after
Lecture outline: Section 3 Chemical reactions: chemical changes that occur when substances react to form new substances 1. Chemical equations 2. Atomic and molecular 3. Chemical calculations Law of conservation
More informationChapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Lecture Presentation
Lecture Presentation Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College Cottleville, MO Law of Conservation of Mass We may lay it down as an
More informationAnnouncement. Quiz # 1 and 2 on Friday, 28 November. Please bring a blue book!
Announcement Quiz # 1 and 2 on Friday, 28 November. Please bring a blue book! 1 Borax is the common name of an industrial cleaner, sodium tetraborate, Na 2 B 4 O 7. Suppose you have 20.0 g of borax. Calculate
More information9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY Work directly from Zumdahl (Chapter 3). Work through exercises as required, then summarise the essentials of the section when complete. A chemical equation is
More informationChemistry Chapter 3. Stoichiometry. (three sections for this chapter)
Chemistry Chapter 3 Stoichiometry (three sections for this chapter) Chemistry Chapter 3 Stoichiometry Section 1 3.1-3.4 Average Atomic Mass The Mole Molar Mass Average Atomic Mass Average mass of objects
More informationChapter 3 Stoichiometry
Chapter 3: Phenomena Phenomena: When some substances are mixed together other substances form. Below is data for the reaction: A(s) + 2B(aq) C(aq) + D(aq) Look at the data below and identify any patterns
More informationName: Date: AP Questions for Chapter 2
Name: Date: AP Questions for Chapter 2 Multiple Choice Identify the choice that best completes the statement or answers the question. You must show all work on looseleaf and attach. 1. The mass of a single
More informationChapter 3 Chemical Reactions and Reaction Stoichiometry
Chapter 3 Chemical Reactions and Reaction Stoichiometry 2015 Pearson Education, Inc. Chemical Reactions and Reaction Stoichiometry 3.1 Chemical Equations 3.2 Simple Patterns of Chemical Reactivity 3.3
More information23.9 (mm) = mm = 2.01 X10 2 g/mol
#18 Notes Unit 3: Stoichiometry Ch. continued III. Percent Composition Ex. 1) Find the % composition of (NH 4 ) 2 C 4 H 4 O 4 2 N = 2 (14.007 g) = 28.014 g N 8+4= 12 H = 12 ( 1.0080 g) = 12.096 g H 4 C
More informationLecture outline: Section 3
Lecture outline: Section 3 Chemical reactions: chemical changes that occur when substances react to form new substances 1. Chemical equations 2. Atomic and molecular mass 3. Chemical calculations 1 Law
More informationChapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry
Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are
More informationChapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11)
C h e m i s t r y 1 A : C h a p t e r 3 P a r t B P a g e 1 Chapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11) Homework: Read Chapters 3. Work out sample/practice
More informationThe Atom, The Mole & Stoichiometry. Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination.
Unit 2: The Atom, The Mole & Stoichiometry Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination. Postulates of the atomic theory: 1. All matter
More informationChapter 3. Mass Relationships, Stoichiometry and Chemical Formulas. Announcements. Learning Objectives MOLE
Announcements HOUR EXAM 1 --Critical To Understand Chapter 3 July 18 6-7:30PM --Skip Combustion Analysis & Isomers (p.82-83 in Principles of Chemistry Text) See me if you donʼt understand! Chapter 3 Relationships,
More informationIGCSE (9-1) Edexcel - Chemistry
IGCSE (9-1) Edexcel - Chemistry Principles of Chemistry Chemical Formulae, Equations and Calculations NOTES 1.25: Write word equations and balanced chemical equations (including state symbols): For reactions
More informationName: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2
Name: Class: _ Date: _ Chpt 12 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is conserved in the reaction shown below? H 2 + Cl 2 2HCl a.
More information15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g
CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO
More informationMass Relationships in Chemical Reactions
Reading Assignments: Chapter 3 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Mass Relationships in Chemical Reactions Or Related topics in other textbooks. Consultation outside lecture room: Office
More informationMole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units )
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units ) N A 6.0 10 mol -1 1 mol substance contains N A Molar mass (g/mol)
More informationChapter 3. Mass Relationships in Chemical. Reactions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill
Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 3 Mass Relationships in Chemical Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry
More informationChemical Equations. Chemical Reaction: Interaction between substances that results in one or more new substances being produced
Chemical Equations Chemical Reaction: Interaction between substances that results in one or more new substances being produced Example: hydrogen + oxygen water Reactants of a Reaction: Starting materials
More informationUNIT 5: MOLES & STOICHIOMETRY
*KEY* UNIT 5: MOLES & STOICHIOMETRY *KEY* VOCABULARY: 1. Mole 2. Formula mass (FM) 3. Gram formula mass (GFM) 4. Coefficient 5. Subscript 6. Species 7. Law of conservation of mass 8. Law of conservation
More informationChapter 3 C 2 H 4 O2. Mass Relationships, Stoichiometry and Chemical Formulas. Announcements. Learning Objectives. C x H y Oz
Announcements HOUR EXAM 1 --Want me to do recitation again? July 18 6-7:30PM --Skip Combustion Analysis & Isomers (p.82-83 in Principles of Chemistry Text) See me if you donʼt understand! Chapter 3 Relationships,
More information3 Stoichiometry: Calculations with Chemical Formulas and Equations
3 Stoichiometry: Calculations with Chemical Formulas and Equations 3.1 Chemical Equations Balance chemical equations. 3. Simple Patterns of Reactivity Predict products of a chemical reaction in a combination
More informationCalculations with Chemical Formulas and Equations
Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows the chemist
More informationSIC CONCEPTS TS OF CHEMISTRY. Unit. I. Multiple Choice Questions (Type-I)
Unit 1 SOME BASIC B SIC CONCEPTS CONCEP TS OF CHEMISTRY CHEMIS I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings
More informationChapter 3. Molecules, Moles, and Chemical Equations
Chapter 3 Molecules, Moles, and Chemical Equations Law of Conservation of Matter Matter is neither created nor destroyed. In chemistry the number of atoms going into a chemical reaction must be the same
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3 : Calculations with Chemical Formulas and Equations AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier Law of Conservation of Mass We may lay it down as an incontestable axiom that,
More informationUnit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction.
Unit 10: Stoichiometry Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Info given by a chemical equation: Chemical changes involve
More informationCh 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated
More informationUnit-1 SOME BASIC CONCEPTS OF CHEMISTRY
Unit-1 SOME BASIC CONCEPTS OF CHEMISTRY 1. Question based on significant numbers,precision,accuracy, ScientificNotation, laws of chemical combinations, SI units 1.1 What are the SI unit of mass, length
More informationChapter 3 : Stoichiometry
Chapter : Stoichiometry 14 KMnO 4 + 4 C H 5 (OH) --> 7 K CO + 7 Mn O + 5 CO + 16 H O + HEAT Chemical changes : Why they occur? How fast? => Need to know chemical stoicheometry Stoichiometry - The study
More informationCHEMICAL ARITHMATICS MODULE - 1. Objectives. Chemical Arithmatics. Atoms, Molecules and Chemical Arithmatics. Notes
2 MODULE - 1 CHEMICAL ARITHMATICS W e know that atoms of different elements combine in simple whole-number ratios to form molecules. For example, hydrogen and oxygen atoms combine in the mass ratio of
More informationINTRO AND BACKGROUND: Reactions, Moles, Stoichiometry, and Solutions. Chemical Reaction Atoms are REARRANGED to form a different substance
INTRO AND BACKGROUND: Reactions, Moles, Stoichiometry, and Solutions Chemical Reaction Atoms are REARRANGED to form a different substance Changes the way atoms are joined together Atoms CANNOT be created
More informationCounting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
More informationChapter 3 Molecules, Compounds, and Chemical Equations
Chapter 3 Molecules, Compounds, and Chemical Equations 3.7 Formula Mass versus Molar mass Formula mass The average mass of a molecule or formula unit in amu also known as molecular mass or molecular weight
More informationStudent Version Notes: Unit 5 Moles & Stoichiometry
Name: Regents Chemistry: Mr. Palermo Student Version Notes: Unit 5 Moles & Stoichiometry Name: KEY IDEAS A compound is a substance composed of two or more different elements that are chemically combined
More informationChemistry 142A, Autumn 2011 Worksheet #3 Answer Key Ch. 3, start of Ch. 4
Chemistry 142A, Autumn 2011 Worksheet #3 Answer Key Ch. 3, start of Ch. 4 1) There are several important compounds that contain only nitrogen and oxygen. Calculate the mass percent of nitrogen in each
More information7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.
Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation
More informationChapter 3 Calculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Contents and Concepts Mass and Moles of Substances Here we will establish a critical relationship between the mass of a chemical substance and
More informationUNIT 5: STOICHIOMETRY
UNIT 5: STOICHIOMETRY Outline The Mole Molar Mass, Mass and atoms Molar Mass of Compounds Empirical Formula, Molecular Formula (Not Hydrates) Stoichiometry, Mole Ratios Limiting Reactants, Percent Yield
More informationChapter 3 The Mole and Stoichiometry
Chapter 3 The Mole and Stoichiometry Chemistry, 7 th Edition International Student Version Brady/Jespersen/Hyslop Brady/Jespersen/Hyslop Chemistry7E, Copyright 015 John Wiley & Sons, Inc. All Rights Reserved
More informationStudent Number Initials N. G Z. Mc Z. Mo T. N H. R M. S M. T.
Student Number Section 003 Initials 5037785 N. G. 50417065 Z. Mc. 50419357 Z. Mo. 50418455 T. N. 50184967 H. R. 503899 M. S. 5038787 M. T. Find Jan or Sandy asap in the Chem. labs Section 006 Student Number
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 informationUNIT 5: STOICHIOMETRY
UNIT 5: STOICHIOMETRY Outline The Mole Molar Mass, Mass and atoms Molar Mass of Compounds Empirical Formula, Molecular Formula (Not Hydrates) Stoichiometry, Mole Ratios Limiting Reactants, Percent Yield
More informationChemical Equations. Chemical Equations. Chemical Equations. Combination Reactions. Decomposition Reactions
John W. Moore Conrad L. Stanitski Peter C. Jurs http://academic.cengage.com/chemistry/moore Chemical Equations Reactants yeast Products C 6 H 1 O 6 (aq) C H 5 OH(l) + CO (g) glucose ethanol carbon dioxide
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationREVIEW of Grade 11 Chemistry
REVIEW of Grade 11 Chemistry SCH4U_08-09 NAME: Section A: Review of Rules for Significant Digits All measurements have a certain degree of associated with them. All the accurately known digits and the
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationChem 101 Review. Fall 2012
Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table
More informationIsotope: An atom of an element that has the same number of protons as the element, but different numbers of neutrons.
SCH 4CI Determining the Mass of Atoms Isotope: An atom of an element that has the same number of protons as the element, but different numbers of neutrons. Example Oxygen 16 O 8 17 O 8 18 O 8 Isotopic
More information