Molar Mass Worksheet Answer Key


 Terence Walker
 1 years ago
 Views:
Transcription
1 Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl g/mol 5) BF g/mol 6) CCl 2 F g/mol 7) Mg(OH) g/mol 8) UF g/mol 9) SO g/mol 10) H 3 PO 4 98 g/mol 11) (NH 4 ) 2 SO g/mol 12) CH 3 COOH 60 g/mol 13) Pb(NO 3 ) g/mol 14) Ga 2 (SO 3 ) g/mol
2 Avogadro s Number and the Mole 1) How many moles of water does 6.02 x molecules represent? 2) Convert 3.01 x molecules of C 2 H 6 to moles 3) How many moles of glucose does 1.2 x molecules represent? 4) How many moles of CaCl 2 does 2.41 x formula units represent 5) How many atoms does 2.0 moles of He represent? 6) How many sodium ions are in 3.0 moles of NaCl? 7) How many molecules are in 0.25 moles of CH 4? 8) How many total atoms are in 1.0 moles of H 2 O?
3 Mass and the Mole Answer Key 1) How many moles are in 15 grams of lithium? 0.46 moles 2) How many grams are in 2.4 moles of sulfur? 77.0 grams 3) How many moles are in 22 grams of argon? 0.55 moles 4) How many grams are in 88.1 moles of magnesium? 2141 grams 5) How many moles are in 2.3 grams of phosphorus? moles 6) How many grams are in 11.9 moles of chromium? grams 7) How many moles are in 9.8 grams of calcium? 0.24 moles 8) How many grams are in 238 moles of arsenic? 17,826 grams What are the molecular weights of the following compounds? 9) NaOH 40.1 grams 12) H 3 PO grams 10) H 2 O 18.0 grams 13) Mn 2 Se grams 11) MgCl grams 14) (NH 4 ) 2 SO grams 15) How many grams are in 4.5 moles of sodium fluoride, NaF? 189 grams 16) How many moles are in 98.3 grams of aluminum hydroxide, Al(OH) 3? 1.26 moles 17) How many grams are in 0.02 moles of beryllium iodide, BeI 2? 5.2 grams 18) How many moles are in 68 grams of copper (II) hydroxide, Cu(OH) 2? 0.70 moles 19) How many grams are in 3.3 moles of potassium sulfide, K 2 S? grams 20) How many moles are in 1.2 x 10 3 grams of ammonia, NH 3? 70.6 moles 21) How many grams are in 2.3 x 104 moles of calcium phosphate, Ca 3 (PO 3 ) 2? grams 22) How many moles are in 3.4 x 107 grams of silicon dioxide, SiO 2? 5.66 x 109 moles 23) How many grams are in 1.11 moles of manganese sulfate, Mn 3 (SO 4 ) 7? grams
4 Combined Mole Calculations Answer Key 1) How many molecules are there in 24 grams of FeF 3? 1.28 x molecules 2) How many molecules are there in 450 grams of Na 2 SO 4? 1.91 x molecules 3) How many grams are there in 2.3 x atoms of silver? 421 grams 4) How many grams are there in 7.4 x molecules of AgNO 3? 209 grams 5) How many grams are there in 7.5 x molecules of H 2 SO 4? 122 grams 6) How many molecules are there in 122 grams of Cu(NO 3 ) 2? 3.92 x molecules 7) How many grams are there in 9.4 x molecules of H 2? 312 grams 8) How many molecules are there in 230 grams of CoCl 2? 1.07 x molecules 9) How many molecules are there in 2.3 grams of NH 4 SO 2? 1.69 x molecules 10) How many grams are there in 3.3 x molecules of N 2 I 6? 430 grams 11) How many molecules are there in 200 grams of CCl 4? 7.82 x molecules 12) How many grams are there in 1 x molecules of BCl 3? 195 grams 13) How many grams are there in 4.5 x molecules of Ba(NO 2 ) 2? 17.1 grams 14) How many molecules are there in 9.34 grams of LiCl? 1.33 x molecules 15) How many grams do 4.3 x molecules of UF 6 weigh? 2.51 grams 16) How many molecules are there in 230 grams of NH 4 OH? 3.96 x molecules
5 More Combined Mole Calculations Solutions 1. Calculate the mass of mole of CaCl g/mol 2. Calculate grams in moles of CO g 3. Calculate number of moles in 32.0 g of CH mol 4. Determine mass in grams of 40.0 moles of Na 2 CO g 5. Calculate moles in g of HgS 0.722mol 6. Calculate moles in g of Al 2 S mol 7. How many moles are in g of H 2 O 1.50mol 8. Determine the mass in grams of Avogadro number of C 12 H 22 O g/mol 9. Find mass in grams of 9.03 moles of H 2 S 308g 10. Determine grams in mole of NH g Consider the molecule CuNH 4 Cl 3 as you answer Name the elements present. Copper, Nitrogen, Hydrogne, Chlorine 12. How many atoms form the molecule? Nine 13. How many of each atom in the molecule? Cu1, N1, H4, Cl How many hydrogen atoms in one mole of molecules? 2.41 x atoms 15. How many chlorine atoms in six moles of molecules? x atoms 16. What is the molar mass of this molecule? g/mol 17. What is the mass in grams of one molecule? x g 18. How many moles would be in 6.84 g of this substance? mol 19. You need mole of lead (II) chromate. How much should you weigh on the scale? 3.23g 20. Given 6.40 g of HBr. How many moles is this? mol Write the correct formula for calcium acetate and then answer based on it. 21. What is the mass of exactly one mole of calcium acetate? Ca(C 2 H 3 O 2 ) 2 158g/mol 22. How many moles are contained in 1.58 g of the substance in #23? 0.01mol 23. How much does mole of #23 weigh? 63.3g 24. Write the formula for oxygen gas. O How many atoms (and moles) are represented by the formula in #24? 2 atoms, 1/N A mole of molecules 26. What is the mass of Avogadro Number of oxygen molecules? g/mol
6 The Mole Review (Solutions) 1) Define mole x of anything, usually atoms or molecules. 2) How many moles are present in 34 grams of Cu(OH) 2? 0.35 moles 3) How many moles are present in 2.45 x molecules of CH 4? 0.41 moles 4) How many grams are there in 3.4 x molecules of NH 3? 96 grams 5) How much does 4.2 moles of Ca(NO 3 ) 2 weigh? 689 grams 6) What is the molar mass of MgO? 40.3 grams/mole 7) How are the terms molar mass and atomic mass different from one another? Molar mass is used to describe the mass of one mole of a chemical compound, while atomic mass is used to describe the mass of one mole of an element or the mass of one atom of an element. 8) Which is a better unit for expressing molar mass, amu or grams/mole? Grams/mole is better, because any macroscopic amount of a substance is better expressed in grams than amu.
Moles, Molecules, and Grams Worksheet Answer Key
Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3
More informationLabs: Chalk Lab Bubble Gum Lab Mole Lab the Works. Activities: Mole Airlines Flight Ebola Mole. Quizzes:
The Mole **Make sure you get your daily work signed off on. That way, when we test you'll have the grade you earned instead of Videos freaking out about 50's in the book. #1  The Mole #2  Particles
More informationMOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]
MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH
More informationStudy Guide For Chapter 7
Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance
More informationB. Elements: We cannot determine how many electrons are lost for the elements b/c their in their valence electrons can change.
Unit 6 Notepack: Chapters 9 &10 Chemical Quantities 9.1 Naming Ions NAME Period: A. ions: Ions made of single. B. Elements: There is a pattern in predicting how many electrons are lost and gained for the
More informationSNC2D Chemistry Review
SNC2D Chemistry Review Name: Draw the BohrRutherford diagram for each of the following atoms and determine the valence charge of their ions: Sodium: Aluminum: Sulfur: Fluorine: From your periodic table/chemistry
More informationAP Chemistry Prep  Summer Assignment 2013
AP Chemistry Prep  Summer Assignment 2013 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which value has only 4 significant digits? a. 6.930 c. 8450
More informationBalancing Chemical Equations
Balancing Chemical Equations 1. sodium carbonate + calcium hydroxide sodium hydroxide + calcium carbonate Na 2 CO 3 + Ca(OH) 2 2 NaOH + CaCO 3 2. carbon dioxide + water carbonic acid CO 2 + H 2 O H 2 CO
More information= 11.0 g (assuming 100 washers is exact).
CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula
More informationChemical Quantities: The Mole Chapter 7 Assignment & Problem Set
Chemical Quantities: The Mole Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Quantities: The Mole 2 Study Guide: Things You Must Know
More informationSYMBOLS, FORMULAS AND MOLAR MASSES
SYMBOLS, FORMULAS AND MOLAR MASSES OBJECTIVES 1. To correctly write and interpret chemical formulas 2. To calculate molecular weights from chemical formulas 3. To calculate moles from grams using chemical
More informationChapter 4 Chemical Composition
Chapter 4 Chemical Composition 4.1 (a) mole; (b) Avogadro s number; (c) empirical formula; (d) solute; (e) molarity; (f) concentrated solution 4. (a) molar mass; (b) percent composition by mass; (c) solvent;
More informationCHEMICAL QUANTITIES. Chapter 10
CHEMICAL QUANTITIES Chapter 10 What is a mole? A unit of measurement in chemistry 1 mole of a substance = 6.02 x 10 23 (Avagadro s number) representative particles of a substance Representative particle
More informationHow much does a single atom weigh? Different elements weigh different amounts related to what makes them unique.
How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique. What units do we use to define the weight of an atom? amu units of atomic weight. (atomic
More informationChapter 7 Part II: Chemical Formulas and Equations. Mr. Chumbley Chemistry 12
Chapter 7 Part II: Chemical Formulas and Equations Mr. Chumbley Chemistry 12 SECTION 3: USING CHEMICAL FORMULAS Molecules and Formula Unit We have not yet discussed the different ways in which chemical
More information1. Balance the following equation. What is the sum of the coefficients of the reactants and products?
1. Balance the following equation. What is the sum of the coefficients of the reactants and products? 1 Fe 2 O 3 (s) + _3 C(s) 2 Fe(s) + _3 CO(g) a) 5 b) 6 c) 7 d) 8 e) 9 2. Which of the following equations
More informationMOLECULAR MASS AND FORMULA MASS
1 MOLECULAR MASS AND FORMULA MASS Molecular mass = sum of the atomic weights of all atoms in the molecule. Formula mass = sum of the atomic weights of all atoms in the formula unit. 2 MOLECULAR MASS AND
More information1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)
1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)
More informationBalancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
More informationCHAPTER 11  CHEMICAL QUANTITIES
I. THE MOLE CONCEPT CHAPTER 11  CHEMICAL QUANTITIES A. What is a mole? 1. a mole is the SI unit of measurement of counting; just like a dozen is a measurement 2. a mole is a number a. 6.02 x 10 23 is
More informationProblem Solving. Mole Concept
Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When
More informationSCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGrawHill Ryerson, 2001
SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGrawHill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample
More informationAtomic mass and the mole
Atomic mass and the mole An equation for a chemical reaction can provide us with a lot of useful information. It tells us what the reactants and the products are in the reaction, and it also tells us the
More informationChemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.
1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.
More informationChapter 6 Chemical Composition
Chapter 6 Chemical Composition 1. 100 washers 0.110 g 1 washer = 11.0 g (assuming 100 washers is exact) 100. g 1 washer 0.110 g = 909 washers 2. 500. g 1 cork 1.63 g = 306.7 = 307 corks 500. g 1 stopper
More informationChemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1
Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500
More informationneutrons are present?
AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest
More information1. How many hydrogen atoms are in 1.00 g of hydrogen?
MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 1024 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?
More informationMODERN CHEMISTRY. 8. What is the formula for aluminum sulfate? 9. What is the formula for barium hydroxide?
MODERN CHEMISTRY Date Name Period Multiple Choice  Identify the choice that best completes the statement or answers the question. Use answerkey worksheet (Page 6) to key in answers to questions. 1. A
More informationCHM1 Review for Exam 9
Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules
More informationU3LM2BWS Molar Mass and Conversions
U3LM2BWS Molar Mass and Conversions Name: KEY 1. The molar mass of chlorine is: 2 x 35.45 g/mol Cl = 70.90 g/mol Cl 2 (Remember that chlorine exists as a diatomic molecule in nature) 2. The molar mass
More informationCHAPTER 3 COMPOUNDS AND MOLECULES
Chapter 3 Compounds and Molecules Page 1 CHAPTER 3 COMPOUNDS AND MOLECULES 31. Octane, a component of gasoline, has eight carbon atoms and eighteen hydrogen atoms per molecule. Its formula is written
More informationBalance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O
Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent
More informationCh. 10 The Mole I. Molar Conversions
Ch. 10 The Mole I. Molar Conversions I II III IV A. What is the Mole? A counting number (like a dozen) Avogadro s number (N A ) 1 mole = 6.022 10 23 representative particles B. Mole/Particle Conversions
More informationQuantitative aspects of chemical change: Moles and molar mass
OpenStaxCNX module: m38717 1 Quantitative aspects of chemical change: Moles and molar mass Free High School Science Texts Project This work is produced by OpenStaxCNX and licensed under the Creative
More informationb. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.
CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following
More informationUnit 5 Chemical Quantities & The Mole
Unit 5 Chemical Quantities & The Mole Molar mass is the mass of one mole of a substance. Molar Mass Other names for molar mass include *formula mass *gram formula mass *molecular weight Molar Mass One
More informationCHEMISTRY CP Name: KEY Period: UNIT 5: TEST REVIEW SHEET MOLE CONVERSIONS, EMPIRICAL/MOLECULAR FORMULA, STOICHIOMETRY
CHEMISTRY CP Name: KEY Period: UNIT 5: TEST REVIEW SHEET MOLE CONVERSIONS, EMPIRICAL/MOLECULAR FORMULA, STOICHIOMETRY MOLES AND MOLE CONVERSIONS 1. Things to Know: a. What is a mole? Avogadro s number
More informationDescription of the Mole Concept:
Description of the Mole Concept: Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called
More informationStoichiometry Review
Stoichiometry Review There are 20 problems in this review set. Answers, including problem setup, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) > 2NH 3 (g) a. nitrogen
More informationChapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations
CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1
More informationName Block THE MOLE. Who s Counting Lab. Mole Notes. Mole Calculations. Mixed Mole Conversions. % Comp, Emp, and Molecular Calcuations
Name Block THE MOLE Who s Counting Lab Mole Notes Mole Calculations Mixed Mole Conversions % Comp, Emp, and Molecular Calcuations Mole Notes, Part 1 1. The Mole is just a long word for changing units
More informationChemical Reactions and Equations. Chapter 8
Chemical Reactions and Equations Chapter 8 Describing Chemical Reactions A chemical reaction is the process by which one or more substances are changed into different substances Reactants Products When
More informationMolecular Formula: Example
Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical
More informationChapter 5  Molecules and Compounds
Chapter 5  Molecules and Compounds How do we represent molecules? In pictures In formula In name Ionic compounds Molecular compounds On the course website, you will find a list of ions that I would like
More informationTUTORIAL 51 HELP. Mass of sodium = 23.0 g/mol x 3 mol = 69.0 g of sodium. Percent mass of sodium = 69.0 g x 100% = 42.
TUTORIAL 51 HELP ANSWER TO QUESTION 1 ON TUTORIAL 51: Question 1. Find the percent composition by mass of sodium phosphate, Na 3 PO 4. Step 1: Find the molar mass of Na 3 PO 4 (The mass of one mole of
More informationChapter 8 Chemical Quantities
Chapter 8 Chemical Quantities Introductory Info The atomic masses of the elements on the periodic table are in the units. These measurements are based on the mass of the standard isotope of the element,
More informationChapter 3 Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative
More informationHOMEWORK 4A. Definitions. OxidationReduction Reactions. Questions
HOMEWORK 4A OxidationReduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric
More informationMole Notes.notebook. October 29, 2014
1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the
More information1. P 2 O 5 2. P 5 O 2 3. P 10 O 4 4. P 4 O 10
Teacher: Mr. gerraputa Print Close Name: 1. A chemical formula is an expression used to represent 1. mixtures, only 3. compounds, only 2. elements, only 4. compounds and elements 2. What is the total number
More informationStoichiometry. Lecture Examples Answer Key
Stoichiometry Lecture Examples Answer Key Ex. 1 Balance the following chemical equations: 3 NaBr + 1 H 3 PO 4 3 HBr + 1 Na 3 PO 4 2 C 3 H 5 N 3 O 9 6 CO 2 + 3 N 2 + 5 H 2 O + 9 O 2 2 Ca(OH) 2 + 2 SO 2
More informationBalancing Chemical Equations
Balancing Chemical Equations Aluminum reacts with copper(ii) chloride, CuCl 2, to form copper metal and aluminum chloride, AlCl 3 1. Identify the reactants and products. Aluminum and copper(ii) chloride
More informationChemistry PostEnrolment Worksheet
Name: Chemistry PostEnrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
More informationUnit 10A Stoichiometry Notes
Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations
More informationBALANCING CHEMICAL EQUATIONS
BALANCING CHEMICAL EQUATIONS The Conservation of Matter states that matter can neither be created nor destroyed, it just changes form. If this is the case then we must account for all of the atoms in a
More informationSolution. Practice Exercise. Concept Exercise
Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of
More informationName: Class: Date: 2 4 (aq)
Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of
More informationThe Mole IT IS JUST A STANDARD NUMBER OF ATOMS/MOLECULES
The Mole S 6.02 X 10 23 IT IS JUST A STANDARD NUMBER OF ATOMS/MOLECULES Relative Masses To understand relative scales, let s s ignore electrons and compare atoms by total number of nuclear particles. Hydrogen,
More informationMole  Mass Relationships in Chemical Systems
Chapter 3: Stoichiometry Mole  Mass Relationships in Chemical Systems 3.1 The Mole 3.2 Determining the Formula of an Unknown Compound 3.3 Writing and Balancing Chemical Equations 3.4 Calculating the Amounts
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationName Class Date. Step 3: Write the equation using formulas for the elements and compounds in the word equation. Al CuCl 2 : AlCl 3 Cu
Skills Worksheet Math Skills Balancing Chemical Equations After you study each sample problem and solution, work out the practice problems on a separate sheet of paper. Write your answers in the spaces
More informationSTOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g.
PERCENTAGE COMPOSITION STOICHOMETRY UNIT 3 1. A sample of magnesium weighing 2.246 g burns in oxygen to form 3.724 g of magnesium oxide. What are the percentages of magnesium and oxygen in magnesium oxide?
More informationChemical Reactions Chapter 8 Assignment & Problem Set
Chemical Reactions Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the
More informationCK12 FOUNDATION. Stoichiometry. Say Thanks to the Authors Click (No sign in required) Parsons
CK12 FOUNDATION Stoichiometry Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) Parsons To access a customizable version of this book, as well as other interactive content,
More informationNames & Formulas for Ionic Compounds
Names & s for Ionic Compounds Determine the correct NAME for the ionic compounds listed below: Chemical Name Chemical Name NaCl Sodium chloride CaCl 2 Calcium chloride CaO Calcium oxide FeF 3 Iron (III)
More informationPractice questions for Ch. 3
Name: Class: Date: ID: A Practice questions for Ch. 3 1. A hypothetical element consists of two isotopes of masses 69.95 amu and 71.95 amu with abundances of 25.7% and 74.3%, respectively. What is the
More informationChapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole
Chapter 4 Chemical Composition Chapter 4 Topics 1. Mole Quantities 2. Moles, Masses, and Particles 3. Determining Empirical Formulas 4. Chemical Composition of Solutions Copyright The McGrawHill Companies,
More informationChapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGrawHill 2009 1
Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGrawHill 2009 1 3.1 Molecular and Formula Masses Molecular mass  (molecular weight) The mass in amu
More informationChapter 4 Chemical Composition. Moles of Various Elements and Compounds Figure 4.8
Chapter 4 Chemical Composition Mole Quantities Moles, Masses, and Particles Determining Empirical and Molecular Formulas Chemical Composition of Solutions 41 Copyright The McGrawHill Companies, Inc.
More informationName: Block: Date: Test Review: Chapter 8 Ionic Bonding
Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fillintheblank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity
More informationChem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses
Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro
More informationAtoms and Ions. 1) a) State the charges of ALL three ions, Ca 2+, F  and K + in terms of electron arrangement and number of protons.
Atoms and Ions 1) a) State the charges of ALL three ions, Ca 2+, F  and K + in terms of electron arrangement and number of protons. b) Use their positions on the periodic table to explain why two of the
More informationUnit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test
Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?
More informationUnit 6: Reactions and Stoichiometry (Link to Prentice Hall Text: Chapters 7, 8 & 9)
R e a c t i o n s a n d S t o i c h i o m e t r y N o t e s P a g e 1 Unit 6: Reactions and Stoichiometry (Link to Prentice Hall Text: Chapters 7, 8 & 9) Name: Date Due Assignments Page Number: Problem
More informationSTOICHIOMETRY STOICHIOMETRY. Measurements in Chemical Reactions. MoleMole Relationships. MassMass Problem. MoleMole Relationships
STOICHIOMETRY STOICHIOMETRY The analysis of the quantities of substances in a chemical reaction. Stoichiometric calculations depend on the MOLE MOLE relationships of substances. Measurements in Chemical
More informationProgramme in mole calculation
Programme in mole calculation Step 1 Start at the very beginning Atoms are very small indeed! If we draw a line 1 metre long, 6,000,000,000 (6 billion) atoms could be lined end to end. So a scientist cannot
More informationCh. 6 Chemical Composition and Stoichiometry
Ch. 6 Chemical Composition and Stoichiometry The Mole Concept [6.2, 6.3] Conversions between g mol atoms [6.3, 6.4, 6.5] Mass Percent [6.6, 6.7] Empirical and Molecular Formula [6.8, 6.9] Bring your calculators!
More informationThe Mole Concept and Atoms
Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly
More informationThe Mole. 6.022 x 10 23
The Mole 6.022 x 10 23 Background: atomic masses Look at the atomic masses on the periodic table. What do these represent? E.g. the atomic mass of Carbon is 12.01 (atomic # is 6) We know there are 6 protons
More informationBalancing Equations Notes
. Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written
More informationCHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT
CHAPTER 3 Calculations with Chemical Formulas and Equations MOLECULAR WEIGHT (M. W.) Sum of the Atomic Weights of all atoms in a MOLECULE of a substance. FORMULA WEIGHT (F. W.) Sum of the atomic Weights
More information4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.
1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.
More informationFormula Stoichiometry. Text pages
Formula Stoichiometry Text pages 237250 Formula Mass Review Write a chemical formula for the compound. H 2 CO 3 Look up the average atomic mass for each of the elements. H = 1.008 C= 12.01 O = 16.00 Multiply
More informationMOLES AND MOLE CALCULATIONS
35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product
More informationc. PCl 3 (l) + 3H 2 O(l) H 3 PO 3 (l) + 3HCl(g)
Chapter 9 Chemical Quantities 1. Although we define mass as the amount of matter in a substance, the units in which we measure mass are a human invention. Atoms and molecules react on an individual particlebyparticle
More informationSuggested Resources Textbook: Chapter 6 (6.3, 6.4, 6.5 & 6.6)
The Mole Big Picture Ideas: 1. The mole is a unit of count. 2. Using conversion factors, one can convert between mass, moles, particles and volume for a given substance. 3. Empirical data including percent
More informationName Class Date. Chapter: Chemical Equations and Reactions
Assessment Chapter Test A Chapter: Chemical Equations and Reactions In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. You
More informationCHM101A Exam 2 Version 1 October 10, 2006
CHM101A Exam 2 Version 1 1. Which of the following statements is incorrect? A. SF 4 has ¼ as many sulfur atoms as fluorine atoms. B. Ca(NO 3 ) 2 has six times as many oxygen atoms as calcium ions. C.
More information= 16.00 amu. = 39.10 amu
Using Chemical Formulas Objective 1: Calculate the formula mass or molar mass of any given compound. The Formula Mass of any molecule, formula unit, or ion is the sum of the average atomic masses of all
More informationMoles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:
Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)
More informationMonatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:
Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cateyeon
More informationChapter 5, Calculations and the Chemical Equation
1. How many iron atoms are present in one mole of iron? Ans. 6.02 1023 atoms 2. How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic weight: S, 32.06 amu] Ans. 4.81 g 3. How many moles
More informationName Class Date. Chapter: Chemical Equations and Reactions
Assessment Chapter Test B Chapter: Chemical Equations and Reactions PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question
More informationNotes: Formula Mass and Percent Composition
Notes: Formula Mass and Percent Composition Formula mass  the mass of one mole of a compound, atom or ion. also called: gram formula mass, molecular mass, gram molecular mass, formula weight, gram formula
More informationThe Mole. Chapter 2. Solutions for Practice Problems
Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of
More information1 dozen eggs = eggs 1 dozen donuts = donuts 1 dozen carbon atoms = carbon atoms
Chapter 6 Page 1 Chapter 6: Chemical Composition We buy beans by the pound and eggs by the dozen. WHY? Because these are convenient ways of purchasing these items. Two ways of specifying quantity: 1) Mass
More information2. Draw the BohrRutherford diagrams for the following Ions: S 2, Al +3, Li +1, P 3
1. Complete the following table: ATOMIC STRUCTURE Name Symbol # protons # neutrons # electrons Net charge Sodium ion Na +1 +1 Oxygen atom Gold ion +3 C Cl 1 Cesium ion +1 12 +2 162 18 +1 10 0 Ba +2 Helium
More informationPractice Reaction Type and Predicting the Products
Practice Reaction Type and Predicting the Products For each of the following: The first one is an example. a. Determine the TYPE of reaction by looking at your Reaction Type Sheets and write the type in
More informationWRITE IN THE CORRECT FORMULA THEN BALANCE THE CHEMICAL EQUATIONS
WRITE IN THE CORRECT FORMULA THEN BALANCE THE CHEMICAL EQUATIONS 1. Hydrogen Oxygen Water METALLIC OXIDE WATER BASE 2. Sodium oxide Water Sodium hydroxide 3. Calcium oxide Water Calcium hydroxide 4. Potassium
More information