# Practice questions for Chapter 8

Save this PDF as:

Size: px
Start display at page:

## Transcription

1 Practice questions for Chapter 8 2) How many atoms of nickel equal a mass of g? (Refer to the Periodic Table.) A) 1 B) 28 C) D) 59 E) 6.02 x 1023 Answer: E Section: 8.1 Avogadro's Number 6) What is the number of sulfur atoms that equal a mass of amu? A) 1 B) 16 C) 32 D) 6.02 x 1023 Section: 8.1 Avogadro's Number 9) What is the number of manganese atoms that equal a mass of g? A) 1 B) 25 C) 55 D) 6.02 x 1023 Section: 8.1 Avogadro's Number 13) Which of the following is equal to 1.00 mole of substance? A) 6.02 x 1023 sodium atoms, Na B) 6.02 x 1023 iodine molecules, I2 C) 6.02 x 1023 sodium iodide formula units, NaI D) all of the above Section: 8.2 Mole Calculations I 14) Which of the following is equal to 1.00 mole of substance? A) 6.02 x 1023 lithium atoms, Li B) 6.02 x 1023 fluorine molecules, F2 C) 6.02 x 1023 lithium fluoride formula units, LiF D) all of the above Section: 8.2 Mole Calculations I

2 17) How many molecules of methane are in mol of CH4 gas? A) 1.20 x 1023 molecules B) 1.20 x 1024 molecules C) 3.01 x 1022 molecules D) 3.01 x 1023 molecules E) 3.01 x 1024 molecules Section: 8.2 Mole Calculations I 20) How many moles of ammonia contain 1.51 x 1024 NH3 molecules? A) mol B) mol C) 2.51 mol D) 3.99 mol E) 25.1 mol Section: 8.2 Mole Calculations I 24) What is the molar mass of cholesterol, C27H45OH? A) g/mol B) g/mol C) g/mol D) g/mol E) g/mol Section: 8.3 Molar Mass 26) What is the molar mass of aluminum chlorate, Al(ClO3)3? A) g/mol B) g/mol C) g/mol D) g/mol E) g/mol Section: 8.3 Molar Mass 31) What is the mass of 4.50 x 1022 atoms of gold, Au? A) g B) g C) 13.3 g D) 14.7 g E) 2640 g Section: 8.4 Mole Calculations II 32) What is the mass of 3.30 x 1023 atoms of silver, Ag? A) g

3 B) 25.8 g C) 59.1 g D) 85.7 g E) 197 g Section: 8.4 Mole Calculations II 37) How many molecules of bromine liquid, Br2, have a mass equal to 31.8 g? A) 1.20 x 1023 molecules B) 1.51 x 1024 molecules C) 1.91 x 1025 molecules D) 2.40 x 1023 molecules E) 3.03 x 1024 molecules Section: 8.4 Mole Calculations II 43) What is the mass in grams of a single formula unit of silver chloride, AgCl? A) 1.16 x g B) 1.66 x g C) 2.38 x g D) 4.21 x 1021 g E) 8.61 x 1025 g Section: 8.4 Mole Calculations II 45) Which of the following gases occupies 22.4 L at STP? A) 1 mol hydrogen, H2 B) 1 mol nitrogen, N2 C) 1 mol of oxygen, O2 D) all of the above Section: 8.5 Molar Volume 46) Which of the following gases occupies 22.4 L at STP? A) 1 mol helium, He B) 1 mol neon, Ne C) 1 mol xenon, Xe D) all of the above Section: 8.5 Molar Volume 54) How many xenon atoms are in 10.0 L of Xe gas at STP? A) 1.35 x 1024 atoms B) 2.69 x 1021 atoms

4 C) 2.69 x 1023 atoms D) 6.02 x 1022 atoms E) 6.02 x 1024 atoms 55) How many hydrogen molecules are in 2.75 L of H2 gas at STP? A) 1.66 x 1024 molecules B) 2.19 x 1023 molecules C) 4.90 x 1024 molecules D) 7.39 x 1022 molecules E) 9.77 x 1021 molecules 59) What is the mass of 455 ml of ethane gas, C2H6, at STP? A) g B) g C) 2.95 g D) 10.2 g E) 65.9 g 66) What is the density of fluorine gas, F2, at STP? A) g/l B) g/l C) 1.18 g/l D) 1.70 g/l E) 22.4 g/l 70) If the density of an unknown gas is 1.96 g/l at STP, what is its molar mass? A) 11.4 g/mol B) 19.6 g/mol C) 22.4 g/mol D) 43.9 g/mol E) 196 g/mol 79) The formula for mustard gas used in chemical warfare is C4H8SCl2 ( g/mol). What is the percentage of carbon in the compound? A) 5.08% B) 7.55% C) 20.16%

5 D) 30.20% E) 44.57% Section: 8.7 Percent Composition 80) The formula for mustard gas used in chemical warfare is C4H8SCl2 ( g/mol). What is the percentage of hydrogen in the compound? A) 0.635% B) 5.08% C) 20.16% D) 30.20% E) 44.57% Section: 8.7 Percent Composition 89) If mol of lead combines with mol of sulfur, what is the empirical formula of the lead sulfide product? A) PbS B) Pb2S C) PbS2 D) Pb3S3 Section: 8.8 Empirical Formula 97) If g of tin metal reacts with g of fluorine gas, what is the empirical formula of the product? A) SnF B) SnF2 C) SnF4 D) SnF10 E) Sn2F3 Section: 8.8 Empirical Formula

6 Chapter 9 1) What term refers to the amount of product experimentally measured in a laboratory procedure? A) actual yield B) percent yield C) stoichiometric yield D) theoretical yield 4) What principle states that mass is neither gained or lost during a chemical reaction? A) Avogadro s theory B) law of combining volumes C) law of conservation of mass D) law of constant composition 5) What is the term for the substance in a chemical reaction that controls the maximum amount of product? A) limiting reactant B) limiting product C) maximum reactant D) maximum product 6) What term refers to a type of stoichiometry calculation that relates the masses of two substances according to a balanced chemical equation? A) mass-mass problem B) mass-volume problem C) mole-mole problem D) volume-volume problem 7) What term refers to a type of stoichiometry calculation that relates the mass of a substance to the volume of a gas according to a balanced chemical equation? A) mass-mass problem B) mass-volume problem C) mole-mole problem

7 D) volume-volume problem 8) What term refers to the mass of 1 mol of substance expressed in grams? A) gram-atomic mass B) gram-molecular mass C) gram-formula mass D) molar mass 9) What term refers to the volume occupied by 1 mol of any gas at STP? A) Avogadro s volume B) molar volume C) standard volume D) STP volume 11) What is the term for the actual yield compared to the theoretical yield expressed as a percent? A) experimental yield B) percent yield C) ratio yield D) stoichiometric yield 13) What is the term for the relationship of quantities (i.e., mass of substance or volume of gas) in a chemical reaction according to the balanced chemical equation? A) mass-mass problem B) mass-volume problem C) volume-volume problem D) stoichiometry 50) What is the mass of iron(iii) bromide ( g/mol) that yields g of silver bromide ( g/mol) precipitate? FeBr3(s) + AgNO3(aq) AgBr(s) + Fe(NO3)3(aq) A) g B) g C) g

8 D) g E) g Section: 9.4 Mass-Mass Problems 58) What is the mass of aluminum metal that reacts to give 11.1 g of manganese metal? MnO2(l) + Al(l) A) 3.64 g B) 4.09 g C) 5.45 g D) 7.27 g E) 8.18 g Section: 9.4 Mass-Mass Problems Mn(l) + Al2O3(s) 59) What is the mass of hydrogen gas released from 2.70 g of aluminum metal and hydrochloric acid? Al(s) + HCl(aq) AlCl3(aq) + H2(g) A) g B) g C) g D) g E) g Section: 9.4 Mass-Mass Problems 97) Considering the limiting reactant, what is the mass of manganese produced from 25.0 g of manganese(iv) oxide (86.94 g/mol) and 25.0 g of aluminum metal? 3 MnO2(l) + 4 Al(l) 3 Mn(l) + 2 Al2O3(s) A) 15.8 g B) 38.2 g C) 47.4 g D) 50.9 g E) 67.8 g Section: 9.8 Limiting Reactant Problems 6) How many moles of oxygen react with 1.00 mol of butane, C4H10? C4H10(g) + O2(g) A) 1.00 mol B) 6.50 mol C) 13.0 mol D) 26.0 mol Section: General Exercises CO2(g) + H2O(g)

9 117) How many moles of oxygen gas react with 6.00 mol of propane, C3H8? C3H8(g) + O2(g) A) 3.00 mol B) 4.00 mol C) 5.00 mol D) 6.00 mol Answer: E Section: General Exercises CO2(g) + H2O(g) 118) How many moles of oxygen gas react with 6.00 mol of pentane, C5H12? C5H12(g) + O2(g) CO2(g) + H2O(g) A) 1.00 mol B) 5.00 mol C) 6.00 mol D) 8.00 mol Answer: E Section: General Exercises 119) How many moles of carbon dioxide are produced from 1.00 mol butane, C4H10? C4H10(g) + O2(g) A) 1.00 mol B) 4.00 mol C) 8.00 mol D) 16.0 mol Section: General Exercises CO2(g) + H2O(g)

### STOICHIOMETRY STOICHIOMETRY. Measurements in Chemical Reactions. Mole-Mole Relationships. Mass-Mass Problem. Mole-Mole 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

### Solution. 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

### Unit 9 Stoichiometry Notes (The Mole Continues)

Unit 9 Stoichiometry Notes (The Mole Continues) 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

### Stoichiometry Chapter 9 Assignment & Problem Set

Stoichiometry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Stoichiometry 2 Study Guide: Things You Must Know Vocabulary (know the definition

### 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?

Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance

### Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358)

Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.

### Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

### Subscripts and Coefficients Give Different Information

Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Chemical equations (Balancing REVIEW) 2. Some simple patterns of reactivity 3. Formula weights (REVIEW) 4. Avogadro's

### Calculating Atoms, Ions, or Molecules Using Moles

TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

### Chemistry Stoichiometry. 45 points. Do not turn page until told to do so.

Chemistry 2010 Stoichiometry 45 points Do not turn page until told to do so. Stoichiometry Multiple Choice (Each worth 2 points) Identify the letter of the choice that best completes the statement or

### 1. 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

### CHAPTER 12 GASES AND THEIR BEHAVIOR

Chapter 12 Gases and Their Behavior Page 1 CHAPTER 12 GASES AND THEIR BEHAVIOR 12-1. Which of the following represents the largest gas pressure? (a) 1.0 atm (b) 1.0 mm Hg (c) 1.0 Pa (d) 1.0 KPa 12-2. Nitrogen

### Unit 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?

### 2 Stoichiometry: Chemical Arithmetic Formula Conventions (1 of 24) 2 Stoichiometry: Chemical Arithmetic Stoichiometry Terms (2 of 24)

Formula Conventions (1 of 24) Superscripts used to show the charges on ions Mg 2+ the 2 means a 2+ charge (lost 2 electrons) Subscripts used to show numbers of atoms in a formula unit H 2 SO 4 two H s,

### Mass and Moles of a Substance

Chapter Three 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

### Ex: 1. 1 mol C H O g C H O. Ex: mol C H O mol C H O.

Example of how to solve a mass-to-mass stoichiometry problem Example Problem: If 1.00 gram of the simple sugar fructose (C 6 H 12 O 6 ) is burned in atmospheric oxygen of (O 2 ), what mass of carbon dioxide

### Chapter 3: STOICHIOMETRY: MASS, FORMULAS, AND REACTIONS

Chapter 3: STOICHIOMETRY: MASS, FORMULAS, AND REACTIONS Problems: 3.1-3.8, 3.11, 3.14-3.90, 3.103-3.120, 3.122-3.125, 3.128-3.131, 3.134, 3.137-36.138, 3.140-3.142 3.2 THE MOLE Stoichiometry (STOY-key-OM-e-tree):

### INTRODUCTORY CHEMISTRY Concepts and Critical Thinking

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 9 The Mole Concept by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 9 1 Avogadro s Number Avogadro

### 4. 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.

### Chemical Quantities: The Mole Chapter 7 Assignment & Problem Set

Chemical Quantities: The Mole Name Warm-Ups (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

### W1 WORKSHOP ON STOICHIOMETRY

INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

### Mole 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

### 11-1 Stoichiometry. Represents

11-1 Stoichiometry What is stoichiometry? Calculations that relate the quantities of substances. It is the study of quantitative (measurable amounts) relationships in chemical reactions and equations.

### Chem 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

### Unit 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

### AT Chapter 3 Notes 15.notebook. September 29, Measuring Atomic Masses

Measuring Atomic Masses Mass Spectrometer used to isolate isotopes of an element and determine their mass. 1 An element sample is heated to vaporize it and the gaseous atoms are zapped with an electron

### CP Chemistry Review for Stoichiometry Test

CP Chemistry Review for Stoichiometry Test Stoichiometry Problems (one given reactant): 1. Make sure you have a balanced chemical equation 2. Convert to moles of the known substance. (Use the periodic

### Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

### Chapter 3 Chemical Reactions and Reaction Stoichiometry. 許富銀 ( Hsu Fu-Yin)

Chapter 3 Chemical Reactions and Reaction Stoichiometry 許富銀 ( Hsu Fu-Yin) 1 Stoichiometry The study of the numerical relationship between chemical quantities in a chemical reaction is called stoichiometry.

### 0.786 mol carbon dioxide to grams g lithium carbonate to mol

1 2 Convert: 2.54 x 10 22 atoms of Cr to mol 4.32 mol NaCl to grams 0.786 mol carbon dioxide to grams 2.67 g lithium carbonate to mol 1.000 atom of C 12 to grams 3 Convert: 2.54 x 10 22 atoms of Cr to

### Daily Practice Review 2/28-29/08

Daily Practice Review 2/28-29/08 1. Why is it not correct to balance an equation by changing the subscripts in one or more of the formulas? If you change the subscripts in a formula you change the chemical

### IB 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

### Test 3 Formula and math of formula review. 2. The oxide of metal X has the formula XO. Which group in the Periodic Table contains metal X?

Name: Sunday, November 04, 2007 Test 3 Formula and math of formula review 1. Which is an example of a binary compound? 1. acetic acid 3. potassium hydroxide 2. nitric acid 4. potassium oxide 2. The oxide

### Stoichiometry. What is the atomic mass for carbon? For zinc?

Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12

### MOLES 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

### Molecular 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

### Chapter 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

### Chemical Equations & Stoichiometry

Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term

### CHEMICAL 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

### Chapter 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

### Stoichiometry (greek): Stoicheion element, metry to measure

Stoichiometry Stoichiometry (greek): Stoicheion element, metry to measure Balanced Chemical equation: Skills Tells Ex. formula writing balancing equations substances involved in the chemical rxn relationship

### 21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11

21 st Century Chemistry Multiple Choice Question in Topic 3 Metals Unit 11 1. Consider the equation: 2Ca(s) + O 2 (g) 2CaO(s) Which of the following statements are correct? (1) Calcium and oxygen are reactants.

### 2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant.

UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in

### 7.1 Stoichiometry and Percent Yield

score /10 pts. Name Class Date 7.1 Stoichiometry and Percent Yield Mole Ratios An example: The combustion of propane is used to heat many rural homes in winter. Balance the equation below for the combustion

### STOICHIOMETRY. - the study of the quantitative aspects of chemical

STOICHIOMETRY - the study of the quantitative aspects of chemical GENERAL PLAN FOR STOICHIOMETRY Mass reactant Mass product Moles reactant Stoichiometric factor Moles product STOICHIOMETRY It rests on

### 4. Magnesium has three natural isotopes with the following masses and natural abundances:

Exercise #1 Atomic Masses 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. In a sample that contains 90.0% new and 10.0% old pennies,

### SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

### 1. 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 10-24 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?

### Exploring Gas Laws. Chapter 12. Solutions for Practice Problems. Student Textbook page 477

Chapter 12 Exploring Gas Laws Solutions for Practice Problems Student Textbook page 477 1. Problem At 19 C and 100 kpa, 0.021 mol of oxygen gas, O 2(g), occupy a volume of 0.50 L. What is the molar volume

### 1. 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

### MOLE 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

### Chapter 3. Chemical Reactions and Reaction Stoichiometry. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT

Lecture Presentation Chapter 3 Chemical Reactions and Reaction James F. Kirby Quinnipiac University Hamden, CT The study of the mass relationships in chemistry Based on the Law of Conservation of Mass

### Chemistry Stoichiometry Lesson 8 Lesson Plan David V. Fansler

Chemistry Stoichiometry Lesson 8 Lesson Plan David V. Fansler The Arithmetic of Equations Objectives: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses,

### IB 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

### CHEM J-2 June /01(a) What is the molarity of the solution formed when 0.50 g of aluminium fluoride is dissolved in ml of water?

CHEM1001 2014-J-2 June 2014 22/01(a) What is the molarity of the solution formed when 0.50 g of aluminium fluoride is dissolved in 800.0 ml of water? 2 The molar mass of AlF 3 is: molar mass = (26.98 (Al)

### PERIODIC TABLE OF ELEMENTS. 4/23/14 Chapter 7: Chemical Reactions 1

PERIODIC TABLE OF ELEMENTS 4/23/14 Chapter 7: Chemical Reactions 1 CHAPTER 7: CHEMICAL REACTIONS 7.1 Describing Reactions 7.2 Types of Reactions 7.3 Energy Changes in Reactions 7.4 Reaction Rates 7.5 Equilibrium

### Formulas, Equations, and Moles. + "reacts with" "to produce" Equations must be balanced. Equal amounts of each element on each side of the equation.

Chapter 3 Formulas, Equations, and Moles Chemical Equations 2 2 + 2 2 2 reactants products + "reacts with" "to produce" coefficients - indicate amount of substance Equations must be balanced. Equal amounts

### Problem Solving. Stoichiometry of Gases

Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.

### Chemical Calculations: Formula Masses, Moles, and Chemical Equations

Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic

### Chemical calculations

Chemical calculations Stoichiometry refers to the quantities of material which react according to a balanced chemical equation. Compounds are formed when atoms combine in fixed proportions. E.g. 2Mg +

### Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

### Chapter 4 Chemical Equations & Stoichiometry

Chapter 4 Chemical Equations & Stoichiometry Chemical reactions are best described using equations which tells us what compounds we started with (reactants), what we did to them (reaction conditions) and

### Practice 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

### AP 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

### The Mole Concept. The Mole. Masses of molecules

The Mole Concept Ron Robertson r2 c:\files\courses\1110-20\2010 final slides for web\mole concept.docx The Mole The mole is a unit of measurement equal to 6.022 x 10 23 things (to 4 sf) just like there

### Chemical Reactions. Chemical Equations. Mole as Conversion Factor: To convert between number of particles and an equivalent number of moles:

Quantities of Reactants and Products CHAPTER 3 Chemical Reactions Stoichiometry Application of The Law of Conservation of Matter Chemical book-keeping Chemical Equations Chemical equations: Describe proportions

### Chapter 1 The Atomic Nature of Matter: Selected Answersc for Practice Exam.

Chapter 1 The Atomic Nature of Matter: Selected Answersc for Practice Exam. MULTIPLE CHOICE 50. 5.80 g of dioxane (C 4 H 8 O 2 ) is how many moles of dioxane? 0.0658 mol 0.0707 mol 0.0725 mol d. 0.0804

### 602X10 21 602,000,000,000, 000,000,000,000 6.02X10 23. Pre- AP Chemistry Chemical Quan44es: The Mole. Diatomic Elements

Pre- AP Chemistry Chemical Quan44es: The Mole Mole SI unit of measurement that measures the amount of substance. A substance exists as representa9ve par9cles. Representa9ve par9cles can be atoms, molecules,

### CHEMICAL EQUATIONS and REACTION TYPES

31 CHEMICAL EQUATIONS and REACTION TYPES The purpose of this laboratory exercise is to develop skills in writing and balancing chemical equations. The relevance of this exercise is illustrated by a series

### Atomic Masses. Chapter 3. Stoichiometry. Chemical Stoichiometry. Mass and Moles of a Substance. Average Atomic Mass

Atomic Masses Chapter 3 Stoichiometry 1 atomic mass unit (amu) = 1/12 of the mass of a 12 C atom so one 12 C atom has a mass of 12 amu (exact number). From mass spectrometry: 13 C/ 12 C = 1.0836129 amu

### Chemical Reactions Chapter 8 Assignment & Problem Set

Chemical Reactions Name Warm-Ups (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

### Chapter 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) + 2O 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

### Mole - 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

### The Mole Concept and Atoms

Copyright The McGraw-Hill 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

### Chapter 6 Chemical Calculations

Chapter 6 Chemical Calculations 1 Submicroscopic Macroscopic 2 Chapter Outline 1. Formula Masses (Ch 6.1) 2. Percent Composition (supplemental material) 3. The Mole & Avogadro s Number (Ch 6.2) 4. Molar

### Sample Exercise 3.1 Interpreting and Balancing Chemical Equations

Sample Exercise 3.1 Interpreting and Balancing Chemical Equations The following diagram represents a chemical reaction in which the red spheres are oxygen atoms and the blue spheres are nitrogen atoms.

### Lecture Notes Chemistry E-1. Chapter 3

Lecture Notes Chemistry E-1 Chapter 3 http://inserbia.info/news/wp-content/uploads/2013/05/tamiflu.jpg http://nutsforhealthcare.files.wordpress.com/2013/01/tamiflu-moa.jpg The Mole A mole is a certain

### CHEMICAL INDUSTRY HOMEWORK

CHEMICAL INDUSTRY HOMEWORK 1. Which of the following can be classed as a raw material in the chemical industry? A. Iron ore B. Ammonia C. Methanol D. Petrol 2. Which of the following costs would be classed

### Chemical Proportions in Compounds

Chapter 3 Chemical Proportions in Compounds 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

### MASS RELATIONSHIPS IN CHEMICAL REACTIONS

MASS RELATIONSHIPS IN CHEMICAL REACTIONS 1. The mole, Avogadro s number and molar mass of an element. Molecular mass (molecular weight) 3. Percent composition of compounds 4. Empirical and Molecular formulas

### Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

### Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction

Reactions Chapter 8 Combustion Decomposition Combination Chapter 9 Aqueous Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte

### Calculations and Chemical Equations. Example: Hydrogen atomic weight = 1.008 amu Carbon atomic weight = 12.001 amu

Calculations and Chemical Equations Atomic mass: Mass of an atom of an element, expressed in atomic mass units Atomic mass unit (amu): 1.661 x 10-24 g Atomic weight: Average mass of all isotopes of a given

### B. 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

### Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

### Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Goal is to understand and become proficient at working with: 1. Avogadro's Number, molar mass and converting between mass and moles (REVIEW). 2. empirical formulas from analysis.

### Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.

### The mass of the formula unit is called the formula mass Formula masses are calculated the same way as molecular masses

Chapter 4: The Mole Atomic mass provides a means to count atoms by measuring the mass of a sample The periodic table on the inside cover of the text gives atomic masses of the elements The mass of an atom

### Mole Calculations Multiple Choice Review PSI Chemistry

Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela

### Ch.4 Solutions. Solutions for Practice Problems p Consider the following reaction. 2H 2(g) + O 2(g) 2H 2 O (l)

Solutions for Practice Problems p. 114 Ch.4 Solutions 1. Consider the following reaction. 2H 2(g) + O 2(g) 2H 2 O (l) (a) Write the ratio of H 2 molecules: O 2 molecules: H 2 Omolecules. The ratio is given

### Formulas, Equations and Moles

Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule

### Chapter 3 Calculation with Chemical Formulas and Equations

Chapter 3 Calculation with Chemical Formulas and Equations Practical Applications of Chemistry Determining chemical formula of a substance Predicting the amount of substances consumed during a reaction

### Chapter 4: Chemical and Solution Stoichiometry

Chapter 4: Chemical and Solution Stoichiometry (Sections 4.1-4.4) 1 Reaction Stoichiometry The coefficients in a balanced chemical equation specify the relative amounts in moles of each of the substances

### Stoichiometry. 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

### Appendix D. Reaction Stoichiometry D.1 INTRODUCTION

Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules

### The 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

### Solution : 22.4 dm 3 of a gas at STP 1 mol of gas molar mass of the gas Now, 4.48 dm 3 of NH 3 at STP 3.49 g dm 3 of NH 3 at STP.

Formulae 1. One mole of atoms Mass of elements Atomic mass Atomic mass 2. Mass of one atom 3 6.022 10 2 3. Number of moles (n) Mass of substance Molar mass of substance 4. Number of molecules n Avogadro

### HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A Oxidation-Reduction 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