Name: 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

Size: px
Start display at page:

Download "Name: 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"

Transcription

1 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. mass only b. mass and moles only c. mass, moles, and molecules only d. mass, moles, molecules, and volume 2. What is the first step in most stoichiometry problems? a. add the coefficients of the reagents b. convert given quantities to moles c. convert given quantities to volumes d. convert given quantities to masses 3. In the reaction 2CO + O 2 2CO 2, 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 4. Which of the following is true about the reaction shown below? C 5 (l) + 8O 2 5CO 2 + 6H 2 O a. 9 moles of reactants chemically change into 11 moles of product. b. 9 grams of reactants chemically change into 11 grams of product. c. 9 liters of reactants chemically change into 11 liters of product. d. 9 atoms of reactants chemically change into 11 atoms of product. 5. Which of the following is an INCORRECT interpretation of the balanced equation shown below? 2S + 3O 2 2SO 3 a. 2 atoms S + 3 molecules O 2 2 molecules SO 3 b. 2 g S + 3 g O 2 2 g SO 3 c. 2 mol S + 3 mol O 2 2 mol SO 3 d. 5 mol of reactants 2 mol of products 6. How many moles of aluminum are needed to react completely with 1.2 mol of FeO? 2Al + 3FeO 3Fe + Al 2 O 3 a. 1.2 mol b. 0.8 mol c. 1.6 mol d. 2.4 mol 1

2 Name: 7. Calculate the number of moles of Al 2 O 3 that are produced when 0.60 mol of Fe is produced in the following reaction. 2Al + 3FeO 3Fe + Al 2 O 3 a mol b mol c mol d mol 8. How many moles of glucose, C 6, can be "burned" biologically when 10.0 mol of oxygen is available? C 6 + 6O 2 6CO 2 + 6H 2 O(l) a mol b mol c mol d mol 9. Hydrogen gas can be produced by reacting aluminum with sulfuric acid. How many moles of sulfuric acid are needed to completely react with 15.0 mol of aluminum? 2Al + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 a mol b mol c mol d mol 10. When iron rusts in air, iron(iii) oxide is produced. How many moles of oxygen react with 2.4 mol of iron in the rusting reaction? 4Fe + 3O 2 2Fe2O 3 a. 1.2 mol b. 1.8 mol c. 2.4 mol d. 3.2 mol 11. At STP, how many liters of oxygen are required to react completely with 3.6 liters of hydrogen to form water? 2H 2 + O 2 2H 2 O a. 1.8 L b. 3.6 L c. 2.0 L d. 2.4 L 12. Which type of stoichiometric calculation does not require the use of the molar mass? a. mass-mass problems b. mass-volume problems c. mass-particle problems d. volume-volume problems 2

3 Name: 13. Aluminum reacts with sulfuric acid to produce aluminum sulfate and hydrogen gas. How many grams of aluminum sulfate would be formed if 250 g H 2 SO 4 completely reacted with aluminum? 2Al + 3H 2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 a g b. 290 g c. 450 g d. 870 g 14. How many liters of hydrogen gas are needed to react with CS 2 to produce 2.50 L of CH 4 at STP? 4H 2 +CS 2 (l) CH 4 + 2H 2 S a L b L c L d L 15. Which conversion factor do you use first to calculate the number of grams of CO 2 produced by the reaction of 50.6 g of CH 4 with O 2? The equation for the complete combustion of methane is: CH 4 + 2O 2 CO 2 +2H 2 O(l) a. 1 mol CH 4 /16.0 g CH 4 b. 2 mol O 2 /1 mol CO 2 c g CH 4 /1 mol CO 4 d g CO 2 /2 mol CO How many liters of NH 3 are needed to react completely with 30.0 L of NO (at STP)? 4NH 3 + 6NO 5N 2 + 6H 2 O a. 5.0 L b L c. 7.5 L d L 17. Glucose, C 6, is a good source of food energy. When it reacts with oxygen, carbon dioxide and water are formed. How many liters of CO 2 are produced when 126 g of glucose completely react with oxygen? C 6 + 6O 2 6CO 2 + 6H 2 O(l) kcal a L b L c L d L 3

4 Name: 18. Calcium oxide, or lime, is produced by the thermal decomposition of limestone in the reaction CaCO 3 Δ CaO + CO 2. What mass of lime can be produced from kg of limestone? a kg b kg c. 8.4 kg d. none of the above 19. How many grams of chromium are needed to react with an excess of CuSO 4 to produce 27.0 g Cu? 2Cr + 3CuSO 4 (aq) Cr 2 (SO 4 ) 3 (aq) + 3Cu a g b g c g d g 20. How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water.) Be + 2H 2 O(l) Be(OH) 2 (aq) + H 2 a g b g c. 162 g d. 324 g 21. What is the maximum number of grams of PH 3 that can be formed when 6.2 g of phosphorus reacts with 4.0 g of hydrogen to form PH 3? P 4 + 6H 2 4PH 3 a g b. 6.8 g c. 270 g d. 45 g 22. Methane and hydrogen sulfide form when hydrogen reacts with carbon disulfide. Identify the excess reagent and calculate how much remains after 36 L of H 2 reacts with 12 L of CS 2. 4H 2 + CS 2 CH 4 + 2H 2 S a. 3 L CS 2 b. 6 L CS 2 c. 9 L CS 2 d. 12 L H 2 4

5 Name: 23. Which of the following would be the limiting reagent in the reaction shown below? 2H 2 + O 2 2H 2 O a. 50 molecules of H 2 b. 50 molecules of O 2 c. Neither a nor b is limiting. d. Both a and b are considered limiting reagents. 24. Which of the following is true about "yield"? a. The value of the actual yield must be given in order for the percent yield to be calculated. b. The theoretical yield is always the same as the actual yield. c. The percent yield may be different from the theoretical yield because reactions do not always go to completion. d. The actual yield may be different from the theoretical yield because insufficient limiting reagent was used. 25. Hydrogen gas is produced when zinc reacts with hydrochloric acid. If the actual yield of this reaction is 85%, how many grams of zinc are needed to produce 112 L of H 2 at STP? Zn + 2HCl(aq) ZnCl 2 + H 2 a. 95 g b. 180 g c. 280 g d. 380 g 5

6 Chpt 12 review Answer Section MULTIPLE CHOICE 1. ANS: D PTS: 1 DIF: L2 REF: p. 389 OBJ: Describe the quantities you can use to interpret a balanced chemical equation. 2. ANS: B PTS: 1 DIF: L1 REF: p. 394 BLM: knowledge 3. ANS: C PTS: 1 DIF: L2 REF: p ANS: A PTS: 1 DIF: L2 REF: p. 386 p. 387 OBJ: Describe the quantities you can use to interpret a balanced chemical equation. 5. ANS: B PTS: 1 DIF: L2 REF: p. 386 p. 387 OBJ: Describe the quantities you can use to interpret a balanced chemical equation. 6. ANS: B PTS: 1 DIF: L2 REF: p. 390 p ANS: A PTS: 1 DIF: L2 REF: p. 390 p ANS: B PTS: 1 DIF: L2 REF: p. 390 p ANS: D PTS: 1 DIF: L2 REF: p. 390 p ANS: B PTS: 1 DIF: L2 REF: p. 390 p ANS: A PTS: 1 DIF: L2 REF: p. 394 p ANS: D PTS: 1 DIF: L2 REF: p. 396 BLM: comprehension 13. ANS: B PTS: 1 DIF: L2 REF: p. 392 p ANS: D PTS: 1 DIF: L2 REF: p

7 15. ANS: A PTS: 1 DIF: L2 REF: p ANS: B PTS: 1 DIF: L2 REF: p ANS: D PTS: 1 DIF: L2 REF: p. 392 p ANS: B PTS: 1 DIF: L2 REF: p. 392 p ANS: A PTS: 1 DIF: L2 REF: p ANS: C PTS: 1 DIF: L2 REF: p ANS: B PTS: 1 DIF: L2 REF: p ANS: A PTS: 1 DIF: L2 REF: p ANS: B PTS: 1 DIF: L2 REF: p ANS: D PTS: 1 DIF: L2 REF: p. 405 OBJ: Explain what the percent yield of a reaction measures. 25. ANS: D PTS: 1 DIF: L3 REF: p. 406 p. 408 OBJ: Explain what the percent yield of a reaction measures. 2

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date» Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent

More information

Slide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass

Slide 1 / 90. Slide 2 / 90. Slide 3 / 90 A B. percent yield stoichiometry A B. atoms and mass Stoichiometry HW Slide 1 / 90 Grade:«grade» Subject: ate:«date» 1 The calculation of quantities in chemical equations is called. Slide 2 / 90 accuracy and precision dimensional analysis percent composition

More information

CHAPTER 12. Chemists use balanced to calculate how much reactant is needed or product is formed in a reaction. + 3H 2NH. Hon Chem 12.

CHAPTER 12. Chemists use balanced to calculate how much reactant is needed or product is formed in a reaction. + 3H 2NH. Hon Chem 12. CHAPTER 12 Stoichiometry is the calculation of quantities using different substances in chemical equations. Based on the Law of Conservation of Mass. Mg(s) + How many moles of H Chemists use balanced to

More information

Practice Problems Stoich!

Practice Problems Stoich! Practice Problems Stoich! Name: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS

More information

UNIT 1 Chemical Reactions Part II Workbook. Name:

UNIT 1 Chemical Reactions Part II Workbook. Name: UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the

More information

Name Date Class. Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line.

Name Date Class. Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. 12 STOICHIOMETRY Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. 1. 2. 3. 4. 5. Column A the substance

More information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs

More information

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry Stoichiometry The quantitative study of reactants and products in a chemical reaction 1 Stoichiometry Whether the units given for reactants or products are moles, grams, liters (for gases), or some other

More information

Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass,

Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, Stoichiometry Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, volume, and heat of reaction. Stoichiometry

More information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for

More information

Mole Conversions Worksheet

Mole Conversions Worksheet Mole Conversions Worksheet There are three mole equalities. They are: 1 mol = 6.02 x 10 particles 1 mol = g-formula-mass (periodic table) 1 mol = 22.4 L for a gas at STP Each equality can be written as

More information

Study Guide: Stoichiometry

Study Guide: Stoichiometry Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE

More information

(DO NOT WRITE ON THIS TEST)

(DO NOT WRITE ON THIS TEST) Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation

More information

Answer questions 1a 1d. Color leaf one the color that corresponds to the answer that is used twice.

Answer questions 1a 1d. Color leaf one the color that corresponds to the answer that is used twice. Station 1 Answer questions 1a 1d. Color leaf one the color that corresponds to the answer that is used twice. Outline the leaf in one of the other colors. Polka-dot the leaf in the third color. 1a. Which

More information

Unit 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 information

Chapter 9: Stoichiometry The Arithmetic ti Of Equations

Chapter 9: Stoichiometry The Arithmetic ti Of Equations Chapter 9: Stoichiometry The Arithmetic of Equations Chemical Calculations Limiting Reagent and Percent Yield The Arithmetic ti Of Equations -- The Arithmetic of Equations -- Using Everyday Equations Stoichiometry

More information

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +

More information

Stoichiometric Calculations

Stoichiometric Calculations Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Table of Contents Click on the topic to go to that section Stoichiometry Calculations with Moles Stoichiometry Calculations with Particles

More information

Stoichiometric Calculations

Stoichiometric Calculations Slide 1 / 109 Slide 2 / 109 Stoichiometric Calculations Slide 3 / 109 Slide 4 / 109 Table of Contents Stoichiometry Calculations with Moles Click on the topic to go to that section Stoichiometry Calculations

More information

General Chemistry 1 CHM201 Unit 2 Practice Test

General 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 information

11 Stoichiometry. Section 11.1 What is stoichiometry?

11 Stoichiometry. Section 11.1 What is stoichiometry? 11 Stoichiometry Section 11.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1.. 3. 4. 5. The study of the quantitative

More information

Name Date Class THE ARITHMETIC OF EQUATIONS

Name Date Class THE ARITHMETIC OF EQUATIONS 12.1 THE ARITHMETIC OF EQUATIONS Section Review Objectives Calculate the amount of reactants required or product formed in a nonchemical process Interpret balanced chemical equations in terms of interacting

More information

Practice questions for Ch. 3

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

More information

Ch 9 Stoichiometry Practice Test

Ch 9 Stoichiometry Practice Test Ch 9 Stoichiometry Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A balanced chemical equation allows one to determine the a. mole ratio

More information

SIC CONCEPTS TS OF CHEMISTRY. Unit. I. Multiple Choice Questions (Type-I)

SIC 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 information

Name Date Class STUDY GUIDE FOR CONTENT MASTERY

Name Date Class STUDY GUIDE FOR CONTENT MASTERY Stoichiometry Section 12.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1. The study of the quantitative relationships

More information

Chapter 9 STOICHIOMETRY

Chapter 9 STOICHIOMETRY Chapter 9 STOICHIOMETRY Section 9.1 The Arithmetic of Equations OBJECTIVE Calculate the amount of reactants required or product formed in a nonchemical process. Section 9.1 The Arithmetic of Equations

More information

Honors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?

Honors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula

More information

Chapter 12 Stoichiometry. Mr. Mole

Chapter 12 Stoichiometry. Mr. Mole Chapter 12 Stoichiometry Mr. Mole Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double or triple the amount

More information

Chemical Equations 10/30/13. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions

Chemical Equations 10/30/13. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions. Types of Chemical Reactions Chemical Equations A chemical equation just like a mathematical equation is a way to express, in symbolic form, the reactions occurring in a chemical system. n Balancing chemical equations n Reaction stoichiometry

More information

Example Exercise 10.1 Interpreting Chemical Equation Calculations

Example Exercise 10.1 Interpreting Chemical Equation Calculations Example Exercise 10.1 Interpreting Chemical Equation Calculations Given the chemical equation for the combustion of methane, CH 4, balance the equation and interpret the coefficients in terms of (a) moles

More information

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product?

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product? Unit 6: Stoichiometry How do manufacturers know how to make enough of their desired product? Chocolate Chip Cookies Using the following recipe, complete the questions. Cookie Recipe 1.5 c sugar 1 c. butter

More information

5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams.

5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams. CHEMISTRY TEST NAME: MASS AND VOLUME DATE: EQUATION RELATIONSHIPS Directions: For each of the following questions, choose the number that best answers the question and place it on your answer sheet. Directions:

More information

Chapter 9. Stoichiometry. Mr. Mole. NB page 189

Chapter 9. Stoichiometry. Mr. Mole. NB page 189 Chapter 9 Stoichiometry Mr. Mole NB page 189 review Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double

More information

Unit 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. 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 information

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

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

More information

Usual Atomic Charges of Main Group Elements

Usual Atomic Charges of Main Group Elements Usual Atomic Charges of Main Group Elements +1 +2 +3 +4 +5 +6 +7-5 -4-3 -2-1 Examples SO 3 sulfur trioxide CO 2 carbon dioxide Al 2 O 3 aluminum trioxide IF 7 iodine heptafluoride Fig. 2-6, p.63 Chemical

More information

Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Chem. I Notes Ch. 11 STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 11.1 notes 1 MOLE = 6.02 x 10 23 representative particles representative particles

More information

Stoichiometry. Mr. Mole

Stoichiometry. Mr. Mole Stoichiometry Mr. Mole Let s make some Cookies! When baking cookies, a recipe is usually used, telling the exact amount of each ingredient. If you need more, you can double or triple the amount Thus, a

More information

Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Ch. 10 Notes STOICHIOMETRY NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles representative particles = ATOMS, IONS,

More information

Quantity Relationships in Chemical Reactions

Quantity Relationships in Chemical Reactions Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number

More information

UNIT 9 - STOICHIOMETRY

UNIT 9 - STOICHIOMETRY General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

Stoichiometry. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas.

Stoichiometry. Consider the reaction in which the reactants are nitrogen gas and hydrogen gas. They produce the product ammonia gas. 1 1. Interpreting Chemical Equations Stoichiometry Calculations using balanced equations are called stoichiometric calculations. The starting point for any problem involving quantities of chemicals in

More information

Name. Practice Test 2 Chemistry 111

Name. Practice Test 2 Chemistry 111 Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba

More information

2. In which of these compounds are there twice as many oxygen atoms as hydrogen atoms? a. H 3 PO 4 c. HClO 3 b. H 2 SO 4 d. H 2 O

2. In which of these compounds are there twice as many oxygen atoms as hydrogen atoms? a. H 3 PO 4 c. HClO 3 b. H 2 SO 4 d. H 2 O Test Review Unit 3_3: Law of conservation of mass Identify the letter of the choice that best completes the statement or answers the question. At the end of the file you can find chemical equations to

More information

AP Chemistry: Chapter 3 Notes Outline

AP Chemistry: Chapter 3 Notes Outline AP Chemistry: Chapter 3 Notes Outline Objectives: Balance chemical equations Use dimensional analysis to solve stoichiometric problems Use dimensional analysis to do limiting reactant problems Use dimensional

More information

Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a

Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts

More information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information

actual yield (p. 372) excess reagent (p. 369) mole-mole relationship for ag bw: x mol G b mol W a mol G xb a mol W Organizing Information 12 Study Guide 12 Study Guide Study Tip Prioritize Schedule your time realistically. Stick to your deadlines. If your class subscribes to the Interactive Textbook with ChemASAP, your students can go online

More information

Chemistry B11 Chapter 5 Chemical reactions

Chemistry 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 information

TOPIC 4: THE MOLE CONCEPTS

TOPIC 4: THE MOLE CONCEPTS TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal

More information

Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations

Chapter 9. Table of Contents. Stoichiometry. Section 1 Introduction to Stoichiometry. Section 2 Ideal Stoichiometric Calculations Stoichiometry Table of Contents Section 1 Introduction to Stoichiometry Section 2 Ideal Stoichiometric Calculations Section 3 Limiting Reactants and Percentage Yield Section 1 Introduction to Stoichiometry

More information

CHAPTER 11 Stoichiometry Defining Stoichiometry

CHAPTER 11 Stoichiometry Defining Stoichiometry CHAPTER 11 Stoichiometry 11.1 Defining Stoichiometry Stoichiometry is the study of quantitative relationships between amounts of reactants used and products formed by a chemical reaction. Stoichiometry

More information

Unit 9 Stoichiometry Notes

Unit 9 Stoichiometry Notes Unit 9 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 to

More information

Unit IV: Stoichiometry

Unit IV: Stoichiometry Unit IV: Stoichiometry D. Calculations from chemical equations 1. Mol-mol calculations 2. Mol-gram calculations 3. Gram-gram calculations E. Limiting reactant (or reagent) F. Other applications of stoichiometry

More information

The Mole. Relative Atomic Mass Ar

The 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 information

CH. 12 STOICHIOMETRY

CH. 12 STOICHIOMETRY CH. 12 STOICHIOMETRY Balanced Chemical Equations Used to calculate: How much of each reactant is needed How much product will form If you know one quantity you can calculate the rest. Quantity may be in

More information

Unit 4: Reactions and Stoichiometry

Unit 4: Reactions and Stoichiometry Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)

More information

Chapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard

Chapter 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 information

CH 221 Chapter Four Part II Concept Guide

CH 221 Chapter Four Part II Concept Guide CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are

More information

Unit Five MC Practice Dec. 5, 2016

Unit Five MC Practice Dec. 5, 2016 Unit Five: Stoichiometry Name Unit Five MC Practice Dec. 5, 2016 In the space provided, write the letter of the term or phrase that best completes each sentence or best answers each question. 1. Stoichiometry

More information

Limiting Reactants. and Percentage Yield. Section 3

Limiting Reactants. and Percentage Yield. Section 3 GO ONLINE Section 3 8E Main Ideas One reactant limits the product of a reaction. Comparing the actual and theoretical yields helps chemists determine the reaction s efficiency. 8E perform stoichiometric

More information

3. Carbon disulfide is an important organic solvent. It can be produced from sulfur dioxide, a byproduct of buring coal.

3. Carbon disulfide is an important organic solvent. It can be produced from sulfur dioxide, a byproduct of buring coal. L3 Chemistry: Stoichiometry: Unit 8: Name Page 1 Mol mol problems: (use only step 2 on the back)! (Chapter 9, p. 237-244)! 4 P + 5 O 2 > 2 P 2 O 5! How many mol of P 2 O 5 are made from 12 mol P? 12 mol

More information

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance

More information

Notes: Balancing Chemical Equations

Notes: Balancing Chemical Equations Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely

More information

Chapter 3 The Mole and Stoichiometry

Chapter 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 information

9.2 Chemical Calcualtions. Chapter 9 Stoichiometry. 9.1 The Arithmetic of Equations. 9.2 Chemical Calculations. 9.3 Limiting Reagent and Percent Yield

9.2 Chemical Calcualtions. Chapter 9 Stoichiometry. 9.1 The Arithmetic of Equations. 9.2 Chemical Calculations. 9.3 Limiting Reagent and Percent Yield 9.2 Chemical Calcualtions Chapter 9 Stoichiometry 9.1 The Arithmetic of Equations 9.2 Chemical Calculations 9.3 Limiting Reagent and Percent Yield 1 Copyright Pearson Education, Inc., or its affiliates.

More information

Name: Unit 9- Stoichiometry Day Page # Description IC/HW

Name: Unit 9- Stoichiometry Day Page # Description IC/HW Name: Unit 9- Stoichiometry Day Page # Description IC/HW Due Date Completed ALL 2 Warm-up IC 1 3 Stoichiometry Notes IC 1 4 Mole Map IC X 1 5 Mole to Mole Practice IC 1 6 Mass to Mole Practice IC 1/2 X

More information

Chapter 9 The Chemical Reaction Equation and Stoichiometry 9.1 Stoichiometry

Chapter 9 The Chemical Reaction Equation and Stoichiometry 9.1 Stoichiometry Chapter 9 The Chemical Reaction Equation and Stoichiometry 9.1 Stoichiometry The stoichiometric coefficients in the chemical reaction equation Is (1 for C 7 H 16, 11 for O 2 and so on). Another way to

More information

Calculations with Chemical Formulas and Equations

Calculations 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 information

Name AP Chemistry September 30, 2013

Name AP Chemistry September 30, 2013 Name AP Chemistry September 30, 2013 AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the blue side of your scantron for each of the

More information

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg? 1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams

More information

CHAPTER 9: STOICHIOMETRY

CHAPTER 9: STOICHIOMETRY 9.1 Interpreting a chemical Equation CHAPTER 9: STOICHIOMETRY H 2 (g) + Cl 2 (g) 2 HCl (g) 1 molecule 1 molecule 2 molecules N 2 + 3 H 2 (g) 2 NH 3 (g) molecule(s) molecule(s) molecule(s) It follows that

More information

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.

TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses

More information

General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction

General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information

Balancing Chemical Reactions. CHAPTER 3: Quantitative Relationships in Chemical Reactions. Zn + HCl ZnCl 2 + H 2. reactant atoms product atoms

Balancing 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 information

Stoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT

Stoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT Unit 10 Resournces Name Academic Chemistry Stoichiometry Homework On-Time LATE DATE ASSIGNMENT 100 70 10.1 10.2 10.3 10.4 10.5 10.6 EC 16 cincochem.pbworks.com Stoichiometry Live in the now. Garth Algar

More information

Chapter 3. Stoichiometry

Chapter 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 information

Stoichiometry Chapter 9 Practice Assessment B

Stoichiometry Chapter 9 Practice Assessment B NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions:

More information

Chapter 9. Chemical Quantities

Chapter 9. Chemical Quantities Chapter 9 Chemical Quantities Section 9.1 Information Given by Chemical Equations A balanced chemical equation gives relative numbers (or moles) of reactant and product molecules that participate in a

More information

AP Chapter 3 Study Questions

AP Chapter 3 Study Questions Class: Date: AP Chapter 3 Study Questions True/False Indicate whether the statement is true or false. 1. The mass of a single atom of an element (in amu) is numerically EQUAL to the mass in grams of 1

More information

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq)

1) Write the reaction for Calcium and nitrogen reacting. 3) What element on the periodic table is the largest? 3)Name these. a) H2S (aq) b) HNO 3 (aq) 1) Write the reaction for Calcium and nitrogen reacting 3) What element on the periodic table is the largest? 3)Name these a) H2S (aq) b) HNO 3 (aq) Stoichiometry: mathematical relationships in formulas

More information

Quantitative Relationships in Chemical Reactions Chapter 7

Quantitative Relationships in Chemical Reactions Chapter 7 Quantitative Relationships in Chemical Reactions Chapter 7 The burning of charcoal releases heat (thermal energy) that grills our food. But the combustion of charcoal and fossil fuels also releases CO

More information

CH 221 Chapter Four Part I Concept Guide

CH 221 Chapter Four Part I Concept Guide 1. Balancing Chemical Equations CH 221 Chapter Four Part I Concept Guide Description When chlorine gas, Cl 2, is added to solid phosphorus, P 4, a reaction occurs to produce liquid phosphorus trichloride,

More information

Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri

Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How

More information

CHEM 120: Introduction to Inorganic Chemistry. Chapters Covered and Test dates. The mole concept and atoms. Avogadro s number

CHEM 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 information

Chapter 3: Chemical Reactions and the Earth s Composition

Chapter 3: Chemical Reactions and the Earth s Composition Chapter 3: Chemical Reactions and the Earth s Composition Problems: 3.1-3.3, 3.5, 3.11-3.86, 3.95-3.115, 3.119-3.120, 3.122, 3.125-3.128, 3.132, 3.134, 3.136-3.138-3.141 3.2 The Mole Stoichiometry (STOY-key-OM-e-tree):

More information

Chemistry I Chapter 9 Stoichiometry Objective Sheet. Equation 1. Objectives: 1. Define stoichiometry

Chemistry I Chapter 9 Stoichiometry Objective Sheet. Equation 1. Objectives: 1. Define stoichiometry Chemistry I Chapter 9 Stoichiometry Objective Sheet Equation 1 2 C 2 H 2 (g) + 5 O 2 (g) 4 CO 2 (g) + 2 H 2 O (g), at STP C 2 H 2 (acetylene) 26 g/mol O 2 32 g/mol CO 2 44 g/mol H 2 O 18 g/mol Objectives:

More information

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,

More information

Unit 6: React ions & St oichiom et ry, Chapt er s 11 & 12. Nam e: Period: Description Reaction Types Activty

Unit 6: React ions & St oichiom et ry, Chapt er s 11 & 12. Nam e: Period: Description Reaction Types Activty Unit 6: React ions & St oichiom et ry, Chapt er s 11 & 12 Nam e: Period: Unit Goals- As you work through this unit, you should be able to: 1. Write formula equations from word equations using appropriate

More information

1 Some Basic Concepts of Chemistry

1 Some Basic Concepts of Chemistry 1 Some Basic Concepts of Chemistry Multiple Choice Questions (MCQs) Q. 1 Two students performed the same experiment separately and each one of them recorded two readings of mass which are given below.

More information

A. Correct. You successfully completed the stoichiometry problem. B. Incorrect. There are 2 moles of AgCl produced for each mole of CaCl 2 reacted.

A. Correct. You successfully completed the stoichiometry problem. B. Incorrect. There are 2 moles of AgCl produced for each mole of CaCl 2 reacted. MCAT General Chemistry Problem Drill 18: Stoichiometry Question No. 1 of 10 1. How many grams of AgCl will precipitate out if 0.27 mole is reacted? + 2 AgNO 3 2 AgCl + Ca(NO 3 ) 2 Question #01 (A) 77 g

More information

Basic Concepts of Chemistry Notes for Students [Chapter 7, page 1] D J Weinkauff - Nerinx Hall High School

Basic Concepts of Chemistry Notes for Students [Chapter 7, page 1] D J Weinkauff - Nerinx Hall High School Basic Concepts of Chemistry Notes for Students [Chapter 7, page 1] Chapter 7 Quantitative Relationships in Chemical Reactions As you have begun to see, chemistry is a quantitative science involving a great

More information

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 10 Chemical Equation Calculations by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 10 1 What

More information

VOCABULARY Define. 1. stoichiometry. 2. composition stoichiometry. 3. reaction stoichiometry. 4. unknown. 5. mole ratio

VOCABULARY Define. 1. stoichiometry. 2. composition stoichiometry. 3. reaction stoichiometry. 4. unknown. 5. mole ratio CHAPTER 9 HOMEWORK 9-1 (pp. 275 279) Define. 1. stoichiometry 2. composition stoichiometry 3. reaction stoichiometry 4. unknown 5. mole ratio SKILL BUILDER On a separate sheet of paper, write five possible

More information

Stoichiometry. 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 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 information

(2 x 22.4 L H 2 ) + (1 x 22.4 L O 2 ) (2 OBJECTIVES:

(2 x 22.4 L H 2 ) + (1 x 22.4 L O 2 ) (2 OBJECTIVES: Chapter 9 The calculations of quantities in a chemical reaction chemical bookkeeping Section 9.1 The Arithmetic of Equations OBJECTIVES: Calculate the amount of reactants required, or product formed, in

More information

**continued on next page**

**continued on next page** Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants

More information

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 )

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 ) Homework Stoichiometry 1.) An oxide of iron has the formula Fe 3 O 4. What mass percent of iron does it contain? (72.360%) 2.) Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed

More information

General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction

General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

More information