O 2. Cl 2. SbCl 3. NaBr. NaCl
|
|
|
- Cordelia Briggs
- 6 years ago
- Views:
Transcription
1 Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations 6.6 The Mole 1. Mg + O 2 à MgO Mg, O 2, and MgO are there? Mg: MgO? Mg O 2 MgO O 2:Mg? 2. Sb + Cl 2 à SbCl 3 Sb Cl 2 SbCl 3 Sb: Cl 2? 3. NaBr + Cl 2 à NaCl + Br 2 NaBr Cl 2 NaCl Br 2 NaBr: Br 2? Br 2: NaBr? 4. NaClO 3 à NaCl + O 2 NaClO 3 NaCl O 2 NaCl: NaClO 3? 5. Fe + HCl à FeCl 2 + H 2 Fe HCl Fe: FeCl 2?
2 FeCl 2 H 2 6. N 2 + O 2 à N 2O 5 N 2 O 2 N 2O 5 N 2O 5: N 2? 7. MgCO 3 à MgO + CO 2 MgCO 3 MgO CO 2 MgO: CO 2? CO 2 : MgO? 8. MgBr 2 + Cl 2 à MgCl 2 + Br 2 MgBr 2 Cl 2 MgCl 2 Br 2 MgBr 2 : MgCl 2? 9. Zn + CuSO 4 à Cu + ZnSO 4 Zn CuSO 4 Cu ZnSO 4 Cu: Zn? 10. NH4NO2 à N2 + H2O NH4NO2 N2 H2O H2O : NH4NO2?
3 Example 1: Using the chemical equation below: Stoichiometry Part I: Mole to Mole 2 Al + 3 CuSO 4 à Al 2(SO 4) Cu What is the number of moles of Al needed if 9 moles of Cu is produced? Step 1. Write the given (include units!). Step 2. What are we looking for (include units!) Given= Want to know: Step 3. What is the mole-to-mole ratio between the given and the compound we are looking for? Step 4: List the given first and then multiply it by the ratio we found in step 3 so that the unit for what we want to know is the only factor left over. Example 2: Using the chemical equation below: 4Fe(s) + 3O 2(g) à 2Fe 2O 3(s) If 10 moles of Fe is used, how many moles of Fe 2O 3 is produced? Step 1. Write the given (include units!). Given= Step 2. What are we looking for (include units!) Want to know: Step 3. What is the mole-to-mole ratio between the given and the compound we are looking for? Step 4: List the given first and then multiply it by the ratio we found in step 3 so that the unit for what we want to know is the only factor left over. Example 3: Using the chemical equation below: N 2O 5 + H 2O à 2HNO 3 HNO 3 is produced if 17 moles of H 2O is reacted? Example 4: Given the reaction: Ca + 2H 2O Ca(OH) 2 + H 2 What is the total number of moles of Ca needed to react completely with 4.0 moles of H 2O? (1) 1.0 (2) 2.0 (3) 0.50 (4) 4.0
4 Practice Part I: Mole-to-mole conversion (complete on loose leaf!) 1. Determine the number of moles of Ca produced when you start with 3 moles of CaCl 2 in the chemical reaction: CaCl 2 à Ca + Cl 2 2. Determine the number of moles of MgO produced when you start with 4 moles of Mg in the chemical reaction: 2 Mg + O 2 à 2 MgO 3. Determine the number of moles of MgO produced when you start with 5 moles of O 2 in the chemical reaction: 2 Mg + O 2 à 2 MgO. 4. Some dry chemicals can be used to put out forest fires. One of these chemicals is NaHCO 3. When NaHCO 3(s) is heated, one of the products is CO 2(g), as shown in the balanced equation below. 2 NaHCO 3 + heat à Na 2CO 3 (s) + H 2O (g) + CO 2 (g) a) Show the correct numerical setup for calculating the percent composition by mass of carbon in the product Na 2CO 3. b) Determine the total number of moles of CO 2(g) produced when 7.0 moles of NaHCO 3(s) is completely reacted. Stoichiometry Part II: Moles Grams! Example 1: What is the mass of 4.76 moles of Na 3PO 4 (gram-formula mass = 164 grams/mole)? Step 1. List the given. (Write units!) Given = Need to find = Well in this case, we already have it: Gram formula mass of = Step 4. Set up by listing the given first and multiply it the gram-formula mass we found in step 3 so that the unit for what we want to know is the only factor left over. Example 2: What is the mass of 5.36 moles of H 2O? Step 1. List the given. (Write units!) Given = Need to find =
5 Gram formula mass of = Step 4. Set up by listing the given first and multiply it the gram-formula mass we found in step 3 so that the unit for what we want to know is the only factor left over. Stoichiometry Part III: Gram-to-mole conversions We can convert from gram-to-mole using the same method. Example 1: Determine the total number of moles of CH 3Br in 19 grams of CH 3Br (gram-formula mass = 95 grams/mol). Step 1. List the given. (Write units!) Given = Need to find = Well in this case, we already have it: Gram formula mass of = Step 4. Set up by listing the given first and multiply it by the gram-formula mass we found in step 3 so that the unit for what we want to know is the only factor left over. Example 2: What is the total number of moles in 80.0 grams of C 2H 5Cl (gram-formula mass = 64.5 grams/mol). Step 1. List the given. (Write units!) Given = Need to find =
6 Well in this case, we already have it: Gram formula mass of = Step 4. Set up by listing the given first and multiply it by the gram-formula mass we found in step 3 so that the unit for what we want to know is the only factor left over. Part II: Mole-to-gram Conversions Practice! 5. What is the mass of 4 moles of Li? 6. Approximately how many grams of HCl do you have if there are 3 moles of HCl? 7. Approximately how many grams of H 2SO 4 do you have if there are 2 moles of H 2SO 4? Part III: Gram-to-mole conversion 8. Approximately how many moles of Na do you have if there are 69 grams of Na? 9. Approximately how many moles of KCl do you have if there are 150 grams of KCl? 10. Approximately how many moles of H 2SO 4 do you have if there are 392 grams of H 2SO 4? Additional Practice/Homework: 1. According to the reaction 2Al + 3H 2SO 4 à 3H 2 + Al 2(SO 4) 3, the total number of moles of H 2SO 4 needed to react completely with 5 mol of Al is (1) 2.5 mol (2) 5 mol (3) 7.5 mol (4) 9 mol 2. Given the equation N 2 + 3H 2 à 2NH 3, what is the total number of moles of NH 3 produced when 10 mol of H 2 reacts completely with N 2? (1) 2 mol (2) 3 mol (3) 6.7 mol (4) 15 mol 3. The process of photosynthesis can be represented by the following equation, 6CO 2 + 6H 2O + energy à C 6H 12O 6 + 6O 2 If 4 mol of C 6H 12O 6 is produced by the process, how many moles of CO 2 and H 2O were used? 4. Given the equation Mg + 2HCl à MgCl 2 + H 2, how many moles of HCl are needed to react with 0.5 mol of magnesium? (1) 0.5 mol (2) 1 mol (3) 2 mol (4) 4 mol 5. Consider the following equation: 2C 2H 6 + O 2 à 4CO 2 + 6H 2O When 4 mol of C 2H 6 are burned the number of moles of CO 2 produced will be (1) 2 mol (2) 6 mol (3) 7 mol (4) 8 mol
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
Practice Packet Unit 6: Moles & Stoichiometry
Regents Chemistry: Mr. Palermo Practice Packet Unit 6: Moles & Stoichiometry 1 LESSON 1: Moles and Molar Mass 1. Put an M if the substance is molecular/covalent, an I if ionic under the formula listed.
Chemical Reactions. Chemical Reactions 5 signs/evidence of chemical reactions:
Chemical Reactions Chemical Reactions 5 signs/evidence of chemical reactions: Chemical Reaction: a process in which one or more substances are converted into new substances with different chemical and
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
What is stoichiometry? It comes from the Greek word stoicheion, which means element, and metron, meaning measure.
Stoichiometry What is stoichiometry? It comes from the Greek word stoicheion, which means element, and metron, meaning measure. It involves the mass relationships between reactants and products in a chemical
Practice Packet Unit 7: Moles & Stoichiometry
PRACTICE PACKET: Unit 7 Moles & Stoichiometry Regents Chemistry: Practice Packet Unit 7: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 6: Lesson 2: Lesson 4A: Lesson 4B: Lesson 3: Lesson 5: www.chempride.weebly.com
15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g
CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO
Chemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
CHAPTER 1 QUANTITATIVE CHEMISTRY
Page 4 Ex 4 (a) element; (b) mixture; (c) compound; (d) element; (e) compound 5. (a) mixture; (b) compound; (c) mixture; (d) element; (e) compound. Page 5 Ex 1.1 3. C 4. D 5. C 6. D 7. a) 0.20 b) 1.2 10
AP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry
Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry Name /108 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing
Unit 5: Chemical Equations and Reactions & Stoichiometry
pg. 10 Unit 5: Chemical Equations and Reactions & Stoichiometry Chapter 8: Chemical Equations and Reactions 8.1: Describing Chemical Reactions Selected Chemistry Assignment Answers (Section Review on pg.
Chemistry. Bridging the Gap Summer Homework. Name..
Chemistry Bridging the Gap Summer Homework Name.. Standard Form Number Number in standard form 0.008 8 x 10-3 0.07 7 x 10-2 0.55 5.5 x 10-1 0.000052 0.048 0.0086 0.00086 0.000086 0.0000000001 0.000455
Solutions to the Extra Problems for Chapter 8
Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.
The coefficients of a balanced chemical equation tell us how many of each species are involved in the reaction.
Stoichiometry Chemical Equations Reactants are written on the left side of the arrow and products are written on the right side of the arrow. The Law of Conservation of Mass tells us that the number of
Concentration of Solutions
Solutions We carry out many reactions in solutions Remember that in the liquid state molecules move much easier than in the solid, hence the mixing of reactants occurs faster Solute is the substance which
Worksheet 1: REPRESENTATIVE PARTICLES
Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is
1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
Practice Packet Unit 3: Moles & Stoichiometry
PRACTICE PACKET: Unit 3 Moles & Stoichiometry Regents Chemistry: Mr. Palermo Practice Packet Unit 3: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson
Broughton High School
Name: Section: Chapter 21 Chemical Reactions Vocabulary Words 1. Balanced Chemical Reactions 2. Catalyst Broughton High School 3. Chemical Equation 4. Chemical Reaction 5. Coefficient 6. Combustion Reaction
Name: Date: Period: Page: Balancing Equations
Name: Date: Period: Page: Balancing Equations In a chemical reaction, one or more reactants change into one or more products. Chemists use chemical equations as a quick shorthand notation to convey as
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
Questions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..
Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative
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
Problem Set III Stoichiometry - Solutions
Chem 121 Problem set III Solutions - 1 Problem Set III Stoichiometry - Solutions 1. 2. 3. molecular mass of ethane = 2(12.011) + 6(1.008) = 30.07 g 4. molecular mass of aniline = 6(12.011) + 7(1.008) +
Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities
Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Micro World atoms & molecules Macro World grams Atomic mass is the mass of an atom in
Unit Learning Targets (L.T.):
Unit 9: Chemical Equations and Reactions Chapters 8 and 19 Name Block Unit Learning Targets (L.T.): By the end of the unit, students will be able to: Chapter 8: 1. Correctly write and balance chemical
Unit 7: Stoichiometry Homework Packet (85 points)
Name: Period: By the end of the Unit 7, you should be able to: Chapter 12 1. Use stoichiometry to determine the amount of substance in a reaction 2. Determine the limiting reactant of a reaction 3. Determine
Calculations From Chemical Equations
Calculations From Chemical Equations Chapter 9 Hein and Arena Version 1.1 Eugene Passer Chemistry Department Bronx Community 1 College John Wiley and Sons, Inc. A Short Review 2 The molar mass of an element
General Chemistry Multiple Choice Questions Chapter 8
1 Write the skeleton chemical equation for the following word equation: Hydrochloric acid plus magnesium yields magnesium chloride and hydrogen gas. a HClO 4 + Mg --> MgClO 4 + H 2 b HClO 4 + Mg --> MgClO
e) 0.25 f) g) 5000 h) e) 1.5 x 10 3 f) 1.5 x 10-3 g) 1.2 x 10 4 h) 2.2 x 10 5
Name: Chapter 3 The Mole & Stoichiometry Scientific Notation and Significant Figures Practice Problems 1. Rewrite the following numbers in scientific notation. a) 2300 b) 5601 c) 0.00026 d) 0.45013 e)
Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017
![Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017](/thumbs/80/82478584.jpg "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 +
CHEM 12 Unit 3 Review package (solubility)
CHEM 12 Unit 3 Review package (solubility) 1. Which of the following combinations would form an ionic solid? A. Metalloid - metal B. Metal non-metal C. Metalloid metalloid D. Non-metal non-metal 2. Which
Reactions in Aqueous Solution
Reading Assignments: Reactions in Aqueous Solution Chapter 4 Chapter 4 in R. Chang, Chemistry, 9 th Ed., McGraw-Hill, 2006. or previous editions. Or related topics in other textbooks. Consultation outside
Chapter 5 Chemical Reactions
Chapter 5 1 Chapter 5 Chemical Reactions Solutions to In-Chapter Problems 5.1 The process is a chemical reaction because the reactants contain two gray spheres joined (indicating H 2 ) and two red spheres
Review Package #2 Measurement and Communication The Mole Chemical Reactions and Equations Stoichiometry
Chemistry 11 Review Package #2 Measurement and Communication The Mole Chemical Reactions and Equations Stoichiometry 1. Measurement and Communication: A. Scientific Notation: - Conversion of numbers from
Limiting Reactants. In other words once the reactant that is present in the smallest amount is completely consumed the reaction will stop.
In any type of chemical reaction, the amount of product that can be produced is determined by the reactant which is in the smallest amount. In any type of chemical reaction, the amount of product that
PowerPoint to accompany. Chapter 2. Stoichiometry: Calculations with Chemical Formulae and Equations. Dr V Paideya
PowerPoint to accompany Chapter 2 Stoichiometry: Calculations with Chemical Formulae and Equations Dr V Paideya Chemical Equations CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Figure 2.4 Chemical Equations
What is a Representative Particle
Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What
Chemical Reactions Unit
Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e 2 P a g e 3 P a g e 4 P a g e 5 P a g e 6 P a g e Chemistry Balancing Equations Balance the following equations by inserting the
AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry
AP Chemistry Unit 3- Homework Problems Gas Laws and Stoichiometry STP 1. What is standard pressure for each of the following: atm, mm Hg, Torr, kpa, PSI 2. Convert each of the following: a. 700 mm Hg to
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
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.
Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Balancing CHEMICAL EQUATIONS
Balancing CHEMICAL EQUATIONS CHEMICAL REACTIONS involves a chemical change in the identity of one or more chemical species Ex. Rusting of iron (Fe): chemical rxn btwn water and iron involve the breaking
BICOL UNIVERSITY. College of Science Department of Chemistry. CHEM 1 GENERAL CHEMISTRY LECTURE HANDOUT Ver. 1.1 α
BICOL UNIVERSITY College of Science Department of Chemistry CHEM 1 GENERAL CHEMISTRY LECTURE HANDOUT Ver. 1.1 α 20110307 1 mole = 6.022 x 10 23 of molecules (Avogadro's number) A mole is similar to a term
Chem A Ch. 9 Practice Test
Name: Class: Date: Chem A Ch. 9 Practice Test Matching Match each item with the correct statement below. a. product d. balanced equation b. reactant e. skeleton equation c. chemical equation 1. a new substance
Reaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units )
Mole: base unit for an amount of substance A mole contains Avogadro s number (N A ) of particles (atoms, molecules, ions, formula units ) N A 6.0 10 mol -1 1 mol substance contains N A Molar mass (g/mol)
BALANCING EQUATIONS NOTES
BALANCING EQUATIONS NOTES WHY DO WE NEED TO BALANCE CHEMICAL EQUATIONS? The LAW OF CONSERVATION OF MASS says that matter cannot be created or destroyed. In other words, you cannot end up with any more
HW 7 KEY!! Chap. 7, #'s 11, 12, odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones)
HW 7 KEY!! Chap. 7, #'s 11, 12, 15-21 odd, 31, 33, 35, 39, 40, 53, 59, 67, 70, 72-75 all, 77, 82, 84, 88, 89 (plus a couple of unassigned ones) 11) NOTE: I used the solubility rules that I have provided
Equations & Stoichiometry Practice Questions
Equations & Stoichiometry Practice Questions 1. Which substance has the greatest molecular mass? (1) H2O2 (2) NO (3) CF4 (4) I2 2. What is the gram formula mass of Ca(OH)2? (1) 29 g (2) 34 g (3) 57 g (4)
Chemical Reactions. Burlingame High School Chemistry 1
Chemical Reactions 1 Chemical Equations Chemical equations are use to describe: the substances that react, the reactants the substances that are formed, the products the relative amounts of all substances
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
Unit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
Chapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
TASK 1 Writing formulas of ionic compounds. TASK 2 Writing formulas 1. TASK 3 Writing formulas 2. TASK 4 Writing balanced equations 1
TASK 1 Writing formulas of ionic compounds 1 AgBr 2 Na 2CO 3 3 K 2O 4 Fe 2O 3 5 CrCl 3 6 Ca(OH) 2 7 Al(NO 3) 3 8 Na 2SO 4 9 PbO 10 Na 3PO 4 11 Zn(HCO 3) 2 12 (NH 4) 2SO 4 13 Ga(OH) 3 14 SrSe 15 RaSO 4
Types of Chemical Reactions
Why? Types of Chemical Reactions Do atoms rearrange in predictable patterns during chemical reactions? Recognizing patterns allows us to predict future behavior. Weather experts use patterns to predict
Formulas and Models 1
Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Chapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
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)
Problem Solving. Limiting Reactants
Skills Worksheet Problem Solving Limiting Reactants At the beginning of Chapter 8, a comparison was made between solving stoichiometry problems and making turkey sandwiches. Look at the sandwich recipe
Semester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
Unit 6: Mole Assignment Packet Period:
Unit 6: Mole Assignment Packet Name: Period: A1: Mole Conversions 1. Identify the representative particle in each of the following: (atom, molecule, formula unit) a. CuSO 4 b. H 2 O c. NaCl d. Zn e. Cu
1.7 REDOX. Convert these to ionic and half equations and you can see clearly how the electrons are transferred:
1.7 REDOX Oxidation and Reduction: Oxidation and reduction reactions can be identified by looking at the reaction in terms of electron transfer: Our understanding of oxidation and reduction was limited
AMOUNT OF SUBSTANCE. TASK 1 Writing formulas of ionic compounds. TASK 2 Writing formulas 1. TASK 3 Writing formulas 2
AMOUNT OF SUBSTANCE TASK 1 Writing formulas of ionic compounds 1 AgBr 2 Na 2CO 3 3 K 2O 4 Fe 2O 3 5 CrCl 3 6 Ca(OH) 2 7 Al(NO 3) 3 8 Na 2SO 4 9 PbO 10 Na 3PO 4 11 Zn(HCO 3) 2 12 (NH 4) 2SO 4 13 Ga(OH)
Unit 10: Stoichiometry Funsheets. Part A: Balanced Chemical Equations- Balance the following chemical equations.
Unit 10: Stoichiometry Funsheets Part A: Balanced Chemical Equations- Balance the following chemical equations. 1) Al + Cl 2 AlCl 3 2) Mg(ClO) 2 MgCl 2 + O 2 3) FeCl 3 + LiOH Fe(OH) 3 + LiCl 4) Na + O
Ch. 5 Oxidation-Reduction Reactions. Brady & Senese, 5 th Ed.
Ch. 5 Oxidation-Reduction Reactions Brady & Senese, 5 th Ed. 1 Index 5.1. Oxidation-reduction reactions involve electron transfer 5.2. The ion-electron method creates balanced net ionic equations for redox
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
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
This is STOICHIOMETRY.
Balanced equations represent the RATIO in which substances combine. The ratio comes from the COEFFICIENTS of the balanced equation. The combining ratio of substances in any chemical reaction is called
STOICHIOMETRY HONORS CHEMISTRY
STOICHIOMETRY HONORS CHEMISTRY MOLE RATIO A mole ratio is the ratio of coefficients used to compare amounts of reactants and products. 1 ZnCl 2 (aq) + 2 NaOH (aq) 1 Zn(OH) 2 (aq) + 2 NaCl (aq) What is
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
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
Chemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11
Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow
INTRODUCTION TO SOLUBILITY UNIT 3A SOLUBILITY THEORY. There are three classes of compounds which can form ionic solutions:
INTRODUCTION TO SOLUBILITY There are three classes of compounds which can form ionic solutions: Acids: HCl, H 2 SO 4, HNO 3 Bases: NaOH, KOH, NH 3 Chemistry 12 UNIT 3A SOLUBILITY THEORY Salts: NaCl, KMnO
Chapter 9. Calculations from Chemical Equations. to patients Introduction to General, Organic, and Biochemistry 10e throughout the
Chapter 9 Calculations from Chemical Equations Accurate measurement and calculation of the correct dosage are important in dispensing the correct medicine to patients Introduction to General, Organic,
elemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
Q (S) + ML (AQ) L (S) + QM (AQ) Is this reaction exo or endothermic? 2Al 2 O 3(S) + heat 4Al (S) + 3O 2(G) CaCrO 4(AQ) + K (S)
CH 4(G) + 2O 2(G) 2H 2 O (G) + CO 2(G) set up C 5 H 12 + O 2 PQ P + Q 2Mg (S) + O 2(G) 2MgO (S) + heat H 2 O 2 O 2 + H 2 O PF 5(S) P (S) + F 2(G) RZ (AQ) + QP (AQ) RP (AQ) + QZ (S) Fe 2 S 3(S) + heat 2Fe
Stoichiometry Dry Lab
Stoichiometry Dry Lab Name: Mole-Mass Conversions The molar mass of a substance is the conversion factor that allows us to convert between the mass of a substance (in grams) and the number of moles of
AP Chemistry. Mole, Molecular Formula Review One Mole = o This is Avogadro s number. Molar Mass: The mass of one mole of a substance in grams.
AP Chemistry Ms Ye Name Date Block Mole, Review One Mole = o This is Avogadro s number Molar Mass: The mass of one mole of a substance in grams Percent Composition: Identifies the elements present in a
Chapter 8. Chemical Equations. Flames and sparks result when aluminum foil is dropped Into liquid bromine.
Chapter 8 Chemical Equations Flames and sparks result when aluminum foil is dropped Into liquid bromine. Introduction to General, Organic, and Biochemistry 10e John Wiley & Sons, Inc Morris Hein, Scott
Chemical Reactions. Before You Read. Chemical Reactions. Science Journal
Chemical Reactions Before You Read Before you read the chapter, respond to these statements 1 Write an A if you agree with the statement 2 Write a D if you disagree with the statement Before You Read Chemical
UNIT 9. Stoichiometry
UNIT 9 Stoichiometry FORMULA MASS Atomic Mass Unit (u): unit of mass for measuring atoms. (1 u = 1/12 th the mass of a carbon 12 atom) FORMULA MASS FORMULA MASS Example 2: Find the mass of one molecule
What is one of the spectator ions (with correct coefficient)? A)
Chem 101 Exam Fall 01 Section 001 1. Based on the solubility rules Mg (PO 4 ) is A) soluble B) insoluble. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of What is
Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions
Final Exam Study Guide Honors Chemistry Semester 1 2017 60 Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal)
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHM 210 Chemistry Homework #3 Compounds and Their Bonds (Ch. 4) Due: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The octet rule indicates that
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Unit 5. Chemical reactions
Unit 5. Chemical reactions Index 1.- Physical and chemical phenomena...2 2.- What is a chemical reaction?...2 2.1. Chemical equation...2 2.2.- Balance of chemical reactions. Law of conservation of mass...3
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:
Reactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
Mass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
Sample Problem Set. Limiting Reactants
Skills Worksheet Sample Problem Set Limiting Reactants At the beginning of Chapter 8, a comparison was made between solving stoichiometry problems and making turkey sandwiches. Look at the sandwich recipe
Unit 5 Chemical Reactions Notes. Introduction: Chemical substances have physical and chemical properties
Unit 5 Chemical Reactions Notes Introduction: Chemical substances have physical and chemical properties Physical Properties 2 Types of Physical Properties Extensive Physical Properties Intensive Physical
Set 1 Marking Scheme: The Structure of the Atom & Chemical Equation Question Explanation Marks
Set Marking Scheme: The Structure of the Atom & Chemical Equation 200 THE STRUCTURE OF THE ATOMS PAPER 2 : STRUCTURE Question Explanation Marks (a)(i) Diffusion Molecules - Made of tiny / discrete particles/
Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products)
Unit 8: Balancing and Identifying Chemical Reactions Packet Name: 1. Law of Conservation of Mass atoms going into the reaction (reactants) must equal atoms coming out of the reaction (products) C O 2 CO
BONDING AND BALANCING
BONDING AND BALANCING Physical Science Spring 2017 NAME: CLASS PERIOD: TEACHER: ASSIGNMENT PAGE NUMBERS DUE DATE HW POINTS EARNED LAB POINTS EARNED Learning Targets: Chemical Bonding 1-2 Atomic Structure
Review of Chemistry 11
Review of Chemistry 11 HCl C 3 H 8 SO 2 NH 4 Cl KOH H 2 SO 4 H 2 O AgNO 3 PbSO 4 H 3 PO 4 Ca(OH) 2 Al(OH) 3 P 2 O 5 Ba(OH) 2 CH 3 COOH 1. Classify the above as ionic or covalent by making two lists. Describe
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