Unit Two Worksheet WS DC U2

Size: px
Start display at page:

Download "Unit Two Worksheet WS DC U2"

Transcription

1 Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed symbols for states of matter and catalysts. 1. Solid iron (III) oxide and hydrogen gas react to produce iron metal and liquid water. 2. When nitric acid is poured into magnesium hydroxide solution, a reaction occurs in which magnesium nitrate and water are produced. 3. When barium metal is dropped into hydrochloric acid, barium chloride is created with hydrogen gas being given off. 4. Aqueous sodium chloride and sulfuric acid react to yield sodium sulfate and hydrochloric acid, both of which are aqueous. 5. Solid phosphorus reacts with oxygen gas to produce solid diphosphorus pentoxide. page 1 WS DC U2

2 6. Pure copper metal can be produced by heating solid copper (II) sulfide in the presence of oxygen gas from the air. Sulfur dioxide gas is also produced in this reaction. 7. Metal iron reacts with oxygen gas to produce solid iron (III) oxide. 8. Aqueous potassium hydroxide and aqueous barium chloride will react to produce aqueous potassium chloride and solid barium hydroxide. 9. Metal barium reacts with aqueous silver nitrate to produce metal silver and aqueous barium nitrate. 10. Sulfur dioxide gas reacts with oxygen gas to produce sulfur trioxide gas. 11. Aluminum metal will react with copper (II) sulfate solution to produce copper metal and aluminum sulfate solution. page 2 WS DC U2

3 12. Solid silver oxide is heated to produce solid silver and oxygen gas. 13. Aqueous solutions of cadmium bromide and sodium sulfide react to produce aqueous sodium bromide and solid cadmium sulfide. Short Answer [Writing]. Balance the following chemical reactions by filling in the coefficients as needed. If no coefficient is needed, write 1 in the blank. Then identify the reaction type. 14. N 2 O 5 + H 2 O HNO 3 Balanced equation: N 2 O 5 + H 2 O HNO P + O 2 P 2 O 5 Balanced equation: P + O 2 P 2 O Fe(OH) 3 Fe 2 O 3 + H 2 O Balanced equation: Fe(OH) 3 Fe 2 O 3 + H 2 O 17. NiCO 3 NiO + CO 2 Balanced equation: NiCO 3 NiO + CO H 2 + Fe 3 O 4 Fe + H 2 O Balanced equation: H 2 + Fe 3 O 4 Fe + H 2 O page 3 WS DC U2

4 19. Fe + Cl 2 FeCl 3 Balanced equation: Fe + Cl 2 FeCl NaOH + HCl NaCl + H 2 O Balanced equation: NaOH + HCl NaCl + H 2 O 21. Al + H 2 SO 4 Al 2 (SO 4 ) 3 +H 2 Balanced equation: Al + H 2 SO 4 Al 2 (SO 4 ) 3 + H NH 4 NO 3 N 2 O + H 2 O Balanced equation: NH 4 NO 3 N 2 O + H 2 O 23. Zn + AgNO 3 Zn(NO 3 ) 2 + Ag Balanced equation: Zn + AgNO 3 Zn(NO 3 ) 2 + Ag Short Answer. Complete the reaction, including indicating states of matter correctly. Then balance the reaction. Finally, identify the kind of reaction. 24. Pb(NO 3 ) 2 (aq) + H 2 SO 4 (aq) 25. Cu (s) + AgNO 3 (aq) 26. Al 2 (SO 4 ) 3 (aq) + NH 4 OH (aq) page 4 WS DC U2

5 27. Br 2 (aq) + FeI 3 (aq) 28. Fe(NO 3 ) 3 (aq) + NaOH (aq) 29. H 2 SO 4 (aq) + BaCl 2 (aq) 30. Sr (s) + N 2 (g) 31. CaCl 2 (aq) + Pb(NO 3 ) 2 (aq) 32. Ca (s) + O 2 (g) Short Answer. Answer the following questions. 33. How is the law of conservation of mass related to the balancing of a chemical equation? 34. Explain why the following is true: 2Na + 2HCl 2NaCl + H 2 Ag + HCl No reaction page 5 WS DC U2

6 35. How do you show, in a chemical equation, that the reaction is reversible? 36. What information would be lost in the description of a chemical reaction if chemical formulas were not used in chemical equations? 37. How can the ability to predict formulas from ionic charge be helpful in predicting the products of a chemical reaction? 38. The equation for the formation of water from its elements, H 2 (g) + O 2 (g) H 2 O (l), can easily be balanced by changing the formula of the product to H 2 O 2. Explain why this is incorrect. 39. How do you predict the correct formula for the combination reaction between a Group A metal and a nonmetal? Calculations. Answer the following questions. Show work or receive no credit. Include proper units and significant figures. Find the gram formula mass or gram molecular mass of each compound. 40. Li 2 O (lithium oxide) 42. C 6 H 12 O 6 (fructose) 41. (NH 4 ) 2 SO 3 (ammonium sulfite) 43. Fe(OH) 3 (iron (III) hydroxide) page 6 WS DC U2

7 44. NH 4 NO 3 (ammonium nitrate) 45. FeCl 3 (iron (III) chloride) How many oxygen atoms are in a representative particle of each substance? 46. N 2 O 5 (dinitrogen pentoxide) 47. NH 4 NO 3 (ammonium nitrate) 48. C 3 H 5 (NO 3 ) 3 (nitroglycerin) 49. C 6 H 5 COOH (benzoic acid) 50. C 8 H 8 O 4 (acetylsalicylic acid) 51. Al(OH) 3 (aluminum hydroxide) Make the following conversions. Show work or receive no credit. Include proper units and significant figures. 52. Convert molecules NH 3 to moles NH Convert 1 trillion ( ) molecules O 2 to moles O Convert molecules Br 2 to moles of bromine atoms (NOTE: NOT Br 2 ). 55. Convert atoms Li to moles of lithium atoms. page 7 WS DC U2

8 56. Convert mol H 2 O 2 to milligrams H 2 O Convert 6.07 mol Ca(NO 3 ) 2 to grams of Ca(NO 3 ) Convert 26.0 L CH 4, at standard temperature and pressure, into grams of CH Convert 779 cg SnF 2 into number of formula units of SnF Convert g Li 2 HPO 4 into the number of atoms in Li 2 HPO Convert molecules Cl 2, at standard temperature and pressure, into volume, in milliliters, of Cl 2. page 8 WS DC U2

9 62. Convert 0.77 mol C 2 H 6, at standard temperature and pressure, into volume, in liters, of C 2 H Convert three molecules of aspirin (C 9 H 8 O 4 ) into nanograms of aspirin. 64. Convert 19.9 g SiO 2 into the number of formula units of SiO Moles of 1090 g Ca(C 2 H 3 O 2 ) 2 Answer the following questions, showing relevant work to receive credit, significant figures, and proper units. 66. Find the density of C 3 H 8 (g) at standard temperature and pressure. 67. Find the density of NO 2 (g) at standard temperature and pressure. 68. The densities of gases A, B, and C are 1.25 g/l, 2.86 g/l, and g/l, respectively, at standard temperature and pressure. Calculate the molar mass of each substance (in other words, find the molar mass of gas A, gas B, and gas C). Then identify each substance as ammonia (NH 3 ), sulfur dioxide (SO 2 ), chlorine (Cl 2 ), nitrogen (N 2 ), or methane (CH 4 ). Show work or receive no credit. page 9 WS DC U2

10 Complete the following table. Show relevant work in the box or receive no credit, and circle your final answer in the box. Also include proper units and significant figures. Formula of substance involved Grams dissolved Moles dissolved 72. Volume of solution 76. Molarity LiCl g L Fe(NO 3 ) L 1.00 M Na 3 PO mol 1.50 M Na 2 SO ml 2.4 x 10 2 M page 10 WS DC U2

11 Calculate the percent composition of the compounds that are formed from the following reactions, showing relevant work or receiving no credit, significant figures, and proper units g N combines completely with 77.4 O g Na and 4.04 g Cl are formed by the decomposition of table salt The compound methyl butanoate has a percent composition of 58.8% C, 9.8% H, and 31.4% O. 79. What is methyl butanoate s empirical formula? 80. If methyl butanoate s molar mass is 102 g/mol, what is its molecular formula? page 11 WS DC U2

12 A compound with a mass of 7.36 g has 6.93 g of oxygen while the rest of the mass is hydrogen. 81. What is the compound s empirical formula? 82. If the compound s molar mass is 34.0 g/mol, what is its molecular formula? Calculate the amount of hydrogen, in grams, in the following amounts of the following compounds assuming 225 g of each substance are present. 83. KC 2 H 3 O 2 (potassium acetate) 84. C 12 H 22 O 11 (sucrose, or table sugar) page 12 WS DC U2

13 85. A compound s percent composition is 32.00% C, 42.66% O, 18.67% N, and 6.67 % H. If the molar mass of this compound is g/mol, what is the molecular formula of this compound? Show work or receive no credit. 86. Nitroglycerine contains 60% as many carbon atoms as hydrogen atoms; three times as many oxygen atoms as nitrogen atoms; and the same number of carbon and nitrogen atoms. The number of moles of nitroglycerine in 1 g is What is the molecular formula of nitroglycerine? Show work or receive no credit. Short Answer. Answer the following questions. 87. Would four balloons, each containing the same number of molecules of a different gas at standard temperature and pressure, have the same mass or the same volume? Explain. 88. How can you determine the molar mass of a gaseous compound if you do not know its molecular formula? 89. Why might the term molar mass be used instead of gram molecular mass, gram formula mass, or gram atomic mass? page 13 WS DC U2

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

Balancing Equations Notes

Balancing Equations Notes . Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O

More information

Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.

Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric

More information

Reaction Writing Sheet #1 Key

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

More information

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Name Period CH 180 Practice Test: Chapters 3 and 4

Name Period CH 180 Practice Test: Chapters 3 and 4 Name Period CH 180 Practice Test: Chapters 3 and 4 Multiple Choice: 1. 11. 2. 12. 3. 13. 4. 14. 5. 15. 6. 16. 7. 17. 8. 18. 9. 19. 10. 20. 21. 22. 23. 24. 25. 26. 27. 1 Directions: Answer all questions.

More information

Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY

Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct

More information

1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D.

1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D. 1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D. Covalent bond 2. Ethene (C 2 H 4 ) and cyclohexane (C 6 H 12 ) have

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

More information

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate

More information

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular

More information

Intro to Reactions/ Balancing Equations

Intro to Reactions/ Balancing Equations Intro to Reactions/ Balancing Equations Chemical Reactions Chemical reactions involve change. Evidence of a chemical reaction could include the following Evolution of heat, light, and/or sound Production

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

More information

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?

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

More information

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

More information

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters] 1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 4. Aqueous Reactions and Solution Stoichiometry Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)

More information

Chemical Reactions. Chemical changes are occurring around us all the time

Chemical Reactions. Chemical changes are occurring around us all the time Chemical changes are occurring around us all the time Food cooking Fuel being burned in a car s engine Oxygen being used in the human body The starting materials are called reactants The ending materials

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment AP Chemistry Summer Assignment Due Date: Thursday, September 1 st, 2011 Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number of significant

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

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2

More information

Indicators of chemical reactions

Indicators of chemical reactions Indicators of chemical reactions Emission of light or heat Formation of a gas Formation of a precipitate Color change Emission of odor All chemical reactions: have two parts Reactants - the substances

More information

SOLUTIONS. Solutions - page

SOLUTIONS. Solutions - page SOLUTIONS For gases in a liquid, as the temperature goes up the solubility goes. For gases in a liquid, as the pressure goes up the solubility goes. Example: What is the molarity of a solution with 2.0

More information

Unit 6: Mole Assignment Packet Period:

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

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

Chemical Reactions CHAPTER Reactions and Equations

Chemical Reactions CHAPTER Reactions and Equations CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number

More information

Chemical Reactions and Equations

Chemical Reactions and Equations Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new

More information

Chapter 8 Chemical Reactions

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

More information

Lesson 13: Ionic Equations & Intro to the Mole with Conversions

Lesson 13: Ionic Equations & Intro to the Mole with Conversions NOTES Name: Date: Class: Lesson 13: Ionic Equations & Intro to the Mole with Conversions Box 1: Balance: 1. Mg + O2 MgO 2. KClO3 KCl + O2 3. C2H6 + O2 CO2 + H2O Write and balance the equation that represents

More information

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022 CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)

More information

26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O

26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +

More information

TYPES OF CHEMICAL REACTIONS

TYPES OF CHEMICAL REACTIONS TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

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) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2

More information

ACP Chemistry (821) - Mid-Year Review

ACP Chemistry (821) - Mid-Year Review ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference

More information

Sophomore AP Chem Practice Problems

Sophomore AP Chem Practice Problems Due on 8/17/18 Sophomore AP Chem Practice Problems Scientific notation and significant figures Determine the number of Significant Figures in the following numbers: 00034 2431. 8900 0.0094 Convert the

More information

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question.

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question. Unit 4 Multiple Choice Identify the choice that best completes the statement or answers the question. 39. Changing a subscript in a correctly written chemical formula a. changes the number of moles represented

More information

Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions

Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are

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

WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS

WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS REVIEW: Polyatomic ions, writing names from formulas, oxidation number rules I. WRITING FORMULAS FROM NAMES: A. Rules: 1. Know

More information

Practice Problems: Set #3-Solutions

Practice Problems: Set #3-Solutions Practice Problems: Set #3-Solutions IIa) Balance the following equations:(10) 1) Zn (s) + H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + H 2 (g) 3Zn (s) + 2H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + 3H 2 (g) 2. Mg 3 N 2 (s)

More information

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of

More information

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic

More information

Chem A Ch. 9 Practice Test

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

More information

CHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances

CHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have

More information

SNC2D Chemistry Review

SNC2D Chemistry Review SNC2D Chemistry Review 1. For each of the following elements: (a) Draw the Bohr-Rutherford diagram for the neutral atom (b) Determine the charge of the ion each element forms (c) Draw the Lewis dot diagram

More information

CHEMpossible. 101 Exam 2 Review

CHEMpossible. 101 Exam 2 Review CHEMpossible 1. Circle each statement that applies to thermal energy and heat: a. Thermal energy is the average kinetic energy of its molecules due to their motion b. High thermal energy is reflected in

More information

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common

More information

Part 01 - Notes: Reactions & Classification

Part 01 - Notes: Reactions & Classification Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,

More information

Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions

Chemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In

More information

PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE

PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The

More information

Chem 1A Dr. White Fall Handout 4

Chem 1A Dr. White Fall Handout 4 Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular

More information

AP CHEMISTRY THINGS TO KNOW

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

More information

CHE 105 FA17 Exam 2. How many moles of beryllium are in 15.0 grams of Be?

CHE 105 FA17 Exam 2. How many moles of beryllium are in 15.0 grams of Be? CHE 105 FA17 Exam 2 Your Name: Your ID: Question #: 1 How many moles of beryllium are in 150 grams of Be? A 66 B 13515 C 901 D 0601 Question #: 2 Vanillin, C8H8O3, is the molecule responsible for the vanilla

More information

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. 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

More information

Exam 1 Worksheet Chemistry 102

Exam 1 Worksheet Chemistry 102 Exam 1 Worksheet Chemistry 102 Chapter 1 Introduction 1. Convert: a. 650 nm to inches b. 650 km to miles c. 345 mg to lb d. 145 lb to μg e. 4.50 10 10 km to μm f. 8.09 10 8 mg to Mg g. 9.00 10 5 ml to

More information

Name Date Class. representative particle molar mass representative particles

Name Date Class. representative particle molar mass representative particles 10.1 THE MOLE: A MEASUREMENT OF MATTER Section Review Objectives Relate Avogadro s number to a mole of a substance Calculate the mass of a mole of any substance Describe methods of measuring the amount

More information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

CHAPTER 9 CHEMICAL QUANTITIES

CHAPTER 9 CHEMICAL QUANTITIES Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

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

6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide.

6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide. 6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide. (d) C 6 H 14 is hexane. 7. (a) C 8 H 18 is octane. (b) P 2 S 3 is diphosphorus trisulfide. (c) OF 2 is oxygen

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

CP Chemistry Final Exam Review

CP Chemistry Final Exam Review I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at

More information

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON

Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the

More information

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.

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

More information

CHM 1045 Qualifying Exam

CHM 1045 Qualifying Exam CHM 1045 Qualifying Exam 1. Which of the following is the basic unit of volume in the metric system? A) liter B) kilogram C) meter D) centimeter E) gram 2. Which of the following is the largest unit? A)

More information

Solubility & Net Ionic review

Solubility & Net Ionic review Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds

More information

6.02 X Memorize this Number

6.02 X Memorize this Number Honors Chemistry - Unit 6 Chapters 3 & 7 The Mole Math with Chemical Formulas Voc. Assignment Due: Quiz Date(s): TBA Problem Set (UT Quest) Due: Test Date: Unit 6 Packet - Page 1 of 14 **VOCABULARY Assignment**

More information

Unit (2) Quantitative Chemistry

Unit (2) Quantitative Chemistry Unit (2) Quantitative Chemistry Chapter (1) :The mole & chemical equation Lesson (1) Mole and chemical equation Chemical equation: The chemical symbols and formulas of the reactants and products which

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

Chemistry 20 Lesson 36 The Whole Enchilada

Chemistry 20 Lesson 36 The Whole Enchilada Unit I: Science 10 Review Chemistry 20 Lesson 36 The Whole Enchilada 1. Classify the substances as ionic (i), molecular (m), or acid (a) and provide the IUPAC name and the state of matter at SATP where

More information

C2.6 Quantitative Chemistry Foundation

C2.6 Quantitative Chemistry Foundation C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen

More information

Percent Composition, Empirical Formula, Molecular Formula, Hydrates

Percent Composition, Empirical Formula, Molecular Formula, Hydrates Name: Percent Composition, Empirical Formula, Molecular Formula, Hydrates Essential Questions How can one explain the structure, properties, and interactions of matter? How do substances combine or react

More information

BALANCING EQUATIONS NOTES

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

More information

CH 221 Sample Exam Exam II Name: Lab Section:

CH 221 Sample Exam Exam II Name: Lab Section: Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,

More information

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T

Gas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided

More information

Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide

Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10

More information

AP Chemistry Semester 1 Practice Problems

AP Chemistry Semester 1 Practice Problems AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3

More information

Net Ionic Equations. Making Sense of Chemical Reactions

Net Ionic Equations. Making Sense of Chemical Reactions Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are

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

Station 2: Matter, Scientific Method, and Density

Station 2: Matter, Scientific Method, and Density Station 1: Chapter 2 1. How many significant figures in the following measurements a) 1.5000 x 10 23 gold atoms b) 1,500 grams of gold c) 15 gold bars d) 0.00150 cm 3 of gold e) 10,050,000 cm of gold 2.

More information

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide. Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the

More information

Worksheet 1: REPRESENTATIVE PARTICLES

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

More information

Unit Learning Targets (L.T.):

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

More information

NCERT Solutions for Atoms and Molecules

NCERT Solutions for Atoms and Molecules 1 NCERT Solutions for Atoms and Molecules Question 1. In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium

More information

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book

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

Honors Chemistry - Unit 7 Chapter 11 Chemical Reactions

Honors Chemistry - Unit 7 Chapter 11 Chemical Reactions Honors Chemistry - Unit 7 Chapter 11 Chemical Reactions Vocab Assignment Due: Unit 7 Packet - Page 1 of 15 UT Quest(s): Quiz on Diatomic Molecules & Balancing: Prediction Quiz : Test Date: VOCABULARY Assignment

More information

Name Date Hour Honors Chemistry Final Exam Study Guide. For problems 1-4, express each number in scientific notation

Name Date Hour Honors Chemistry Final Exam Study Guide. For problems 1-4, express each number in scientific notation Name Date Hour Honors Chemistry Final Exam Study Guide For problems 1-4, express each number in scientific notation 1.) 0.00000000007461 m 2.) 0.0000158 mi 3.) 0.00000632 m 4.) 0.000015 m ----------------------------------------------------------------------------------------------------------------------

More information

What type of solution that contains all of the

What type of solution that contains all of the What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution What type of solution that contains less solute than it is able to hold at a given temperature?

More information

Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.

Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:

More information

REVIEW OF BASIC CHEMISTRY ANSWER KEY

REVIEW OF BASIC CHEMISTRY ANSWER KEY REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F

More information

Unit IV: Chemical Equations & Stoichiometry

Unit IV: Chemical Equations & Stoichiometry Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations

More information

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES

5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES 5072 CHEMISTRY (NEW PAPERS WITH SPA) BASIC TECHNIQUES 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) BASIC TECHNIQUES LEARNING OUTCOMES a) Be able to write formulae of simple compounds b) Be able to write

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

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

4. Magnesium has three natural isotopes with the following masses and natural abundances: Exercise #1. Determination of Weighted Average Mass 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. Suppose that a bag of pennies

More information

Unit V: Solutions. A. Properties of Solutions. B. Concentration Terms of Solutions. C. Mass Percent Calculation. D. Molarity of Solutions

Unit V: Solutions. A. Properties of Solutions. B. Concentration Terms of Solutions. C. Mass Percent Calculation. D. Molarity of Solutions Unit V: Solutions A. Properties of Solutions B. Concentration Terms of Solutions C. Mass Percent Calculation D. Molarity of Solutions E. Solution Stoichiometry F. Dilution Problems 5-A Properties of Solutions

More information

Dr. Rick Fletcher. Clearly print your name in the name section of the Scantron answer sheet.

Dr. Rick Fletcher. Clearly print your name in the name section of the Scantron answer sheet. Dr. Rick Fletcher Homework 2 Chemistry 101 March 6, 2009 There is one most correct response to each of the multiple choice questions. Choose the best answer. Each of the twenty-five questions is worth

More information