CHAPTER 4 CHEMICAL REACTIONS & STOICHIOMETRY

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "CHAPTER 4 CHEMICAL REACTIONS & STOICHIOMETRY"

Transcription

1 Review Questions: Chemical Reactions and Stoichiometry Page 1 CHAPTER 4 CHEMICAL REACTINS & STICHIMETRY 1 Antimony can react with chlorine gas to give antimony trichloride Sb + Cl 2 SbCl 3 (l) Which of the following is the most correct set of stoichiometric coefficients to balance this equation (a) 1, 1, 1 (b) 1, 3, 2 (c) 4, 6, 4 (d) 2, 3, 2 2 ctane burns in air to give carbon dioxide and water C 8 H 18 (l) + 2 C 2 + H 2 Which of the following is the most correct set of stoichiometric coefficients to balance this equation (a) 2, 25, 16, 18 (b) 2, 12, 8, 9 (c) 1, 12, 8, 9 (d) 1, 6, 8, 9 3 The original method of making ammonia was to react calcium cyanamide with water according to the following reaction CaCN 2 + H 2 (l) CaC + NH 3 Which of the following is the most correct set of stoichiometric coefficients to balance this equation (a) 2, 6, 2, 4 (b) 4, 2, 6, 2 (c) 1, 3, 1, 2 (d) 1, 1, 1, 1 4 Write and balance the equation for the combustion of ascorbic acid (C 6 6, vitamin C) in oxygen to give C 2 and H 2 (a) (b) (c) (d) C C H 2 C C H 2 2 C C H 2 C C 2 + H 2 5 Write and balance the equation for the combustion of ferrocene, C 10 Fe, in oxygen to give iron(iii) oxide, carbon dioxide, and water (a) C 10 Fe Fe C H 2 (b) (c) (d) C 10 Fe Fe + 10 C H 2 2 C 10 Fe Fe C H 2 4 C 10 Fe Fe C H 2

2 Review Questions: Chemical Reactions and Stoichiometry Page 2 15 Nitrogen oxide is oxidized in air to give brown nitrogen dioxide 2 N N 2 If you have 22 moles of N, (a) you need 22 moles of 2 for complete reaction and produce 22 moles of N 2 (b) you need 11 moles of 2 for complete reaction and produce 22 moles of N 2 (c) you need 11 moles of 2 for complete reaction and produce 33 moles of N 2 (d) you need 10 moles of 2 for complete reaction and produce 20 moles of N 2 16 Aluminum reacts with oxygen to give aluminum(iii) oxide 4 Al Al 2 If you have 60 moles of Al, (a) you need 30 moles of 2 for complete reaction and produce 20 moles of Al 2 (b) you need 180 moles of 2 for complete reaction and produce 120 moles of Al 2 (c) you need 30 moles of 2 for complete reaction and produce 20 moles of Al 2 (d) you need 45 moles of 2 for complete reaction and produce 30 moles of Al 2 17 The very stable compound SF 6 is made by burning sulfur in an atmosphere of fluorine S F 2 8 SF 6 If you need 250 moles of SF 6, you will need to use (a) 0313 moles of S 8 and 750 moles of F 2 (b) 100 moles of S 8 and 240 moles of F 2 (c) 0125 moles of S 8 and 300 moles of F 2 (d) 800 moles of S 8 and 240 moles of F 2 18 Many metals react with halogens to give metal halides For example, Fe + Cl 2 FeCl 2 If you begin with 100 g of iron, (a) you will need 100 g of Cl 2 for complete reaction and will produce 227 g of FeCl 2 (b) you will need 127 g of Cl 2 for complete reaction and will produce 100 g of FeCl 2 (c) you will need 127 g of Cl 2 for complete reaction and will produce 227 g of FeCl 2 (d) you will need 100 g of Cl 2 for complete reaction and will produce 100 g of FeCl 2 19 Like many metals, aluminum reacts with a halogen to give a metal halide 2 Al + 3 Br 2 (l) Al 2 If you begin with 256 g of Al, how many grams of Br 2 (molar mass = 1598 g/mol) are required for complete reaction (a) 384 g (b) 101 g (c) 151 g (d) 227 g

3 Review Questions: Chemical Reactions and Stoichiometry Page 3 20 Many metals react with halogens to give metal halides For example, 2 Al + 3 Br 2 (l) Al 2 If you begin with 256 g of Al, how many grams of Al 2 (molar mass = 5334 g/mol) could you produce if you use excess Br 2 (a) 177 g (b) 201 g (c) 253 g (d) 506 g 21 Many metal halides react with water to produce the metal oxide (or hydroxide) and the appropriate hydrogen halide For example, TiCl 4 (l) + 2 H 2 Ti HCl If you begin with 140 g of TiCl 4 (molar mass = 1897 g/mol), (a) you will need 266 g of H 2 for complete reaction and will produce 590 g of Ti 2 and 108 g of HCl (b) you will need 133 g of H 2 for complete reaction and will produce 590 g of Ti 2 and 108 g of HCl (c) you will need 266 g of H 2 for complete reaction and will produce 88 g of Ti 2 and 88 g of HCl (d) you will need 133 g of H 2 for complete reaction and will produce 77 g of Ti 2 and 77 g of HCl 22 Assume you allow 280 g of titanium(iv) chloride (molar mass = 1897 g/mol) to react with 600 g of water What is theoretical yield of titanium(iv) oxide TiCl 4 (l) + 2 H 2 Ti HCl (a) 590 g (b) 600 g (c) 118 g (d) 133 g 23 Gaseous sulfur dioxide, S 2, can be removed from smokestacks by treatment with limestone and oxygen 2 S CaC CaS C 2 (i) How many grams of CaC are required to remove 150 g of S 2 (a) 117 g (b) 150 g (c) 234 g (d) 468 g (ii) How many grams of CaS 4 are formed when 150 g of S 2 is consumed completely (a) 150 g (b) 136 g (c) 159 g (d) 319 g 24 The reaction of methane and water is one way to prepare hydrogen CH H 2 C H 2 If you begin with 995 g of CH 4 and 2510 g of water, what is the maximum theoretical yield of H 2 (a) 125 g (b) 500 g (c) 281 g (d) 562 g

4 Review Questions: Chemical Reactions and Stoichiometry Page 4 25 Ammonia gas can be prepared by the following reaction: Ca + 2 NH 4 Cl 2 NH 3 + H 2 + CaCl 2 If you mix 112 g of Ca and 224 g of NH 4 Cl, what is the theoretical yield of NH 3 (a) 340 g (b) 355 g (c) 680 g (d) 712 g 26 Aluminum chloride, AlCl 3, can be produced by treating scrap aluminum with chlorine gas 2 Al + 3 Cl 2 2 AlCl 3 If you start with 540 g of Al and 810 g of Cl 2, what is the maximum number of grams of AlCl 3 (molar mass = 1333 g/mol) that can be produced (a) 101 g (b) 135 g (c) 266 g (d) 540 g 27 Uranium(VI) oxide reacts with bromine trifluoride to give uranium(iv) fluoride, an important step in the purification of uranium ore 6 U + 8 BrF 3 (l) 6 UF Br 2 (l) If you begin with 365 g each of U and BrF 3, what is the maximum yield theoretically possible for UF 4 (a) 534 g (b) 401 g (c) 837 g (d) 1120 g 28 Aspirin is produced by the reaction of salicylic acid (M = 1381 g/mol) and acetic anhydride (M = 1802 g/mol) 2 C 7 + C 4 (l) 2 C H 2 (l ) salicylic acid acetic anhydride aspirin If you mix 100 g of each of the reactants, how many grams of aspirin (M = g/mol) can theoretically be obtained (a) 652 g aspirin (b) 130 g aspirin (c) 200 g aspirin (d) 236 g aspirin 29 Phosphoric acid is made from phosphate rock, one form of which is apatite, Ca 5 (P 4 ) 3 F (molar mass = 5043 g/mol) Ca 5 (P 4 ) 3 F + 5 H 2 S 4 (aq) 5 CaS H 3 P 4 (aq) + HF(aq) If you use 100 g of apatite and 500 g of sulfuric acid (molar mass = 9807 g/mol), what is the maximum possible yield of phosphoric acid (9799 g/mol) (a) 300 g (b) 194 g (c) 582 g (d) 600 g 30 Hydrazine, N 2 H 4, is an important industrial reagent It is synthesized by the Raschig process 2 NaH + Cl NH 3 N 2 H NaCl + 2 H 2 If you combine 100 g each of NaH, Cl 2, and NH 3, some amount of two of the three reactants will be left when the reaction is complete The two reactants that are left over are (a) NaH and Cl 2 (b) NaH and NH 3 (c) Cl 2 and NH 3

5 Review Questions: Chemical Reactions and Stoichiometry Page 5 31 Ammonia gas can be prepared by the reaction of a basic oxide like calcium oxide with ammonium chloride, an acidic salt Ca + 2 NH 4 Cl 2 NH 3 + H 2 + CaCl 2 If you isolate exactly 100 g of NH 3, but should have isolated 136 g in theory, what is the percentage yield of ammonia (a) 368% (b) 735% (c) 900% (d) 712% 32 The valuable compound diborane, B 2, can be made by the reaction 2 NaBH 4 + I 2 B NaI + H 2 You use 1203 g of NaBH 4 and excess iodine If you isolate 0295 g of B 2, the percentage yield of B 2 is (a) 950% (b) 671% (c) 500% (d) 335% 33 Nitrogen gas can be prepared in the laboratory by the reaction of ammonia with copper(ii) oxide according to the following unbalanced equation NH 3 + Cu N 2 + Cu + H 2 If you pass 263 g of gaseous NH 3 over a bed of solid Cu (in stoichiometric excess), how many grams of N 2 can be isolated (a) 216 g (b) 288 g (c) 433 g (d) 865 g 34 Disulfur dichloride can be made by allowing chlorine gas to react with molten sulfur S 8 (l) + 4 Cl 2 4 S 2 Cl 2 If you begin with 120 g of S 8 and 635 g of Cl 2, and you isolate only 799 g of S 2 Cl 2, what is the percentage yield of S 2 Cl 2 (a) 804% (b) 487% (c) 301% (d) 601% g of a metal carbonate, containing an unknown metal M, were heated to give the metal oxide and 0376 g C 2 MC + heat M + C 2 What is the identity of the metal M (a) M = Ni (b) M = Cu (c) M = Zn (d) M = Ba 36 Styrene, the building block of polystyrene, is a hydrocarbon, a compound consisting only of C and H If you burn 0438 g of the compound, and find that it produces 1481 g of C 2 and 0303 g of H 2, determine the empirical formula of the compound (a) CH (b) C 2 H (c) C 8 (d) C 7

6 Review Questions: Chemical Reactions and Stoichiometry Page 6 37 Mesitylene is a liquid hydrocarbon, a compound consisting only of C and H If you burn 0115 g of the compound, and find that it produces 0379 g of C 2 and g of H 2, determine the empirical formula of the compound (a) CH (b) C 2 H 3 (c) C 3 H 4 (d) C 9 38 Phenanthrene is a hydrocarbon, a compound consisting only of C and H If you burn 0215 g of the compound, and find that it produces 0747 g of C 2 and 0109 g of H 2, determine the empirical formula of the compound (a) CH 3 (b) C 2 H (c) C 7 (d) C 7 39 Toluene is an aromatic hydrocarbon, a compound composed only of C and H If you burn 0366 g of the compound, and find that it produces 122 g of C 2 and 0286 g of H 2, determine the empirical formula of the compound (a) CH (b) C 3 (c) C 5 H 7 (d) C 7 40 Propionic acid is an organic acid, a compound containing only C, H, and If you burn 0236 g of the acid completely, and isolate 0421 g of C 2 and 0172 g of H 2, what is the empirical formula of the acid (a) CH 2 (b) C 3 H 3 2 (c) C 3 2 (d) CH 3 41 Quinone, which is used in the dye industry and in photography, is an organic compound containing only C, H, and What is the empirical formula of the compound if you find that 0105 g of the compound give 0257 g of C 2 and g of H 2 when burned completely (a) C 3 H 2 (b) C 2 H 2 (c) CH (d) CH 2 42 Vinyl acetate, a compound containing only C, H, and, is the basis of certain plastics To determine its empirical formula you burn 0178 g and find it produces 0364 g of C 2 and 0112 g of H 2 What is the empirical formula of vinyl acetate (a) C 3 H 2 (b) C 2 H 3 (c) C 2 H 2 (d) CH 2 43 Silicon and hydrogen form a series of interesting compounds, Si x To find the formula of one of them, you take a 622 g sample of the compound and burn it in oxygen n doing so, all of the Si is converted to 1164 g of Si 2 and all of the H to 6980 g of H 2 What is the empirical formula of the silicon compound (a) SiH 4 (b) SiH 3 (c) Si 3 (d) Si 2

7 Review Questions: Chemical Reactions and Stoichiometry Page 7 44 To find the formula of a compound composed of iron and carbon monoxide, Fe x (C) y, you burn the compound in pure oxygen according to the following, unbalanced equation Fe x (C) y + 2 Fe 2 + C 2 If you burn 1959 g of Fe x (C) y and find 0860 g of Fe 2 and 2133 g of C 2, what is the empirical formula of Fe x (C) y (a) Fe(C) 4 (b) Fe 2 (C) 9 (c) Fe(C) 5 (d) Fe(C) 6 45 Boron forms an extensive series of compounds with hydrogen, all with the general formula B x To analyze one of these compounds you burn it in air and isolate the boron in the form of B 2 and the hydrogen in the form of water according to the following unbalanced equation B x + excess 2 B 2 + H 2 If you find that 0148 g of B x give 0422 g of B 2 when burned in excess 2, what is the empirical formula of B x (a) BH 3 (b) B 2 (c) B 3 (d) B 5 H 7 46 You have a mixture of CuS 4 and CuS 4 5 H 2 The mixture has a mass of 1245 g, but, after heating to drive off all the water, the mass is only 0832 g What is the weight percent of CuS 4 5 H 2 in the mixture (a) 919% (b) 500% (c) 810% (d) 362% 47 Diborane, B 2, can be made by the reaction 2 NaBH 4 + I 2 B NaI + H 2 If you use 1203 g of NaBH 4 and 3750 g of iodine, what is the maximum theoretical yield of B 2 (a) 0409 g (b) 0440 g (c) 0204 g (d) 0880 g 48 Aluminum bromide is a valuable laboratory chemical If you use 250 ml of liquid bromine (density = g/ml) and excess aluminum metal, what is the maximum theoretical yield of Al 2 2 Al + 3 Br 2 (l) Al 2 (a) 647 g (b) 129 g (c) 863 g (d) 259 g

8 Review Questions: Chemical Reactions and Stoichiometry Page 8 49 Bromine trifluoride reacts with metal oxides to evolve oxygen quantitatively For example, 3 Ti BrF 3 (l) 3 TiF Br 2 (l) Suppose you wish to use this reaction to determine the weight percent of Ti 2 in a sample of ore To do this you collect the 2 gas from the reaction If you find that 2367 g of the Ti 2 -containing ore evolve 143 mg of 2, what is the weight percent of Ti 2 in the sample (a) 754% (b) 151% (c) 302% (d) 849% 50 Electrolysis of aqueous sodium chloride is an important industrial process, since the products are commercially important chlorine, hydrogen, and sodium hydroxide 2 NaCl(aq) + 2 H 2 (l) Cl 2 + H NaH(aq) Assuming you begin with 293 g of NaCl, answer the following questions: (i) How many grams of Cl 2 are theoretically obtainable (a) 710 g (b) 147 g (c) 178 g (d) 710 g (ii) How many grams of NaH are theoretically obtainable (a) 383 g (b) 201 g (c) 100 g (d) 400 g (iii) How many grams of water must be consumed for complete reaction (a) 180 g (b) 360 g (c) 903 g (d) 180 g (iv) If you have actually isolated only 350 g of H 2, the percentage yield of H 2 is (a) 900% (b) 691% (c) 350% (d) 140% ANSWERS CHAPTER 4 1 d 11 d 21 a 2 a 12 b 22 c 3 c 13 c 23 i = c, ii = d 4 b 14 d 24 b 5 d 15 b 25 c 6 b 16 d 26 a 7 c 17 a 27 b 8 a 18 c 28 b 9 d 19 d 29 c 10 b 20 c 30 c 31 b 41 a 32 b 42 b 33 a 43 a 34 d 44 b 35 b 45 d 36 a 46 a 37 c 47 b 38 c 48 c 39 d 49 b 40 c 50 i = c, ii = b, iii = c, iv = b

Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses

Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro

More information

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

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

More information

CHAPTER 12 GASES AND THEIR BEHAVIOR

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

More information

Molecular Formula: Example

Molecular Formula: Example Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

0.786 mol carbon dioxide to grams g lithium carbonate to mol

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

More information

Calculating Atoms, Ions, or Molecules Using Moles

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

More information

Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

More information

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

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

More information

Chemical Equations & Stoichiometry

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

More information

Unit 2: Quantities in Chemistry

Unit 2: Quantities in Chemistry Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find

More information

Unit 9 Stoichiometry Notes (The Mole Continues)

Unit 9 Stoichiometry Notes (The Mole Continues) Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

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

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

More information

Chemical calculations

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

More information

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations CHE11 Chapter Chapter Stoichiometry: Calculations with Chemical Formulas and Equations 1. When the following equation is balanced, the coefficients are. NH (g) + O (g) NO (g) + H O (g) (a). 1, 1, 1, 1

More information

CHAPTER 3 COMPOUNDS AND MOLECULES

CHAPTER 3 COMPOUNDS AND MOLECULES Chapter 3 Compounds and Molecules Page 1 CHAPTER 3 COMPOUNDS AND MOLECULES 3-1. Octane, a component of gasoline, has eight carbon atoms and eighteen hydrogen atoms per molecule. Its formula is written

More information

Chapter 1 The Atomic Nature of Matter

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

More information

1. How many hydrogen atoms are in 1.00 g of hydrogen?

1. How many hydrogen atoms are in 1.00 g of hydrogen? MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 10-24 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?

More information

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH

More information

1. P 2 O 5 2. P 5 O 2 3. P 10 O 4 4. P 4 O 10

1. P 2 O 5 2. P 5 O 2 3. P 10 O 4 4. P 4 O 10 Teacher: Mr. gerraputa Print Close Name: 1. A chemical formula is an expression used to represent 1. mixtures, only 3. compounds, only 2. elements, only 4. compounds and elements 2. What is the total number

More information

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe: Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

More information

AP Chem Unit 1 Assignment 3 Chemical Equations

AP Chem Unit 1 Assignment 3 Chemical Equations Symbols used in chemical equations: Symbol Meaning + used to separate one reactant or product from another used to separate the reactants from the products - it is pronounced "yields" or "produces" when

More information

Chapter 5, Calculations and the Chemical Equation

Chapter 5, Calculations and the Chemical Equation 1. How many iron atoms are present in one mole of iron? Ans. 6.02 1023 atoms 2. How many grams of sulfur are found in 0.150 mol of sulfur? [Use atomic weight: S, 32.06 amu] Ans. 4.81 g 3. How many moles

More 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

Problem Solving. Stoichiometry of Gases

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

More information

Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations. Learning outcomes. you should be able to: Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

More information

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

Chemical Reactions. Chemical Equations. Mole as Conversion Factor: To convert between number of particles and an equivalent number of moles: Quantities of Reactants and Products CHAPTER 3 Chemical Reactions Stoichiometry Application of The Law of Conservation of Matter Chemical book-keeping Chemical Equations Chemical equations: Describe proportions

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Formulae, stoichiometry and the mole concept

Formulae, stoichiometry and the mole concept 3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

W1 WORKSHOP ON STOICHIOMETRY

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

More information

Lecture Notes Chemistry E-1. Chapter 3

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

More information

Chapter 3 Calculation with Chemical Formulas and Equations

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

More information

MOLES AND MOLE CALCULATIONS

MOLES AND MOLE CALCULATIONS 35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

More information

Practice questions for Chapter 8

Practice questions for Chapter 8 Practice questions for Chapter 8 2) How many atoms of nickel equal a mass of 58.69 g? (Refer to the Periodic Table.) A) 1 B) 28 C) 58.69 D) 59 E) 6.02 x 1023 Answer: E Section: 8.1 Avogadro's Number 6)

More information

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

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

More information

Stoichiometry. Unit Outline

Stoichiometry. Unit Outline 3 Stoichiometry Unit Outline 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis

More information

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

More information

Formulas, Equations and Moles

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

More information

CP Chemistry Review for Stoichiometry Test

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

More information

Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.

Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects. Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of

More information

Mass and Moles of a Substance

Mass and Moles of a Substance Chapter Three Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows

More information

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

Name Date Class STOICHIOMETRY. SECTION 12.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) Name Date Class 1 STOICHIOMETRY SECTION 1.1 THE ARITHMETIC OF EQUATIONS (pages 353 358) This section explains how to calculate the amount of reactants required or product formed in a nonchemical process.

More information

Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)

Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4) Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical

More information

Chapter 3! Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry

Chapter 3! Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry Chapter 3! : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

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

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

More information

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

CONSERVATION OF MASS During a chemical reaction, matter is neither created nor destroyed. - i. e. the number of atoms of each element remains constant

CONSERVATION OF MASS During a chemical reaction, matter is neither created nor destroyed. - i. e. the number of atoms of each element remains constant 1 CHEMICAL REACTINS Example: Hydrogen + xygen Water H + H + + - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. reactants products + H + H (balanced equation)

More information

Chapter 3 Stoichiometry

Chapter 3 Stoichiometry Chapter 3 Stoichiometry 3-1 Chapter 3 Stoichiometry In This Chapter As you have learned in previous chapters, much of chemistry involves using macroscopic measurements to deduce what happens between atoms

More information

Writing, Balancing and Predicting Products of Chemical Reactions.

Writing, Balancing and Predicting Products of Chemical Reactions. Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical

More information

Molarity of Ions in Solution

Molarity of Ions in Solution APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.

More information

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

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

More information

Chapter Three: STOICHIOMETRY

Chapter Three: STOICHIOMETRY p70 Chapter Three: STOICHIOMETRY Contents p76 Stoichiometry - The study of quantities of materials consumed and produced in chemical reactions. p70 3-1 Counting by Weighing 3-2 Atomic Masses p78 Mass Mass

More information

CHEMICAL EQUATIONS and REACTION TYPES

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

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

THE MOLE / COUNTING IN CHEMISTRY

THE MOLE / COUNTING IN CHEMISTRY 1 THE MOLE / COUNTING IN CHEMISTRY ***A mole is 6.0 x 10 items.*** 1 mole = 6.0 x 10 items 1 mole = 60, 00, 000, 000, 000, 000, 000, 000 items Analogy #1 1 dozen = 1 items 18 eggs = 1.5 dz. - to convert

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of

More information

Chemistry: Chemical Equations

Chemistry: Chemical Equations Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

More information

11-1 Stoichiometry. Represents

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

More information

CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!!

CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!! CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!! 1. Complete reaction, determine the compounds, check oxidation numbers of each

More information

Moles and Chemical Reactions. Moles and Chemical Reactions. Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol

Moles and Chemical Reactions. Moles and Chemical Reactions. Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol We have used the mole concept to calculate mass relationships in chemical formulas Molar mass of ethanol (C 2 H 5 OH)? Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol Mass percentage of

More information

Chemical Calculations: Formula Masses, Moles, and Chemical Equations

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

More information

Moles, Molecules, and Grams Worksheet Answer Key

Moles, Molecules, and Grams Worksheet Answer Key Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3

More information

APPENDIX B: EXERCISES

APPENDIX B: EXERCISES BUILDING CHEMISTRY LABORATORY SESSIONS APPENDIX B: EXERCISES Molecular mass, the mole, and mass percent Relative atomic and molecular mass Relative atomic mass (A r ) is a constant that expresses the ratio

More information

The Mole. Chapter 2. Solutions for Practice Problems

The Mole. Chapter 2. Solutions for Practice Problems Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of

More information

Lecture 5, The Mole. What is a mole?

Lecture 5, The Mole. What is a mole? Lecture 5, The Mole What is a mole? Moles Atomic mass unit and the mole amu definition: 12 C = 12 amu. The atomic mass unit is defined this way. 1 amu = 1.6605 x 10-24 g How many 12 C atoms weigh 12 g?

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

Part One: Mass and Moles of Substance. Molecular Mass = sum of the Atomic Masses in a molecule

Part One: Mass and Moles of Substance. Molecular Mass = sum of the Atomic Masses in a molecule CHAPTER THREE: CALCULATIONS WITH CHEMICAL FORMULAS AND EQUATIONS Part One: Mass and Moles of Substance A. Molecular Mass and Formula Mass. (Section 3.1) 1. Just as we can talk about mass of one atom of

More information

CHM-101-A Exam 2 Version 1 October 10, 2006

CHM-101-A Exam 2 Version 1 October 10, 2006 CHM-101-A Exam 2 Version 1 1. Which of the following statements is incorrect? A. SF 4 has ¼ as many sulfur atoms as fluorine atoms. B. Ca(NO 3 ) 2 has six times as many oxygen atoms as calcium ions. C.

More information

Module Seven Including Liquids and Solutions in Stoichiometric Calculations. Chem 170. Stoichiometric Calculations. Module Seven

Module Seven Including Liquids and Solutions in Stoichiometric Calculations. Chem 170. Stoichiometric Calculations. Module Seven Chem 170 Stoichiometric Calculations Module Seven Including Liquids and Solutions in Stoichiometric Calculations DePauw University Department of Chemistry and Biochemistry Page 1 Introduction to Module

More information

Chem 31 Fall 2002. Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Writing and Balancing Chemical Equations

Chem 31 Fall 2002. Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Writing and Balancing Chemical Equations Chem 31 Fall 2002 Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations Writing and Balancing Chemical Equations 1. Write Equation in Words -you cannot write an equation unless you

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X

87 16 70 20 58 24 44 32 35 40 29 48 (a) graph Y versus X (b) graph Y versus 1/X HOMEWORK 5A Barometer; Boyle s Law 1. The pressure of the first two gases below is determined with a manometer that is filled with mercury (density = 13.6 g/ml). The pressure of the last two gases below

More information

Stoichiometry. Lecture Examples Answer Key

Stoichiometry. Lecture Examples Answer Key Stoichiometry Lecture Examples Answer Key Ex. 1 Balance the following chemical equations: 3 NaBr + 1 H 3 PO 4 3 HBr + 1 Na 3 PO 4 2 C 3 H 5 N 3 O 9 6 CO 2 + 3 N 2 + 5 H 2 O + 9 O 2 2 Ca(OH) 2 + 2 SO 2

More information

How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies

How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies Limi$ng reactants How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies How Many Cookies Can I Make? In this

More information

Ca 3 N 2 (s) + 6H 2 O(l) H 2NH 3 (g) + 3Ca(OH) 2 (s) mole ratio 1 : 6 : 2 : 3 molar mass (g/mole)

Ca 3 N 2 (s) + 6H 2 O(l) H 2NH 3 (g) + 3Ca(OH) 2 (s) mole ratio 1 : 6 : 2 : 3 molar mass (g/mole) 1. STOICHIOMETRY INVOLVING ONLY PURE SUBSTANCES For all chemical reactions, the balanced chemical equation gives the mole ratios of reactants and products. If we are dealing with pure chemicals, the molar

More information

Formulae, Equations & Formula Mass

Formulae, Equations & Formula Mass St Peter the Apostle High School Chemistry Department Formulae, Equations & Formula Mass N4 & N5 Homework Questions Answer questions as directed by your teacher. National 4 level questions are first followed

More information

Chemistry Final Study Guide

Chemistry Final Study Guide Name: Class: Date: Chemistry Final Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The electrons involved in the formation of a covalent bond

More information

4.3 Reaction Stoichiometry

4.3 Reaction Stoichiometry 196 Chapter 4 Stoichiometry of Chemical Reactions 4.3 Reaction Stoichiometry By the end of this section, you will be able to: Explain the concept of stoichiometry as it pertains to chemical reactions Use

More information

Tutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution.

Tutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution. T-27 Tutorial 4 SOLUTION STOICHIOMETRY Solution stoichiometry calculations involve chemical reactions taking place in solution. Of the various methods of expressing solution concentration the most convenient

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O

Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Balance the following equation: KClO 3 + C 12 H 22 O 11 KCl + CO 2 + H 2 O Ans: 8 KClO 3 + C 12 H 22 O 11 8 KCl + 12 CO 2 + 11 H 2 O 3.2 Chemical Symbols at Different levels Chemical symbols represent

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

BALANCING CHEMICAL EQUATIONS

BALANCING CHEMICAL EQUATIONS BALANCING CHEMICAL EQUATIONS The Conservation of Matter states that matter can neither be created nor destroyed, it just changes form. If this is the case then we must account for all of the atoms in a

More information

Periodic Table, Valency and Formula

Periodic Table, Valency and Formula Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed

More information

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

Reactions. Balancing Chemical Equations uses Law of conservation of mass: matter cannot be lost in any chemical reaction Reactions Chapter 8 Combustion Decomposition Combination Chapter 9 Aqueous Reactions Exchange reactions (Metathesis) Formation of a precipitate Formation of a gas Formation of a week or nonelectrolyte

More information

Chapter 3: STOICHIOMETRY: MASS, FORMULAS, AND REACTIONS

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

More information

Problem Solving. Percentage Yield

Problem Solving. Percentage Yield Skills Worksheet Problem Solving Percentage Yield Although we can write perfectly balanced equations to represent perfect reactions, the reactions themselves are often not perfect. A reaction does not

More information

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

2. The percent yield is the maximum amount of product that can be produced from the given amount of limiting reactant. UNIT 6 stoichiometry practice test True/False Indicate whether the statement is true or false. moles F 1. The mole ratio is a comparison of how many grams of one substance are required to participate in

More information

Chem 171 Review - Exam 1

Chem 171 Review - Exam 1 Chem 171 Review - Exam 1 The following is a list of concepts and terms with which you should be well-acquainted. This is not a substitute for your notes. This list of review topics is not meant to be exhaustive,

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Chemical Reactions in Water

Chemical Reactions in Water Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Acids, Bases and Salts Acids dissolve in water to give H + ions. These ions attach

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1 Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500

More information

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

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

More information

9. The molar mass of hydrazine is 32 g/mol and its empirical formula is NH 2. What is its molecular formula?

9. The molar mass of hydrazine is 32 g/mol and its empirical formula is NH 2. What is its molecular formula? Dr. Rogers Solutions Homework 1. Give the name for the following compounds and state whether they are ionic or not A. Ba(NO 3 ) 2 B. NaH C. PCl 5 D. CO E. NH 4 OH F. Ca(MnO 4 ) 2 G. N 2 O 4 H. NaHSO 4

More information

Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction

Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction Worksheet # 11 1. A solution of sodium chloride is mixed with a solution of lead (II) nitrate. A precipitate of lead (II) chloride results, leaving a solution of sodium nitrated. Determine the class of

More information