Percent Composition. % Composition, from masses (Practice) From masses (Example)
|
|
|
- Ashlynn Hamilton
- 5 years ago
- Views:
Transcription
1 From masses (Example) Percent Composition A sample of steel wool is placed in an aluminum pan and ignited. The following data is collected: Determine the following: 1. of iron in the product. (g) A Aluminum pan B Al pan with steel wool C Al pan and product Composition, from masses (Practice) A g sample of aluminum is reacted with sulfuric acid. Aluminum sulfate is separated from the resulting solution and dried. The mass of the aluminum sulfate is found to be g. Determine the percent aluminum and percent sulfate in this compound. A Aluminum B Aluminum sulfate Determine the mass of sulfate in the product: (g) 2. of oxygen in the product. 3. of the product. 4. Percent composition of the product. a. Iron. Determine the percent composition by mass: Aluminum ions Sulfate ions of (g) by mass of =? b. xygen 5. Check your work: Do the percentages add up to 100? Table Format: or (Element, Ion, Atom, Polyatomic Ion, molecule,, etc.) (g) (rounded) Al Total Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 1 of 11 Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 2 of 11
2 Composition, from a chemical name or formula (Example) Determine the percent composition of manganese(iii) oxide. Formula: Mn of s mass of (6 significant digits) =? From masses (Example) Determining Empirical Formulas A sample of steel wool is placed in an aluminum pan and ignited. The following data is collected: (g) A Aluminum pan B Al pan with steel wool C Al pan and product Determine the empirical formula for the compound formed. Fe Composition, from a chemical name or formula (Practice) Determine the percent composition of manganese(iv) phosphate. Formula: Chemical Formula: Chemical Name: Mn P of s mass of (6 significant digits) =? Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 3 of 11 Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 4 of 11
3 Review: / / Empirical Formulas, from masses (Practice) A g sample of aluminum is reacted with sulfuric acid. Aluminum sulfate is separated from the resulting solution and dried. The mass of the aluminum sulfate is found to be g. Determine the percent of aluminum and percent sulfate in this compound. Al (or Al +3 ) S 4-2 Chemical Formula: Chemical Name: Smaller = Recognize fractions and their decimal equivalents: Name Fraction Decimal Decimal Range (±0.050) Halves x / Thirds x / , or Fourths x / , or Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 5 of 11 Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 6 of 11
4 Determining Molecular Formulas (Type III [N-N] and rganic [C x H y ]) Steps: 1. Determine Empirical Formula. 2. Find ratio of molar mass to empirical mass: Molar = R = Empirical 3. Distribute R into empirical formula to find molecular formula: Molecular Formula = (Empirical Formula) R Example: 1.50 g of an unknown white powder is analyzed and found to contain phosphorus and oxygen. Through further testing the mass of oxygen in the compound is determined to be 0.85 g and the molar mass of the compound is found to be 284 g/mol. Determine the molecular formula for this compound. P Empirical Formula: Empirical : Practice: A compound containing chlorine, carbon, and hydrogen is used as an additive for gasoline to help prevent engine knock. This compound shows the following percentage composition: Cl C? H The molar mass is known to be g. Determine the molecular formula for this compound. When given percent composition, assume 100 g. This makes the percents into masses. Cl C H Empirical Formula: Empirical : R = Molar / Empirical = / = = Molecular Formula Possibilities ( ) R where R ε {1, 2, 3,, x} R=1 ( ) R = ( ) 1 = P *1 *1 = P M 1 = g R=2 ( ) R = ( ) 2 = P *2 *2 = P M 2 = g R=3 ( ) R = ( ) 3 = P *3 *3 = P M 3 = g R=x ( ) R = ( ) x = P *x *x = P x x M x = * x Molar R = = = = Empirical Molecular Formula = (P ) R = ( ) = P Name this compound: Molecular Formula = (Cl C H ) R Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 7 of 11 Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 8 of 11
5 Hydrates Water and Molecular Formula From masses: (Example) Water in a Hydrate (from formula): Formula: CoCl 2 6 A g sample of hydrated cobalt(ii) chloride is heated to remove the water. nce cool, the anhydrous crystal is found to have a mass of 6.95 g. Determine the percent water and the formula of the hydrate. of s of (6 significant digits) CoCl 2 x Anhydrous cobalt(ii) chloride Water of hydration (g) CoCl 2 = 100? Percent Water: (g) (rounded) CoCl 2 Formula of a Hydrate (from masses): CoCl 2 x Atomic or Molar CoCl 2 Formula: CoCl 2 Name: cobalt( ) chloride hydrate Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 9 of 11 Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 10 of 11
6 Water and Formula From masses: (Practice) A 3.68 g sample of hydrated calcium sulfate is heated to remove the water. nce cool, the anhydrous crystal is found to have a mass of 2.91 g. Determine the percent water and the formula of the hydrate. CaS 4 x Anhydrous calcium sulfate Water of hydration (g) Percent Water: (g) (rounded) CaS 4 Formula of a Hydrate (from masses): CaS 4 x Atomic or Molar CaS 4 Formula: CaS 4 Name: calcium sulfate hydrate Ch 06 Notes.doc 10/16/2009 9:47:00 AM Page 11 of 11
CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units
CHAPTER 11 The Mole 11.1 The Mole: Measurement of Matter Matter is measured in one of three ways: (How many?) Mole SI unit that measures the amount of a substance 6.02 x 10 particles of that substance.
AP WORKSHEET 4s: Calculations Summary
AP WORKSHEET 4s: Calculations Summary TYPE 1: Those involving Avogadro s number (the mole concept). Question 1 A sample of Ge is found to contain 9.7 x 10 23 atoms of Ge. How many moles of Ge atoms are
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
Hydrates, Percent Composition, and Empirical and Molecular Formulas
Hydrates, Percent Composition, and Empirical and Molecular Formulas Hydrates Hydrates are ionic cmpds (salts) that have water molecules bound to their ions. Examples: CuSO 4 5H 2 O Fe(NO 3 ) 3 9H 2 O CoCl
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
Molar Conversions & Calculations
Molar Conversions & Calculations Ch. 11 The Mole 1 A. What is the Mole? A counting number (like a dozen) Avogadro s number (n) 1 mol = 6.02 x 10 23 items A VERY large amount!!!! 2 A. What is the Mole?
Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas
Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas In Chemistry, a Mole is: the unit that measures the amount of a substance - equals 6.022 x 10 23 particles of
Finding Formulas. using mass information about a compound to find its formula
Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula
23 carbon atoms The number is known as Avogadro s d Number.
THE MOLE (a counting unit).again! i A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon
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
THE MOLE (a counting unit).again!
Name: Period: Date: THE MOLE (a counting unit).again! A mole represents a, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon
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
Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas
Composition Stoichiometry Composition Stoichiometry NOTES 1 So far, we ve studied the products of a chemical reaction in terms of their identity. Stoichiometry is a branch of chemistry dealing with quantities.
THE MOLE (a counting unit)
MOLE AND MATH THE MOLE (a counting unit) A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mole eggs = 6.022 x 10 23 eggs 1 dozen
Unit 5. Chemical Composition
Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles
Solutions to the Extra Problems for Chapter 8
Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.
Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets
Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For
Unit 5 Percent Composition, Empirical Formulas, and Reactions
Chemistry 1 West Linn High School Unit 5 Packet and Goals Name: Period: Unit 5 Percent Composition, Empirical Formulas, and Reactions Unit Goals: As you work through this unit, you should be able to: 1.
Name: Date: Pd: Topic 1.2: The Mole Concept and Empirical Formula
Name: Date: Pd: Topic 1.2: The Mole Concept and Empirical Formula Relative Atomic Mass- A r - the weighted average of one atom of an element relative to 1/12 of an atom of carbon-12. A r values do not
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitri
Moles Revisited Name Date Molar Mass How do you calculate the formula mass of a compound? Examples Potassium fluoride Strontium nitrate Aluminum nitride Magnesium phosphate Mole Conversions One-step How
Determining Chemical Formulas
SECTION 7.4 Determining Chemical Formulas When scientists discover or produce a new compound, they analyze it to learn its composition. Often what they measure is the percentage composition of the substance.
Chemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom.
Average Atomic Mass Since atoms are so small and the mass of individual atoms is also very small, it is not useful to use the units of grams or kilogram. A new unit called the atomic mass unit (amu) was
UNIT 7 CHEMICAL FORMULAS WRITING FORMULAS NOTES. EXAMPLES: 1. carbon tetrachloride 2. calcium oxide. 3. iron (III) bromide 4.
WRITING FORMULAS NOTES EXAMPLES: 1. carbon tetrachloride 2. calcium oxide 3. iron (III) bromide 4. lead (II) nitrate 5. aluminum hydroxide 6. ammonium chromate Notes- HONORS 1 NAMING COMPOUNDS NOTES EXAMPLES:
Stoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)
Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number
3.1 Percent Composition
3.1 Percent Composition The percentage composition of a compound refers to the relative mass of each element in a compound. The Law of Definite Proportions states that the elements in a given chemical
AP Chemistry - Summer Assignment
AP Chemistry - Summer Assignment NOTE: a. MUST SHOW ALL WORK FOR CREDIT!! b. Where work is required, do on a separate sheet of paper c. These are the foundational things you should be able to do when you
Unit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
Note Taking Guide: Episode 701. Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.) Avogadro s Number - the = the number
Note Taking Guide: Episode 701 Name Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.)? grains of rice = 1.94 g Avogadro s Number - the = the number Molar Mass the of one of
CHAPTER 6 CHEMICAL COMPOSITION
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 6 CHEMICAL COMPOSITION Day Plans for the day Assignment(s) for the day 1 Begin Chapter
Student Version Notes: Unit 5 Moles & Stoichiometry
Name: Regents Chemistry: Mr. Palermo Student Version Notes: Unit 5 Moles & Stoichiometry Name: KEY IDEAS A compound is a substance composed of two or more different elements that are chemically combined
c formula units of potassium iodide a moles of beryllium b moles of calcium c mole of sulfur a. 6.
Chapter 11 1. Identify and calculate the number of representative particles in each of the following quantities. a. 2.15 moles of gold 2.15 mol Au 1.29 10 24 atoms Au b. 0.151 mole of nitrogen oxide 0.15O
How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?
1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams
Background: Understanding the Mole
Background: Understanding the Mole 1. Why was it important for scientists to know the number of atoms in a sample of matter? 2. What was chosen to use as the standard on which to base the atomic masses
It s just like finding out your test score!!!
It s just like finding out your test score!!! 97 correct out of 100 questions = 97 x 100 = 97% 100 Total of something x 100 = % TOTAL The chemical composition can be expressed as the mass percent of each
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
If you're given a mass percent, you can use it as a conversion factor between the element and the compound
Announcements Wednesday, September 23, 2009 MasteringChemistry due dates (all at 11:59 pm): Ch 3: Fri, Sep 25 Exam 1: next Mon, Sep 28. 20-25 multiple choice questions Short answer (naming, chemical equations)
Unit 3 Chemical Quantities THE MOLE
Chemistry NAME Date Hour Unit 3 Chemical Quantities THE MOLE Practice Test Form C Second Half of Chapter 7 Objective 7 Use the mole to convert among measurements of mass, volume, and number of particles.
Proportions in Chemical Compounds
Chapter 6 Proportions in Chemical Compounds Section 6.1 Chemical Proportions and Percentage Composition Solutions for Practice Problems Student Edition page 260 1. Practice Problem (page 260) Calculate
Chemical reactions: Chemical reactions change substances into other substances.
Chemical reactions: Chemical reactions change substances into other substances. A chemical equation is used to represent a reaction. This has the form: reactants à products Word equations use the names
7 Quantitative Composition of Compounds. Chapter Outline. The Mole. Slide 1. Slide 2. Slide 3
1 7 Quantitative Composition of Compounds Black pearls are composed of calcium carbonate, CaCO 3. The pearls can be measured by either weighing or counting. Foundations of College Chemistry, 14 th Ed.
SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions
SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions [Exam ID:25FPCV 1 When a strontium atom loses its valence electrons, it has the same electron configuration as which element?
AP Chemistry: Chapter 3 Notes Outline
AP Chemistry: Chapter 3 Notes Outline Objectives: Balance chemical equations Use dimensional analysis to solve stoichiometric problems Use dimensional analysis to do limiting reactant problems Use dimensional
Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance.
I. Measuring Matter Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. As you know, atoms and molecules are extremely
Part 01 - Notes: The Mole and Its Calculations
Part 01 - Notes: The Mole and Its Calculations Objectives: Identify, define, and explain: mole, Avogadro s number, representative particle, gram atomic mass, gram molecular mass, gram formula mass, molar
6.02 x 1023 CHAPTER 10. Mole. Avogadro s Number. Chemical Quantities The Mole: A Measurement of Matter Matter is measured in one of three ways:
Chapter 10 Notes CHAPTER 10 10.1 The Mole: A Measurement of Matter Matter is measured in one of three ways: Chemical Quantities Mole SI unit that measures the amount of a substance A mole of a substance
Percent Composition and Empirical Formulas
Percent Composition and Empirical Formulas Content Objectives SWBAT calculate the percent composition by mass of each element in a compound. SWBAT calculate the empirical formula of a compound based on
How many carbon atoms are in 1 mol of sucrose (C 12 H 22 O 11 )? A) 7.23 x B) 6.02 x C) 5.02 x D) 12 E) 342
Question 1 How many carbon atoms are in 1 mol of sucrose (C 12 H 22 O 11 )? A) 7.23 x 10 24 B) 6.02 x 10 23 C) 5.02 x 10 22 D) 12 E) 342 3-1 Question 2 Calculate the mass % of hydrogen in ammonium bicarbonate.
Chapter 3 - Molecules, Compounds and Chemical Equations
Chapter 3 - Molecules, Compounds and Chemical Equations Section 3.2 two general types of bonding between atoms found in compounds, ionic and covalent ionic bonds result when electrons have been transferred
Notes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl -
Name I. Essential Terminology Notes: The Mole Period Chemistry Pre-AP The smallest particle of an element is the atom. Diatomic elements (like O 2 ) are the main exception to this. We say that diatomic
UNIT 1 Chemical Reactions Part II Workbook. Name:
UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the
Chemistry 65 Chapter 6 THE MOLE CONCEPT
THE MOLE CONCEPT Chemists find it more convenient to use mass relationships in the laboratory, while chemical reactions depend on the number of atoms present. In order to relate the mass and number of
Unit 6 Part 2. Mole Related Calculations
Unit 6 Part 2 Mole Related Calculations Several mole related calculations % composition Find the % of each element in a compound Empirical Formula Determine the simplest formula from mass or % composition
7 Quan'ta've Composi'on of Compounds. Chapter Outline. The Mole. The Mole. The Mole. The Mole. Advanced Chemistry
7 Quan'ta've Composi'on of Compounds Chapter Outline 7.1 The Mole 7.2 7.3 Percent Composition of Compounds 7.4 Calculating Empirical Formulas 7.5 Calculating the Molecular Formula from Black pearls are
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
The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume.
The Mole Concept The mole is a convenient unit A mole is the number of atoms present in exactly 12 g of the isotope carbon-12. In 12 g of carbon-12 there are 6.022 x 10 23 carbon atoms It is easily converted
UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY
UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance
Chemistry Stoichiometry and Heat Exam (ver.1) Mr. Thaler. Please do not write on this exam. Mark your answers on the scantron only.
1. Identify from the unbalanced equations below the one that does not represent a redox reaction. a. H 2O 2(aq) + MnO 4 - (aq) O 2(g) + Mn 2+ (aq) b. H 2(g) + N 2(g) NH 3(g) c. NaCl (aq) + AgNO 3(aq) NaNO
Stoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT
Unit 10 Resournces Name Academic Chemistry Stoichiometry Homework On-Time LATE DATE ASSIGNMENT 100 70 10.1 10.2 10.3 10.4 10.5 10.6 EC 16 cincochem.pbworks.com Stoichiometry Live in the now. Garth Algar
Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance.
I. Measuring Matter Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. As you know, atoms and molecules are extremely
WKS 9.1 Calculating Molar Mass (1 page)
WKS 9.1 Calculating Molar Mass (1 page) Find the molar mass (AKA the molecular or formula mass) for each of the following substances. Name of compound Formula of compound Work Molar Mass (g/mol) dichlorine
PERCENTAGE COMPOSITION
PERCENTAGE COMPOSITION Just like any percentage problems you are comparing the part to the whole. In chemistry, percentage composition is based on mass, not on numbers of atoms present. For Example, if
Unit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
CHEMICAL QUANTITIES. Chapter Six
CHEMICAL QUANTITIES Chapter Six Introducing the Mole The dozen is a unit of quantity If I have a dozen atoms, I have 12 atoms by definition. The mole(mol) is a very important unit of quantity in chemistry.
Chapter 9: Stoichiometry The Arithmetic ti Of Equations
Chapter 9: Stoichiometry The Arithmetic of Equations Chemical Calculations Limiting Reagent and Percent Yield The Arithmetic ti Of Equations -- The Arithmetic of Equations -- Using Everyday Equations Stoichiometry
Molar Mass. The total of the atomic masses of all the atoms in a molecule:
Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu
**continued on next page**
Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants
Unit 6: The Mathematics of Chemical Formulas x (6.02 x ) 6.02 x mass: 2 g
Unit 6: The Mathematics of Chemical Formulas # of molecules # of H atoms # of O atoms 1 2 1 2 4 2 3 6 3 100 200 100 6.02 x 10 23 2 (6.02 x 10 23 ) 6.02 x 10 23 mass: 18 g mass: 2 g mass: 16 g molar mass:
Composion Stoichiometry
Composition Stoichiometry blank 3.3.13.notebook Due: Ch 10 RG Hummmm... How do you "measure" bananas? > How many? Count 1 dozen naners or 12 naners Composion Stoichiometry 3 new conversion factors > Avogadro's
Unit 7. Bonds and Naming
Unit 7 Bonds and Naming I. Ionic Bonds Positive ion is attracted to a negative ion; usually a metal & a nonmetal Ionic compound: a substance that has ionic bonds Cation: positive ion Anion: negative ion
MOLES AND EQUATIONS. Answer all questions. Max 51 marks. Mark../51...% Grade. Paddington Academy 1
MOLES AND EQUATIONS Answer all questions Max 51 marks Name.. Mark../51...% Grade Paddington Academy 1 1. In the sixteenth century, a large deposit of graphite was discovered in the Lake District. People
Physical and Chemical Changes and Properties
Physical and Chemical Changes and Properties Practice 1.1 pg. 11 Determine whether each change is physical or chemical. What kind of property (chemical or physical) is demonstrated in each case? a. A copper
Quantitative Chemistry
Quantitative Chemistry When we do experiments to measure something in Chemistry, we: Repeat experiments (usually 3 times) to improve the reliability of the results, by calculating an average of our results.
O(s) CuSO 4. (a) Draw an arrow on the diagram to show where heat is applied. ...
1 The apparatus in the diagram is used to heat a sample of hydrated copper(ii) sulfate crystals, CuSO 4.5H 2 O The equation for the reaction that takes place is hydrated copper(ll) sulfate CuSO 4.5H 2
The quantities in formulas and in chemical reactions can be counted singly or in groups, such as the mole.
CHEM110 Week 4 Notes Mass relationships in Chemical Formulas Page 1 of 5 Recall the Law of Definite Proportions. All samples of a compound have the same atomic composition (or) all samples have the same
EXPERIMENT 6 Empirical Formula of a Compound
EXPERIMENT 6 Empirical Formula of a Compound INTRODUCTION Chemical formulas indicate the composition of compounds. A formula that gives only the simplest ratio of the relative number of atoms in a compound
Chapter 8 Chemical Quantities
Chapter 8 Chemical Quantities Molecular Weight and Moles Find the molecular mass or formula massof each of the following 1. HNO 3 2. Ammonium nitrate 3. Fe 2 O 3 4. Rubidium Sulfite 5. H 3 PO 4 6. Lithium
What is the general term for any negatively charged ion? A) anion B) cation C) monoatomic ion D) polyatomic ion E) none of the above
What is the general term for any negatively charged ion? A) anion B) cation C) monoatomic ion D) polyatomic ion E) none of the above What is the general term for any negatively charged ion? A) anion B)
1. Mole Definition & Background
Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1 1. Mole Definition & Background The mole was developed
Please understand that you will NOT receive another copy of this packet! Name:
Mole Unit Packet Please understand that you will NOT receive another copy of this packet! Name: Period: Introduction to The unit of the Mole is the HEART of all chemistry and most of its calculations.
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
Stoichiometry Practice Problems
Name Period CRHS Academic Chemistry Stoichiometry Practice Problems Due Date Assignment On-Time (100) Late (70) 9.1 9.2 9.3 9.4 9.5 Warm-Up EC Notes, Homework, Exam Reviews and Their KEYS located on CRHS
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
Empirical Formulas and Molecular Formulas. Ch 3.5
Empirical Formulas and Molecular Formulas Ch 3.5 Empirical Formulas are the simplest (lowest) whole number ratio of atoms in a molecule or ionic compound Molecular Formulas are true formulas. For example:
Practice questions for Ch. 3
Name: Class: Date: ID: A Practice questions for Ch. 3 1. A hypothetical element consists of two isotopes of masses 69.95 amu and 71.95 amu with abundances of 25.7% and 74.3%, respectively. What is the
Unit Five MC Practice Dec. 5, 2016
Unit Five: Stoichiometry Name Unit Five MC Practice Dec. 5, 2016 In the space provided, write the letter of the term or phrase that best completes each sentence or best answers each question. 1. Stoichiometry
HW 3 15 Hydrates Notes IC Hydrates HW 4 Water in a Hydrate IC/HW Unit 8 Test Review HW 5 X Unit 8 Test In class on 2/13 and 2/14
Name: Unit 8- The Mole Day Page # Description IC/HW Due Date Completed All 2 Warm-up IC 1 3 4 Notes on the Mole IC 1 5 7 The Mole IC 1 8 9 Chemical Quantities HW 2 10 Percent Composition Notes IC X 2 Gum
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
Show your work for all questions; answer all parts of all questions. No work = no credit.
Quiz: Ch 3 & 4 Name: Version M (32 pts) September 16, 2005 AP Chem Period: 1 2 3 4 Show your work for all questions; answer all parts of all questions. No work = no credit. 1. (10 pts) A compound contains
(i) Calculate the relative formula mass of carbon dioxide, CO 2.. (Relative atomic masses: C = 12, O = 16) (1) CaCO 3.
1 (a) Calcium oxide is manufactured by heating calcium carbonate. The waste product of this process is carbon dioxide. (i) Calculate the relative formula mass of carbon dioxide, CO 2. (Relative atomic
Chapter 9. Chemical Names and Formulas
Chapter 9 Chemical Names and Formulas 9.1 - Naming Ions Monatomic ions: Single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons. - Cations: Groups
Chapter 10 CHEMICAL QUANTITIES The MOLE
Chapter 10 CHEMICAL QUANTITIES The MOLE Avogadro s Hypothesis Equal volumes of gases (@ same T and p) have the same # molecules. The number of 12 C atoms in 12.00 grams of carbon is called Avogadro s 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**
Contents. Content Guidance. Questions & Answers. Getting the most from this book... 4 About this book... 5
Contents Getting the most from this book... 4 About this book.... 5 Content Guidance Atomic structure......................................... 6 Amount of substance....................................
Chem RG Chapter Packet 7 Mole & Chemical Composition. Assign Section # Name Ch 07 Test Review (turn in separately for graded points
Name Period. Chem RG Chapter Packet 7 Mole & Chemical Composition Assign Section # Name 10 5 1. Assignment Sheet printed 2. Notes 7.1 3. Notes 7.2 4. Notes 7.3 5. 7.1 Chapter 7 WS #1 6. 7.2 Chapter 7 WS
The coefficients of a balanced chemical equation tell us how many of each species are involved in the reaction.
Stoichiometry Chemical Equations Reactants are written on the left side of the arrow and products are written on the right side of the arrow. The Law of Conservation of Mass tells us that the number of
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
1.21. Formulae, equations and amounts of substance
1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as
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
The chemical formulas of most of the elements are simply their elemental symbol:
Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.