YEAR 11 CHEMISTRY SEMESTER 1 TITLE: CHEMICAL QUANITITES AND CALCULATIONS (3)
|
|
|
- Hugo McBride
- 5 years ago
- Views:
Transcription
1 YEAR 11 CHEMISTRY SEMESTER 1 TITLE: CHEMICAL QUANITITES AND CALCULATIONS (3) LESSON TITLE OBJECTIVES Check your progress MEG 2 MEG 5 MEG 8 1 Conservation of mass and balancing -Explore ideas about the conservation of mass -Understand what the numbers in stand for -Write balanced symbol State the law of the conservation of mass Explain how to balance in terms of numbers of atoms on both sides of the Explain the meaning of subscripts within a formula and multipliers before a formula in a balanced 2 Relative formula mass 3 Mass changes when gases are in reactions -Review the differences between the isotopes of an element -Distinguish between the mass of an atom and the relative atomic mass of an element -Use relative atomic masses to calculate relative formula masses -Find out how mass can be gained or lost during a reaction -Find the mass of carbon dioxide released per gram of copper carbonate decomposed -Assess the accuracy of measurements Be able to calculate a relative formula mass from the sum of the relative atomic masses Explain that when there is a mass change in a reaction it may be because a gas is given off Calculate the sum of the relative formula masses of reactants and s Explain why there appears to be a mass change when metals carbonates are heated or metals are heated in oxygen Show how the relative formula masses of reactants are equal to the relative formula masses of s Explain observed changes in mass I nonenclosed systems and explain the changes in terms of the particle model
2 4 Chemical measures and uncertainty 5 Moles and amounts of -Explore ideas about the accuracy of measurements -Consider how closely measurements reflect true values -Explore ways of estimating the uncertainty in a set of measurements -Describe the measurements of amounts of s in -Calculate the amount of in a given mass of a -Calculate the mass of a given number of of a Describe that whenever a measurement is made there is always a degree of uncertainty about the result Describe the measurement of amounts of in Represent a distribution of results and make estimates of uncertainty Calculate the number of in a given mass Represent the range of a set of measurements about a mean as a measure of uncertainty Calculate the mass of a given number of 6 Using to balance -calculate the masses of s in a balanced symbol -Calculate the masses of reactants and s from balanced symbol -Calculate the mass of a given reactant or -Convert masses in grams to amounts in -Balance an given the masses of reactants and s -Change the subject of a mathematical Calculate the masses of s in a balanced symbol Calculate the masses of reactants and s from balanced symbol Calculate the mass of a given reactant or
3 Convert masses in grams to amounts in Balance an given the masses of reactants and s Change the subject of a mathematical Concentration of solutions -Relate mass, volume and concentration -Calculate the mass of solute in solution -Relate concentration in mol/dm 3 to mass and volume Relate mass, volume and concentration Calculate the mass of solute in a solution Relate concentration in mol/dm 3 to mass and volume 7 Percentage yield -Calculate the percentage yield from the actual yield -Identify the balanced needed for calculating yields -Calculate theoretical amounts from reactant amounts 8 Atom economy -Identify the balanced of a reaction -Calculate the atom economy of a reaction to form a -Explain why a particular reaction pathway is chosen 9 Using concentrations of solutions -Describe how to carry out titrations -Calculate concentrations in titrations in mol/dm 3 and in g/dm 3 Identify the balanced needed for calculating yields Identify the balanced of a reaction Describe how to carry out titrations Calculate the theoretical amount of s from the amounts of reactants Calculate the atom economy of a reaction to form a desired Calculate concentrations in titrations in mol/dm 3 and in g/dm 3 Calculate the percentage yield from the actual yield and the theoretical yield Explain why a particular reaction pathway is chosen to produce a given the atom economy, yield, rate, equilibrium position and usefulness of bys Explain how the concentration of a solution in mol/dm 3 is related to the mass of
4 10 Amounts of in volumes of gases 11 Amounts in chemistry 12 Change the subject of an -Explain how the concentration of a solution in mol/dm 3 is related to the mass of the solute and the volume of the solution -Explain that the same amount of any gas occupies the same volume at room temperature and pressure (rtp) -Calculate the volume of a gas at rtp from its mass and relative formula mass -Calculate the volumes of gases from a balanced and a given volume of a reactant or -Use atomic masses to calculate formula masses -Explain how formula mass relates to the number of -Explain how the number of relates to other quantities -Use to demonstrate conservation -Rearrange the subject of an -Carry out multi-step calculations KEY TERM LIST: Balanced, conservation of mass, reactants, s Atomic mass, formula mass Explain that the same amount of any gas (in ) occupies the same volume at room temperature and pressure Calculate the volume of a gas at rtp from its mass and relative formula mass the solute and the volume of the solution Calculate the volumes of gases from a balanced and a given volume of a reactant or
5 Gas, mass, particles, thermal decomposition Uncertainty, estimate, distribution of results, range of measurements Mole, chemical amount, relative formula mass, Avogadro number/constant, reactant mass, mass, molar mass, molar volume Balanced, solute, solvent, solution, concentration Yield, percentage yield, theoretical yield, actual yield Atom economy, sustainability, reaction pathway, by- Titration, burette, pipette, indicator Gas volume, room temperature and pressure, decimetre cubed, atmospheric pressure Equation, rearrange, multiply, multi-step calculation MATHEMATICAL SKILLS: Substitute numerical values into Calculate the range and mean of a set of values Use appropriate units for physical quantities Translate information between graphical and numerical form Recognise and use expressions in decimal form Use expressions in standard form Use an appropriate number of significant figures Change the subject of an Use ratios, fractions and percentages Solve simple algebraic Understand and use simple mathematical symbols Construct and interpret frequency tables and diagrams, bar charts and histograms Make estimates of the results of simple calculations
4.3 Quantitative chemistry
4.3 Quantitative chemistry Chemists use quantitative analysis to determine the formulae of compounds and the equations for reactions. Given this information, analysts can then use quantitative methods
4.3.1 Chemical measurements, conservation of mass and the quantitative interpretation of chemical equations
4.3 Quantitative chemistry Chemists use quantitative analysis to determine the formulae of compounds and the equations for reactions. Given this information, analysts can then use quantitative methods
Quantitative analysis Notes
Edexcel GCSE Chemistry Topic 5: Separate chemistry 1 Quantitative analysis Notes 5.8C (HT only) Calculate the concentration of solutions in mol dm -3 and convert concentration in g dm -3 into mol dm -3
Revision Checklist :4.3 Quantitative Chemistry
Revision Checklist :4.3 Quantitative Chemistry Conservation of Mass The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the
Chemistry (separate) for November PPE
1.1 Elements and 1.2 Atoms, formulae and Chapter 1 Atomic Structure and Periodic Table Identify symbols of elements from the periodic table Recognise the properties of elements and. Identify the elements
Part 7- Quantitative Chemistry Application Questions Triple Science
Part 7- Quantitative Chemistry Application Questions Triple Science How bonding and structure are related to the properties of substances A simple model of the atom, symbols, relative atomic mass, electronic
Concentration of Solutions
Concentration of Solutions 1 of 27 Boardworks Ltd 2016 Concentration of Solutions 2 of 27 Boardworks Ltd 2016 Measuring concentrations 3 of 27 Boardworks Ltd 2016 It is not enough to say that one concentration
AQA Chemistry GCSE. Topic 3: Quantitative Chemistry. Flashcards.
AQA Chemistry GCSE Topic 3: Quantitative Chemistry Flashcards What is the law of conservation of mass? What is the law of conservation of mass? The law of conservation of mass states that no atoms are
Revision Checklist :4.3 Quantitative Chemistry
Revision Checklist :4.3 Quantitative Chemistry Conservation of Mass The law of conservation of mass states that no atoms are lost or made during a chemical reaction so the mass of the products equals the
5072 CHEMISTRY (NEW PAPERS WITH SPA) TOPIC 3: FORMULAE, STOICHIOMETRY AND THE MOLE CONCEPT
5072 CHEMISTRY (NEW PAPERS WITH SPA) TOPIC 3: FORMULAE, STOICHIOMETRY AND THE MOLE CONCEPT 5067 CHEMISTRY (NEW PAPERS WITH PRACTICAL EXAM) TOPIC 3: FORMULAE, STOICHIOMETRY AND THE MOLE CONCEPT LEARNING
Edexcel Chemistry A-level
Edexcel Chemistry A-level Topic 5 - Formulae, Equations and Amounts of Substance Flashcards What is the symbol for amount of substance? What is the symbol for amount of substance? n What is the unit used
Concentration of Solutions
Concentration of Solutions 1 of 27 Boardworks Ltd 2016 Concentration of Solutions 2 of 27 Boardworks Ltd 2016 Measuring concentrations 3 of 27 Boardworks Ltd 2016 It is not enough to say that one concentration
IGCSE Double Award Extended Coordinated Science
IGCSE Double Award Extended Coordinated Science Chemistry 4.1 - The Mole Concept The Atomic Mass Unit You need to know the atomic mass unit and the relative atomic mass. In Unit C3.3, 1 atomic mass unit
Quantitative Chemistry. AQA Chemistry topic 3
Quantitative Chemistry AQA Chemistry topic 3 3.1 Conservation of Mass and Balanced Equations Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For
Lesson title Lesson objectives AQA specification reference 1.1 Elements and compounds
1.1 Elements and compounds 1.2 Atoms, formulae and equations Identify symbols of elements from the periodic table Recognise the properties of elements and compounds. Identify the elements in a compound
AQA GCSE (9-1) Combined Chemistry Three Year Scheme of Work
Year 9 Term 1 1/2 1.1 Elements and compounds Year 9 Term 1 1/2 1.2 Atoms, formulae and equations Chapter 1: Atomic structure and the periodic table Identify symbols of elements from the periodic table
GraspIT AQA GCSE Quantitative changes
A. Chemical measurements part 1 Chemical changes and conservation of mass 1. A piece of magnesium was heated in a crucible. a) Write a balance equation to show how the magnesium reacts with oxygen. (2)
FACTFILE: GCSE CHEMISTRY: UNIT 2.6
FACTFILE: GCSE CHEMISTRY: UNIT Quantitative Chemistry Learning outcomes Students should be able to:.1 calculate the concentration of a solution in mol/dm 3 given the mass of solute and volume of solution;.2
The Mole. Relative Atomic Mass Ar
STOICHIOMETRY The Mole Relative Atomic Mass Ar Relative Molecular Mass Mr Defined as mass of one atom of the element when compared with 1/12 of an atom of carbon-12 Some Ar values are not whole numbers
AQA GCSE (9-1) Chemistry Three Year Scheme of Work
This 3-Year Scheme of Work offers a flexible approach for KS4. It is based on three science lessons per fortnight (assuming a two week timetable of two lessons one week and one lesson in the other). Lessons
Chapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
Chapter 3. Atomic Number. Atomic Number. Section 3. Atoms of different elements have different numbers of protons.
Section 3 Atomic Number Atoms of different elements have different numbers of protons. Atoms of the same element all have the same number of protons. The atomic number (Z) of an element is the number of
L = 6.02 x mol Determine the number of particles and the amount of substance (in moles)
1.1 The Mole 1.1.1 - Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 10 23 particles. This number is also known as Avogadro's constant, symbolised
TOPIC 4: THE MOLE CONCEPTS
TOPIC 4: THE MOLE CONCEPTS INTRODUCTION The mass is gram (g) of 1 mole of substances is called its.. 1 mole of substances has.. particles of a substances The mass of 1 mole of substances is always equal
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
Personalised Learning Checklists AQA Chemistry Paper 1
AQA Chemistry (8462) from 2016 Topics C4.1 Atomic structure and the periodic table State that everything is made of atoms and recall what they are Describe what elements and compounds are State that elements
CHEM111 UNIT 1 MOLES, FORMULAE AND EQUATIONS QUESTIONS
Lesson 1 1. (a) Deduce the number of protons, neutrons and electrons in the following species: (i) 37 Cl - (ii) 1 H + (iii) 45 Sc 3+ (b) Write symbols for the following species: (i) 8 protons, 8 neutrons,
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.
(Molar Volume of Gases) (Molarity) (Percent Composition)
list the safety and protective equipment available in the laboratory describe how and when to use each piece of equipment indicate on a school map the location of the nearest fire alarm and appropriate
WJEC England GCSE Chemistry. Topic 3: Chemical formulae, equations and amount of substance. Notes. (Content in bold is for Higher Tier only)
WJEC England GCSE Chemistry Topic 3: Chemical formulae, equations and amount of substance Notes (Content in bold is for Higher Tier only) charges on ions an ion is formed when an atom loses or gains electrons
Name AP CHEM / / Chapter 3 Outline Stoichiometry
Name AP CHEM / / Chapter 3 Outline Stoichiometry Atomic Masses The modern system of atomic masses, instituted in 1961, is based on carbon-12. Carbon-12 is assigned the mass of exactly 12 atomic mass units
Nine tips for scaffolding multi-step calculations
Nine tips for scaffolding multi-step calculations Principles to help students sequence longer maths tasks From Education in Chemistry rsc.li/2paxfig Build up the basics Ensure you have secured the following
Mole Calculations. Specification points. Year 10 Moles I Quantitative Chemistry
Mole Calculations Specification points Year 0 Moles I Quantitative Chemistry Relative formula mass know How to calculate the relative formula mass of a compound What a mole is and Avagadro s number How
Topic 1.2 AMOUNT OF SUBSTANCE
Topic 1.2 AMOUNT OF SUBSTANCE The mole Reacting masses and atom economy Solutions and titrations The ideal gas equation Empirical and molecular formulae Ionic equations Mill Hill County High School THE
Chapter 11. Molecular Composition of Gases
Chapter 11 Molecular Composition of Gases PART 1 Volume-Mass Relationships of Gases Avogadro s Law Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. Recall
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a
Apply the concept of percent yield to stoichiometric problems. Methanol can be produced through the reaction of CO and H 2 in the presence of a catalyst. CO (g) + H 2 (g) CH 3 OH (l) If 75.0 g of CO reacts
IGCSE (9-1) Edexcel - Chemistry
IGCSE (9-1) Edexcel - Chemistry Principles of Chemistry Chemical Formulae, Equations and Calculations NOTES 1.25: Write word equations and balanced chemical equations (including state symbols): For reactions
Name Class Date = + 1 S atom 32.1 amu +
Molar Mass 10. What is the atomic mass of an element? 11. Circle the letter of the phrase that completes this sentence correctly. The atomic masses of all elements a. are the same. b. are based on the
AQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table
AQA GCSE CHEMISTRY (9-1) Topic 1: Atomic Structure and the Periodic Table 4.1.1 Atoms, elements and compounds 4.1.1.1 Atoms, elements and compounds All substances are made of atoms. An atom is the smallest
Mass Relationships in Chemical Reactions
Reading Assignments: Chapter 3 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Mass Relationships in Chemical Reactions Or Related topics in other textbooks. Consultation outside lecture room: Office
Contents. Answers 73. F01 Target 7 Single Science Chemistry WB indd 3
Contents Unit 1 Moles 1 Get started 2 1 How do I describe what a mole is? 3 2 How do I calculate how many moles, or particles, there are in a substance? 4 3 How do I calculate the mass of a reactant or
6 atomic # C symbol Carbon name of element atomic mass. o Examples: # 1 mol C = g # 1 mol O = g # 1 mol H = 1.
7.1 AVOGADRO S NUMBER AND MOLAR CONVERSIONS CHEMISTRY NOTES Identify the mole as the unit used to count particles, whether atoms, ions, or molecules. Use Avogadro s number to convert between amount in
OCR unit 5 revision booklet
OCR unit 5 revision booklet Moles and Molar Mass One mole of any substance contains 6x10 23 particles. For example a mole of carbon atoms would contain 10 x 10 23 carbon atoms. To calculate mole of a substance
ST. FRANCIS SECONDARY SCHOOL HALF YEARLY EXAMINATION SPECIMEN PAPER FORM 4 CHEMISTRY TIME: 2 HOURS. Name: Total Mark from 90:
ST. FRANCIS SECONDARY SCHOOL HALF YEARLY EXAMINATION SPECIMEN PAPER FORM 4 CHEMISTRY TIME: 2 HOURS Name: Total Mark from 90: A copy of the periodic table is provided during the exam. You are reminded of
Combined Science: Trilogy
Co-teaching GCSE Chemistry and GCSE Combined Science: Trilogy This high level co-teaching guide will help you plan your route through the course. You ll be able to see what common themes and topics span
AQA Chemistry (Combined Science) Specification Checklists. Name: Teacher:
AQA Chemistry (Combined Science) Specification Checklists Name: Teacher: Paper 1-4.1 Atomic structure and the periodic table 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic
Atoms, Ions and Molecules Calculations
Atoms, Ions and Molecules Calculations 1. How do you calculate the atomic mass of an element? Atomic Mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope2)(mass of isotope 2)
HOMEWORK 11-1 (pp )
CHAPTER 11 HOMEWORK 11-1 (pp. 333 335) VOCABULARY Define. 1. Gay-Lussac s law of combining volumes of gases 2. Avogadro s law Answer each question. 3. Write and explain the equation that expresses the
Answer ALL questions
Answer ALL questions 01. Most experiments involving electrolysis use inert electrodes, which do not take part in the reactions. However, in some experiments the electrodes do take part in the reactions.
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Lecture Outline 3.1 Chemical Equations The quantitative nature of chemical formulas and reactions is called stoichiometry. Lavoisier
Quantity Relationships in Chemical Reactions
Chapter 10 Relationships in Chemical Reactions Section 10.1 Conversion Factors from a Chemical Equation Goal 1 The coefficients in a chemical equation give us the conversion factors to get from the number
Chemistry. Chapter 17
Chemistry Chapter 17 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Balancing Chemical
Chemistry Chapter 16. Reaction Energy
Chemistry Reaction Energy Section 16.1.I Thermochemistry Objectives Define temperature and state the units in which it is measured. Define heat and state its units. Perform specific-heat calculations.
Chapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
Paper Atomic structure and the periodic table
Paper 1 4.1 Atomic structure and the periodic table 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Use the names and symbols of the first 20 elements in
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
1 Atoms, molecules and stoichiometry try
1 Atoms, molecules and stoichiometry try DEFINITION: Relative atomic mass (Ar) is the average mass of one atom compared to one twelfth of the mass of one atom of carbon-12 DEFINITION: Relative Isotopic
Videos 1. Crash course Partial pressures: YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion:
Videos 1. Crash course Partial pressures: https://youtu.be/jbqtqcunyza?list=pl8dpuualjxtphzz YuWy6fYEaX9mQQ8oGr 2. Crash couse Effusion/Diffusion: https://youtu.be/tlrzafu_9kg?list=pl8dpuualjxtph zzyuwy6fyeax9mqq8ogr
CHEMISTRY- I PUC. Properties of matter and their measurements in chemistry:
CHEMISTRY- I PUC UNIT 1 : Some Basic concepts of Chemistry Matter and its classification: Matter: Anything that occupies space, has mass. The three states of matter are Solids, liquids and gases. Chemical
1. Making the invisible, visible. 2. Enabling the students to witness experiments that they cannot conduct themselves.
Lesson Plan Lesson: Gas Calculations Aim: To investigate the molar and reacting volumes of gases. Learning Outcomes : At the end of the lesson, students will be able to : 1. state the molar volumes of
11B, 11E Temperature and heat are related but not identical.
Thermochemistry Key Terms thermochemistry heat thermochemical equation calorimeter specific heat molar enthalpy of formation temperature enthalpy change enthalpy of combustion joule enthalpy of reaction
At a high temperature, calcium oxide reacts with carbon to form calcium carbide, CaC,.
- ~~Y---~--------'~ '~~L ~ U A-NT, T""?t11 VE. ~ G.-8~Q,-C---,- \ p ic ---,kf r~ ~,,-,----:-r ----"-,. " At a high temperature, calcium oxide reacts with carbon to form calcium carbide, CaC,. CaO(s) +
Chapter 3 Molecules, Compounds, and Chemical Equations
Chapter 3 Molecules, Compounds, and Chemical Equations 3.7 Formula Mass versus Molar mass Formula mass The average mass of a molecule or formula unit in amu also known as molecular mass or molecular weight
Set 1 Structure of the atoms & Chemical Equation Perfect Score F Matter is anything that. and has.
STRUCTURE OF THE ATOMS 1. Matter is anything that. and has. 2. The particle theory of matter state that matter is.. 3. Type of particle Example 4. Property Solid Liquid Gas Diagrammatic representation
Stoichiometry Part 1
Stoichiometry Part 1 Formulae of simple compounds Formulae of simple compounds can be deduced from their ions/valencies but there are some that you should know off by heart. You will learn these and more
If green spheres represent chlorine atoms, yellow-green spheres represent fluorine atoms, and white spheres represent hydrogen atoms,
Understanding the Concepts Balance each of the following by adding coefficients: Balance each of the following by adding coefficients: If red spheres represent oxygen atoms and blue spheres represent nitrogen
GCSE CHEMISTRY REVISION LIST
GCSE CHEMISTRY REVISION LIST OCR Gateway Chemistry (J248) from 2016 Topic C1: Particles C1.1 Describe the main features of the particle model in terms of states of matter and change of state Explain, in
Figure 1. Oxygen. (g) +... (g)... SO 3. The pressure of the reacting gases was increased.
Q1. Figure 1 represents a reaction in the production of sulfuric acid. Figure 1 Oxygen Sulfur dioxide Sulfur trioxide (a) Complete and balance the equation for the reaction.... SO 2 (g) +... (g)... SO
Conservation of Mass
Conservation of Mass 1 of 35 Boardworks Ltd 2016 Conservation of Mass 2 of 35 Boardworks Ltd 2016 What is a chemical reaction? 3 of 35 Boardworks Ltd 2016 A chemical reaction is a change that takes place
Core. Topic 1: Stoichiometric relationships. Essential idea: Physical and chemical properties depend on the ways in which different atoms combine.
Core 32 Essential idea: Physical and chemical properties depend on the ways in which different atoms combine. 1.1 Introduction to the particulate nature of matter and chemical change Nature of science:
Ideal Gas & Gas Stoichiometry
Ideal Gas & Gas Stoichiometry Avogadro s Law V a number of moles (n) V = constant x n Constant temperature Constant pressure V 1 /n 1 = V 2 /n 2 Ammonia burns in oxygen to form nitric oxide (NO) and water
2.1.3 Amount of substance
2.1.3 Amount 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 there are atoms in 12 grams
General Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
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
CHAPTER 2: Atoms, Molecules and Stoichiometry
CHAPTER 2: Atoms, Molecules and Stoichiometry 2.1 Mass of Atoms and Molecules 2.2 Mass Spectrometer 2.3 Amount of Substance 2.4 Empirical Formula and Molecular Formula 2.5 Stoichiometry and Equations Learning
Vijaykumar N. Nazare
Std-XI science Unit 1: Some Basic Concepts of Chemistry Vijaykumar N. Nazare Grade I Teacher in Chemistry (Senior Scale) vnn001@ chowgules.ac.in 1.1 IMPORTANCE OF CHEMISTRY Chemistry is the branch of science
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 8 Chemical Composition
REVISION: GAS LAWS & MOLE CALCULATIONS 18 JUNE 2013
REVISION: GAS LAWS & MOLE CALCULATIONS 18 JUNE 2013 Lesson Description In this lesson we revise how to: apply the gas laws to perform calculations apply the mole concept to perform calculations Key Concepts
Lecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
REVIEW of Grade 11 Chemistry
REVIEW of Grade 11 Chemistry SCH4U_08-09 NAME: Section A: Review of Rules for Significant Digits All measurements have a certain degree of associated with them. All the accurately known digits and the
Chemical Energetics. First Law of thermodynamics: Energy can be neither created nor destroyed but It can be converted from one form to another.
Chemical Energetics First Law of thermodynamics: Energy can be neither created nor destroyed but It can be converted from one form to another. All chemical reactions are accompanied by some form of energy
Smoking at an early age may make it more difficult to quit smoking later. Which of the above statements is an opinion and which is a theory?
Preview Lesson Starter Objectives Foundations of Atomic Theory Law of Conservation of Mass Law of Multiple Proportions Dalton s Atomic Theory Modern Atomic Theory Section 1 The Atom: From Philosophical
The N 2 O 4 -NO 2 Equilibrium
Chemical Equilibria William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 1 Gaseous Chemical Equilibrium For a gaseous chemical equilibrium, more than one gas is present:
Name Date Class STUDY GUIDE FOR CONTENT MASTERY. Use each of the terms below to complete the passage. Each term may be used more than once.
Gases Section 14.1 The Gas Laws In your textbook, read about the basic concepts of the three gas laws. Use each of the terms below to complete the passage. Each term may be used more than once. pressure
CHEM 121 Introduction to Fundamental Chemistry. Summer Quarter 2008 SCCC. Lecture 2
CHEM 121 Introduction to Fundamental Chemistry Summer Quarter 2008 SCCC Lecture 2 Could Stephanie, Liqingqing, Huong, Sophia and Yumiko see me after class for a few minutes. Thanks. Matter, Measurements
Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
Quantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
1.3: Empirical and Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL
1.3: Empirical and Molecular Formulas Ms. Kiely Coral Gables Senior High IB Chemistry SL Practice How heavy are 1.20 x 10²⁵ atoms of potassium? ANSWER How many grams in 1.20 x 10²⁵ atoms of potassium?
Chemistry Chapter 3. Stoichiometry. (three sections for this chapter)
Chemistry Chapter 3 Stoichiometry (three sections for this chapter) Chemistry Chapter 3 Stoichiometry Section 1 3.1-3.4 Average Atomic Mass The Mole Molar Mass Average Atomic Mass Average mass of objects
Chapter 1 IB Chemistry Warm Ups Stoichiometry. Mrs. Hilliard
Chapter 1 IB Chemistry Warm Ups Stoichiometry Mrs. Hilliard Vocabulary 1. Atomic theory 2. Kelvin 3. Mole 4. Relative abundance 5. Molar Mass 6. Empirical formula 7. Molecular formula 8. Stoichiometry
Chemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
UNIT 3 AMOUNT OF SUBSTANCE AND MEASUREMENT UNIT 3. AMOUNT OF SUBSTANCE AND MEASUREMENT Student Version
UNIT 3 AMOUNT OF SUBSTANCE AND MEASUREMENT Student Version Contents a) Introduction b) Safety Precautions in the Laboratory c) Quantities, Units and Measuring Instruments d) Measuring Densities e) The
Chemical Reactions. Chapter 17
Chemical Reactions Chapter 17 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Some equations
Atoms, Molecules, and the Mole
The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting
Thermodynamic and Stochiometric Principles in Materials Balance
Thermodynamic and Stochiometric Principles in Materials Balance Typical metallurgical engineering problems based on materials and energy balance NiO is reduced in an open atmosphere furnace by excess carbon
NCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE
UNIT Atomic Structure & Properties Periodic Table Bonding Chemical Reactions Moles / Stoichiometry Acids and Bases 15 Days 11 Days 16 Days 16 Days 26 Days 9 Days S T A N D A R D S H.1P.1 Explain how atomic
Chemistry *P40135A0116* P40135A. Unit: KCH0/4CH0 Paper: 2C. Edexcel Certificate Edexcel International GCSE. Tuesday 29 May 2012 Morning Time: 1 hour
Write your name here Surname Other names Edexcel Certificate Edexcel International GCSE Chemistry Unit: KCH0/4CH0 Paper: 2C Centre Number Candidate Number Tuesday 29 May 2012 Morning Time: 1 hour You must
AQA GCSE Chemistry Checklist
AQA GCSE Chemistry Checklist Subject content 4.1.1 A simple model of the atom, symbols, relative atomic mass, electronic charge and isotopes Students will be supplied with a periodic table for the exam
General Chemistry I The Mole Map. Dr. Koni Stone Chapter 3, clicker 3
General Chemistry I The Mole Map Dr. Koni Stone Chapter 3, clicker 3 How many moles of sodium carbonate are in 50.5 grams of sodium carbonate? A. 106 moles B. 4.76 x 10-1 moles C. 2.10 moles D. 5.35 x