Quantitative Chemistry. AQA Chemistry topic 3
|
|
- Isaac Lynch
- 6 years ago
- Views:
Transcription
1 Quantitative Chemistry AQA Chemistry topic 3
2 3.1 Conservation of Mass and Balanced Equations
3 Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For example, consider burning methane: Methane + oxygen Carbon dioxide + water Notice that no atoms were made or destroyed in this reaction, they were simply rearranged. Therefore we can write the Law of the Conservation of Mass: Mass of products = mass of reactants
4 Balancing equations Consider the following reaction: Sodium + water sodium hydroxide + hydrogen Na Na + O + H H O H H H This equation doesn t balance there are 2 hydrogen atoms on the left hand side (the reactants and 3 on the right hand side (the products )
5 Balancing equations We need to balance the equation: Sodium + water sodium hydroxide + hydrogen Na H O H O Na H Na + + O H H O Na H H H Now the equation is balanced, and we can write it as: 2Na (s) + 2H 2 O (l) 2NaOH (aq) + H 2(g)
6 Some examples 2 2 Mg + O 2 Zn + 2 HCl 2 Fe + 3 Cl 2 NaOH + HCl CH O 2 Ca + 2 H 2 O NaOH + H 2 SO 4 2 CH 3 OH + 3 O 2 2 MgO ZnCl 2 + H 2 2 FeCl 3 NaCl + H 2 O CO H 2 O Ca(OH) 2 + H 2 Na 2 SO H 2 O 2 CO H 2 O
7 Atomic mass RELATIVE ATOMIC MASS, A r ( Mass number ) = number of protons + number of neutrons SYMBOL PROTON NUMBER = number of protons (obviously)
8 Some simple compounds Methane, CH 4 Ethyne, C 2 H 2 Water, H 2 O Sulphuric acid, H 2 SO 4 Carbon dioxide, CO 2 Key Hydrogen Oxygen Carbon Sulphur
9 Relative formula mass, M r The relative formula mass of a compound is the relative atomic masses of all the elements in the compound added together. E.g. water H 2 O: Relative atomic mass of O = 16 Relative atomic mass of H = 1 Therefore M r for water = 16 + (2x1) = 18 Work out M r for the following compounds: 1) HCl 2) NaOH 3) MgCl 2 4) H 2 SO 4 5) K 2 CO 3 H=1, Cl=35 so M r = 36 Na=23, O=16, H=1 so M r = 40 Mg=24, Cl=35 so M r = 24+(2x35) = 94 H=1, S=32, O=16 so M r = (2x1)+32+(4x16) = 98 K=39, C=12, O=16 so M r = (2x39)+12+(3x16) = 138
10 An example of Conservation of Mass Here s a classic experiment where magnesium is burned in a crucible: 2Mg + O 2 2MgO Mass of magnesium and crucible before burning = 78.25g Mass of magnesium and crucible after burning = 78.56g Mass is always conserved in any reaction, so where did this extra mass come from?
11 Example Questions For each of the following reactions, state whether or not the mass of the total system should go up or down and explain your answer: 1) Iron + oxygen iron oxide 2) Copper carbonate copper oxide + carbon dioxide For higher tier, write a balanced equation for each reaction, given that iron oxide is Fe 2 O 3 and copper carbonate is CaCO 3.
12 Example Questions 1) aluminium + oxygen aluminium oxide If you start with 27g of aluminium and 24g of oxygen, how much aluminium oxide will you make? 51g 2) magnesium + oxygen magnesium oxide If you start with 24g of magnesium and make 40g of magnesium oxide, how much oxygen was used? 16g 3) potassium oxide + water potassium hydroxide If you start with 9g of water and make 56g of potassium hydroxide, how much potassium oxide was used? 47g EXTENSION Write balanced symbol equations for above reactions
13 3.2 Moles (Higher only)
14 Recap Questions Here are carbon and oxygen on the Periodic Table and a picture of carbon dioxide: 1) What is the atomic mass of carbon? 2) What is the atomic mass of oxygen? 3) What is the molecular mass of carbon dioxide? Carbon dioxide, CO 2
15 A Mole in numbers Definition: A mole of a substance is the relative formula mass of that substance in grams, For example, 12g of carbon would be 1 mole of carbon......and 44g of carbon dioxide (CO 2 ) would be 1 mole etc... Q. How many moles are the following? 1. 23g of sodium 2. 48g of magnesium 3. 36g of carbon 4. 28g of iron 1 mol 2 mol 3 mol 0.5 mol
16 A Mole Definition: A mole of a substance ALWAYS contains the same number of molecules/ions/particles/atoms: Avogadro s Constant: 1 mole = 6.02x10 23 molecules Q. How many moles are the following? 1. How many molecules are in 2 moles of carbon? 2. What about 2 moles of magnesium? 3. How many molecules are in 46g of sodium? 4. How many molecules are in 23g of iron? 1.2x x x x10 23
17 Molar Calculations No. of moles = Mass (g) Molar mass (g/mol) N = m M Some example questions: 1) Calculate the mass of 4 mol of lithium 2) Calculate the mass of 2 mol of sodium 3) Calculate the number of moles in 36g of carbon 4) Calculate the number of moles in 88g of carbon dioxide 5) Calculate the number of moles in 27g of water 28g 46g 3 mol 2 mol 1.5 mol
18 Calculating the mass of a product E.g. what mass of magnesium oxide is produced when 60g of magnesium is burned in air? Step 1: READ the equation: 2Mg + O 2 2MgO IGNORE the oxygen in step 2 the question doesn t ask for it Step 2: WORK OUT the relative formula masses (M r ): 2Mg = 2 x 24 = 48 2MgO = 2 x (24+16) = 80 Step 3: LEARN and APPLY the following 3 points: 1) 48g of Mg makes 80g of MgO 2) 1g of Mg makes 80/48 = 1.66g of MgO 3) 60g of Mg makes 1.66 x 60 = 100g of MgO
19 Calculating the mass of a product using moles Let s try this question again but using moles: Step 1: READ the equation: 2Mg + O 2 2MgO 2 moles of magnesium + 1 mole of oxygen forms 2 moles of magnesium oxide Step 2: WORK OUT the relative formula masses (M r ) of MgO: 2MgO = 2 x (24+16) = 80 Step 3: Apply these steps: 1) 60g of Mg is equal to 1.25 moles (60/48) 2) Therefore we will make 1.25 moles of magnesium oxide 3) Therefore we make 100g of MgO (1.25 moles)
20 1) When water is electrolysed it breaks down into hydrogen and oxygen: 204g produces 108g so 100g produces (108/204) x 100 = 52.9g of Al 2 O 3 2H 2 O 2H 2 + O 2 What mass of hydrogen is produced by the electrolysis of 6g of water? Work out M r : 2H 2 O = 2 x ((2x1)+16) = 36 2H 2 = 2x2 = g of water produces 4g of hydrogen 2. So 1g of water produces 4/36 = 0.11g of hydrogen 3. 6g of water will produce (4/36) x 6 = 0.66g of hydrogen 2) What mass of calcium oxide is produced when 10g of calcium burns? 2Ca + O 2 2CaO M r : 2Ca = 2x40 = 80 2CaO = 2 x (40+16) = g produces 112g so 10g produces (112/80) x 10 = 14g of CaO 3) What mass of aluminium is produced from 100g of aluminium oxide? 2Al 2 O 3 4Al + 3O 2 M r : 2Al 2 O 3 = 2x((2x27)+(3x16)) = 204 4Al = 4x27 = 108
21 Another method Try using this equation: Mass of product IN GRAMMES Mass of reactant IN GRAMMES M r of product M r of reactant Q. When water is electrolysed it breaks down into hydrogen and oxygen: 2H 2 O 2H 2 + O 2 What mass of hydrogen is produced by the electrolysis of 6g of water? Mass of product IN GRAMMES 6g 4 36 So mass of product = (4/36) x 6g = 0.66g of hydrogen
22 Using Moles to balance equations Example question: 130g of zinc reacts with 146g of hydrochloric acid (HCl) to form 272g of zinc chloride (ZnCl 2 ) and some hydrogen (H 2 ). Answer the following: 1) How much hydrogen was produced? 4g 2) How many moles of each substance were reacted/produced? 1 of Zn, 2 of HCl, 1 of ZnCl 2, 1 of H 2 3) Write a balanced chemical equation for this reaction. Zn + 2HCl ZnCl 2 + H 2
23 Recap questions Carbon Methane, CH 4 Water, H 2 O Oxygen, O dioxide, CO 2 2 1) What are the molecular masses of these four compounds? Key Hydrogen 2) How many grams of each compound would you have if you had one mole of each one? 3) Which mole is the heaviest? Oxygen Carbon Sulphur
24 Limiting Reactants What if we don t get the ratios right? Example question: Consider the reaction you have when you burn methane: CH 4 + 2O 2 CO 2 + 2H 2 O A student burns 32g of methane in 72g of oxygen. Which reactant is used up completely? 32g of methane is 2 moles. 72g of oxygen is 2.25 moles of O 2. Therefore this reaction is limited by the 2 moles of methane the limiting reactant. Q. How much CO 2 would we expect to produce? 2 moles (88g)
25 A note about volume The two most commonly used units of volume in chemistry are the cm 3 and the dm 3 : 1cm 3 1dm 3 (= 1000cm 3 ) 1) Convert 1250cm 3 into dm 3 2) Convert 1cm 3 into dm 3 3) Convert 0.056dm 3 into cm 3 4) Convert 1.28dm 3 into cm 3
26 Concentration Concentration means how much of a chemical there is in a fixed volume and can be measured in g/dm 3 or mol/dm 3. A solution of low concentration ( dilute ) A solution of high concentration ( strong )
27 Questions on Concentration To calculate the concentration of a substance you could use one of these formulae: Conc. = Mass of substance (g) Volume of solvent (dm 3 ) Conc. = Amount of solute (mol) Volume of solvent (dm 3 ) Calculate, with units, the concentration of the following: 1) A solution of 10g salt in 1dm 3 of water 2) 2mol of hydrochloric acid in 500cm 3 of water 3) 10kg of salt in 200dm 3 of water 4) 0.5mol of sodium hydroxide in 100cm 3 of water
28 Converting concentrations To convert g/dm 3 into mol/dm 3 you can use the following formula: Concentration = Concentration (g/dm 3 ) (mol/dm 3 ) Molar mass Convert the following: 1) 0.5mol/dm 3 of sodium hydroxide into g/dm 3. 2) 2mol/dm 3 of HCl into g/dm 3. 3) 20g/dm 3 of NaCl into mol/dm 3. 4) 500g/dm 3 of CaCl 2 into mol/dm 3.
29 Changing a Concentration Wow that s a strong acid! How can I make it less concentrated? What would you do to change an acid of concentration 1 mol/dm 3 to an acid of concentration 0.1 mol/dm 3? Can you think of some examples where dilution is needed in food?
30 3.3 Yield and Atom Economy of Chemical Reactions (Chem only)
31 Problems with calculating mass Calculating the amount of a product or reactant may not always give you a reliable answer... 1) The reaction may not have completely 2) The reaction may have been 3) Some of the product may have been 4) Some of the reactants may have produced other The amount of product that is made is called the. This number can be compared to the maximum theoretical amount as a percentage, called the percentage yield. Words lost, yield, finished, reversible, products
32 Percentage Yield Percentage yield = Actual yield Predicted yield X 100% Some example questions: 1) The predicted yield of an experiment to make salt was 10g. If 7g was made what is the percentage yield? 70% 2) Dave is trying to make water. If he predicts to make 15g but only makes 2g what is the percentage yield? 13% 3) Sarah performs an experiment and has a percentage yield of 33%. If she made 50g what was she predicted to make? 150g
33 Percentage Yield (harder) Theoretical yield = the amount of product that should be made as calculated from the masses of atoms Actual yield = what was actually produced in a reaction Percentage yield = actual yield (in g) Example question: theoretical yield 65g of zinc reacts with 73g of hydrochloric acid and produces 102g of zinc chloride. What is the percentage yield? Zn + 2HCl ZnCl 2 + H 2 The theoretical yield is 136g (using Cl = 35.5) so the % yield is 75%
34 Atom Economy Percentage atom economy = Relative formula mass of useful product Total masses of products Calculate the atom economies of the following: 1) Converting ethanol into ethene (ethene is the useful bit): C 2 H 5 OH C 2 H 4 + H % 2) Making zinc chloride from zinc and hydrochloric acid: Zn + 2HCl ZnCl 2 + H 2 99%
35 3.4 Using Concentrations in mol/dm 3 (Chemistry only)
36 Revision about Moles Consider two liquids: 20cm 3 of 0.1mol/dm 3 of hydrochloric acid Now consider two gases: 20cm 3 of 0.1mol/dm 3 of sodium hydroxide These two beakers contain the same number of moles 20cm 3 of helium at room temperature and pressure 20cm 3 of argon at room temperature and pressure These two gases contain the same number of moles
37 Titration 1) Fill a burette with sodium hydroxide solution of known concentration 2) Accurately measure out 25cm3 of acid and place it in the conical flask 3) Add phenolphthalein indicator to the flask 4) Slowly add the alkali until the mixture in the flask turns pink (down to the next drop!) 5) Repeat until you get similar results
38 Titration Equations Q. 0.05dm 3 of HCl neutralises 0.1dm 3 of NaOH of concentration 0.5mol/dm 3. What is the concentration of the acid? The key steps: 1) Look at the equation to compare the numbers of moles: HCl + NaOH NaCl + H 2 O Notice that 1 mole of HCl neutralises 1 mole of NaOH 2) Use this equation: No. of moles = concentration x volume a) So, the number of moles of NaOH is (0.5 x 0.1) = 0.05mol b) According to the equation, this will neutralise 0.05mol of HCl c) Therefore we have (0.05mol/0.05dm 3 ) = 1mol/dm 3 HCl
39 Titration Equations 1) 0.2dm 3 of HCl neutralises 0.1dm 3 of NaOH of concentration 0.5mol/dm 3. What is the concentration of the acid? HCl + NaOH NaCl + H 2 O 0.25mol/dm 3 2) H 2 SO 4 of concentration 0.4mol/dm 3 neutralises 0.1dm 3 of NaOH of concentration 0.2mol/dm 3. How much acid was used? H 2 SO 4 + 2NaOH Na 2 SO 4 + 2H 2 O 0.025mol/dm 3
40 3.5 Amounts of substances in relation to volumes
41 Calculating Volumes of Gases An important fact: 1 mole of a gas at room temperature (20 O C) and pressure (1 atm) occupies a volume of 24dm 3. 1) What is the volume of 2 moles of oxygen? 2) What is the volume of 0.25 moles of carbon dioxide? 3) How many moles would be in 8dm 3 of nitrogen? 4) How much volume would 80g of argon occupy? 5) A balloon contains 12dm 3 of carbon dioxide. What is the mass of this much CO 2? 48dm 3 6dm 3 1/3 mol 48dm 3 22g
42 Calculating the volume of a product REMEMBER THIS - At normal temperature and pressure the Relative Formula Mass (M r ) of a gas will occupy a volume of 24 litres e.g. 2g of H 2 has a volume of 24 litres 32g of O 2 has a volume of 24 litres 44g of CO 2 has a volume of 24 litres etc Q. When water is electrolysed it breaks down into hydrogen and oxygen: 2H 2 O 2H 2 + O 2 What VOLUME of hydrogen is produced by the electrolysis of 6g of water? From previous work Calculating the mass of a product we find that the MASS of hydrogen produced was 0.66g 2g of hydrogen (H 2 ) will occupy 24 litres (from the red box above), So 0.66g will occupy 0.66/2 x 24 = 8 litres
43 Example questions 1) What volume of hydrogen is produced when 18g of water is electrolysed? 2H 2 O 2H 2 + O 2 24dm 3 2) Marble chips are made of calcium carbonate (CaCO 3 ). What volume of carbon dioxide will be released when 500g of CaCO 3 is reacted with dilute hydrochloric acid? CaCO 3 + 2HCl CaCl 2 + H 2 O + CO 2 120dm 3 3) Magnesium will react with hydrochloric acid. What volume of hydrogen would be produced if you reacted 1g of magnesium with excess acid? Mg + 2HCl MgCl 2 + H 2 1dm 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
More informationRevision 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
More information2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with
Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12
More informationFACTFILE: 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
More informationGraspIT 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)
More informationIGCSE (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
More informationQuantitative 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.
More informationC4 Quick Revision Questions
C4 Quick Revision Questions H = Higher tier only SS = Separate science only Question 1... of 50 Write the equation which shows the formation of iron oxide Answer 1... of 50 4Fe + 3O 2 2Fe 2 O 3 Question
More informationPart 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
More informationAQA 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
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationChapter 5 Chemical Calculations
Calculating moles Moles and elements Moles and compounds Moles and gases Moles and solutions Calculating formulae Finding the formula Chapter 5 Chemical Calculations Moles and chemical equations Checklist
More informationIGCSE 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
More informationStoichiometry 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
More informationWhat is this booklet for: This is simply designed to be a bridging Chemistry booklet. It has work to prepare you for the A level you are starting in
1 What is this booklet for: This is simply designed to be a bridging Chemistry booklet. It has work to prepare you for the A level you are starting in September. It contains a series of topics that you
More informationUnit 1 SOME BASIC CONCEPTS OF CHEMISTRY I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings of mass which are given
More informationLower Sixth Chemistry. Sample Entrance Examination
Lower Sixth Chemistry Sample Entrance Examination Time allowed: 60 minutes Name: Total : 60 Marks INSTRUCTIONS : Answer all questions Answers should be written in the spaces provided Dictionaries or reference
More informationSIC CONCEPTS TS OF CHEMISTRY. Unit. I. Multiple Choice Questions (Type-I)
Unit 1 SOME BASIC B SIC CONCEPTS CONCEP TS OF CHEMISTRY CHEMIS I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings
More informationThe 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
More informationOutcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass,
Stoichiometry Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, volume, and heat of reaction. Stoichiometry
More informationChemical measurements QuestionIT
Chemical measurements QuestionIT 1. What is the law of conservation of mass? Mass of reactants = mass products. 2. Why might some reactions appear to show a change in mass? A reactant or a product is a
More informationThe Masses of chemicals
The Masses of chemicals Boardworks Ltd 2003 WILF To give a definition of relative formula mass M r. To calculate relative formula mass if its formula and the relative atomic mass are given. To give a full
More information3. Which postulate of Dalton s atomic theory is the result of the law of conservation of mass?
1 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 ethanoate. Show that these observations are in
More informationCHEM111 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,
More informationNATIONAL 5 CHEMISTRY
Farr High School NATIONAL 5 CHEMISTRY Unit 1 Chemical Changes and Structure Question Booklet 1 Rates of Reaction 1. Explain how the following would affect the rate of the reaction between 1.0 g of magnesium
More informationPersonalised 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
More informationNCERT Solutions for Atoms and Molecules
1 NCERT Solutions for Atoms and Molecules Question 1. In a reaction, 5.3 g of sodium carbonate reacted with 6 g of ethanoic acid. The products were 2.2 g of carbon dioxide, 0.9 g water and 8.2 g of sodium
More informationEnd of chapter exercises
End of chapter exercises Problem 1: Write only the word/term for each of the following descriptions: 1. the mass of one mole of a substance 2. the number of particles in one mole of a substance Answer
More informationRepresenting Chemical Change
Representing Chemical Change As we have already mentioned, a number of changes can occur when elements react with one another. These changes may either be physical or chemical. One way of representing
More information1.24 Calculations and Chemical Reactions
1.24 Calculations and Chemical Reactions Converting quantities between different substances using a balanced equation A balanced chemical equation tells us the number of particles of a substance which
More informationSeparate Science: Chemistry Paper 1. Knowledge Organisers. Chemistry Paper 1 17 th May AM 1h 45min. Atomic Structure The Periodic Table
Separate Science: Chemistry Paper 1 Chemistry Paper 1 17 th May AM 1h 45min Topics in the Paper: C1 C2 Atomic Structure The Periodic Table Knowledge Organisers C3 C4 C5 C6 C7 Structure and Bonding Chemical
More informationburette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3
1 Crystals of sodium sulphate-10-water, Na 2 SO 4.10H 2 O, are prepared by titration. burette filled with sulphuric acid conical flask 25.0 cm 3 of sodium hydroxide(aq) concentration 2.24 mol / dm 3 (a)
More informationCHEM111 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,
More informationMoles, calcula/ons in gaseous and solu/on and acids and bases
Moles, calcula/ons in gaseous and solu/on and acids and bases Moles and calcula/ons 1 Objec/ves All Define rela/ve molecular mass and rela/ve formula mass Most Describe Avogadro s constant and the terms
More informationFormulae of simple compounds
4. Stoichiometry Formulae of simple compounds Formulae of simple compounds can be deduced from their ions but there are some that you should know off by heart. You must learn the following formulae: Carbon
More informationHow 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
More informationSummer Preparatory Tasks for A Level Chemistry 2017.
Summer Preparatory Tasks for A Level Chemistry 2017. Task One: Why have you chosen to complete an A Level in Chemistry? Research your future career and what subjects and grades are required to achieve
More informationChemical 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
More information4.3.1 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
More informationFigure 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
More informationA-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS
A-LEVEL TRANSITION COURSE SUMMER 2018 PART 2: USING CHEMICAL EQUATIONS MASS AQUEOUS VOLUME ` MOLAR MASS GASEOUS VOLUME MOLES CONCENTRATION REVISION FROM LESSON 1 How many moles? 1) Jahin weighs a sample
More informationTopic 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
More information2.1.3 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
More informationClass IX Chapter 3 Atoms and Molecules Science
Class IX Chapter 3 Atoms and Molecules Science 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
More informationTHE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School
THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY AT Myton School Introduction Before you start the AS Chemistry course in September you should have completed this new bridging course for Chemists. It has been
More informationPRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE
PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The
More informationFormulae and Equations
Formulae and Equations 1 of 41 Boardworks Ltd 2016 Formulae and Equations 2 of 41 Boardworks Ltd 2016 Forming different compounds 3 of 41 Boardworks Ltd 2016 Elements are made up of just one type of atom.
More information4.4. Revision Checklist: Chemical Changes
4.4. Revision Checklist: Chemical Changes Reactivity of metals When metals react with other substances the metal atoms form positive ions. The reactivity of a metal is related to its tendency to form positive
More informationSCIENCE JSUNIL TUTORIAL CLASS 9. Activity 1
Activity Objective To understand, that there is a change in mass when a chemical change takes place. (To understand law of conservation of mass experimentally). Procedure. Take one of the following sets,
More informationUnit of Pressure (P):Pa Unit of Volume (V): m 3 Unit of Temp (T): K n= moles R = Converting temperature. C K add 273
1.2 Calculations 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 of carbon-12.
More informationClass XI Chapter 1 Some Basic Concepts of Chemistry Chemistry
Question 1.1: Calculate the molecular mass of the following: (i) H 2 O (ii) CO 2 (iii) CH 4 (i) H 2 O: The molecular mass of water, H 2 O = (2 Atomic mass of hydrogen) + (1 Atomic mass of oxygen) = [2(1.0084)
More informationMole Concept 5.319% = = g sample =
Mole - a counting system Avogadro s number = 6.0 10 3 Mole Concept Chemical calculation involving mass: Empirical formula: The simplest formula that shows the relative numbers of the different kinds of
More informationOCR 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
More informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More informationName: DEADLINE: 1 st lesson back, September term
Name: DEADLINE: 1 st lesson back, September term The aim of this preparation work is to revise GCSE chemistry topics that you will need for A Level course. Part A is for everyone to complete. Part B is
More informationSet 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
More informationUNIT 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
More informationLondon Examinations IGCSE
Centre No. Candidate No. Paper Reference 4 3 3 5 2 H Paper Reference(s) 4335/2H London Examinations IGCSE Chemistry Paper 2H Higher Tier Wednesday 21 May 2008 Afternoon Time: 2 hours Surname Signature
More informationUnit 5. Chemical reactions
Unit 5. Chemical reactions Index 1.- Physical and chemical phenomena...2 2.- What is a chemical reaction?...2 2.1. Chemical equation...2 2.2.- Balance of chemical reactions. Law of conservation of mass...3
More information4.3 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
More informationREACTION RATES AND REVERSIBLE REACTIONS
NAME SCHOOL INDEX NUMBER DATE REACTION RATES AND REVERSIBLE REACTIONS 1. 1989 Q 4 P1 The graph shows the loss in total mass of a mixture of marble chips and dilute hydrochloric acid with time at 250C Loss
More informationUnit of Pressure (P):Pa Unit of Volume (V): m 3 Unit of Temp (T): K n= moles R = Converting temperature. C K add 273
1.2 Calculations 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 of carbon-12.
More informationStoichiometric relationships 1
Stoichiometric relationships 1 Chapter outline Describe the three states of matter. Recall that atoms of diff erent elements combine in fi xed ratios to form compounds which have diff erent properties
More informationChapter 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
More informationStoichiometry. 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
More information1 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
More informationTHE BRIDGING COURSE TO SIXTH FORM CHEMISTRY Birchwood High School
THE BRIDGING COURSE TO SIXTH FORM CHEMISTRY Birchwood High School Mrs Ryan Chemistry Please also access the website below which is a link to a really good PPT that will help to bridge the gap between GCSE
More informationTOPIC 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
More informationConcentration 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
More informationChemistry. Bridging the Gap Summer Homework. Name..
Chemistry Bridging the Gap Summer Homework Name.. Standard Form Number Number in standard form 0.008 8 x 10-3 0.07 7 x 10-2 0.55 5.5 x 10-1 0.000052 0.048 0.0086 0.00086 0.000086 0.0000000001 0.000455
More information1.22 Concentration of Solutions
1.22 Concentration of Solutions A solution is a mixture formed when a solute dissolves in a solvent. In chemistry we most commonly use water as the solvent to form aqueous solutions. The solute can be
More informationUnit 4. Chemical Calculations
Index Unit 4. Chemical Calculations 1.- Chemical reactions...2 1.1.- What is a chemical reaction?...2 1.2 The law of conservation of mass...2 1.3 Balance of chemical reactions...2 1.4.- Rate of reaction...3
More informationNo Brain Too Small. Credits: Four
No Brain Too Small Level 1 Science 2015 90944 Demonstrate understanding of aspects of acids and bases Credits: Four Achievement Achievement with Merit Achievement with Excellence Demonstrate understanding
More informationBullers Wood School. Chemistry Department. Transition to A Level Chemistry Workbook. June 2018
Bullers Wood School Chemistry Department Transition to A Level Chemistry Workbook June 2018 This booklet contains questions for you to work through and answer over the summer to prepare for the A level
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
More informationIf Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?
If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,
More informationSet 4 Marking Scheme: Acid Bases & Salts 2010
Set 4 Marking Scheme: Acid Bases & Salts 00 ACID AND BASES PAPER : STRUCTURE (a) Neutralisation KOH + H SO 4 K SO 4 + H O Correct formulae of reactants and products Balanced equation i. H +, OH -, K +
More informationNine 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
More information(DO NOT WRITE ON THIS TEST)
Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationYear 12 Chemistry Summer Work 2018
Year 12 Chemistry Summer Work 2018 Complete this multiple choice quiz, using your own knowledge in 1 hour you will need a periodic table and a calculator for some of the questions. Record your answers
More informationName... Requirements for the task and Chemistry lessons
Name... HAUTLIEU SCHOOL CHEMISTRY Pre AS and IB Diploma Task Expectations All sections of the task will be attempted please check you have answered all questions (even those on the back page) Answers should
More informationChemistry Calculations CHEMISTRY A L C U T I O N S. 1. Methods. These sheets belong to. KHS Oct 2013 page 1. N5 - Book 1
CHEMISTRY A L C U LA T I N S C 1. Methods These sheets belong to KHS ct 2013 page 1 This is the first of hopefully two booklets written to teach the calculations for National 5 Chemistry as taught in Scotland.
More informationPersonalised Learning Checklists AQA Trilogy Chemistry Paper 1
AQA TRILOGY Chemistry (8464) from 2016 Topics T5.1 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
More informationFunsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017
Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +
More informationC2.6 Quantitative Chemistry Foundation
C2.6 Quantitative Chemistry Foundation 1. Relative masses Use the periodic table to find the relative masses of the elements below. (Hint: The top number in each element box) Hydrogen Carbon Nitrogen Oxygen
More informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:
More informationAtomic Structure and the Periodic Table. AQA Chemistry topic 1
Atomic Structure and the Periodic Table AQA Chemistry topic 1 1.1 Atoms, elements and compounds The structure of the atom Everything in the universe is basically made up of atoms. An atom is the smallest
More information4.4.1 Reactivity of metals Metal oxides The reactivity series. Key opportunities for skills development.
4.4 Chemical changes Understanding of chemical changes began when people began experimenting with chemical reactions in a systematic way and organising their results logically. Knowing about these different
More informationmohd faisol mansor/chemistry form 4/chapter 7 CHAPTER 7 ACIDS AND BASES HCl (g) H 2 O H + (aq) + Cl - (aq) NaOH(s) H 2 O Na + (aq) + OH - (aq)
CHAPTER 7 ACIDS AND BASES Arrhenius Theory An acid is a chemical compound that produces hydrogen ions, H + or hydroxonium ions H3O + when dissolve in water. A base defined as a chemical substance that
More information1 Some Basic Concepts of Chemistry
1 Some Basic Concepts of Chemistry Multiple Choice Questions (MCQs) Q. 1 Two students performed the same experiment separately and each one of them recorded two readings of mass which are given below.
More informationSymbols. Table 1 A set of common elements, their symbols and physical state
Symbols Symbols are a kind of shorthand system for writing down elements and compounds. Each element has a particular one or two letter symbol. The first letter of a symbol is always capital, and if there
More informationYear 10 Chemistry Exam June 2011 Multiple Choice. Section A Mulltiple Choice
Year 10 Chemistry Exam June 2011 Multiple Choice Section A Mulltiple Choice 1. An aqueous solution is obtained when: a. a substance dissolves in any liquid b. a substance is dissolved in water c. when
More informationStoichiometry CHAPTER 12
CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs
More information1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER. Homogeneous (SOLUTIONS)
TOPIC 1: STOICHIOMETRIC RELATIONS 1.1 Introduction to the Particulate Nature of Matter and Chemical Change MATTER Mass Volume Particles Particles in constant motion MATTER Pure Matters Mixtures ELEMENTS
More informationA Level Chemistry. Ribston Hall High School. Pre Course Holiday Task. Name: School: ii) Maths:
A Level Chemistry Ribston Hall High School Pre Course Holiday Task Name: School: GCSE Grades in i) Chemistry or Science: ii) Maths: 1 The following are a series of questions on topics you have covered
More informationIB Topics 1 & 11 Multiple Choice Practice
IB Topics 1 & 11 Multiple Choice Practice 1. How many atoms of nitrogen are there in 0.50 mol of (NH 4) 2CO 3? 1 2 3.01 10 23 6.02 10 23 2. What is the value of x when 32.2 g of Na 2SO 4 xh 2O are heated
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More informationTOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry.
TOPIC 9. CHEMICAL CALCULATIONS III - stoichiometry. Stoichiometric calculations. By combining a knowledge of balancing equations with the concept of the mole, it is possible to easily calculate the masses
More information