MARIYA INTERNATIONAL SCHOOL. Work sheet II. Term II. Level 8 Chemistry [Paper IV] Name:
|
|
- Patricia Blake
- 5 years ago
- Views:
Transcription
1 MARIYA INTERNATIONAL SCHOOL Work sheet II Term II Level 8 Chemistry [Paper IV] Name: 1. Chemists use the concept of the mole to calculate the amounts of chemicals involved in a reaction. a) Define mole. b) 3.0 g of magnesium was added to 12.0 g of ethanoic acid. Mg + 2CH3COOH (CH3COO)2 Mg + H2 The mass of one mole of Mg is 24 g. The mass of one mole of CH3COOH is 60 g. i. Which one, magnesium or ethanoic acid, is in excess? You must show your reasoning. ii. How many moles of hydrogen were formed?
2 iii. Calculate the volume of hydrogen formed, measured at r.t.p. 2. In an experiment, 25.0cm 3 of aqueous sodium hydroxide, 0.4mol /dm 3, was neutralized by 20.0cm 3 of aqueous oxalic acid, H2C2O4. 2NaOH + H2C2O4 Na2C2O4 + 2H2O Calculate the concentration of the oxalic acid in mol /dm 3 i. Calculate the number of moles of NaOH in 25.0 cm 3 of 0.4 mol /dm 3 solution.
3 ii. Use your answer to (i) and the mole ratio in the equation to find out the number of moles of H2C2O4 in 20 cm 3 of solution. iii. Calculate the concentration, mol /dm 3, of the aqueous oxalic acid. 3. Propene reacts with hydrogen iodide to form 2 - iodopropane. CH3 CH = CH2 + HI CH3 CHI CH3 1.4 g of propene produced 4.0 g of 2 - iodopropane. Calculate the percentage yield. Moles of CH3 CH=CH2 reacted =.. Maximum moles of CH3 CHI CH3 that could be formed = Mass of one mole of CH3 CHI CH3 = 170 g Maximum mass of 2 - iodopropane that could be formed = Percentage yield % =..
4 4. 6.0g of ethanoic acid, Mr = 60, was reacted with 5.5 g of ethanol, Mr = 46. Determine which is the limiting reagent and the maximum yield of ethyl ethanoate, Mr = 88. Number of moles of ethanoic acid =... Number of moles of ethanol =... The limiting reagent is... Number of moles of ethyl ethanoate formed =... Maximum yield of ethyl ethanoate =...
5 5. What is the maximum mass of silver(i) chromate(vi) which could be obtained from 20cm 3 of aqueous silver(i) nitrate, concentration 0.2 mol /dm 3? 2AgNO3 (aq) + K2CrO4 (aq) Ag2CrO4 (s) + 2KNO3 (aq) Number of moles of AgNO3 used =... Number of moles of Ag2CrO4 formed =... Mass of one mole of Ag2CrO4 = 332 g Mass of Ag2CrO4 formed =... g
6 6. Strontium chloride-6-water can be made from the insoluble compound, strontium carbonate, by the following reactions. SrCO3 (s) + 2HCl SrCl2 (aq) + CO2 (g) + H2O (l) SrCl2 (aq) + 6H2O SrCl2. 6H2O In the above experiment, 50.0cm 3 of hydrochloric acid of concentration 2.0mol/dm 3 was used. 6.4 g of SrCl2.6H2O was made. Calculate the percentage yield. Number of moles of HCl used =... Number of moles of SrCl2.6H2O which could be formed =... Mass of one mole of SrCl2.6H2O is 267g Theoretical yield of SrCl2.6H2O =...g Percentage yield =...%
7 7. Dilute hydrochloric acid reacts with sodium carbonate solution. i. Calculate how many moles of hydrochloric acid were used.... mol ii. Use your answer to (i) and the equation for the reaction to calculate the number of moles of sodium carbonate that reacted.... mol iii. Use your answer to (ii) to calculate the concentration of the sodium carbonate solution in mol / dm mol / dm 3
8 iv. In another experiment, mol of sodium carbonate were reacted with excess hydrochloric acid. Calculate the maximum volume (at r.t.p.) of carbon dioxide gas that could be made in this reaction. 8. Calcium chloride can be made by reacting calcium carbonate with hydrochloric acid.... dm 3 An excess of calcium carbonate was added to 50.0 cm 3 of mol / dm 3 hydrochloric acid. The solution was filtered to remove the excess calcium carbonate. (a) How many moles of HCl were used in this reaction? (b) Deduce the number of moles of carbon dioxide gas made in this reaction.... mol... mol
9 (c) Calculate the mass of carbon dioxide made in this reaction.... g (d) Calculate the volume, in dm 3, of carbon dioxide made in this reaction at room temperature and pressure (r.t.p.).... dm 3 9. Chlorine, bromine and iodine are halogens. (a) Chlorine can be made in the laboratory by heating manganese (IV) oxide with concentrated hydrochloric acid. Calculate the volume of 8.00 mol / dm 3 HCl (aq) needed to react with 3.48 g of MnO2. moles of MnO2 used... mol
10 moles of HCl needed... mol volume of HCl needed... cm g of a hydrate, Cu(NO3)2.xH2O, formed 2.4 g copper(ii) oxide. Number of moles of CuO formed =... Number of moles of Cu (NO3)2.xH2O in 7.26 g =... Mass of 1 mole of Cu (NO3)2.xH2O =... g Mass of 1 mole of Cu (NO3)2 is 188 g The value of x in this hydrate =...
least reactive magnesium
1 One way of establishing a reactivity series is by displacement reactions. (a) A series of experiments was carried out using the metals lead, magnesium, zinc and silver. Each metal was added in turn to
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 informationAnhydrous strontium chloride is not used in toothpaste because it absorbs water from the atmosphere. The hexahydrate, SrCl 2.6H 2O, is preferred.
Q1.(a) Anhydrous strontium chloride is not used in toothpaste because it absorbs water from the atmosphere. The hexahydrate, SrCl 2.6H 2O, is preferred. A chemist was asked to determine the purity of 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 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 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 informationDescribe the structure and bonding in a metallic element. You should include a labelled diagram in your answer. ... [3] ...
3 Gallium is a metallic element in Group III. It has similar properties to aluminium. (a) (i) Describe the structure and bonding in a metallic element. You should include a labelled diagram in your answer.
More informationDescribe in full the colour change at the end-point of this titration. ... (1)
Q1. (a) A solution of barium hydroxide is often used for the titration of organic acids. A suitable indicator for the titration is thymol blue. Thymol blue is yellow in acid and blue in alkali. In a titration
More informationChem!stry. Assignment on Acids, Bases and Salts #
Chem!stry Name: ( ) Class: Date: / / Assignment on Acids, Bases and Salts #5 Write your answers in the spaces below: 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. 17. 18. 19. 20. 1. Which of the
More informationPRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions. Dr Chris Clay
PRACTICAL QUESTIONS TEST TUBE REACTIONS 4&11 Questions Dr Chris Clay http://drclays-alevelchemistry.com/ Q1.(a) A sample of solid chromium(iii) hydroxide displays amphoteric character when treated separately
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 informationF321: Atoms, Bonds and Groups Redox
F321: Atoms, Bonds and Groups Redox 39 Marks 1. The element strontium forms a nitrate, Sr(NO 3 ) 2, which decomposes on heating as shown below. 2Sr(NO 3 ) 2 (s) 2SrO(s) + 4NO 2 (g) + O 2 (g) Using oxidation
More informationFor the element X in the ionic compound MX, explain the meaning of the term oxidation state.
1. (a) By referring to electrons, explain the meaning of the term oxidising agent.... For the element X in the ionic compound MX, explain the meaning of the term oxidation state.... (c) Complete the table
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 informationTIME 1 hour 30 minutes, plus your additional time allowance.
Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education 2012 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC112] WEDNESDAY
More informationwhite precipitate white precipitate, dissolves in excess of NaOH brown precipitate Identity of Q Identity of R Identity of S...
Q1.The table below shows observations of changes from some test-tube reactions of aqueous solutions of compounds Q, R and S with five different aqueous reagents. The initial colours of the solutions are
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 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 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 informationPage 2. Q1.The following pairs of compounds can be distinguished by simple test tube reactions.
Q1.The following pairs of compounds can be distinguished by simple test tube reactions. For each pair of compounds, give a reagent (or combination of reagents) that, when added separately to each compound,
More informationF321: Atoms, Bonds and Groups Moles and Equations
F321: Atoms, Bonds and Groups Moles and Equations 108 Marks 1. (a) A student carries out a titration to find the concentration of some sulfuric acid. The student finds that 25.00 cm 3 of 0.0880 mol dm
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 information2.67 g (Total 1 mark)
Q1. The chloride of an element Z reacts with water according to the following equation. Zl 4(l) + 2H 2O(l) ZO 2(s) + 4Hl(aq) 1.304 g sample of Zl 4 was added to water. The solid ZO 2 was removed by filtration
More informationMOLES 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
More informationName a solid which can reduce copper(ii) oxide to copper.
1 The law of constant composition states that all pure samples of a compound contain the same elements in the same proportion by weight. A typical experiment to test this law is to prepare the same compound
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 information2017 Enrolment The 3rd. Japan University Examination. Chemistry. Do not open the examination booklet until the starting signal for the exam is given.
2017 Enrolment The 3rd Japan University Examination Examination Date: July 2016 Chemistry (60 min) Do not open the examination booklet until the starting signal for the exam is given. Please read the following
More informationFormulae,Stoichiometry and The Mole Concept
Formulae,Stoichiometry and The Mole Concept FORMULAE AND CHEMICAL EQUATIONS: 1. The following is an example of a balanced chemical equation with state symbols. Na 2 CO 3 (s) + 2HCl(aq) 2NaCl(aq) + CO 2
More informationB410U10-1 S17-B410U10-1. CHEMISTRY AS component 1 The Language of Chemistry, Structure of Matter and Simple Reactions
Surname Centre Number Candidate Number Other Names 2 GCE AS NEW B410U10-1 S17-B410U10-1 CHEMISTRY AS component 1 The Language of Chemistry, Structure of Matter and Simple Reactions FRIDAY, 26 MAY 2017
More informationComplete the table to show the relative charge of each particle and the number of each particle found in a 140 Ce 2+ ion.
1 This question is about the elements with atomic numbers between 58 and 70 (a) Cerium, atomic number 58, is a metal Complete the table to show the relative charge of each particle and the number of each
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 information2 Answer all the questions. How many neutrons are there in an atom of chlorine-37?... [1] How many electrons are needed to fill one orbital?
2 Answer all the questions 1 The answer to each part of this question is a number (a) (i) How many neutrons are there in an atom of chlorine-37? [1] (ii) How many electrons are needed to fill one orbital?
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 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 informationElements in the Periodic Table show a periodic trend in atomic radius. In your answer you should use appropriate technical terms, spelled correctly.
1 The Periodic Table is arranged in periods and groups (a) Elements in the Periodic Table show a periodic trend in atomic radius State and explain the trend in atomic radius from Li to F In your answer
More informationTHE MOLE - PART 2. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.
THE MOLE - PART 2 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which one of the following statements is a quantitative observation? a.
More informationChem!stry. Mole Calculations Assignment Twelve
Chem!stry Name: ( ) Class: Date: / / Mole Calculations Assignment Twelve 1. A gas is 46.2% carbon and 53.8% nitrogen. Under conditions of room temperature and pressure (r.t.p.) the volume of the gas is
More informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
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 informationAngel International School - Manipay 1 st Term Examination November, 2015
Grade 11B Angel International School - Manipay 1 st Term Examination November, 2015 Chemistry - I Duration: 1.00 Hour Part 1 1) A liquid boils at a temperature of 100 o C. Which other property of the liquid
More information+ 10Cl 2Mn H 2 O + 5Cl 2. Deduce the half-equation for the oxidation of chloride ions to chlorine.
Q1.Chlorine is an important industrial chemical. (a) Chlorine is formed when KMnO 4 reacts with hydrochloric acid. The ionic equation for this redox reaction is 16H + + 2MnO 4 + 10Cl 2Mn 2+ + 8H 2 O +
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 informationSome standard enthalpies of formation are given in the table below
Q1. Barium can be extracted from barium oxide (BaO) in a process using aluminium. A mixture of powdered barium oxide and powdered aluminium is heated strongly. The equation for this extraction process
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 informationCHERRY HILL TUITION AQA CHEMISTRY A2 PAPER Section A (2 marks) (1 mark) (Extra space) Property
2 Section A Answer all questions in the spaces provided. 1 (a) Define the term lattice enthalpy of dissociation. 1 (b) Lattice enthalpy can be calculated theoretically using a perfect ionic model. Explain
More informationA student wanted to make 11.0 g of copper chloride
Q1.A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride. (a) Describe how a sample of copper
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More information(a) Bleach can be made by reacting chlorine with cold aqueous sodium hydroxide. A solution of bleach contains the chlorate compound NaClO. ...
1 The chlor-alkali industry is an important part of the UK chemical industry. The raw material is brine, a concentrated aqueous solution of sodium chloride, NaCl(aq). Two products that can be manufactured
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 informationOCR A Chemistry A-Level Module 5 - Physical Chemistry & Transition Elements
OCR A Chemistry A-Level Module 5 - Physical Chemistry & Transition Elements Acids and Bases Notes and Example Calculations Answers given at the end of the booklet ph Acid Calculations Strong Acids To calculate
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 informationQuestions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..
Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative
More informationCh 4-5 Practice Problems - KEY
Ch 4-5 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
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 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 informationA student wanted to make 11.0 g of copper chloride
Q1.A student investigated the reactions of copper carbonate and copper oxide with dilute hydrochloric acid. In both reactions one of the products is copper chloride. (a) Describe how a sample of copper
More informationCHAPTER 1 QUANTITATIVE CHEMISTRY
Page 4 Ex 4 (a) element; (b) mixture; (c) compound; (d) element; (e) compound 5. (a) mixture; (b) compound; (c) mixture; (d) element; (e) compound. Page 5 Ex 1.1 3. C 4. D 5. C 6. D 7. a) 0.20 b) 1.2 10
More informationCandidate Name Centre Number Candidate Number. Energy, Rate and Chemistry of Carbon Compounds
AS CHEMISTRY Specimen Assessment Materials 21 Candidate Name Centre Number Candidate Number AS CHEMISTRY COMPONENT 2 Energy, Rate and Chemistry of Carbon Compounds SPECIMEN PAPER 1 hour 30 minutes ADDITIONAL
More informationExtra Questions. Chemical Formula IUPAC Name Ionic, Molecular, or Acid. ethanol. sulfurous acid. titanium (IV) oxide. gallium sulfate.
Chemistry 30 Recap Chemistry 20 Complete the following chart: Extra Questions Name: Chemical Formula IUPAC Name Ionic, Molecular, or Acid PbI2 (s) ethanol NaHS (aq) sulfurous acid H2O2 (l) titanium (IV)
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 informationUnit-8 Equilibrium. Rate of reaction: Consider the following chemical reactions:
Unit-8 Equilibrium Rate of reaction: Consider the following chemical reactions: 1. The solution of sodium chloride and silver nitrate when mixed, there is an instantaneous formation of a precipitate of
More informationSO 4... [2], to an excess of dilute sulfuric acid. A student adds a sample of solid potassium carbonate, K [3]
1 Chemicals called acids have been known throughout history The word acid comes from the Latin acidus meaning sour Dilute sulfuric acid, H 2 SO 4, is a common laboratory acid (a) State the formulae of
More informationCHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
More informationChemical calculations
Chemical calculations Basic concepts: 1 Those ions that are not involved in a chemical reaction are called Spectator ions 2 The relationship between the amounts (measured in moles) of reactants and products
More information, for C 2. COOH is mol dm [1] COOH by adding water until the total volume is cm 3. for C 2 COOH.
1 A student is supplied with 0.500 mol dm 3 potassium hydroxide, KOH, and 0.480 mol dm 3 propanoic acid, C 2 COOH. The acid dissociation constant, K a, for C 2 COOH is 1.35 10 5 mol dm 3. (a) C 2 COOH
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More information# Ans Workings / Remarks
# Ans Workings / Remarks 1 B Atomic mass and temperature affects the rate of diffusion of gas. The lower the atomic mass, the lighter the substance. The higher the temperature, the higher the rate of collision
More informationCHAPTER 8 SALTS. NaCl. A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion.
CHAPTER 8 SALTS A salt is an ionic substance produced when the hydrogen ion of the acid is replaced by metal ion or an ammonium ion. The salt consists of two parts, cation from base and anion from acid.
More informationA student adds the following volumes of aqueous sodium thiosulfate, dilute hydrochloric acid and distilled water to the conical flask.
1 When aqueous sodium thiosulfate and dilute hydrochloric acid are mixed, a precipitate of insoluble sulfur is produced. This makes the mixture difficult to see through. Na 2 S 2 O 3 (aq) + 2HCl (aq) S(s)
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 information2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds
2 Answer all the questions. 1 Born Haber cycles can be used to determine lattice enthalpies of ionic compounds. (a) Define, in words, the term lattice enthalpy............. [2] (b) The Born Haber cycle
More informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More information(a) Explain what is happening in stages 1 and 2. (3) (b) (i) Identify the products formed in stages 5, 6 and 7.
1 Hydrated magnesium nitrate, Mg(NO 3 ) 2.6H 2 O, is heated in a boiling tube and the following observations are made. Stage 1 Stage 2 Stage 3 Stage 4 Stage 5 Stage 6 Stage 7 The white solid forms a clear,
More informationA level Chemistry Preparation Work
A level Chemistry Preparation Work This booklet is designed to help you prepare for you re A level studies in chemistry. Tasks have been selected to improve your grounding in key skills and concepts that
More information5072 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
More informationK (Total 1 mark)
Q1.A sample of 2.18 g of oxygen gas has a volume of 1870 cm 3 at a pressure of 101 kpa. What is the temperature of the gas? The gas constant is R = 8.31 J K 1 mol 1. A 167 K B 334 K C 668 K D 334 000 K
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 informationPractice Problems Stoich!
Practice Problems Stoich! Name: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE IN QUESTIONS
More informationF321: Atoms, Bonds and Groups Group 7
F321: Atoms, Bonds and Groups Group 7 93 Marks 1. Chlorine and bromine are elements in Group 7 of the Periodic Table. Chlorine is used in water treatment. State one advantage and one disadvantage of using
More informationF321: Atoms, Bonds and Groups Acids
F321: Atoms, Bonds and Groups Acids 49 Marks 1. A student carries out experiments using acids, bases and salts. Calcium nitrate, Ca(NO 3 ) 2, is an example of a salt. The student prepares a solution of
More informationIB Topics 9 & 19 Multiple Choice Practice
IB Topics 9 & 19 Multiple Choice Practice 1. What are the oxidation states of chromium in (NH 4) 2Cr 2O 7 (s) and Cr 2O 3 (s)? 2. Which of the following is a redox reaction? 3Mg (s) + 2AlCl 3 (aq) 2Al
More informationLesson (1) Mole and chemical equation
Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)
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 informationExcellence International School Chemistry Academic Year Grade 9 Revision sheet 3 Topic: unit 8 speed of reaction
Unit 9 : 9.1&9.2 Name:... Class:.. Date: Paper 2 Excellence International School Chemistry Academic Year 2016-2017 Grade 9 Revision sheet 3 Topic: unit 8 speed of reaction 1 st term 1. A student was investigating
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 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 informationPlease hand your completed booklet to your Chemistry tutor when you begin A Level Chemistry in September
#THIS I S TH E P L AC E A-LEVEL CHEMSITRY NAME: You should complete this work ready for starting Year 1 A Level Chemistry. If there are any questions that you cannot do, even after using your GCSE notes
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 informationNECTA A-Level CHEMISTRY 2 May 2004
NECTA A-Level CHEMISTRY 2 May 2004 [04/2] SECTION A 1. (a) Draw a sketch of a cell formed by combining Zn 2+ (aq)/zn(s) and Cu 2+ (aq)/cu(s) half-cells. Indicate on the sketch the following: The positive
More informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More information... [1] (ii) Draw a dot-and-cross diagram to show the bonding in NH 3
1 Chemists have developed models for bonding and structure which are used to explain different properties. (a) Ammonia, NH 3, is a covalent compound. Explain what is meant by a covalent bond. Draw a dot-and-cross
More informationSolutions Solubility. Chapter 14
Copyright 2004 by Houghton Mifflin Company. Solutions Chapter 14 All rights reserved. 1 Solutions Solutions are homogeneous mixtures Solvent substance present in the largest amount Solute is the dissolved
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 informationWhich of the following answers is correct and has the correct number of significant figures?
Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant
More informationChem!stry. Assignment on Redox
Chem!stry Name: ( ) Class: Date: / / Assignment on Redox Question 1: Which one of the following elements is the most powerful reducing agent? A Aluminium B Copper C Lead D Potassium Question 2: Which of
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 informationTopic 1a Atomic Structure Revision Notes
Topic 1a Atomic Structure 1) Fundamental particles Atoms consist of protons, neutrons and electrons Protons and neutrons are found in the nucleus which contains most of the mass of the atom and all of
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 information1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4.
1 Zirconium (Zr) is a metal in Period 5. Its main oxidation state is +4. (a) The following are all zirconium atoms: 90 40Zr, 91 40Zr and 92 40Zr. In terms of numbers of electrons, neutrons and protons,
More informationCHERRY HILL TUITION AQA CHEMISTRY A2 PAPER Section A. Answer all questions in the spaces provided.
2 Section A Answer all questions in the spaces provided. 1 This question is about bond dissociation enthalpies and their use in the calculation of enthalpy changes. 1 (a) Define bond dissociation enthalpy
More information