Chemistry KS4 Quantitative Chemistry Homework Booklet Name: _________________________________________ Class: _________________________________________ Teacher: _______________________________________ Page 1 of 29 Homework Task Due Date Teache r Signat ure Qu01 Relative Mass and Moles Qu02 Equations and Calculations Qu03 From masses to balanced equations Qu04 The yield of a chemical reaction Qu05 Atom economy Qu06 Expressing concentration Qu07 Titrations RP Qu08 Titration Calculations Qu09 Volumes of Gases
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· Web viewHomework Task Due Date Teacher Signature Qu01 Relative Mass and Moles Qu02 Equations and Calculations Qu03 From masses to balanced equations Qu04 The yield of a chemical
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Read the Qu01 sections on your knowledge organisers before you begin.
Comprehension Task Iron has three oxides with the following formulae:
Iron (II) Oxide, FeO Iron (III) Oxide, Fe2O3
Iron (II,III) Oxide, Fe3O4
Calculate the relative formula mass of each oxide of Iron.Page 1 of 25
Homework Task Due Date
Teacher Signature
Qu01 Relative Mass and MolesQu02 Equations and CalculationsQu03 From masses to balanced equationsQu04 The yield of a chemical reactionQu05 Atom economyQu06 Expressing concentrationQu07 Titrations RPQu08 Titration CalculationsQu09 Volumes of Gases
Qu 01
Relative Mass and Moles – I should know… R A G
How to calculate the relative atomic mass of an element using the proportions of isotopes
How to calculate relative formula mass of an element [H] How to calculate the number of moles (or mass) of a
substance, using its mass (or number of moles) and relative formula mass
[H] What Avogadro’s constant tells us about moles
Qu01 Relative Mass and Moles Exam Question Practise
Q1.
(a) What is the relative formula mass (Mr) of titanium dioxide, TiO2?
Relative atomic masses (Ar): O = 16 Ti = 48
Tick one box.
64
80
128
768
(1)
Comprehension Task Iron has three oxides with the following formulae:
Iron (II) Oxide, FeO Iron (III) Oxide, Fe2O3
Iron (II,III) Oxide, Fe3O4
Calculate the relative formula mass of each oxide of Iron.
Page 2 of 25
(b) How many atoms are present in one mole of fluorine atoms?
Tick (✔) one box.
2.03 × 1026
2.06 × 1023
6.02 × 1023
6.02 × 1026
(1)
(c) An element has three isotopes.
The table shows the mass numbers and percentage of each isotope.
Isotope 1 Isotope 2 Isotope 3
Mass number 24 25 26
Percentage (%) 78.6 10.1 11.3
Calculate the relative atomic mass (Ar) of the element.
Give your answer to 3 significant figures.(2)
(d) Complete the table below to show the number of atoms of carbon and oxygen in the formula of zinc carbonate, ZnO3
Element Number of atoms in
Page 3 of 25
the formula ZnCO3
zinc, Zn 1
carbon, C
oxygen, O
(2)
(e) When 125 g zinc carbonate is heated, 81 g zinc oxide is produced.
Calculate the mass of carbon dioxide produced.(1)
(f) Calculate the relative formula mass (Mr) of the hydrocarbon in the diagram above.
Relative atomic masses (Ar): H = 1 C = 12(2)
(g) Calculate the relative formula mass (Mr) of aluminium sulfate Al2(SO4)3
(h) Calculate the relative formula mass (Mr) of lead nitrate Pb(NO3)2
Relative atomic masses (Ar): N = 14 O = 16 Pb = 207(2)
Page 4 of 25
Qu 02
Equations and Calculations – I should know… R A G
[H] What balanced equations tell you about chemical reactions
[H] How to use balanced equations to calculate masses of reactants and products
Qu 03
From Masses to Balanced Equations – I should know… R A G
[H] How to work out a balanced equation using the masses of the reactants and products
[H] Why a limiting reactant affects the amount of a product that can be obtained from a reaction
Read the Qu02 and Qu03 and keyword sections on your knowledge organisers before you begin.
Comprehension Task
The image above shows copper reacting with oxygen. Balance the equation below so that it matches
Page 5 of 25
TYPE HERE
Qu02/Qu03 Balanced Equations and Calculations Exam Question Practise
Q1.
(a) In industry, methanol is produced by reacting carbon monoxide with hydrogen.
The equation for the reaction is:
CO(g) + 2H2(g) ⇌ CH3OH(g)
How many moles of carbon monoxide react completely with 4.0 × 103 moles of hydrogen?
Tick one box.
1.0 × 103 moles
2.0 × 103 moles
Comprehension Task
The image above shows copper reacting with oxygen. Balance the equation below so that it matches
Page 6 of 25
4.0 × 103 moles
8.0 × 103 moles
(1)
(b) Nitrogen and hydrogen are passed over iron to produce ammonia in the Haber Process.
Balance the equation for the reaction.
N2 + H2 → NH3
(1)
(c) Some iron ores contain iron oxide (Fe2O3).
Complete and balance the equation for a reaction to produce iron from iron oxide.
_____ Fe2O3 + _____ C → ___________ + _____ CO2
(2)
(d) Nitrogen dioxide reacts to produce nitrogen and oxygen in catalytic converters.
Complete the equation for this reaction.
The equation should be balanced.
____ NO2 (g) ⟶ ____________ + ____ O2 (g)(2)
(e) The reaction of hydrogen with carbon monoxide is shown below:
Balance the equation for the reaction.
H2 + CO ⟶ C6H14 + H2O(1)
Q2. A student wanted to make 11.0 g of copper chloride.
The equation for the reaction is:
CuCO3 + 2HCl → CuCl2 + H2O + CO2
Relative atomic masses, Ar: H = 1; C = 12; O = 16; Cl = 35.5; Cu = 63.5
Calculate the mass of copper carbonate the student should react with dilute hydrochloric acid to make 11.0 g of copper chloride.
You should show your working
Page 7 of 25
(4)
Q3. In a reaction, 40 kg of titanium chloride was added to 20 kg of sodium.
The equation for the reaction is:
TiCl4 + 4 Na ⟶ Ti + 4 NaCl
Relative atomic masses (Ar): Na = 23 Cl = 35.5 Ti = 48
Explain why titanium chloride is the limiting reactant.
You must show your working.(4)
Qu 04
Yield of a Chemical Reaction. [CHEMISTRY ONLY] – I should know… R A G
What is meant by the yield of a chemical reaction What factors affect the yield How to calculate theoretical yield of a reaction How to calculate percentage yield of a reaction
Read the Qu 04 sections on your knowledge organisers before you begin.
Comprehension Task Percentage yield of a chemical reaction is given by the following formula:
Percentage yield = (actual yield ÷ theoretical yield) x 100
A student carried out a reaction to produce a chemical. She calculated the yield for the reaction as 106%
Explain why this yield is incorrect. Page 8 of 25
Qu 04 Yield Exam Question Practise
Q1.
(a) A company calculates that 500 g of titanium dioxide should produce 1.2 kg of titanium chloride.
However, the company finds that 500 g of titanium dioxide only produces 900 g of titanium chloride.
Calculate the percentage yield.(2)
(b) For a reaction the percentage yield was 92.3%
Comprehension Task Percentage yield of a chemical reaction is given by the following formula:
Percentage yield = (actual yield ÷ theoretical yield) x 100
A student carried out a reaction to produce a chemical. She calculated the yield for the reaction as 106%
Explain why this yield is incorrect.
Page 9 of 25
The theoretical maximum mass of titanium produced in this batch was 13.5 kg.
Calculate the actual mass of titanium produced.(2)
(c) A student tried to make 11.0 g of copper chloride.
The percentage yield of copper chloride was 79.1 %.
Calculate the mass of copper chloride the student actually produced.(2)
Q2.
(a) Calculate the minimum mass of zinc that needs to be added to 0.500 g of iodine so that the iodine fully reacts.
The equation for the reaction is:
Zn + I2 ⟶ ZnI2
Relative atomic masses (Mr): Zn = 65 I = 127(3)
Page 10 of 25
A scientist obtains 12.5 g of zinc iodide using the above reaction
The percentage yield in this reaction is 92.0%.
(b) What is the maximum theoretical mass of zinc iodide produced in this reaction?(3)
(c) Suggest one reason why the percentage yield in this reaction is not 100%.(1)
Qu 05
Atom Economy [CHEMISTRY ONLY] – I should know…
How to calculate the atom economy of a reaction with respect to a desired product
Why atom economy is important in industrial processes
Read the Qu 05 sections on your knowledge organisers before you begin.
Comprehension Task The image below shows 2 ways of producing 1-phenylethanol, which is an important chemical feedstock. It is used to make styrene, the monomer for polystyrene. (you do not need to know about this structure for your GCSE)
Page 11 of 25
Qu05 Atom Economy Exam Question Practise
Q1.
(a) The percentage atom economy for a reaction is calculated using:
The equation for the reaction of copper carbonate and sulfuric acid is:
Comprehension Task The image below shows 2 ways of producing 1-phenylethanol, which is an important chemical feedstock. It is used to make styrene, the monomer for polystyrene. (you do not need to know about this structure for your GCSE)
Page 12 of 25
Calculate the percentage atom economy for making copper sulfate from copper carbonate.
(3)
(b) An equation for a reaction is:
NiO + C ⟶ Ni + CO
Calculate the percentage atom economy for the reaction to produce nickel.
Relative atomic masses (Ar): C = 12 Ni = 59
Relative formula mass (Mr): NiO = 75
Give your answer to 3 significant figures.(3)
Q2.
Zinc sulfate can be made by two methods.
The equations for the two methods are:
Method 1: ZnO + H2SO4 ⟶ ZnSO4 + H2O
Method 2: ZnCO3 + H2SO4 ⟶ ZnSO4 + H2O + CO2
(a) Calculate the percentage atom economy for making zinc sulfate in Method 1.
The concentration of the sodium hydroxide was 0.102 mol / dm 3
Concordant results are those within 0.10 cm 3 of each other.
Calculate the concentration of the citric acid in mol / dm 3
Use only the concordant results from the table in your calculation.
You must show your working.(5)
Page 20 of 25
Q3.
A student titrated 25.0 cm3 portions of dilute sulfuric acid with a 0.105 mol/dm3 sodium hydroxide solution.
The table below shows the student’s results.
Titration1
Titration2
Titration3
Titration4
Titration5
Volume of sodium hydroxide solution in cm3 23.50 21.10 22.10 22.15 22.15
The equation for the reaction is:
2 NaOH + H2SO4 ⟶ Na2SO4 + 2 H2O
Calculate the concentration of the sulfuric acid in mol/dm3
Use only the student’s concordant results.
Concordant results are those within 0.10 cm3 of each other.(5)
Qu 09 Volumes of Gases [CHEMISTRY ONLY] – I should know… R A G
[H] How to calculate the volume (in dm3) of a gas at room temperature and pressure from its mass (in g) and relative formula mass
[H] How to calculate volumes (in dm3) of gaseous reactants
Page 21 of 25
and products from a balanced equation and a given volume (in dm3) of a gaseous reactant or product
Qu09 Gas Volumes Exam Question Practise
Q1.
Read the Qu09 sections on your knowledge organisers before you begin.
Comprehension Task 44 grams of CO2 and 32 grams of O2 occupy the same volume.
Explain why, and how it is possible when the gases have different sized molecules.
Page 22 of 25
A student measured the volumes of gases collected every minute for 20 minutes.
The graph below shows the student’s results.
Calculate the amount in moles of chlorine collected after 20 minutes.
Use the graph above
The volume of one mole of any gas at room temperature and pressure is 24.0 dm3
Give your answer in standard form.(3)
Q2.(a) Sodium carbonate reacts with dilute hydrochloric acid:
Na2CO3 + 2HCl → 2NaCl + H2O + CO2
Page 23 of 25
The carbon dioxide was collected at room temperature and pressure.The volume of one mole of any gas at room temperature and pressure is 24.0 dm3.
How many moles of carbon dioxide is 95.0 cm3?
Give your answer to three significant figures.(2)
(b) Calculate what mass of Sodium Carbonate (Na2CO3) was needed to produce 0.95cm3 of carbon dioxide
Relative atomic masses, Ar: Na = 23; C = 12; O = 16; (3)
Q3.Air bags are used to protect the passengers in a car during an accident. When the crash sensor detects an impact it causes a mixture of chemicals to be heated to a high temperature. Reactions take place which produce nitrogen gas. The nitrogen fills the air bag.
The mixture of chemicals contains sodium azide (NaN3) which decomposes on heating to form sodium and nitrogen.
2NaN3 → 2Na + 3N2
A typical air bag contains 130 g of sodium azide.
Calculate the volume of nitrogen that would be produced when 130 g of sodium azide decomposes.
Relative atomic masses (Ar): N = 14; Na = 23
Page 24 of 25
The volume of one mole of any gas at room temperature and pressure is 24.0 dm3.