Q1.
This question is about metals and metal compounds.
(a) Iron pyrites is an ionic compound.
The diagram below shows a structure for iron pyrites.
Determine the formula of iron pyrites.
Use the diagram above.
___________________________________________________________________
(1)
(b) An atom of iron is represented as
Give the number of protons, neutrons and electrons in this atom of iron.
Number of protons _______________________
Number of neutrons _______________________
Number of electrons _______________________
(3)
(c) Iron is a transition metal.
Sodium is a Group 1 metal.
Give two differences between the properties of iron and sodium.
1. _________________________________________________________________
___________________________________________________________________
2. _________________________________________________________________
___________________________________________________________________
(2)
Nickel is extracted from nickel oxide by reduction with carbon.
(d) Explain why carbon can be used to extract nickel from nickel oxide.
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Page 1 of 45
, ___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(e) An equation for the 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.
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___________________________________________________________________
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Percentage atom economy = _____________________ %
(3)
(Total 11 marks)
Q2.
Titanium is a transition metal.
Titanium is extracted from titanium dioxide in a two-stage industrial process.
Stage 1 TiO2 + 2 C + 2 Cl2 ⟶ TiCl4 + 2 CO
Stage 2 TiCl4 + 4 Na ⟶ Ti + 4 NaCl
(a) Suggest one hazard associated with Stage 1.
___________________________________________________________________
___________________________________________________________________
(1)
(b) Water must be kept away from the reaction in Stage 2.
Give one reason why it would be hazardous if water came into contact with sodium.
___________________________________________________________________
Page 2 of 45
, ___________________________________________________________________
(1)
(c) Suggest why the reaction in Stage 2 is carried out in an atmosphere of argon and
not in air.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(d) Titanium chloride is a liquid at room temperature.
Explain why you would not expect titanium chloride to be a liquid at room
temperature.
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___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
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(3)
In Stage 2, sodium displaces titanium from titanium chloride.
(e) Sodium atoms are oxidised to sodium ions in this reaction.
Why is this an oxidation reaction?
___________________________________________________________________
___________________________________________________________________
(1)
(f) Complete the half equation for the oxidation reaction.
Na ⟶ ____________ + ____________
(1)
(g) In Stage 2, 40 kg of titanium chloride was added to 20 kg of sodium.
The equation for the reaction is:
TiCl4 + 4 Na ⟶ Ti + 4 NaCl
Page 3 of 45
, Relative atomic masses (Ar): Na = 23 Cl = 35.5 Ti = 48
Explain why titanium chloride is the limiting reactant.
You must show your working.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
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(4)
(h) For a Stage 2 reaction the percentage yield was 92.3%
The theoretical maximum mass of titanium produced in this batch was 13.5 kg.
Calculate the actual mass of titanium produced.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Mass of titanium = ______________________ kg
(2)
(Total 15 marks)
Q3.
Older cars are tested each year to measure the amount of pollutants contained in exhaust
fumes.
The table below shows the maximum allowed percentages of exhaust pollutants for petrol
cars.
Maximum allowed percentage
Age of car (%) of exhaust pollutant
in years Carbon Unburned
monoxide hydrocarbons
16−24 0.30 0.02
3−16 0.20 0.02
Page 4 of 45
This question is about metals and metal compounds.
(a) Iron pyrites is an ionic compound.
The diagram below shows a structure for iron pyrites.
Determine the formula of iron pyrites.
Use the diagram above.
___________________________________________________________________
(1)
(b) An atom of iron is represented as
Give the number of protons, neutrons and electrons in this atom of iron.
Number of protons _______________________
Number of neutrons _______________________
Number of electrons _______________________
(3)
(c) Iron is a transition metal.
Sodium is a Group 1 metal.
Give two differences between the properties of iron and sodium.
1. _________________________________________________________________
___________________________________________________________________
2. _________________________________________________________________
___________________________________________________________________
(2)
Nickel is extracted from nickel oxide by reduction with carbon.
(d) Explain why carbon can be used to extract nickel from nickel oxide.
___________________________________________________________________
Page 1 of 45
, ___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(e) An equation for the 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.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Percentage atom economy = _____________________ %
(3)
(Total 11 marks)
Q2.
Titanium is a transition metal.
Titanium is extracted from titanium dioxide in a two-stage industrial process.
Stage 1 TiO2 + 2 C + 2 Cl2 ⟶ TiCl4 + 2 CO
Stage 2 TiCl4 + 4 Na ⟶ Ti + 4 NaCl
(a) Suggest one hazard associated with Stage 1.
___________________________________________________________________
___________________________________________________________________
(1)
(b) Water must be kept away from the reaction in Stage 2.
Give one reason why it would be hazardous if water came into contact with sodium.
___________________________________________________________________
Page 2 of 45
, ___________________________________________________________________
(1)
(c) Suggest why the reaction in Stage 2 is carried out in an atmosphere of argon and
not in air.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(2)
(d) Titanium chloride is a liquid at room temperature.
Explain why you would not expect titanium chloride to be a liquid at room
temperature.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
(3)
In Stage 2, sodium displaces titanium from titanium chloride.
(e) Sodium atoms are oxidised to sodium ions in this reaction.
Why is this an oxidation reaction?
___________________________________________________________________
___________________________________________________________________
(1)
(f) Complete the half equation for the oxidation reaction.
Na ⟶ ____________ + ____________
(1)
(g) In Stage 2, 40 kg of titanium chloride was added to 20 kg of sodium.
The equation for the reaction is:
TiCl4 + 4 Na ⟶ Ti + 4 NaCl
Page 3 of 45
, 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)
(h) For a Stage 2 reaction the percentage yield was 92.3%
The theoretical maximum mass of titanium produced in this batch was 13.5 kg.
Calculate the actual mass of titanium produced.
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Mass of titanium = ______________________ kg
(2)
(Total 15 marks)
Q3.
Older cars are tested each year to measure the amount of pollutants contained in exhaust
fumes.
The table below shows the maximum allowed percentages of exhaust pollutants for petrol
cars.
Maximum allowed percentage
Age of car (%) of exhaust pollutant
in years Carbon Unburned
monoxide hydrocarbons
16−24 0.30 0.02
3−16 0.20 0.02
Page 4 of 45
