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WorksheetsQ1 - Metal Reactivity
Total questions: 29
Worksheet time: 15mins
When iron reacts with oxygen, iron oxide is made. i. Write the word equation for this reaction.
Iron + Oxygen → Iron oxide
Iron + Hydrogen → Iron oxide
Iron + Oxygen → Iron chloride
Iron + Nitrogen → Iron oxide
What type of reaction occurs when a metal reacts with oxygen?
Oxidation reaction
Reduction reaction
Neutralization reaction
Precipitation reaction
Calculate the relative formula mass of iron oxide, Fe₂O₃ (relative atomic masses: Fe = 56, O = 16)
160
120
144
176
Order these metals from most to least reactive.
Potassium > Lithium > Gold
Gold > Potassium > Lithium
Lithium > Potassium > Gold
Gold > Lithium > Potassium
When lithium is added to water, bubbles of hydrogen gas are given off. Describe the test for hydrogen gas.
A lit splint produces a 'pop' sound in the presence of hydrogen gas.
A glowing splint relights in the presence of hydrogen gas.
Hydrogen gas turns limewater milky.
Hydrogen gas changes blue litmus paper to red.
When testing the reactivity of metals with water, the same volume of water must be used. i. State the name of the piece of apparatus used to measure the volume of water.
Measuring cylinder
Burette
Beaker
Test tube
When testing the reactivity of metals with water, the same volume of water must be used. ii. Describe one other variable that must be controlled in this reaction.
The mass or amount of metal used must be controlled.
The color of the metal must be controlled.
The shape of the container must be controlled.
The temperature of the room must be controlled.
When gold is added to water, nothing happens. Explain why.
Gold is unreactive and does not react with water.
Gold dissolves in water to form a solution.
Gold reacts vigorously with water to produce hydrogen gas.
Gold changes color when added to water.
When testing the reactivity of metals with water, the same volume of water must be used. Complete the equation by adding state symbols.
2Li (s) + 2H₂O (l) → 2LiOH (aq) + H₂ (g)
2Li (l) + 2H₂O (g) → 2LiOH (s) + H₂ (aq)
2Li (aq) + 2H₂O (s) → 2LiOH (g) + H₂ (l)
2Li (g) + 2H₂O (aq) → 2LiOH (l) + H₂ (s)
Hydrogen and nitrogen used in the Haber process are obtained from:
Hydrogen from water, nitrogen from air
Hydrogen from air, nitrogen from water
Both from air
Both from water
Describe the conditions needed for the haber process.
450°C, 200 atmospheres, and an iron catalyst.
100°C, 1 atmosphere, and a platinum catalyst.
700°C, 500 atmospheres, and a copper catalyst.
300°C, 50 atmospheres, and a nickel catalyst.
Balance the equation for the Haber process. N₂ + ....H₂ → ...NH₃
N₂ + 3H₂ → 2NH₃
N₂ + 2H₂ → 2NH₃
N₂ + 3H₂ → NH₃
N₂ + H₂ → 2NH₃
When nitrogen and hydrogen are reacted together, the reaction can reach a dynamic equilibrium. This is when the forward and __________ reverse reaction happen at the same _______.
rate
temperature
pressure
volume
Which of the following metals is usually found uncombined in the Earth’s crust?
silver
lithium
calcium
copper
State why lead can be extracted by heating lead oxide with carbon.
Because lead oxide is less reactive than carbon
Because lead oxide is more reactive than carbon
Because carbon is less reactive than lead
Because carbon cannot reduce lead oxide
Lead is extracted by heating lead oxide with carbon. Electrolysis is not used to extract lead because:
lead is too reactive
lead is not reactive enough
electrolysis is too expensive
carbon cannot reduce lead oxide
During electrolysis of a solution, hydrogen can be made at the cathode. i. State the name of the gas that can be produced at the anode.
Oxygen
Hydrogen
Chlorine
Nitrogen
State what is meant by the term electrolysis.
Electrolysis is the process of using electricity to break down a compound into its elements or simpler compounds.
Electrolysis is the process of combining elements to form a compound using heat.
Electrolysis is the process of filtering mixtures using a sieve.
Electrolysis is the process of separating solids from liquids by evaporation.
During electrolysis of a solution, hydrogen can be made at the cathode. iii. Copper sulfate solution was made by dissolving 16.43 g of copper sulfate in water to make 500 cm³ of solution. Calculate the concentration of this solution in g dm⁻³. Give your answer to three significant figures.
32.9 g dm⁻³
8.22 g dm⁻³
16.4 g dm⁻³
65.8 g dm⁻³
Solid copper sulfate is dissolved in water to be electrolysed. i. State why copper sulfate solution, rather than solid copper sulfate, must be used in this experiment.
Because only ions in solution can move freely to conduct electricity and allow electrolysis to occur.
Because solid copper sulfate is more reactive than its solution.
Because water increases the mass of copper sulfate.
Because solid copper sulfate is a better conductor than its solution.
Solid copper sulfate is dissolved in water to be electrolysed. ii. Which of the following ions from the copper sulfate solution will be attracted to the negatively charged cathode:
Cu2+
SO4 2-
H+
OH-
Molten zinc iodide is electrolysed. i. State the two products formed in this reaction.
Zinc and iodine.
Zinc and chlorine.
Zinc and bromine.
Zinc and oxygen.
Which of the following best describes how to conduct electrolysis of a molten compound in the laboratory?
By passing an electric current through the molten compound using suitable electrodes
By heating the compound in the presence of air
By dissolving the compound in water and filtering it
By mixing the compound with acid and observing the reaction
State whether the zinc is oxidised or reduced in this reaction.
Oxidised
Reduced
Calculate the maximum mass of zinc that can be obtained from 173 tonnes of iron oxide, ZnO. (relative atomic masses: O = 16, Zn = 65)
143 tonnes
156 tonnes
101 tonnes
65 tonnes
Aluminium cannot be extracted by heating its oxide with carbon. Aluminium has to be extracted from its oxide by electrolysis. Explain why.
Aluminium is more reactive than carbon, so carbon cannot displace aluminium from its oxide. Therefore, electrolysis is required to extract aluminium from its oxide.
Aluminium oxide is too soft to be reduced by carbon, so electrolysis is required.
Carbon reacts with aluminium oxide to form aluminium carbide, so electrolysis is required.
Aluminium cannot conduct electricity, so only electrolysis can extract it.
Magnesium is above aluminium in the reactivity series. Suggest the method used to extract magnesium from its ore.
Electrolysis is used to extract magnesium from its ore because it is very reactive.
It is extracted by heating with carbon.
It is extracted by roasting in air.
It is extracted by reduction with hydrogen.
State the 4 stages of a life cycle assessment, in order.
The 4 stages are: 1. Raw material extraction, 2. Manufacturing and processing, 3. Use and maintenance, 4. Disposal or recycling.
The 4 stages are: 1. Product design, 2. Packaging, 3. Transportation, 4. Marketing.
The 4 stages are: 1. Research and development, 2. Sales, 3. Customer feedback, 4. Product recall.
The 4 stages are: 1. Concept development, 2. Testing, 3. Launch, 4. Promotion.
Evaluate the advantages of recycling instead of extracting metals from the Earth’s crust.
Recycling metals saves energy, reduces environmental impact, conserves natural resources, and reduces waste compared to extracting metals from the Earth's crust.
Recycling metals increases energy consumption and depletes natural resources.
Recycling metals causes more pollution than extracting metals from the Earth's crust.
Recycling metals has no effect on waste reduction or resource conservation.
