A student investigates the decomposition of hydrogen peroxide.
0.2 g of oxygen gas is produced in the reaction.
The student uses 0.5 g of manganese(IV) oxide as a catalyst in the reaction.
How much manganese(IV) oxide remains at the end of the reaction?
A 0.2 g
B 0.3 g
C 0.5 g
D 0.7 g
[1]
Hydrogen gas, H2, reacts with oxygen gas, O2, to make water, H2O.
What is the atom economy for this reaction?
Mr: H2 = 2, O2 = 32, H2O = 18
A 50%
B 53%
C 89%
D 100%
[1]
Crude oil is separated into fractions by fractional distillation.
Look at the diagram of the fractions made in fractional distillation.
Which of these fractions has the strongest intermolecular forces?
A Bitumen
B Diesel oil
C Gases
D Kerosene
[1]
What is the general formula of the fractions produced by the fractional distillation of crude oil?
A CnH2n
B CnH2n+2
C C2H2n+1OH
D C2n+2H2
[1]
[1]
Enzymes are a type of catalyst.
Which of the following catalysts is an example of an enzyme?
A Amylase – a catalyst found in human saliva.
B Iron – a catalyst used in the Haber process.
C Manganese(IV) oxide – a catalyst used in the decomposition of hydrogen peroxide.
D Vanadium(V) oxide – a catalyst used in the Contact process.
[1]
Look at the structure of glycine.
Glycine is a monomer that reacts to form proteins.
Glycine contains two different functional groups that allow it to undergo polymerisation.
What are the two functional groups?
A −NH2 and −C=O
B −NH2 and −CH2−
C −NH2 and −OH
D −NH2 and −COOH
[1]
[1]
The Contact process produces sulfur trioxide, SO3, in an exothermic reaction.
The temperature in the reaction vessel is usually 450 °C.
What happens as the temperature is increased to 600 °C?
A Higher rate of reaction and increased yield of sulfur trioxide.
B Higher rate of reaction and decreased yield of sulfur trioxide.
C Higher rate of reaction and no change in yield of sulfur trioxide.
D Lower rate of reaction and decreased yield of sulfur trioxide.
[1]
A student reacts a hydrocarbon with bromine water.
The formula of the product is C3H6Br2.
Which is the displayed formula of the hydrocarbon?
[1]
Which of these homologous series can react together to form addition polymers?
A Alcohols and carboxylic acids
B Alkenes only
C Alkenes and alkanes
D Carboxylic acids only
[1]
Which is the correct expression for calculating the concentration of a solution in g / dm3? 12
[1]
Chemists often have a choice of reaction pathway when making a new product.
Which factor do chemists consider when choosing a reaction pathway?
A Disposal of product
B Price they can charge for the product
C Rate of reaction
D Usefulness of waste reactants
[1]
What is the formula of the functional group in alcohols ?
A −CH3
B −COOH
C −CO2
D −OH
[1]
The rate of reaction of marble chips with dilute hydrochloric acid depends on the surface area of the marble chips.
Which surface area of the marble chips gives the highest rate of reaction?
0.673 mm2 A
1030 mm2 B
[1]
This question is about the properties of materials.
Look at the table. It shows information about two materials.
| Polymer | Metal | |
| Melting Point (°C) | 100–260 | 1100 |
| Density (kg / m3) | 940 | 8940 |
| Relative electrical conductivity (10 = good, 1 = poor) | 2 | 10 |
| Flexibility | high | high |
Electrical cables are made of metal wires surrounded by a polymer coating.
Explain why
• the wire is made of metal
• the metal wire is coated with a polymer.
Use information from the table in your answer.
[3]
Aluminium is a metal.
Aluminium is extracted from an ore called bauxite.
Electrolysis is used to extract the aluminium.
Use the reactivity series to explain why aluminium cannot be extracted from bauxite by heating the bauxite with carbon.
[1]
Drinks cans are often made from aluminium.
4.0 kg of bauxite makes 1.0 kg of aluminium.
285 000 kJ of energy is needed to make 1.0 kg of aluminium from bauxite.
Aluminium can be recycled.
4.0 kg of recycled aluminium makes 3.8 kg of aluminium.
14 250 kJ of energy is needed to produce 1 kg of aluminium from recycled aluminium.
Describe how aluminium is recycled.
[2]
Describe and explain two advantages of recycling aluminium.
Use the information in the question in your answer.
[3]
The Haber process is used to manufacture ammonia, NH3.
Ammonia is used to make fertilisers, which farmers use on their crops.
Explain why fertilisers are so important in the agricultural production of crops.
[2]
Ammonium sulfate is a fertiliser made from ammonia and sulfuric acid.
The diagram shows the stages in the industrial production of ammonium sulfate.
Complete the diagram to show the raw materials in the production of ammonium sulfate.
Raw Materials
[2]
Ammonium nitrate, NH4NO3, is another fertiliser made from ammonia.
Ammonium nitrate is made by reacting ammonia with nitric acid.
Calculate the mass of ammonium nitrate that could be made from 25.5 tonnes of ammonia.
Ar: H = 1.0, N = 14.0, O = 16.0
Mass of ammonium nitrate =........ tonnes
[3]
A student makes some ammonium nitrate in the laboratory.
He predicts that he should make 12.5 g of ammonium nitrate.
His percentage yield is 80%.
Calculate the actual mass of ammonium nitrate that the student makes.
[2]
Sodium is in Group 1 of the Periodic Table.
Sodium reacts with water to make sodium hydroxide, NaOH, and hydrogen.
Write the balanced symbol equation for the reaction between sodium and water.
[2]
Sodium ions, Na +, are formed when sodium reacts with water. (b)
Look at the equation. It shows how a sodium ion is formed from a sodium atom.
The symbol e− means an electron.
The formation of a sodium ion from a sodium atom is an example of oxidation.
Explain why.
[1]
Rubidium is another element in Group 1.
Rubidium reacts much faster than sodium does.
Explain why.
Use ideas about electrons in your answer.
[2]
Another student also investigates the rate of reaction between dilute hydrochloric acid and magnesium carbonate.
He also wants to find out how the concentration of the acid changes the rate of reaction. He uses a different method.
Describe the method he uses.
Include a labelled diagram of the set‑up of the apparatus he uses.
[5]
Plot a graph of the results on the grid. Draw a line of best fit.
[4]
What happens to the rate of reaction as the temperature increases?
[1]
Explain your answer to (b)(ii).
Use ideas about collisions between particles in your answer.
[3]
Which two compounds are members of the same homologous series ?
[1]
Write down two reasons for your answer in (a)(i).
[2]
Many molecules of compound C react together to form a polymer.
This reaction is called addition polymerisation.
Draw the displayed formula of the polymer formed by compound C.
[2]
Another type of polymerisation is condensation polymerisation.
Describe one difference between addition polymerisation and condensation polymerisation.
[1]
* A student has unlabelled samples of three liquids.
The student knows that the three liquids are:
• pentane, C5H12
• pentene, C5H10
• ethanoic acid, CH3COOH.
Describe tests that the student should do to identify each of the three liquids.
Include balanced symbol equations for the reactions described.
[6]
A student neutralises potassium hydroxide with dilute sulfuric acid in a titration experiment.
Look at the student’s method for her experiment.
• Measure 25.0 cm3 of 0.200 mol / dm3 potassium hydroxide into a conical flask using a pipette.
• Add a few drops of universal indicator to the potassium hydroxide.
• Fill the burette to above the 0.00 cm3 line with dilute sulfuric acid.
• Quickly add the dilute sulfuric acid to the potassium hydroxide until the indicator changes colour.
• Repeat the experiment.
Describe and explain one improvement the student should make to her method to get a more accurate titration result.
[2]
The student repeats the experiment four times.
Look at the student’s results.
| Titration number | 1 | 2 | 3 | 4 |
| Volume of acid (cm3) | 25.75 | 23.60 | 23.70 | 23.65 |
Calculate the accurate volume of the acid that reacts with the alkali.
[2]
Look at the equation for the reaction between sulfuric acid and potassium hydroxide.
Use your answer from part (b)(i) to calculate the concentration of the dilute sulfuric acid, H2SO4, that reacted with the 25.0 cm3 of 0.200 mol / dm3 potassium hydroxide.
Give your answer to 3 significant figures.
Concentration of dilute sulfuric acid =........ mol / dm3
[4]
A student investigates the reactivity of four metals, A, B, C and D.
He adds a small piece of each metal to cold water.
He then adds a small piece of each metal to dilute hydrochloric acid.
Look at his results.
| Metal Observations in water | Observations in dilute hydrochloric acid |
| A slow bubbling | very fast bubbling |
| B no reaction | no reaction |
| C fast bubbling | very fast bubbling |
| D no change | slow bubbling |
Write down the order of reactivity of the four metals A, B, C and D.
[2]
Calculate the number of moles of hydrogen gas produced.
One mole of any gas occupies 24 dm3 at room temperature and pressure.
[2]
Use your answer from (b)(i) to calculate the mass of hydrogen gas produced.
[1]
Chromium metal, Cr, reacts with nickel sulfate solution, NiSO4. Solid nickel is made.
Two possible equations for this reaction are:
10.40 g of chromium metal reacts with excess nickel sulfate solution to make 17.61 g of nickel.
Deduce which equation, 1 or 2, represents the reaction which takes place.
Ar: Cr = 52.0, Ni = 58.7
[3]
Bioleaching is one method used to extract copper from ores.
Reactions involving bacteria slowly convert copper sulfide to a mixture of copper sulfate solution and sulfuric acid.
Describe two advantages of extracting copper using bioleaching instead of traditional mining.
[2]
Suggest one reason why the sulfuric acid produced during bioleaching may be harmful to the environment.
[1]
Evaluate the information shown in the graph.
To what extent does the graph support a link between carbon dioxide levels and global warming?
[2]
Describe and explain what is meant by the greenhouse effect.
[3]
Many scientists believe an enhanced greenhouse effect is caused by human activities.
State a human activity that can cause an enhanced greenhouse effect.
[1]
State two environmental effects of an enhanced greenhouse effect.
[2]
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