Chemistry – Year 11 – Track 2 – 2019 Page 1 of 16
DEPARTMENT FOR CURRICULUM,
LIFELONG LEARNING AND EMPLOYABILITY
Directorate for Learning and Assessment Programmes
Educational Assessment Unit
Annual Examinations for Secondary Schools 2019
YEAR 11 CHEMISTRY TIME: 2 hours
Name: _____________________________ Class: _______________
Useful
Data
Atomic numbers and relative atomic masses are shown in the periodic table printed below.
One mole of any gas occupies 22.4 dm3 at standard temperature (0 °C / 273 K) and pressure
(1 atm. / 760 mmHg / 101.3 kPa).
Faraday constant = 96500 C mol-1 Q = I t
PERIODIC TABLE
Marks Grid [For Examiner’s use only]
Question
No.
Section A Section B
1 2 3 4 5 6 7 8 9 10
Max
Mark 7 10 10 7 10 6 10 20 20 20
Theory
Total
Actual
Mark
Theory Paper: 85% Practical: 15% Final Score: 100%
Track 2 Track 2 Track 2
Page 2 of 16 Chemistry – Year 11 – Track 2 – 2019
Section A: Answer ALL questions in the spaces provided.
This section carries 60 marks.
1) Complete:
a) _________________ is a yellow-green gas that turns damp blue litmus paper
red and then bleaches it to white. (1)
b) When electrons are gained in a reduction reaction, this results in a
_________________ in oxidation number. (1)
c) Rhombic and monoclinic are the terms used to describe ________________ of
sulfur. (1)
d) A ____________________ series is a group of organic compounds with the
same functional group and similar chemical properties. (1)
e) ___________________ is the process by which long-chain hydrocarbons are
broken down into simpler molecules. (1)
f) A solution of ______________________ ____________________ gives a
muddy green precipitate with sodium hydroxide solution and a yellow
precipitate with acidified silver nitrate solution. (1)
g) When heated, ______________________ ______________________
decomposes to give a white powder which is heat stable, water vapour and a
gas which turns limewater milky. It also gives a lilac flame colour in a Bunsen
flame. (1)
Total: 7 marks
2) The following question is about nitrogen dioxide.
a) Nitrogen dioxide can be prepared in the laboratory by gently heating white
lead(II) nitrate powder. Besides nitrogen dioxide, a solid and another gas that
relights a glowing splint are formed. Complete and balance the reaction for this
chemical change:
__ Pb(NO3)2(s) → _________ (__) + __ NO2 (__) + ________ (g) (3)
Chemistry – Year 11 – Track 2 – 2019 Page 3 of 16
b) The apparatus used for the experiment mentioned in part (a) is shown below. If
the mixture of gases obtained is cooled, the two gases formed can be separated
since one of the gases is liquefied (liquid A).
i) Suggest one safety precaution when carrying out this experiment.
______________________________________________________________
__________________________________________________________ (1)
ii) From the diagram, identify Liquid A and Gas B.
Liquid A: _________________________________________
Gas B: ___________________________________________ (2)
c) Nitrogen dioxide is a brown gas and is found in equilibrium with colourless
dinitrogen tetroxide. This can be represented as follows:
2NO2 (g) ⇌ N2O4 (g) ∆H = negative
The forward reaction is exothermic (i.e. heat energy is released).
Assuming the above equilibrium is occurring in a closed gas syringe, state
how the colour would change, giving reasons, when:
i) the syringe is heated while the volume is kept constant
• colour change:
__________________________________________________
• reason:
__________________________________________________________
__________________________________________________________
__________________________________________________________
______________________________________________________ (2)
Page 4 of 16 Chemistry – Year 11 – Track 2 – 2019
ii) the volume of the gas syringe is decreased to increase pressure
• colour change:
__________________________________________________________
• reason:
__________________________________________________________
__________________________________________________________
__________________________________________________________
______________________________________________________ (2)
Total: 10 marks
3) This question is about ammonia.
In the Haber process, nitrogen and hydrogen form an equilibrium in which
ammonia is produced.
a) Give a balanced chemical equation.
___________________________________________________________ (2)
b) Is nitrogen oxidised or reduced in the process? Explain.
_______________________________________________________________
___________________________________________________________ (2)
c) State the conditions used in the process, including the catalyst.
_______________________________________________________________
___________________________________________________________ (3)
d) Draw a dot cross diagram of an ammonia (NH3) molecule (draw outer electron
shells only).
(3)
Total: 10 marks
Chemistry – Year 11 – Track 2 – 2019 Page 5 of 16
4) The following question is about sulfuric acid.
a) The Contact Process is used to produce sulfuric acid on an industrial scale. The
process consists of four steps (chemical reactions) that lead to the production of
concentrated sulfuric acid.
i) The second step involves a reversible reaction in which sulfur dioxide gas,
SO2, is oxidised to sulfur trioxide gas, SO3. Give the name or formula of the
catalyst used in this step.
_________________________________________________________ (1)
ii) State and explain whether the use of a catalyst influences the position of
equilibrium.
_____________________________________________________________
_____________________________________________________________
_________________________________________________________ (2)
b) The table below shows reactions involving sulfuric acid:
A CuO + H2SO4 → CuSO4 + H2O
B CuSO4.5H2O 𝑠𝑢𝑙𝑓𝑢𝑟𝑖𝑐 𝑎𝑐𝑖𝑑 → CuSO4 + 5H2O
C Cu + 2H2SO4 → CuSO4 + 2H2O + SO2
Using the letters, A, B and C show where sulfuric acid is acting as:
i) a dehydrating agent: __________________
ii) an acid: _______________
iii) an oxidizing agent: __________________ (3)
c) In two of the reactions shown in the table above, sulfuric acid must be used in
concentrated form. In the other reaction it may be used in dilute form.
Identify the reaction where sulfuric acid may be used in dilute form.
___________________________________________________________ (1)
Total: 7 marks
Page 6 of 16 Chemistry – Year 11 – Track 2 – 2019
5) Two students put a conical flask with sodium thiosulfate solution (Na2S2O3) on the
window sill of the laboratory. The students can clearly see a tree in the school field
through the flask. They add hydrochloric acid to the flask and the following
reaction occurs:
Na2S2O3(aq) + 2HCl(aq) → S(s) + SO2(g) + 2NaCl(aq) + H2O(l)
The mixture becomes cloudy due to the insoluble sulfur that forms and as a result,
after some time, the students can no longer see the tree through the flask.
a) The students repeat the experiment using the exact same quantities of
reactants on three different days. They measure the time taken for the tree to
disappear and obtain the following results:
Exp. Day 1: 120 s Exp. Day 2: 200 s Exp. Day 3: 150 s
Which experiment was done on the hottest day? ____________________ (1)
b) The following week, the students perform the three experiments, under the
same conditions using the same chemicals. However, they use different
concentrations of sodium thiosulfate solution. The results for the time taken for
the tree to disappear are as follows:
Exp. 1: 110 s Exp. 2: 100 s Exp. 3: 150 s
i) Which experiment had the strongest solution? ___________________ (1)
ii) Explain your answer using the Collision Theory.
____________________________________________________________
____________________________________________________________
________________________________________________________ (1)
iii) The strongest solution of Na2S2O3 had a concentration of 2.5 mol dm-3 and
50 cm3 of solution were used. Calculate the number of moles of sodium
thiosulfate that react.
(Assume that the acid is present in excess.)
____________________________________________________________
________________________________________________________ (1)
Chemistry – Year 11 – Track 2 – 2019 Page 7 of 16
iv) Calculate the amount in grams of sulfur that precipitates.
____________________________________________________________
____________________________________________________________
________________________________________________________ (2)
v) Calculate the volume of sulfur dioxide gas produced at stp.
____________________________________________________________
____________________________________________________________
________________________________________________________ (2)
vi) The students wanted to confirm that the gas produced was indeed SO2.
Describe a test to identify SO2.
____________________________________________________________
________________________________________________________ (1)
c) The students decided to use the same reaction to investigate the rate of
reaction by measuring the volume of SO2 gas produced with time. They used
50 cm3 of 2.5 mol dm-3 Na2S2O3 solution. They obtained the following graph.
The students repeated the experiment using 50 cm3 of 3.5 mol dm-3 Na2S2O3
solution. On the same graph above, draw a sketch of the pattern you would
expect the students to obtain.
(Assume that the acid is in excess in both experiments and that all the SO2 is
released as a gas.) (1)
Total: 10 marks
Page 8 of 16 Chemistry – Year 11 – Track 2 – 2019
6) Two students wanted to determine the reactivity of metals
by investigating the rate of reaction of water at room
temperature with sodium and calcium.
a) Look at the diagram and suggest which metal would be
in test tube A.
________________________________________ (1)
b) Explain your answer above using your knowledge about the position of metals
in the periodic table.
______________________________________________________________
______________________________________________________________
__________________________________________________________ (1)
c) Given that the experiment is repeated using magnesium and calcium:
i) Which of the two will be more reactive?
________________________________________________________ (1)
ii) Explain your answer with respect to their atomic structure.
____________________________________________________________
____________________________________________________________
________________________________________________________ (1)
d) Given that the reaction between sodium and water is as follows:
2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)
i) State whether sodium has been oxidised or reduced.
_______________________________________________________ (1)
ii) Give the ionic half equation for sodium in this reaction.
_______________________________________________________ (1)
Total: 6 marks
7) This question is about crude oil and the chemicals obtained from it.
a) Many of the hydrocarbon fractions obtained from crude oil belong to the alkane
group.
i) What is the general formula of alkanes?
_________________________________________________________ (1)
Chemistry – Year 11 – Track 2 – 2019 Page 9 of 16
ii) Alkanes have only single bonds in their molecules. Are they saturated or
unsaturated?
_________________________________________________________ (1)
iii) The fourth member of alkanes is butane, C4H10. Draw the structural
formulae for two isomers of this hydrocarbon.
(2)
b) Propane is another useful gas obtained from crude oil. But it can also be
prepared by hydrogenation of propene.
i) Complete the equation below for this reaction, by drawing the structures of
propene and propane.
+ H2 →
(2)
ii) What kind of reaction is this?
________________________________________________________ (1)
iii) Mention ONE use of propane.
________________________________________________________ (1)
c) Consider the following compounds.
CH3CH2CH=CH2 CH3CH2CH2CH2CH2CH3 HC≡CH
A B C
i) Write the compounds A, B and C in order of their boiling points, putting the
one with the lowest boiling point first.
________________________________________________________ (1)
ii) Which of A, B or C is most likely to be a liquid at room temperature and
pressure?
________________________________________________________ (1)
Total: 10 marks
Page 10 of 16 Chemistry – Year 11 – Track 2 – 2019
Section B: Answer any TWO questions only on the foolscaps provided. This
section carries 40 marks.
8) Lactic acid is a weak acid which can be produced by the
body when it is undergoing hard exercise. It causes
muscle pain known as ‘stitch’. For every molecule of
lactic acid that ionises in water one H+ ion is produced.
a)
i) What term is used to describe acids which release one H+ ion per molecule?
_________________________________________________________ (1)
ii) What is the meaning of the term ‘weak acid’?
_________________________________________________________ (2)
iii) Give another example of a weak acid?
_________________________________________________________ (1)
b) During a practical session, a student was asked to prepare a 1 litre standard
solution of concentration 0.5 mol dm-3 using powdered lactic acid.
i) Find the mass of one mole of lactic acid. (RAM C=12, H=1, O=16)
_____________________________________________________________
_________________________________________________________ (2)
ii) Calculate the mass of 0.5 moles of lactic acid which should be used to
prepare this solution.
_____________________________________________________________
_________________________________________________________ (1)
iii) Make a list of 6 pieces of apparatus which are needed for such a
preparation.
_____________________________________________________________
_________________________________________________________ (3)
Chemistry – Year 11 – Track 2 – 2019 Page 11 of 16
iv) Arrange the sentences in the following table in the correct order to give the
proper method used to prepare a standard solution. Use the numbers 1 to 5.
(5)
Add some distilled water to the beaker and stir with the stirring rod to dissolve the solid.
Top up to the mark with distilled water.
Using the funnel and stirring rod pour the solution into the volumetric flask.
Put a clean dry beaker on an electronic balance.
Add the calculated amount of lactic acid powder.
c) The lactic acid solution was then used to find the concentration of a solution of
sodium hydroxide using the following procedure.
• 25 cm3 NaOH were transferred to a conical flask.
• Drops of phenolphthalein was added to the conical flask.
• This NaOH was titrated using the lactic acid solution. 20.45 cm3 of the
lactic acid solution were required.
The equation for the neutralisation of lactic acid with NaOH follows:
NaOH + CH3CHOHCOOH → CH3CHOHCOONa + H2O
i) What is the name of the indicator used in this titration?
__________________________________________________________ (1)
ii) Find the number of moles present in 20.45 cm3 lactic acid solution whose
concentration was 0.5 mol dm-3.
_____________________________________________________________
_________________________________________________________ (1)
iii) Given that the acid and alkali react in the ratio of 1:1, state the number of
moles of NaOH which reacted.
__________________________________________________________ (1)
iv) This amount in moles of NaOH was present in 25 cm3 of solution. Find the
concentration by calculating how many moles of NaOH were present in
1000 cm3.
_____________________________________________________________
__________________________________________________________ (2)
Total: 20 marks
Page 12 of 16 Chemistry – Year 11 – Track 2 – 2019
9) The following article written by Claire Caruana was published last year in a local
newspaper.
Pollution in Malta continues to be among the worst in Europe, with the island
having the fourth highest levels of particles in the air compared to all
Member States. …
According to the agency, road transport, agriculture, power plants,
industries and households are the biggest emitters of air pollution. Heart
disease and stroke are the most common reasons for premature death
attributed to air pollution, followed by lung disease and lung cancer.
Times of Malta, Oct 16th, 2017
a)
i) Give the name and percentage abundance of the two most common gases
found in air.
__________________________________________________________ (2)
ii) Sulfur dioxide is one of the gases which causes atmospheric pollution. From
the article above find two sources of this gas.
__________________________________________________________ (2)
b) Carbon dioxide is a gas required by plants, but humans are now producing large
quantities of it and this is causing problems.
i) Name a human activity that is contributing to the increase of CO2 in air.
__________________________________________________________ (1)
ii) Name the effect that excess CO2 levels are having on our planet and give
one consequence of it.
_____________________________________________________________
__________________________________________________________ (2)
Chemistry – Year 11 – Track 2 – 2019 Page 13 of 16
c) Fossil fuels such as butane (C4H10) are used for cooking in Malta.
i) Name the separation technique which is used to obtain butane and other
fractions from crude oil.
__________________________________________________________ (1)
ii) Copy and balance the following equation which shows the complete
combustion of butane. (2)
_C4H10 + _O2 → _CO2 + _H2O
iii) When gas heaters are used to heat rooms in winter, without proper
ventilation, poisonous carbon monoxide can be produced. Explain why.
_____________________________________________________________
__________________________________________________________ (2)
iv) The following diagram shows the apparatus which can be used to separate
two miscible liquids X and Y. On the diagram below, label the thermometer,
condenser, fractionating column, beaker and round bottomed flask. (5)
v) Liquids X and Y have boiling points 85 °C and 120 °C respectively. Which
liquid would you expect to come out of the condenser first?
__________________________________________________________ (1)
d) Write two suggestions which you would give to the Maltese people to limit and
reduce pollution.
_______________________________________________________________
____________________________________________________________ (2)
Total: 20 marks
Page 14 of 16 Chemistry – Year 11 – Track 2 – 2019
10) In industry, aluminium is extracted by means of electricity from an ore which
contains aluminium oxide.
a) Name the ore from which aluminium is extracted.
___________________________________________________________ (1)
b) Explain why cryolite is added to the aluminium ore during the process.
___________________________________________________________ (1)
c) The anodes are made of graphite and they react with the oxygen produced by
the reaction. Complete the following equation. Include state symbols: (2)
C(__) + O2(__) → ______ (__)
d) The following half equations show the reactions at the electrodes.
Half equation 1: 2O2- - 2e- → O2
Half equation 2: Al3+ + 3e- → Al
i) Which reaction shows reduction?
_________________________________________________________ (1)
ii) Which reaction occurs at the anode?
_________________________________________________________ (1)
iii) The 1st half equation shows that 2 moles of electrons are required to release
1 mole of oxygen gas. How many moles of oxygen are produced if 10 moles
of electrons pass through the system?
__________________________________________________________ (2)
Chemistry – Year 11 – Track 2 – 2019 Page 15 of 16
iv) At stp 1 mole of oxygen occupies a volume of 22.4 dm3. Using your answer
to (iii), calculate the volume of oxygen produced in the reaction.
__________________________________________________________ (2)
v) From the 2nd equation one notes that 3 moles of electrons produce 27 g of
aluminium. Calculate the mass of aluminium produced when 30 moles of
electrons pass through the system.
_____________________________________________________________
__________________________________________________________ (2)
e) Aluminium is found in Period 3 of the Periodic table. It is a metal and conducts
electricity.
i) The following table shows the relative electrical conductivity of the elements
in period 3. Use the graph paper provided to plot a graph of Element
(x-axis) against relative electrical conductivity (y-axis). (4)
Element Relative electrical conductivity
Sodium 0.25
Magnesium 0.41
Aluminium 1.00
Silicon 0.10
Phosphorus 0
Sulfur 0
Chlorine 0
Argon 0
ii) Chlorine is non-metal. Draw a dot cross diagram of the chlorine molecule
and use it to explain why it does not conduct electricity.
_____________________________________________________________
__________________________________________________________ (4)
Total: 20 marks
Page 16 of 16 Chemistry – Year 11 – Track 2 – 2019