ABOVE AND BEYOND
FIRST CHOICE GROUP OF SCHOOLS
GENERAL CERTIFICATE OF EDUCATION ORDINARY LEVEL
CHEMISTRY 4024/2
PAPER 2 Theory FORM 4
TIME: 2 HOURS
Additional materials: Electronic calculator
Answer paper
JANUARY 2025 MOCK EXAMINATIONS
INSTRUCTIONS TO CANDIDATES
Write your name, Centre number and candidate number in the answer sheet provided.
Answer all questions.
INFORMATION FOR CANDIDATES
The number of marks is given in brackets ( ) at the end of each question.
This question paper consists of 7 printed pages
FIRST CHOICE GROUP OF SCHOOLS EXAMINATIONS BOARD©
Section A
Answer all questions
1. (i). An element M is in period 3 of the Periodic table and has 3 valence electrons.
Give the name and nuclide notation of the element.
(2)
(ii) Write the formula of the oxide formed by the element when it reacts with oxygen and state its
acid base nature.
(2)
(b i). Write a balanced chemical equation for the reaction when zinc reacts with dilute hydrochloric
acid.
(2)
(ii). Describe a test for one of the products.
(2)
2. (a). A white powder X is strongly heated and a gas that turns lime water milky white was produced.
(i). State with a reason the identity of X.
(2)
(ii). Write a chemical equation for the reaction when X is heated strongly
(2)
(iii). Describe a chemical test to show the presence of
1. Fe ²+
2. Cu²+ (4)
3. (a). Table 1 shows a record of some industrial gases in some manufacturing processes, their uses
and how they can be identified.
Name of gas Method of Use of gas Identification of gas
manufacturing
Oxygen ......... Steel manufacturing .......
...... ...... ...... Turns lime water milky white
...... Electrolysis of water Manufacturing of ammonia .......
(7)
(b) Explain why high temperature is used in the manufacturing of ammonia even though a greater
yield is obtained at lower temperatures?
(1)
4. Fig 1 shows a general diagram that can be used for carrying out electrolysis in a school laboratory
Complete the table below
Electrolyte Electrode X Electrode Y Anode Cathode
reaction reaction
Lead(ii) Bromide Graphite Graphite
Copper(ii) sulphate Blister Copper Pure Copper
Aluminium oxide in Graphite
molten cryolite
(7)
(b). Describe the observations made during the electrolysis of molten lead (ii) Bromide
(1)
5. (a). In a titration experiment 25cm³ of aqueous ammonia required 21.50cm³ of 0.1mol/dm³ of
sulphuric acid for complete neutralisation,
H2SO4 + 2NH4OH (NH4)2SO4 + 2H2O
(i) Calculate the number of moles of sulphuric acid
(ii) Deduce the moles of ammonia
(iii) Calculate the concentration of ammonia in 25cm³ of solution
(6)
(b i). Give one physical property that is similar between carbon dioxide and sulphur dioxide. (1)
(ii). Name the process by which carbon dioxide is obtained from air. (1)
Section B
Answer 4 questions from the section
6. Fig 2 shows a set up to show how some metals reacts with chlorine
(a Name the substance than can be used as the drying agent (1)
(b). When Iron is used, the chloride produced contains 34.5% Iron.
(i). Define the term Empirical formula
(ii). Calculate the Empirical formula of the chloride
(iii).Given that the relative formula mass of the chloride is 325, Deduce the molecular mass of the
chloride
(iv).Use the molecular formula deduced above to write the chemical equation of the reaction (7)
(c). Table 4 shows some characteristics of diamond and graphite
Graphite Diamond
Electrical Conductivity Good Poor
Hardness Soft Hard
Density 2.2g/cm³ 3.5g/cm³
(i) Describe the structure of
1. Graphite
2. Diamond
(ii) Use the structure in (i) to explain the differences in the physical properties listed in the
table above (5)
(iii) State any one use of
1. Graphite
2. Diamond (2)
7. In an experiment to investigate the rate of reaction between Iron fillings and sulphuric acid,
100cm³ of 0.2 mol/dm³ sulphuric acid was added to 5g of Iron fillings. The gas produced was recorded
in time intervals as shown in table 5 below
Time/min 0 30 60 90 120 150 180
Volume 0.00 12.00 24.67 36.67 43.99 48.00 48.00
of
gas/cm³
(a) Draw a labelled diagram of the apparatus that can be used to measure the volume of gas
produced (2)
(b) (i) Plot a graph of the gas produced against tine taken. (3)
(ii) Estimate the volume of gas produced at 50min. (1)
(iii Deduce the rate of reaction at t = 60min. (3)
(iv)On the same axis sketch two more graphs to show how the graph would look like when
1. 5g of powdered Iron is used
2. 5g of granules of Iron is used. (2)
(c) State and explain two other ways of increasing the rate of reaction. (4)
8. The diagram below shows some reactions of Barium
(a)(i). Identify L, M, X and Y. (4)
(ii). Write balanced chemical equations for the formation of M, X and Y. (3)
(b). Copy and complete the table to show the two main alloys of copper, their composition and uses.
Alloy Composition Use
..... .... ....
..... .... ...
(6)
(c).Describe the biological and industrial importance of iron (2)
7. (a)(i) Copy and complete the table to show the raw materials for the production of nitric acid
Raw material Source
.... ...
... ...
(4)
(ii) State the conditions for the production of nitric acid (2)
(iii).Write 3 equations involved in the production of nitric acid. (3)
(b). Calculate the oxidation state of sulphur in
1. H2S
2. H2SO4. (2)
(c)(i). Write the chemical formula of ammonium nitrate (1)
(ii). Name the 3 bonds in ammonium nitrate. (3)
8. (a)(i) Name the chemical process used to obtain Iron in the blast furnace. (1)
(ii). Explain why
1. Silicon dioxide is used to make bricks for the walls of the furnace. (1)
2. Magnesium Oxide is used in the refractory lining of the blast furnace (1)
3. The blast furnace is never extinguished. (1)
(b)(i). Give the chemical formula of slag. (1)
(ii). State the role of slag in the blast furnace (1)
(iii).State two advantages of using alloys over pure metals. (2)
(c).(i) State the physical state of the following halogens
1. Chlorine
2. Bromine
3. Iodine (3)
(ii) Name one source of Chlorine (1)
(iii).State any two uses of Chlorine. (2)
(d) A hydrocarbon X has the relative molecular formula 42 and has 85.7% carbon
Calculate 1. The Empirical formula and
2. Molecular formula of the hydrocarbon. (2)
