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Kansbag Chemistry Paper 2 Question Paper

Kansbag Chemistry Paper 2

Course:Secondary Level

Exam Year:2009

Name Admission Number Class

233/2
CHEMISTRY
Paper 2
TIME: 2 Hours

KANSBAG PROJECTIONS FORM FOUR ENTRY TERM 1 EXAMINATION 2009
Kenya Certificate of Secondary Education
CHEMISTRY
PAPER 2
TIME: 2 Hours

Instructions
- Answer all the questions in the spaces provided.
- Mathematical tables / electronic calculators may be used.
- All working must Clearly be shown

For Examiner’s Use Only
Question Maximum Score Candidate’s Score
1
2
3
4
5
6
Total Score

1) a) The grid below represents part of the periodic table study it and answer the questions that follow. (The letters do not represent the actual symbols of the elements).
A
B
C D E
F

i) What name is given to the group of elements to which C and F belong? (1mk)

ii) Which letter represents the element that is the least reactive? (1mk)

iii) What type of a bond is formed when B and E react? Explain. (2mks)

iv) Write the formula of the compound formed when element D and oxygen react.
(1mk)

v) On the grid indicate with a tick the position of element G which is in the third period of periodic table and forms G3– ions. (1mk)

b) Study the information in the table below and answer the questions that follow.
Substance Melting point (°C) Boiling Point (°C) Solubility in water Density at room temp. g/cm3
H -117 78.5 very soluble 0.8
J -78 -33 very soluble 0.77 x 10-3
K -23 77 insoluble 1.6
L -219 -133 slightly soluble 1.33 x 10-3
i) Which substance would dissolve in water and would be separated from solution by fractional distillation? Give a reason. (2mk)

ii) Which substance is a liquid at room temperature and when mixed with water two layers would be formed? Explain. (2mks)

iii) Which letter represents a substance that is a gas at room temperature and which can be collected;
a) Over water? Explain. (2mks)

b) By downward displacement of air? (Density of air 1.29 x 10-3 g/cm3 of room temperature) (1mk)

2) The diagram below shows the laboratory preparation of Sulphur (IV) Oxide.

a) i) Identify the mistake in the set-up and correct it. (2mks)

ii) Name solid X. (1mk)

iii) Write an equation for the reaction giving the gas (1mk)

b) i) Describe an experiment to show that sulphur (IV) oxide gas contains sulphur. Write an equation. (3mks)

ii) How would you test gas to show it is sulphur (IV) oxide? (1mk)

iii) Give two uses of sulphur (IV) oxide. (2mks)

c) Sulphur is mostly found in underground deposits.
i) Name the method used for its extraction. (1mk)

ii) Name the two allotropes of sulphur (1mk)

iii) Give any two uses of sulphur. (2mks)

d) Concentrated sulphuric acid (IV) acid is added to sugar. Describe the observation made.
(2mks)

3) a) Name the following compounds. (2mks)
i) CH3(CH2)2CHClCH3

ii) CH3CCCHBrCHBrCH3

b) Give the structural formula of; (2mks)
i) 2 – lodo – 3,4 dimethyl hexane.

ii) 1, 1, 2, 2, tetrachloro ethane

c) i) What is meant by isomerism? (1mk)

ii) Draw and name two isomers of butane. (2mks)

d) Study the schemes below and answer the questions that follow:

i) Name the reagents used in. (3mks)
Step I
Step II
Step IV
ii) Write an equation for complete combustion of (1mk)

iii) Explain one disadvantage of the continued use of items made from the compound formed in step III. (2mks)

4) a) Name one raw material from which sodium hydroxide is manufactures. (1mk)

b) Sodium hydroxide pellets were accidentally mixed with sodium chloride. 17.6g of the mixture was dissolved in water to make one litre of solution. 100cm3 of the solution was neutralized by 40cm3 of 0.5M sulphuric acid.
i) Write an equation for the reaction that took place. (1mk)

ii) Calculate the;
I. Number of moles of the substance that reacted with sulphuric acid. (2mks)

II. Number of moles of the substance that would react with sulphuric acid in one litre of solution. (1mk)

III. Mass of unreacted substances in the one litre of solution (H = 1.0; Na = 23.0; Cl = 35.5, O =.16.0) (2mks)

c) The diagram below shows an incomplete set-up to prepare and collect ammonia gas.

i) Name solid M (1mk)

ii) Complete the diagram to show how a dry sample of ammonia gas can be obtained. (2mks)

d) In an experiment, excess ammonia gas was passed over heated copper (III) oxide in a combustion tube.
i) State the observation that was made in the combustion tube at the end of the experiment. (1mk)

ii) What property of ammonia is shown in the above reaction? (1mk)

iii) Name one use of ammonia. (1mk)

5) Use the flow chart below to answer the questions that follow.

a) i) Name substances X and Y. (2mks)

ii) Name any two substances being recycled in the process. (1mk)

iii) Name the processes that take place at S and R. (2mks)

iv) Name the chamber labeled Q. (1mk)

v) Write the equations for the reaction taking place in:
I. Q:
II. T: (2mks)
b) Sodium carbonate produced is stored as washing soda.
i) What is the chemical name of washing soda? (1mk)

ii) State Two uses of Sodium carbonate. (2mks)

6) In an experiment; a piece of Magnesium ribbon was cleaned with steel wool: 2.4g of the clean Magnesium ribbon was placed in a crucible and completely burnt in oxygen. After cooling, the product weighed 4.0g.
a) Explain why it is necessary to clean the Magnesium ribbon. (1mk)

b) Why was there increase in mass? (1mk)

c) Why was there increase in mass? (1mk)

d) Write the equation for the reaction which took place in the crucible. (1mk)

e) The product in the crucible was shaken with water and filtered. Explain the observation which was made when blue and red litmus paper were dropped into the filtrate (3mks)

f) Calculate the volume of oxygen gas used during the burning (O = 16; Molar gas volume is 24,000cm3 atom r.t.p.) (4mks)

g) When 1.08g of aluminum foil were heated in a stream of chlorine gas; the mass of the product formed was 3.47g. Calculate the;
i) Maximum mass of the product if chlorine was in excess. (3mks)

ii) Percentage yield of the product formed. (1mk)

Kansbag Chemistry Paper 2 Question Paper

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