(a) Give two differences between luminous and non-luminous flames.(2 marks)
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(b) How is the non-luminous flame produced? (1 mark)
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(a) The apparatus below were used to separate a mixture of liquid A and B.

State two properties of liquids that make it possible to separate using such
apparatus. (2 marks)
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(b) Give the name of the above apparatus. (1 mark)
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(a) Explain why solid Carbon (IV) oxide is preferred over ordinary ice for use by ice
cream venders. (1 mark)
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(b) Name one piece apparatus used to measure volume of gases. (1 mark)
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(c) Draw a diagram of a deflagrating spoon. (1 mark)

The table below shows the pH values of solutions P, R, Q and S.

(a) Which solution represent:
(i) Strong base - ……………………………………………… (1 mark)
(ii) Weak acid - ………………………………………………. (1 mark)
(b) Give an example of solution S. (1 mark)
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6.95g of hydrated iron (II) sulphate FeSO₄. nH₂O was dissolved in 250 cm³ solution
resulting into a 0.1M solution. Determine the value of n.
(Fe = 56, O = 16, S = 32, H = 1).

Rusting leads to fast wearing out of farm tools and equipment as well as buildings.
(a) Give the chemical name of rust. (1 mark)
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(b) What two conditions accelerate rusting process? (2 marks)
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Study the diagram below and answer the questions that follow.

(a) Write an equation for the reaction that take place in the combustion tube.
(1 mark)
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(b) Why would it not be advisable to use potassium in place of iron in the set-up?
(1 mark)
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(c) Glass wool should be heated before heating iron. Explain. (1 mark)
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I. Name the following organic compounds.
(a) (1 mark)
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(b) HOCH₂- CHOH - CH₂OH (1 mark)
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II. Given
A CH₃(CH₂)₁₆ COO^- Na⁺
B CH₃(CH₂)₆ CH(CH₃)CH₂ SO^-3 Na⁺
Identify detergent
A - ………………………………………………………………………. (1 mark)
B - ………………………………………………………………………. (1 mark)

In terms of structure and bonding, explain the following.
(a) Graphite is used as a lubricant. (1 mark)
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(b) Alluminium is better conductor of electricity then magnesium. (1 mark)
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(c) Water is a liquid at room temperature while hydrogen sulphide is a gas.
(1 mark)
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(a) Define the term molar latent heat of fusion. (1 mark)
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(b) The molar heat of fusion of ice at O0C is 6kJ mol^-1. Calculate the heat change
when 36g of ice is converted to 36g of water at 100C. (3 marks)
(SHC = 4.2^-1g K^-1, density = 1.0g/cm³3, H = 1.0, O = 16.0)
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Draw a well labeled diagram showing how blister copper is purified.

Gas Q with a relative molecular mass of 48 took 50 seconds to diffuse through a porous
diaphragm. How long will it take for the same amount of hydrogen Chloride (HCl) to
diffuse through the same diaphragm under similar conditions? (H = 1.0, Cl = 35.5).

(a) Calculate the oxidation state of chromium in the ion Cr₂ O₂^-. (1 mark)
(b) Using oxidation numbers, determine from the equation below the species which
undergoes oxidation and reduction.
2FeCl_2(aq) + Cl_{2 (g)} 2Fe Cl_{3 (aq)}
Oxidation - ……………………………………………………………… (1 mark)
Reduction - ……………………………………………………………… (1 mark)

Given elements A, B and C with atomic numbers 11, 19 and 13 respectively.
(a) Compare the atomic radius of A and C. Explain. (2 marks)
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(b) Compare reactivity of A and B. (1 mark)
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Haber process (the manufacture of ammonia gas) is given by the following equation.
N_{2 (g)} + 3H_{2 (g)} 2NH_{3 (g)} ΔH = -92kJ mol-1.
State and explain the effect of:
(a) Introducing some drops of water to the equilibrium. (1 mark)
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(b) Pumping nitrogen gas to the equilibrium mixture. (1 mark)
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(c) Lowering the temperature of the reaction. (1 mark)
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Elements P and Q have the following atomic numbers 19 and 8 respectively.
(i) Using dot ( ) and cross draw a diagram to show how the elements form bonds.
(1 mark)

Describe how sodium sulphate crystals can be prepared starting with 50cm³ of 2M
sodium hydroxide and 1M sulphuric (VI) acid.
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Write ionic equations to show how;
(a) (i) Excess ammonia solution reacts with a solution containing Copper II ions. (1 mark)
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(ii) Excess sodium hydroxide added to a solution containing Al³⁺ ions.
(1 mark)
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(b) Give the name of the following ion [Zn(NH₃)₄]²⁺ (1 mark)
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(a) Define electrolysis. (1 mark)
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(b) During the electrolysis of molten aluminium oxide, write the equations at the;
Anode - …………………………………………………………………………. (1 mark)
Cathode - …………………………………………………………………………. (1 mark)
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(a) Give any two differences between alpha and beta particles. (2 marks)
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(b) A radioactive isotope T decays by emitting three alpha particles to form ²¹⁴₈₃ Bi
what is the atomic number and mass number T?
Atomic number - …………………………………………………… (1 mark)
Mass number - …………………………………………………… (1 mark)

(a) Using acidified potassium dichromate (VI) solution, describe how you would
differentiate between sulphur (IV) oxide and hydrogen sulphide. (2 marks)
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(b) Identify the catalyst preffered in contact process. Explain. (2 mark)
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Study the following part of the solvay process for the manufacture of sodium carbonate
and answer the questions that follows:

(i) State the main source of Carbon (IV) oxide in the process. (1 mark)
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(ii) Write down the overall equation for the reaction in chamber I. (1 mark)
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(iii) Name process in step 1. (1 mark)
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(a) The following equation involve hydrochloric acid.
MnO_{2 (s)} + 4HCl_(aq) MnCl_{2 (aq)} + 2H₂O_(l) + Cl_{2 (g)}
State the type of reaction taking place in the reaction. (1 mark)
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(b) State two contrasting chemical properties of hydrogen and chlorine.
(2 marks)
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(a) An element O has two isotopes ¹⁶₈ O containing 90% and Isotope ¹⁸₈ O.
(i) What are isotopes? (1 mark)
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(ii) Find the R.A.M of O. (2 marks)

(a) When a hydrocarbon is completely burnt in oxygen 4.2g of Carbon (IV) oxide and 1.71g of water were formed.
(a) Determine the empirical formular of the hydrocarbon. (3 marks)
(b) Given that formula mass of compound above is 28. Find the molecular
formular. (1 mark)

(a) Name the two types of polymerization. (1 mark)
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(b) Study the section of the polymer below and answer the questions that follow.

(i) Give the name of the polymer above. (1 mark)
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