(a) (i)  State the collision theory of reaction rates.

(ii)  Using the collision theory, explain briefly how temperature can affect the rate of a chemical reaction.   

(b) (i) Sketch a graphical representation of Charles’ law.
(ii) Calculate the volume of oxygen that would be required for the complete combustion of 2.5 moles of ethanol at s.t.p.
[molar volume at s.t.p = 22.4 dm\(^3\)]                                        

(c) (i)  Define esterification.  
(ii)  Give two uses of alkanoates.
(iii)  Give the products of the alkaline hydrolysis of ethyl ethanoate.

(d) A tin coated plate and a galvanized plate were exposed for the same length of time.
(i)  Which of the two plates corrodes faster?
(ii)  Explain briefly your answer in 2 (d) (i).                               

(a) Arrange the three states of matter in order of decreasing:
(i)        kinetic energy;
(ii)       force of cohesion.                                                         

(b) Consider the redox reaction equation:

(i)         State the change in oxidation number of:
I.          magnesium;
II.         hydrogen.

(ii)        Which of the species is being:
I.          oxidized;
II.         reduced?

(iii)       Identify the oxidizing agent.                                         

(c) (i) State two differences between boiling and evaporation.
(ii) What will be the effect of reduction of atmospheric pressure on the boiling point of water?                                                        

(d) For a given chemical equilibrium system, what is the significance of the equilibrium constant K?                                                    

(e) Consider the following organic compounds:
C\(_3\)H\(_7\)COOH; (CH\(_3\))\(_3\)COH.

Give the IUPAC name of each compound.                    

(f) Why are organic compounds classified on the basis of functional groups?                          
(g) State three differences between the solubility of solids in liquids and gases in liquids.                                                            

(h) Write a balanced chemical equation for the reaction between fluorine and water.        

(i) Define the term basicity of an acid.                               

(a) A compound of carbon, hydrogen and chlorine contains 0.48 g of carbon, 0.08 g of hydrogen and 1.42 g of chlorine.
(i)  Determine the empirical formula of the compound.
(ii)  If the molar mass of the compound is 99, calculate the molecular formula of the compound.
[H = 1.0, C = 12.0, Cl = 35.5]                                                    

(b) State three properties of NaCl (s) which shows that it is ionic.                   

(c)   Consider the following reaction equation:

(i)        On the same diagram, sketch and label a reaction profile for a catalysed and uncatalysed reaction between H\(_2\) and O\(_2\).
(ii)        Indicate the possible positions of the activated complexes for the reaction profiles in (c)(i).                                    
(d)        The petrochemical industry produces addition polymers using one of the fractions obtained from crude oil.
(i)         Name the fraction used as a raw material for the process.
(ii)        What process is used to obtain the fraction from crude oil?
(iii)       Name two gaseous hydrocarbons that can be used in making polymers.
(iv)       Describe briefly how these hydrocarbons can be obtained.
(v)        Name the polymer produced from one of the hydrocarbons named in (d)(iii).
                                                                                                                                

a) (i) Describe, using the kinetic theory of matter, what happens when potassium chloride dissolves in water.
(ii) Give a reason why the process in (a) (i) is endothermic.                      

(b) (i) An underground iron pipe is less likely to corrode if it is bonded at intervals with magnesium rods. Give reasons for this observation.
(ii)  State the stages involved in the rusting of iron.
(iii) State the condition for the rusting of iron in water.                                 

(c) (i)  What is a spontaneous reaction?
(ii)  State two conditions that could make a reaction spontaneous.
(iii) Explain briefly why one gramme of sodium reacts more rapidly with water at 250C than one gramme of calcium at the same temperature.
(iv)   Write equations for the reactions in (c)(iii).                                        

(d)   What mass of lead (II) trioxocarbonate (IV) would contain 35.0 g of lead?
[C=12.0, O = 16.0, Pb = 207.0]                                                         

(e)  Name the type of intermolecular force present in:

(i)         fluorine;
(ii)        hydrogen fluoride.                                                                   

(a)   Outline the procedures for the treatment of water for town supply.   

(b) (i)  State two main impurities present in bauxite.
(ii)  Give one reason why bauxite is usually preferred as the ore for the extraction of aluminium.
(iii)   Outline the manufacture of aluminium form purified bauxite.            

(c) (i)  Explain briefly the term fine chemical industry.
(ii)  State two differences between a fine chemical and a heavy chemical.

(d) (i)  Write a balanced chemical equation for the combustion of coal.
(ii)   If 5.4 g of coal is burnt completely, calculate the amount of oxygen measured at s.t.p. that would be required for the combustion.
[C = 12.0, O = 16.0, Molar volume of a gas at s.t.p. = 22.4 dm\(^3\)]        

(e) Name two substances which can be used as electrodes during the electrolysis of acidified water.