(a)(i) Describe briefly the laboratory preparation of hydrogen gas from the action of steam on iron.
(ii)    Write the equation for the reaction in (a)(i).
(iii)   List three methods for the industrial preparation of hydrogen gas. 
                                                           
(b)Consider the following reaction equation:
   CO(g)    +   2H\(_{2(g)}\)                CH\(_3\)OH\(_{(g)}\) + 201 kJmol-J

Predict the effect of each of the following factors on the position of equilibrium:

(i)    decrease in temperature;
(ii)   increase in pressure;
(iii)  increase in concentration of CO\(_{(g)}\).                                                   

(c) (i)   Define condensation polymerization.
(ii)   Name two condensation polymers.
(iii)  Write the formula of ethylethanoate.                                                

(d) (i)   Define the term allotropy.
(ii)     Name two crystalline allotropes of carbon.
(iii)    State one use of each of the allotropes named in (d)(ii).     

(e)    State two differences between nitrogen (I) oxide and oxygen.        

(a) (i)  Name the ore mostly used in the extraction of aluminium.
  (ii)  Name two major impurities in the ore named in (a)(i).
  (iii)  Name the material used in making the electrodes in the extraction of aluminium.
  (iv)  Give two reasons why aluminium is commonly recycled.
  (v) Explain briefly why the anode has to be replaced at regular intervals during the extraction of aluminium.         

(b)  A current of 0.75 amperes was passed through an electrolysis containing chromium ions    for one hour and four minutes. If the mass of chromium deposited was 0.52 g, calculate the:

(i)    quantity of electricity passed;
(ii)    moles of chromium deposited;
(iii)  quantity of electricity required to deposit one mole of chromium;
(iv)  charge on the chromium ion.
[Cr = 52.0, 1 F = 96500 C]                                                 

(c)  In the contact process for the manufacture of tetraoxosulphate(VI) acid, the following reaction occurs:
2SO\(_2\)\(_{(g)}\) + O\(_2\)\(_{(g)}\)              2SO\(_3\)\(_{(g)}\)    H = - 197 kJ mol\(^{-1}\)

(i)   Name the catalyst used in the reaction;
(ii)  State the optimum temperature for this reaction;
(iii) What would be the effect on the yield of SO\(_3\) if a temperature higher than the optimum is used?      

(d)(i)  State two chemical methods by which temporary hardness of water can be removed.
(ii)  Write a balanced chemical equation for each of the methods stated in (d)(i).

(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).