Iron is obtained from haematite using a blast furnace shown if figure 5 below.

a) Four raw materials are required for the production of iron. Three of these are iron oxide, hot air and limestone
Give the name of the fourth raw material 
b) Write an equation for the reaction in which carbon (IV) oxide is converted into carbon (II) oxide.
c) Explain why the temperature in the region marked Y is higher than that of the incoming hot air. 
d) State one physical property of molten slag other than density that allows it to be separated from molten iron as shown in figure 5. 
e) One of the components of the waste gases is Nitrogen (IV) oxide describe the adverse effects it has on the environment.
f) Iron from the blast furnace contains about 5% carbon
i) Describe how the carbon content is reduced. 
ii) Why is it necessary to reduce the carbon content?

b) State the observation that would be made in the following tests to distinguish between:
i) Sodium and copper burning pieces of each in air. 
ii) Sodium and Magnesium by placing small pieces of each in cold water which contains two drops of phenolphalein. 
c) The atomic numbers of Na and Mg are 11 and 12 respectively. Which of the elements has a higher ionization energy? Explain. 
d) Naturally occurring uranium consists of three isotopes which are radioactive.

​i) Which of these isotopes has the longest half-life? Give a reason
ii) Calculate the relative atomic mass of uranium

(iv)State one  use of radioactive isotopes in the  paper industry

(a)Figure 3 show the changes that take place between states of matter. Some of them have been identified and others labelled.

i) Give the names of the processes
I H 
II G 
ii) Name one substance that can undergo process F when left in an open container in the laboratory. 
iii) The process J is called deposition. Using water as an example, write an equation that represents the process of deposition. 
b) Figure 4 shows the beating curve for water.

i) Give the names of the intermolecular forces of attraction in the segments;
I MN 
II RS 
ii) The heats of fusion and vaporization of water are 334.4 Jg-1 and 1159.4 Jg-1 respectively.
I Explain why there is a big difference between the two.
II How is the difference reflected in the curve? 
c) Coal, oil and natural gas are major sources of energy. They are known as fossil fuels. Hydrogen is also a source of energy.
i) State and explain two reasons why hydrogen is a very attractive fuel compared to fossils. 
ii) State one disadvantage of using hydrogen fuel instead of fossil fuels.

a) the schematic diagram shows part of the Solvay process used for the manufacture of sodium carbonate.

i) Explain how the sodium chloride required for this process is obtained from sea water. 
ii) Two main reactions take place in UNIT I . The first one is the formation of ammonium hydrogen carbonate.
I. Write an equation for this reaction 
II. Write an equation for the second reaction 
iii) State how the following are carried out: 
I Process I
II) Process II
iv)In an experiment to determine the percentage purity of the sample of sodium carbonate produced in the Solvay process, 2.15 g of the sample reacted completely with 40.0cm3 of 0.5 M sulphuric acid.
I calculate the number of moles of sodium carbonate that reacted. 
II Determine the percentage of sodium carbonate in the sample. (Na= 23.0, C= 12.0, O = 16.0) 
b) Name two industrial uses of sodium carbonate 

The set-up below (figure 2) was used to electrolyse a bromide of metal D DBr2

i) Write equation for the reactions at the
I cathode 
II anode 
ii) The electrodes used in the experiment were made of carbon and metal D. which of the two electrodes was used as the anode? Give a reason. 
iii) Give a reason why this experiment is carried out in a fume cupboard.
iv) When a current of 0.4A was passed for 90 minutes, 2.31 g of metal D were deposited.
I Describe how the amount of metal D deposited was determines.
II Calculate the relative atomic mass of metal D. (I Faraday = 96500 coulombs)

​a) Draw the structures of the following compounds: 
i) 2- methylbut -2 ene;
ii) heptanoic acid
b) Describe a physical test that can be used to distinguish between methanol and hexanol. 
c) Use the flow chart below to answer the questions that follow.

​
i) Name:
(I) the type of reaction that occurs in step II; 
(II) Substance B. 
ii) Give the formula of substance C. 
iii) Give the reagent and the conditions necessary for the reaction in step (IV)

a) Two reagents that can be used to prepare chlorine gas are manganese (IV) oxide and concentrated hydrochloric acid.
i) Write an equation for the reaction. 
ii) Give the formula of another reagent that can be reacted with concentrated hydrochloric acid to produce chlorine gas. 
iii) Describe how the chlorine gas could be dried in the laboratory 
b) In an experiment, dry chlorine gas was reacted with aluminium as shown in figure 1.

i) Name substance A. 
ii) Write an equation for the reaction that took place in the combustion tube. 
iii) 0.84 g of aluminium reacted completely with chlorine gas. Calculate the volume of chlorine gas used (Molar gas volume is 24dm3, Al = 27).
iv) Give two reasons why calcium oxide is used in the set up.

​Starting with red roses, describe how;
(i) a solution  containing the red pigment may be prepared
(ii) the solution can be shown tobe an indicator.

(a) Draw the structure of compound N formed in the following reaction.

​(b) Give one use of compound N.

​The energy level diagram below shows the effect of a catalyst on the reaction path.

a)What does point M represent?
b) With reference to the energy level diagram, explain how a catalyst speeds up the rate of a reaction.

The following reaction is in equilibrium in a closed container

State giving reasons how an increase in pressure would affect the amount of hydrogen.

The graph below shows the relationship between pressure and the temperature of a gas in a fixed volume container.

a) State the relationship between pressure and temperature that can be deduced from the graph. 
b) Using kinetic theory, explain the relationship shown in the graph.

For each of the following reactions, state the observation and write the formula of the
Compound responsible for the observation:
a) Bromine water is added to aqueous potassium iodide; 
b) Excess aqueous ammonia is added to copper (II) hydroxide (precipitate).

The boiling points of some compounds of hydrogen with some elements in groups 4 and 6 of the periodic table are given below.

a) Which of the compounds CH4 and SiH4 has stronger intermolecular forces? 
b) Explain why the boiling points of H2O and H2S show different trends from that of CH4 and SiH4

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

a) What observation would be made in step I? 
b) Name another substance that could be used in step 2. 
c) Give the name of substance H.