(a) Write an equation to show the effect of heat on the nitrate of: 
(i) Potassium
(ii) Silver
(b) The table below gives information about elements Ai, A2, A3, and A4
i) In which period of the periodic table is element A2? Give a reason.

(ii) Explain why the atomic radius of:
I. Ai is greater than that of A2;
II. A4 is smaller than its ionic radius.
(iii) Select the element which is in the same group as A3.
(iv) Using dots (•) and crosses(x) to represent outermost electrons, draw a diagramto show the bonding in the compound formed when Ai reacts with A4. 

b) Describe two chemical tests that can be used to distinguish between ethane and ethane.
c)The following scheme represents various reactions starting with propan-1-ol.
Use it to answer the questions that follow.

​i) Name one substance that can be used in step I.
ii) Give the general formula of X.

iii)Write the equation for the reaction in step IV.
iv) Calculate the mass of propan-1-ol which when burnt completely in air at room temperature and pressure would produce 18dm3 of gas. (C = 12.0; O = 16.0; H = 1.0; Molar gas volume = 24dm3)

The diagram below represents a set up of an electrolytic cell that can be used in the production of aluminium.

​(a) On the diagram, label the anode.
(b)Write the equation for the reaction at the anode.
(c) Give a reason why the electrolytic process is not carried out below 950°C.
(d)Give a reason why the production of aluminium is not carried out using reduction process
(e)Give two reasons why only the aluminium ions are discharged
(f)State two properties of duralumin that makes it suitable for use in aircraft industry.
(g)Name two environmental effects caused by extraction of aluminium.

The set up below can be used to produce sodium hydroxide by electolysing brine.

(i) Identify gas Y.
(ii)Describe how aqueous sodium hydroxide is formed in setup above.
(iii)One of the uses of sodium hydroxide is in manufacture of soaps. State one other use of sodium hydroxide.
(b) Study the information given in the table below and answer the questions that follow.

(i) Construct an electrochemical cell that will produce the highest
(ii) Calculate the emf of the cell constructed in (i) above.
(iii)Why is it not advisable to store a solution containing E+ ions in the container made of H? 

(a) Methanol is manufactured from carbon (IV) oxide and hydrogen gas according to the equation:

The reaction is carried out in the presence of a chromium catalyst at 700K and 30kPa. Under these conditions, equilibrium is reached when 2% of the carbon (IV) oxide is converted to methanol
(i)How does the rate of the forward reaction compare with that of the reverse reaction when 2% of the carbon (IV) oxide is converted to methanol?
(ii)Explain how each of the following would affect the yield of methanol:
I Reduction in pressure
II Using a more efficient catalyst
(iii) If the reaction is carried out at 500K and 30kPa, the percentage of carbon (IV) oxide converted to methanol is higher than 2%
I what is the sign of ΔH for the reaction? Give a reason 
II Explain why in practice the reaction is carried out at 700K but NOT at 500K
(b)Hydrogen peroxide decomposes according to the following equation:

(a) Describe the process by which Nitrogen is obtained from air on a large scale. 
(b) Study the flow chart below and answer the questions that follow.

(i) Identify gas J.
(ii) Using oxidation numbers, show that ammonia is the reducing agent in step (VI)
(iii) Write the equation for the reaction that occurs in step (V).
(iv) Give one use of ammonium nitrate.
(c) The table below shows the observations made when aqueous ammonia was added to cations of elements E, F and G until in excess.

​Use the information in the table below to answer the questions that follow. The letters do not represent the actual symbols of the elements.

​(a) Give reasons why the melting point of:
(i) S is higher than that of R; 
(ii) V is lower than that of U. 
(b) How does the reactivity of W with Chlorine compare with that of R with chlorine? 
Explain.
(c) Write an equation for the reaction between T and excess oxygen.
(d) When 1.15g of R were reacted with water, 600cm3 of gas was produced.
Determine the relative atomic mass of R. (Molar gas volume = 24 000 cm3).
(e) Give one use of element V.

When a student was stung by a nettle plant, a teacher applied an aqueous solution of ammonia to the affected area of the skin and the
student was relieved of pain. Explain. 

​A mixture contains ammonium chloride, copper (II) oxide and sodium chloride. Describe how each of the substances can be obtained form the mixture. 

Describe an experimental procedure that can be used to extract oil from nut seeds. 

Hydrogen sulphide is a highly toxic and flammable gas. It is normally prepared in a fume chamber.
(a) Name two reagents that can be used to prepare hydrogen sulphide in the laboratory.
(b) One of the uses of hydrogen sulphide is to produce sulphur as shown in the following equation:
 2H2S(g) + S02 (g) -> 3S(s) + 2H20(1)
Identify the reducing agent in this reaction and give a reason for your answer. 
(c) Other than production of sulphuric (VI) acid, state one commercial use of sulphur.

Charcoal is a fuel that is commonly used for cooking. When it burns it forms two oxides.
(a) Name the two oxides. 
(b) State one use of the two oxides. 

Given the following substances: wood ash, lemon juice and sodium chloride.
(a) Name one commercial indicator that can be used to show whether wood ash, lemon juice and sodium chloride are acidic, basic or neutral. 
(b) Classify the substances in 15(a) above as acids, bases or neutral.

The set-up below was used to collect a dry sample of a gas

​Give two reasons why the set-up cannot be used to collect carbon (IV) oxide gas.