• A-Gamma rays
• B-Beta rays
• C-Alpha rays

​An experiment was carried out to prepare crystals of magnesium sulphate. Excess magnesium powder was added to 100 cm3 of dilute sulphuric (VI) acid in a beaker and warmed until no further reaction took place. The mixture was filtered and the filtrate evaporated to saturation, then left to cool for crystals to form.
(a) (i) Write an equation for the reaction. 
(ii) Explain why excess magnesium powder was used. 
(iii) State how completion of the reaction was determined. 
(iv) What is meant by a saturated solution? 
(v) Explain why the filtrate was not evaporated to dryness. 
(b) When bleaching powder, CaOCl2, is treated with dilute nitric(V) acid, chlorine gas is released. This reaction can be used to determine the chlorine content of various samples of bleaching powders and liquids.
(i) Write an equation for the reaction of nitric(V) acid with bleaching powder.
(ii) Calculate the volume of chlorine produced when 10g of CaOCl2 is treated with excess nitric (v) acid. (Ca = 40.0; 0 = 16.0; Cl = 35.5; 1 mole of gas occupies 22.4dm3 at s.t.p) 
(c) Apart from use of chlorine gas in bleaches and water treatment, state two other uses of chlorine gas.

​(a) Complete Table I by indicating the observations, type of permanent or temporary change and name of new compound formed.

(b) Use the set-up in Figure 3 to answer the questions that follow. The flask was covered with a cloth that had been soaked in ice-cold water.

(i)State the observation made on the coloured water. Explain.
(ii) Name the gas law illustrated in Figure 3. 
(c)Use the standard electrode potentials in Table 2 to answer the questions that follow.

​(i)Write the half-cell representation for the element whose electrode potential is for hydrogen. 
(ii) Arrange the elements in order of reducing power, starting with the weakest reducing agent. 
(iii) I Select two half cells which combine to give a cell with the least e.m.f. 
II Calculate the e.m.f of the half cells identified in (iii) I. 

The diagram in figure I shows some natural and industrial processes. Study it and answer the questions that follows

​(a) Identify the processes labelled: 
A...................
B...................
C...................
D...................
(b) State the reagents and conditions required for processes B and D.
(i) Process B:
Reagent................
Conditions ............ 
(ii) Process D:
Reagent................
Conditions ............ 
(iii) Describe how process D is carried out.
(iv) State two additives used to improve the quality of soap.
(c) State the reagents required in steps F and G.
(iii) Draw the structure of terylene.
(d) (i) Name the polymer formed in step C.
(ii) State one disadvantage of the polymer formed in (d) (i).

 (a) Name two ores of iron. 
(b) Describe how the amount of iron in a sample of iron(III) oxide can be determined. 

(a) Give the symbols of the o charged particles emitted by a radioactive isotope.

​mass number 
atomic number:

(a) Define molar heat of displacement. 
(b)The following ionic equation represents the reaction between metal Y and an aqueous solution of Z2+.

Draw an energy level diagram to represent the reaction

Metal X and Y have standard electrode Potentials of —0.13 V and —0.76V respectively .The metals were Connected to form a cell as shown in Figure 4.

(a) Name the part labelled z. 
(b) State one functi0 of the part labelled Z. 
(c) Calculate the e.m.f. of the cell. 

 In the Haber process, nitrogen reacts with hydrogen according to the following equation.

(a)What would be the effect of adding a catalyst on the position of the equilibrium? 
(b) Explain why it is not advisable to use temperatures higher than 773 K in the Haber process.

 Study the flow chart in Figure 1 and answer the questions that follow.

Gas N forms a while suspension with aqueous calcium hydroxide.
(a) Name the anion present in the potassium salt. 
(b) Write an ionic equation for the formation of solid M. 
(c) Give one use of gas N.

 The following are formulae of organic compounds. Use the formulae to answer the questions that follow:

​(a) Select:
(i) two compounds which when reacted together produce a sweet smelling compound.
(ii) an unsaturated hydrocarbon. 
(b) Name the compound selected in (a) (ii).

(a) Define a soluble base. 
(b) Aqueous solutions of 2M ethanoic acid and 2M nitric(V) acid were tested for electrical conductivity. Which solution is a better conductor of electricity? Explain.

The decay rates of a sample of a radioisotope of bismuth at different time intervals is indicated in the following table.

(a)(i) Draw a graph of disintegration rate against time. 
(ii) Determine the half-life of bismuth. 
(iii) What would be the effect on the curve if half the amount of sample of bismuth were used. 
(b) Radioactivity has several applications. State one application of radioactivity in: 
(i) Medicine 
(ii) Agriculture 
(iii) Tracers 
(iv) Nuclear power station 
(c) State two dangers associated with radioactivity. 

The following steps were used to analyse a metal ore.
(i) An ore of a metal was roasted in a stream of oxygen. A gas with a pungent smell was formed which turned acidified potassium dichromate(VI) green.
(ii) The residue left after roasting was dissolved in hot dilute nitric(V) acid. Crystals were obtained from the solution.
(iii) Some crystals were dried and heated. A brown acidic gas and a colourless gas were evolved and a yellow solid remained. (iv) The solid was yellow when cold.
(v) The yellow solid was heated with powered charcoal. Shiny beads were formed.
Name the:
(a) gas formed when the ore was roasted in air. 
(b) gases evolved when crystals in step (iii) were heated. 
(c) yellow solid formed in step (iii). 
(d) shiny beads in step (iv). 
(e) The yellow solid from procedure (iii) was separated, dried, melted and the melt electrolysed using graphite electrodes.
I. Describe the observations made at each electrode. 
II. Write the equation for the reaction that took place at the anode. 
(f) Some crystals formed in step (ii) were dissolved in water, and a portion of it reacted with potassium iodide solution. A yellow precipitate was formed. Write an ionic equation for this reaction. 
(g) To another portion of the solution from (f), sodium hydroxide solution was added drop by drop until there was no further change. Describe the observation made. 
(h) To a further portion of the solution from (f), a piece of zinc foil was added.
I. Name the type of reaction taking place. 
II. Write an ionic equation for the above reaction.