(a) Consider the following reaction sequence.

(i) What process leads/tathe formation of K?

(ii) Write the formula of K.

(iii) Write the structural formula of L and name L.

(iv) Name A\(_n\)

(v) Write the structure of M and name M.

(b)(i) What are carbohydrates?

(ii) Give one example each of a I. monosaccharide; II. disaccharide; III. polysaccharide.

(c) Consider the following structure of a simple sugar :

(i) Which functional group makes the compound a reducing agent?

(ii) State what would C = O be observed when I. the compound is mixed with Fehling's solution and boiled;

I. few drops of concentrated H\(_2\)SO\(_4\) is added to the sample of the compound. H—C—OH

(iii) Write an equation for the reaction in (c)(ii)(II).

(d) A hydrocarbon Z with molecular mass 78 on combustion gave 3.385 g of CO\(_2\) and and 0.692 g of H\(_2\)O. Determine the molecular formula of Z. [ H = 1, C = 12, O = 16]

(a)(1) Define covalent bond.

(ii) Give two properties of covalent compounds

(ii) With the aid of a diagram, show how ammonia molecule is formed

(iv) Illustrate with a diagram the formation of ammonium ion?

(v) What type of bond(s) exist(s) in I. ammonia, H. ammonium ion? (\(_1\)H\(_7\)N)

(b)(i) Write three subatomic particles with their corresponding relative masses. CH\(_2\)OH

(ii) Name the possible states in which water can exist.

(c) (i) State Graham's law of diffusion

(ii) Arrange the following gases, He, CH\(_4\) and N\(_2\) in order of increasing rates of diffusion. Give a reason for the order. [ H = 1, He = 4, C = 12, N = 14 ]

(d) Draw the structures of the following compounds:

(i) 2,3-dimethylbutane;

(ii) 1,4-dibromocyclohexane.

(a)(i) What are acidic oxides?

(ii) Give one example of each of the following oxides: I. acidic oxide; II. basic oxide; III. amphoteric oxide; IV. neutral oxide

(b)(i) Define each of the following terms;  I. Heat II. Heat of neutralization

(ii) Weite the above  an equation to illustrate each of the terms in (b)(i) above

(ii) Given that the standard heat of combustion of butane (C\(_4\)H\(_{(10)}\) is + 5877 kJmol\(^{-1}\), calculate the heat of 14.5 g butane. [ H = 1, = 12 ]

(c) (i) Name two allotropes of sulphur

(ii) State one difference between the two allotropes.

(d)(i) Give two characteristics of noble eases

(ii) State one use each of I. He; II. Ar.

(e) State what is observed on warming ammonium trioxonitrate (V) with sodium hydroxide.

 (a)(i) Define hard water

(ii) Name two substances responsible for hardness in water

(iii) Give two methods for the removal of hardness in water.

(b)(i) What are the raw materials require for the manufacture of tetraoxosulphate (VI) acid by the contact process?

(ii) Write an equation for tr reaction that requires a catalyst in the contact process (iii) State the catalyst used in (b)(ii).

(c)(i) Give two uses of sodium tetraoxosulphate (VI) Consider the reaction represented by the following equation:

Na\(_2\)SO\(_4\).10H\(_2\)O\(_{(s)}\)  \(\to\) Na\(_2\)SO\(_4\).H\(_2\)O + 9H\(_2\)O\(_{(g)}\)

(ii) What name is given to this type of reaction?

(iii) Calculate the solubility of Na\(_2\)CO\(_3\) at 25°C. if 30.0 cm\(^3\) of its saturated solution at that temperature gave 1.80 g of the anhydrous salt. [C = 12, 0 = 16, Na = 23]

(d)(i) Define the term activated complex

(ii) State one reason why a collision may not produce a chemical reaction

(iii) The formation of water gas is represented by the following equation:

C\(_{(s)}\) + H\(_2\)O\(_{(g)}\) \(\to\) CO\(_{(g)}\) + H\(_{2(0)}\) \(\Delta\)H= + 131 kJmol\(^{-1}\)

Draw an energy profile diagram for the reaction showing the I. activated complex, II. enthalpy of reactants.

(a) Define the following terms:(i) Saturated solution; (ii) Solubility.

(b) In an experiment to determine the solubility of a given salt Y, the following data were provided:

Mass of dry empty dish = 7.16 g

Mass of dish + saturated solution of salt Y = 17.85 g

Mass of dish + salt Y = 9.30 g Temperature of solution = °C

Molar mass of salt Y = 100

Density of solution Y = 1.00 g cm\(^{-3}\) Calculate the solubility of salt Y in

(i) g dm\(^{-3}\) of solution, (ii) mol dm\(^{-3}\) of solution.

(c) State the type of bond broken on melting each of the following substances: (i) NaCI\(_{(s)}\) (ii) CO\(_{2(s)}\) (iii) SiO\(_{2(s)}\) (iv) Al\(_{(s)}\)

(d) Explain the following observations: (i) the chemical reactivity of alkali metals increases down the group; (ii) Mg has higher melting point than Na; (iii) K is a better reducing agent than Na.

(e)(i) What are isotopes? (ii) Lithium exists as \(^6_3\)Li and \(^7_3\)Li in the ratio 2:25. Calculate the relative atomic mass of the lithium.