Explain the importance of the chemistry syllabus in four points.

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Identify four features of micro-teaching that differentiate it from other teaching practices.

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(a) Explain the difference between homogeneous and heterogeneous equilibria. (b) Given an equilibrium reaction: N2(g) + 3H2(g) <=> 2NH3(g) at 230oC: (i) write an expression of an equilibrium constant, (Kc), (ii) explain what will happen on the equilibrium if NO is removed from the system.

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Explain why, (a) Alkenes are slightly more soluble than their corresponding alkanes (b) the major product of the reaction between 1-butane and hydrogen bromide gas is secondary bromobutane, not primary bromobutane.

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State four merits of classroom tests.

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(a) Explain the concept of soil reaction. (b) Describe two sources of acid in the soil.

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Given the half-reaction equations: MnO4-(aq) + 5e- + 8H+ -> Mn2+(aq) + 4H2O(l) E0 = 1.51V ClO3-(aq) + 2H+ + 2e- -> ClO2-(aq) + H2O(l) E0 = 1.19V (a) Give the overall balanced cell reaction, (b) calculate E0cell.

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(a) Write electronic configuration of: (i) Copper ( Cu), 29 (ii) calcium ion ( Ca2+).

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Identify the property of cyanide ligand CN- that makes it possible to form complexes with such a transition metal.

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State four uses of a lesson plan.

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A solution of 1dm3 was made by dissolving 28.6 g of impure sodium carbonate in distilled water. A 25 cm3 of this solution was completely neutralized by 24.9 cm3 of 3.65 g of hydrochloric acid in 1dm3 solution. (a) Calculate the concentration of pure sodium carbonate in g/dm3. (b) If the impurity in sodium carbonate is water of crystallization, calculate the value of Z in the formula Na2CO3.ZH2O.

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Calculate the wavelength in meter, of a bulb light that is radiated by the energy of 2.76 x 105 Joules.

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(a) Using a relevant example in each case, describe five characteristics of homologous series. (b) Hydrocarbon R was found to contain 84% by mass carbon, and the rest percentage was hydrogen. If its molecular mass was 60 g, find: (i) Empirical formula (ii) molecular formula.

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Suggest five safety precautions for the storage of chemicals in chemistry laboratory.

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Elaborate five principles of teaching and learning chemistry.

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Describe five procedures to be followed when moderating chemistry test items.

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