INSTRUCTIONS
- Write your name and index number in the spaces provided above
- Sign and write date of examination in the space provided.
- All working must be clearly shown where necessary.
- Mathematical tables and silent electronic calculations may be used
- Answer all questions in English.
QUESTIONS
- Give two difference between a thistle funnel and a dropping funnel (2marks)
- Gives names of the following processes used to
- Separate calcium carbonate from water (1mark)
- Separate a mixture of nitrogen and Helium (1mark)
- The table below shows some solutions and their pH value
Solution pH values
P 1.5
Q 6.0
R 14.0
S 8.0
Which of the above solutions is likely to be of- Sodium carbonate (1mark)
- Solution with high concentration of Hydrogen ions (1mark)
- In the laboratory preparation of oxygen gas, Hydrogen peroxide is used.
- Name the catalyst used (1mark)
- Write a balanced chemical equation for the reaction (1mark)
- State three observation made when a piece of potassium metal is dropped into cold water giving a reason for each. (3marks)
- In the extraction of iron, the iron ore is reduced to iron in a blast furnace
- Name the main ore used in extraction of iron (1mark)
- What is the main reducing agent in the blast furnace (1mark)
- Write the equation for the reaction through which the iron ore is reduced to iron in the blast furnace (1mark)
- Draw the structure of the following
- Mg+ (1mark)
- Hydroxonium ion (1mark)
- When 27.8g of hydrated aluminium oxide (AI2O3•XH2O) was heated to a constant mass 20.6 g of aluminium oxide was obtained. Determine the value of X (Al=27, O=16, H=1 (3marks)
- In the haber process, the industrial manufacture of ammonia is given by the following equation
N2(g)+H2(g) 2NH3(g)ΔH=-97KJ/mol- Name one source of nitrogen gas used in this process (1mark)
- Name the catalyst used in the above reaction (1mark)
- What is the effect of increasing temperature on the yield of ammonia? Explain (2marks)
- Describe the correct process of heating a liquid in a test-tube using a bunsen burner. (3marks)
- Draw a labelled diagram of a set up that can be used to prepare dry sample of carbon (IV) oxide using calcium carbonate (3marks)
-
- Draw structural formulae of two positional isomers with molecular formula C4H8 (2marks)
- Study the equation below and answer the questions that follow
C6H14+CL2-C6H13CL+HCL- State the condition under which this reaction occurs (1mark)
- Give the general name of this type of reaction (1mark)
-
- Define hydration energy (1mark)
- Given that the lattice energy of NaCl is +781kJ/mol and hydrated energy of Na+ and Cl- are
-390kJ/mol and -384kJ/mol respectively. Calculate the heat of solution of one mole of NaCl(s) using energy cycle. (3marks)
- 240cm3 of nitrogen (I) oxide gas takes 16 seconds to diffuse through a certain porous pot. 300cm3 of x takes 12 seconds to diffuse through the same pot calculate the relative molecular mass of gas x. (N=14, O=16) (3marks)
- Draw a well labelled diagram that can be used during electrolysis of molten sodium chloride in the laboratory (3marks)
- The figure below describes the manufacture of detergent B
- What type of detergent is B (1mark)
- Draw the structure of detergent B (1marks)
- State two disadvantage of using detergent B (2marks)
- Use the flow chart below to answer the question below
- Explain the observation in step II (1mark)
- Name the process that takes place when flower petals are put into solution T (1mark)
- Reaction in step I takes place only in presence of moisture. Give a reason for this (1mark)
- The diagram below represent a dry cell with Zinc can and graphite as the electrodes and ammonium chloride paste as an electrolyte
- Write an ionic equation for the reaction taking place at
- Anode (1mark)
- Cathode (1mark)
- State the property of carbon powder that make it suitable for use in the cell (1mark)
- State one other substance that could be used in place of manganese (IV) oxide (1mark)
- Write an ionic equation for the reaction taking place at
- The diagram bellow represents part of periodic table. Use it to answer the question that follow
- Write the electronic arrangement for the stable ion formed by X (1mark)
- Write an equation for the reaction between W and Q (1mark)
- Compare the ionization energy of element A and Z. Explain. (2marks)
- Write equations to show the effect of heat on each of the following
- Ammonium nitrate (1mark)
- Potassium nitrate (1mark)
- Anhydrous iron (II) sulphate (1mark)
- When excess chlorine gas is bubbled through diluted sodium hydroxide solution; the resulting solution act as a bleaching agent
- Write an equation for the reaction between chlorine gas and sodium hydroxide solution (1mark)
- Name the bleaching agent (1mark)
- Write an equation to show the bleaching and explain how it occurs (2marks)
- Alpha ()and beta (ß) particles can be distinguished using papers, aluminium foil and an electric field complete the diagram below to show how this is done (3marks)
- During electrolysis of magnesium sulphate, a current of 0.3A was passed for 30 minutes calculate the volume of gas produced at the anode (molar gas volume =24dm3 IF=96500C (3marks)
- Starting with sodium metal, describe how a sample of crystal of sodium hydrogen carbonate may be prepared (3marks)
- When 20cm3 of 0.5M sulphuric (VI) acid was mixed with 20cm3 of 1M NaOH, the temperature of the solution rose from 24.0°C to 32.0°C calculate the molar heat of neutralisation (Specific heat capacity of the solution is 4.2Jg-1density is 1g/cm3 (3marks)
- The table below shows the test carried out on a sample of water and results obtained
Sample
Test
observation
A
Addition of NaOH solution drop wise until in excess
White precipitate souble in exess
B
Adding of NH3(aq) solution
White precipitate
C
Addition of dilute HNO3 followed by Ba(NO3)2
White precipitate
- Identify the anion present in the water (1mark)
- Write the ionic equation for the reaction in C (1mark)
- Write the formula of the complex ion in A (1mark)
MARKING SCHEME
-
- A thistle funnel has no tap while dropping funnel has a tap
- A dropping funnel allows one to add controlled amount of solution while thistle funnel does not
-
- Filtration
- Fractional distillation
-
- S
- P
-
- manganese (iv) oxide
- 2H2O2(I) → MnO2 2H2O(I)O2(g)
(penalise ½ for wrong or missing state symbol
Penalise fully if not balanced
-
- Potassium will float ½- less dense than water.½
- Potassium will melt into a silvery½ ball since reaction exothermic.½
- Produces a hissing sound½ - hydrogen gas produced½
- A lilac (purple)½ flame is produced due to production of potassium½ vapour
Any 3 for 3 marks
-
- Haematite
- Carbon (ii) oxide / Co Accept name or formula
- Fe2O3(x)+3CO(g)→2Fe(I)+3CO2(g)
or
2Fe2O3(x)+3C(x)→4Fe(I)+3CO2(g)
-
-
- AI2O3 H2O
20.6 7.2
102 18
20.6 7.2
102 0.4
0.02 0.4
1 : 0.02
20
AI2O3 • 20H2O -
- Fractional distillation of air/air
- Finely divided iron/iron
- The yield decreases.
The forward reaction is exothermic hence backward reaction is favoured
(the decomposition of ammonia)
- Using a test tube holder
Slanting
Facing away
Heat
Rotate -
Workability – 1
Labelling – 1
Method of collection -1 – downward delivery or use of syringe. -
-
-
- u.v light
- Substitution
-
-
- Hydration energy – energy change that occurs when one mole of gaseous ions becomes hydrated.
-
Total hydration energy =(-390)+(+384)
ΔHsoin =+781+(-774)=+7KJ/mol
- 240→N2O-16sec
300→N2O→300×16/ 240
=20sec
(12/ 20)2 = Mx/ 44
0.33=Mx/ 44
Mx=44×0.36
15.84sec -
Workability
Labelling
Drawing -
- Soap less detergent
-
-
- It is non-biodegradable hence pollutes the environment.
- It causes eutrophication
- It is expensive
-
- Orange acidified potassium dichromate (VI) changes to green
- bleaching
Moisture assists to form ions for reaction to take place.
-
- Anode.
Zn(s)→Zn2+(aq)2e-1
Cathode.
2NH+4(aq)+2e-→2NH3(g)+H2(g)
2NH+4(aq)+2MnO2(aq)+2e-→Mn2O3(aq)+2NH3(g)+H2O(I) - it forms a positive terminal of the cell
- Anode.
-
- 2.8
- 3W(s)+Q2(g)→W3Q2(s)
3Mg(s)+N2(g)→Mg3N2(s) - Z has a lower ionization energy than A , Z has a larger atomic radius than A hence outermost electron in Z is loosely held.½
-
- NH4NO3(s)→N2O(g)+2H2O(g)
- 2KNO3(s)→2KNO2+O2(g)
- 2FeSO4(s)→Fe2O3(s)+SO2(g)+SO3(g)
-
- NaOH(aq)+Cl(g)→NaCl(aq)+NaOCl(aq)+H2O(I)
- Sodium chlorate (I)1
- NaOCl(aq)+dye→NaCL(aq)+NaOCL(aq)+(dye+O)
NaOcl decomposes to give atomic oxygen (O) that bleaches by oxidation.1
-
Angle of deflection 1
Labelling 1
Penetration power 1 - 4OH(aq)→2H2O(I)+O2(g)+4e
Q=0.3 × 30 × 60=540e
Ie=965500C
4e=386000c
386000c-24dm3
540c→24 × 540/ 386000
=0.0335 liters -
- Heat sodium metal (mall pieces) in oxygen to form sodium oxide
- dissolve the oxide in water to form sodium hydroxide
(OR) Add a piece of sodium metal to water in a trough to form sodium hydroxide - bubble excess CO2 into the solution to form sodium hydrogen carbonate
- Warm the solution to concentrate.
- Allow solution to cool and form crystals filter and Dry the crystals between pieces of filter paper
-
mass of solution =(40cm3 1kg/cm3)=40g
ΔT=32-24=8°C
ΔH= 40/ 1000× 4.2 × 8
=1.344KJ
moles of H+ ions = 2(20×0.5)/ 1000 =0.02moles
0.02moles - 1.344/1 × 0.02
ΔHneut=-67.2KJs/mol
Penalize ½ for negative sign ½ for wrong or missing units. -
- SO2-4
- Ba2+(aq)+SO2-4(aq)→BaSO4(s)
- [AI(OH)4]-
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