NAME:……………………………………………INDEX
NO:………………………
CANDIDATES SIGNATURE………………………….
DATE………………………..
SCHOOL………………………………………….
233/1
CHEMISTRY
PAPER 1
MARCH/APRIL 2010
2 HOURS
THE ELDORET EAST INTER SCHOLL
EXAMINATION-2010
Kenya CERTIFICATE OF Secondary
Education.
FORM FOUR
233/1
BIOLOGY
PAPER 1
MARCH/APRIL 2010
2 HOURS
INSTRUCTIONS TO CANDIDATES;
Write your name and index number in
the spaces provided above.
Sign and write the date of
examination in the spaces provided above
Answer All the questions in
the spaces provided in the question paper.
All working Must
BE clearly shown where necessary
Mathematical tables and electronic calculators
may be used
Question
|
Maximum Score
|
Candidates Score
|
1-31
|
80
|
1. The diagram below is a laboratory
set up for preparation of oxygen gas.
(a) Name
(i) The apparatus marled A (1MK)
………………………………………………………………………………………………
(ii) Solid P………………………………………………………………………….
(1mk)
(b) Write an equation for the
reaction that takes place in the flask. (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
2. When magnesium is burnt in air,
it react with both nitrogen and oxygen. Write the formulae of the two products formed
(2mks).
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
3. An element X forms an ion with
the formula X+.The electronic of the ion is 2.8.
(i)Name the chemical family of element
X (1MK)
…………………………………………………………………………………………….
ii) .Write a chemical equation for
the reaction of element X in cold water. (1mk).
……………………………………………………………………………………………………………………………………………………………………………………………..
iii. State and explain the effect
of the resulting solution in(ii) above on litmus paper(1mk)
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
4. Study the set up below and answer
the question that follows.
(i)Name electrode A (1/2)
……………………………………………………………………………………………
ii.Write the half equation in
electrode B when the switch is closed (1mk)
…………………………………………………………………………………………….
iii) .Explain why heating is
necessary in the set up.
(1mk)
………………………………………………………………………………………………
5. Chlorine reacts with ethane as
shown below
C2H6(g0 +
Cl
C2H5CL(g) +HCL(g)
(a) What condition is necessary for
this reaction to occur (1/2mk)
………………………………………………………………………………………………
(b) Name the type of reaction that
occurs (1/2)
………………………………………………………………………………………………
6. a) What is meant by isomerism (1mk)
………………………………………………………………………………………………
(b) Draw and name two isomers of a
compound whose molecular formula is C4H10.(2mks)
7. Alkaline earth metals get
progressively more reactive down the group while halogens get progressively
less reactive down the group. Explain (2mks)
………………………………………………………………………………………………………………………………………………………………………………………………
8. (a) An element P has atomic
number17.It forms compound with element G.Using dots(.)and crosses(x) to represent electrons. Draw a
diagram to show the bonding in the compound. (2mks).
(b) Molecular compounds have lower
melting points compared to ionic compounds.Expalin why this is so.
……………………………………………………………………………………………………………………………………………………………………………………………..
………………………………………………………………………………………………………………………………………………………………………………………………
9. The scheme below shows some
reaction sequence starting with solid N.
(a) Identify solid N.
………………………………………………………………………………………………………………………………………………………………………………………………..
(b) Write the formula of the complex
ion in solution R. (1MK)
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
c).Give an importance of hard water
(1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
……………………………………………………………………………………………….
10. Dry carbon (II) gas react with
lead(II)oxide as shown in the equation
(a)Name the process undergone by
lead (II) oxide (1mk)
…………………………………………………………………………………………….
(b) Give a reason for your answer in (a) above
(1mk)
…………………………………………………………………………………………….
c) Name any other gas that can be
used to perform the same function as carbon (II) oxide gas in above reaction.
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
11. Using the equation below,
identify the substance that cats as a abase in the forward reaction
Substance: (1mk)
…………………………………………………………………………………………..
Reason: (1mk)
……………………………………………………………………………………..
12 a).Nitrogen(IV) Oxide is one
source of environmental pollution. Explain (1mk)
13. Give two main source of nitrogen
(IV) oxide in the atmosphere (1mk)
14.A student was given four
carbonates labeled A,B,C and d to heat and test for carbon(IV) OXIDE GAS. He
obtained the following results.
Carbonates
|
Color before heating
|
Colour after heating
(hot)
|
Test for carbon (IV) Oxide
|
A
|
White
|
White
|
Negative
|
B
|
White
|
Yellow
|
Positive
|
C
|
Green
|
Black
|
Positive
|
D
|
White
|
Red
|
Positive
|
Which carbonate can be used to
soften water? Explain your answer (2mks)
………………………………………………………………………………………………………………………………………………………………………………………………
15.a)Study the equation below and answer the questions
that follow
I2(s) I2(g)
9.( i) What conditions must be
present for the changes represented by the equation above to occur (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
ii.) Name the process represented
by the equation above (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………..
b.) How can the purity of a
substance be determined (1mk)
……………………………………………………………………………………………………………………………………………………………………………………………
16. An atomic of element Q can be
expressed as 31/15Q.The letter dose not represent the actual symbol of the element.
a.) Write down the symbol of the
most stable ion of element Q.
……………………………………………………………………………………………
b).Write down the electronic
arrangement of the ion element Q.
……………………………………………………………………………………………………………………………………………………………………………………………….
17. Zinc metal was reacted with dilute
hydrochloric acid as shown in the figure below. Study it and answer the
question that follows.
a.)
Name gas N..
………………………………………………………………………………………………...
b).How can one tell if all acid has
reacted?(1mk)
……………………………………………………………………………………………………………………………………………………………………………………………….
c) Write down a balanced ionic
equation to show the reaction taking place in the boiling tube.(1mk)
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
18.1.47kg of CaCL was heated to a
constant mass of 1.11G.Find the value of x.
Ca=40, Cl=35.5, H=1, O=16 ( 3MKS.)
19.(a.)Distinguish between the mass
number and the relative atomic mass of an element.
c.) Why is the atomic radius of
magnesium larger that it’s ionic radius.
When a green solid M was heated
strongly in a test, a black residue and a gas which formed a while precipitate
with lime water were formed.
a).Identify solid M (1MK)
………………………………………………………………………………………………...
b) .Write down a balanced chemical
equation to show the reaction between the balck residues and dilute sulphuric
acid (1mk)
20. State and explain why magnesium
continues to burn is SO2 gas.(2mks).
21. Excess chlorine was bubbles
into hot concentrated sodium hydroxide
a. ) Write equation of reaction
above.(1mk)
B).Calculate the oxidation number
of chlorine in the chlorine formed (1mk)
22. Bottles of sodium carbonate,
sodium chloride and sugar have lost their labels student prepares and tests an
aques solution of a sample from each bottle. The results obtained are as shown
in the table below.
Bottle
|
Ph
|
Electrical conductivity
|
Correct label
|
1
|
7
|
CONDUCTS
|
|
2
|
7
|
Dose not conduct
|
|
3
|
10
|
Conduct
|
Complete the table by filling
correct label for each bottle.
23. Bleaching powder is used to
treat water in drinking water supply plants. Briefly explain how it eradicates
the micro-organisms from water.(2mks)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
24. What would you observe when the
following tests are carried out in Iron (II) Sulphate Solution.
i.) little aqueous ammonia is added
to iron (II) sulphate solution.(1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
………………………………………………………………………………………………
ii.) A few drops of concentrated
nitric acid are added to Iron (II) Sulphate solution and warmed gently.(1mk).
………………………………………………………………………………………………………………………………………………………………………………………………..
iii) Excess aqueous ammonia is
added drop wise to the mixture in (II) above(1mk)
………………………………………………………………………………………………………………………………………………………………………………………………..
25. State two uses of Ammonia (2mks).
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
26. Starting from powered sulphur,
describe how you would prepare a sample rhombic sulphur.(3mks).
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
27. The diagram below shows an
experiment to compare the heating effects of luminous and non-luminous flame.
a) .State and explain the
observation made at the bottom of each beaker at the end of the
experiment.(1mk)
b.) The diagram below represents a
luminous flame.
On the diagram, mark and label the
hottest and coolest parts of the flame.(1mk0
c) .When not in use, it is
advisable to put off a non-luminous flame or turn it to a luminous
falme.Expalin.(1mk)
a.)Name any two water pollutants (1mk)
d.)Describe the chemical test for
water.(2mks)28.The molar masses of gases Y and Z are 28.0 and 44.0 Respectively.
If a volume of 280cm3 of gas Y diffuses through a membrane in 70 seconds, how
long will it take 400cm3 of gas Z to diffuse through the same membrane.(3mks)
29. The table below contains some
information about the properties of oxides. Use the information in the table
below to answer the questions that follow. Letters A, B, C, D, E& Z are not
actual symbols of the elements.
a.) The melting pointy of oxide of B is higher
than that of the oxide of A. Why? (1mk)
i.) Write the formula of the chloride
of B. (1mk).
ii.)State one possible use of
calcium oxide (1mk)
30.(a )What is absolute Zero
Temperature? (1mk)
(b.)A gas occupies a volume of 600cm3
pressure of 760mmHg and a Temperature of x. C,at pressure of 780mmHg and
Temperature of 50 C,The gas occupies a volume of 633.66cm3.Determine the value
of x.
NAME:……………………………………………INDEX NO:………………………
CANDIDATES SIGNATURE………………………….
DATE………………………..
SCHOOL………………………………………….
233/2
CHEMISTRY
PAPER 2
MARCH/APRIL 2010
2 HOURS
THE ELDORET EAST INTER SCHOLL EXAMINATION-2010
Kenya CERTIFICATE OF Secondary Education.
FORM FOUR
233/2
CHEMISTRY
PAPER 2
MARCH/APRIL 2010
2 HOURS
INSTRUCTIONS TO CANDIDATES;
Ø
Write your name and index number in the spaces
provided above.
Ø
Sign and write the date of examination in the
spaces provided above
Ø
Answer All the questions in the spaces
provided in the question paper.
Ø
All working Must BE clearly shown where
necessary
Ø
Mathematical tables and electronic calculators
may be used
Question
|
Maximum Score
|
Candidate score
|
1
|
12
|
|
2
|
10
|
|
3
|
06
|
|
4
|
08
|
|
5
|
11
|
|
6
|
12
|
|
7
|
12
|
|
8
|
09
|
|
Total
|
80
|
1. The grids represent parts of the
periodic table. Study it and answer question that follow. The letters do not
represent the actual symbols of the elements.
(a).(i).Write down the electron
configuration of element N (1/2MK)
………………………………………………………………………………………………………………………………………………………………………………………………
ii).Using dots (.)Or crosse(x) to represent electronics,
draw a diagram showing the formation of an ion of element N. (1/2)mk -).
b.)What type of structure could the
oxide of K have? Explain. (2mks)
c.)How does the reactivity of R and
Q Compare? (2mks)
d.)1.2g of K reacted completely
with 1110 cm3 of chlorine gas at s.t.p (1 mole of gas occupies 22.4dm3).
i.) Write a balanced equation for
the reaction between K and chlorine.(1mk)
ii.)Determine the relative atomic
mass K.(3MKS)
ii) .Explain the observation that
would be made if a nitrate of K is heated.(2mks).
2. The flow chart below shows the
industrial preparation of sulphuric (vi) acid. Study it and answer the question
the follow.
a).i.)With the help of an equation,
state one source of sulphur (iv) oxide.(11/2)
ii.)Name a suitable substance that
can be used in the drier.(11/2)
iii).In the catalytic converter,
the temperature is adjusted to about 45.C without external heating.
Explain (1mk)
iv.) Write an Equation for the
process taking place in a absorption tower? (1mk)
v) Why is it not advisable to use
hard water in the diluter?(1mk)
vi.) Name one solid waste produced
in this process.
b.) Nitric (V) acid and hydrogen
chloride can be prepared in the laboratory by heating a nitrate and chloride
respectively with concentrated sulphuric (VI) acid. What property of
concentrated sulphuric (VI) acid makes it suitable for the preparation of nitric
(v) ACID and hydrogen chloride. (1mk)
c.)How does the bleaching affects
of sulphur (VI) oxide gas band chlorine gas compare (2mks)
3. The equation below shows the
molar enthalpies of combustion of carbon, hydrogen
and molar of formation of methane.
a).(i.)Draw the energy cycle
diagram and work out the enthalpy of combustion of methane. (3mks).
b.Given that the ,molar heat of
combustion of butane is-2877KJ/Mol and that C=12,H=1,calacualte heat value in
KJ/gram.
i. Methane (CH4)(1mk)
ii.Butane.(1mk)
ii.
From the results in b(i) and ii above,
which one is the better fuel.(1mk)
4.Auqeous hydrochloric acid was
reacted with sodium sulphite and a gas A evolved when this gas was dried, mixed
with oxygen and then passed over a catalyst B,maintained at 400.Can exothermic
reaction occurred. The product was cooled by an ice-salt mixture and colourless
crystals were formed. When very low PH value resulted.
a.)
Identify (2mks)
A………………………………………………………………………………….
B………………………………………………………………………………..
C………………………………………………………………………………..
D………………………………………………………………………………..
b.)Write equations for the
reactions which led to the formation of (2mks)
A……………………………………………………………………………………..
B……………………………………………………………………………………
c) Suggest a suitable drying agent
for gas A.
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
(d.)State and explain what would
happen to the yield of c if the temperature of the catalysts were raised to
600C. (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
(e.)Write an ionic equation for the
reaction which would occur between solution D and Z and Zinc Metal. (1mk).
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
f) Describe one chemical test which
could be used to identify gas A. (1mk)
…………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………….
5. The flow below represents the
main steps in the preparation of sodium carbonate.
a.) Name the substance labeled. (2mks)
A…………………………………………………………………………………………….
B………………………………………………………………………………………………C……………………………………………………………………………………………
D…………………………………………………………………………………………..
B.Cold water is made to circulate
around X. What does this suggest about the reaction between A and brine(1/2mks)
………………………………………………………………………………………………………………………………………………………………………………………………
c.)What process takes place in
chamber Y.? (½
MK).
……………………………………………………………………………………………..
……………………………………………………………………………………………..
……………………………………………………………………………………………..
d.)Name two by-products that are
recycled in this process. (1MK)
e.)Why is recycling important? (1mk)
……………………………………………………………………………………………………………………………………………………………………………………………..
f.) Write the equation for the
reaction that takes place in the upper part of solvay Tower(1MK)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
g.)Assuming that there was no
recycling in this process, two moles of ammonia would be required for producing
one mole of an hydrous sodium carbonate. Calculate the volume of ammonia at
s.t.p that would be used to produce 10.6 kg of sodium carbonate by a factory
operating at 80% efficiency.
(C=12,O=16.H=1,Na=23,N=14,I mole of
gas occupies 22.4 dm3 at s.t.p) (3mks)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
h.) Give two industrial uses of
sodium carbonate (2mks)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
6.( a) Study the information in the
table below and answer the question that follow.
Number of carbon atoms
|
Relative molecular mass of hydrocarbon
|
2
|
28
|
3
|
42
|
4
|
56
|
i.) Write the general formula of
the hydrocarbons in the table (1mk).
……………………………………………………………………………………………………………………………………………………………………………………………..
ii.) Predict the Relative Molecular
Mass (RMM) of the hydrocarbon with 6 carbon atoms (1mk)
…………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
ii.) Determine the molecular
formula of the hydrocarbon in(ii) above and draw its structural formula (C=12,H=1)
(2mks)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………
b.) The scheme below shows some reactions
of substances. Study it and answer the question that follows.
I.Name the reagent used in
Step
2:………………………………………………………………………..(1mk)
Step
3:……………………………………………………………………….(1mk)
Step 4:……………………………………………………………………….(1mk)
ii.) Write an equation for the
complete combustion of ethyne (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
iii.) Write down the name and
structural formula of compound B. (2MKS)
Structural formula
Name
iv) Give the homologous series that
the compound formed in step 3 and step 2belong to.(1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
v.) Explain what you understand by
the term hydrocarbon.(1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
7. The scheme below shows various
reactions starting with hydrogen and nitrogen gases. Study it and answer the
questions that follow.
a. Name the major source of
i.) Hydrogen (1/2mk)
……………………………………………………………………………………………………………………………………………………………………………………………..
ii).Nitrogen (1/2mk)
……………………………………………………………………………………………………………………………………………………………………………………………..
b.Name the catalysts and explain
why its used in step 1. (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
c.)Identify
i)Solid L (1MK)
……………………………………………………………………………………………………………………………………………………………………………………………….
ii ).Gas J (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
iii.) Process Q (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
d.) (i.)Name compound R and state
one use (1mk).
………………………………………………………………………………………………………………………………………………………………………………………………
ii.Determines the percentage of
nitrogen in compound R.
(N=14, 0, H=1,0 O=16.0) (3mks)
(e) (.i.) Write two equations for
the reaction in step 1. (2mks)
……………………………………………………………………………………………………………………………………………………………………………………………..
ii.) Using an equation explain the
observation made in step II. (2mks)
………………………………………………………………………………………………………………………………………………………………………………………………
8. The solubility of two salts D and
E are given in the following table. In
each case solubility per 100g of water.
Temperature(0c)
|
10
|
20
|
30
|
40
|
50
|
60
|
70
|
80
|
Solubility of D
|
17
|
21
|
24
|
29
|
34
|
40
|
47
|
56
|
Solubility E
|
35.8
|
36.0
|
36.2
|
36.8
|
36.8
|
37.3
|
37.6
|
38.0
|
Using the data, plot solubility
curves (solubility against Temperature) of D and E on the same axes on the graph
paper below. Use your graph to answer the question that follows. (4mks)
(a. ) At what temperature are the solubilities of
the two salts equal? (1mk)
……………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
(b.)Estimate the solubility of D at
0c. (1mk)
………………………………………………………………………………………………………………………………………………………………………………………………
(c.)A saturated solution of E in
50grams of water at 25 was evaporated to dryness .What was the mass of the
residue (1mk).
………………………………………………………………………………………………………………………………………………………………………………………………..
d.)The saturated solution obtained
was each cooled to 20 C.Calculate the total mass of the salts precipitated. (2mks)
………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………………..
NAME…………………………….INDEX NO………………………….
CANDIDATES SIGNATURE……………………….
DATE……………………………………
233/3
CHEMISTRY
PAPER 3
MARCH/APRIL 2010
THE ELDORET EAST INTERSCHOOLS EXAMINATION-2010
END OF TERM 1 2010 FORM FOUR
Kenya certificate of secondary Education
233/3
CHEMISTRY
PAPER 3
MARCH/APRIL 2010
Instructions to candidates
Ø Write
your name and index number in the spaces provided
Ø Sign
and write the date of examination in the spaces provided above
Ø Answer
all questions in the spaces provided in the question paper
Ø You
are NOT allowed to start working with the apparatus for the first 15 minutes of
the 21/4 hours allowed for this paper. This time is to enable you to
read the question paper and make sure you have all the chemicals and apparatus
that you may need.
Ø All
working MUST be clearly shown where necessary.
Ø Mathematical
tables and electronic calculators may be used.
 |
 |
||
Question Maximum score Candidates score
|
1 17
|
2 15
|
3 08
|
233/3
The Eldoret East Inter schools Examinations Form four © 2010
2
1.(a)You are provided with
(b) Solution A 0.03
sodium hydroxide
© Solution B 1m
hydrochloric acid
(d) Solid Q I gram of hydrated metal carbonate M2co3.x
h2o
You are required to determine
Ø The
value of x M2co3.xH2o
Ø The
volume of CO2(g) at room temperature and pressure
Procedure
(i) Using a pipette and pipette filler place 25cm3
of solution B into a conical flask. Carefully add all solid Q and wait for
about four minutes until effervescence stops.
(ii) Transfer the resulting solution into a 250 ml
volumetric flask using a funnel. Rinse the conical flask with a little
distilled water and transfer the washing into the volumetric flask.
(iii) Add more distilled water to the solution in the
volumetric flask to make up to the mark. Shake the resulting solution well and
label it C.
(iv) Rinse the burette with solution C. Using a pipette and pipette filler, place
25cm3 of solution A into a 250ml conical flask. Add 2 drops of
solution A into a 250ml conical flask. Add 2 drops of phenolphthalein indicator
and titrate solution A with solution C. Record your results in the table 1
below.
(v) Repeat the titration two more times to obtain two other
readings and complete the table.
I II III |
Final burette reading (cm3)
|
Initial burette reading (cm3)
|
Volume of solution C (cm3)
|
(a)Calculate the
(i) Average volume of solution C used
(1mk)
(ii) Moles of sodium hydroxide in 25.0cm3 of
solution A used (1mk)
(iii) Moles of hydrochloric acid in the average volume of
solution C used (2mks)
(iv) Moles of hydrochloric acid in 25.0 cm3 of
solution C (1mk)
3
(v) Moles of hydrochloric acid in the original 25cm3
of solution B (2mks)
(vi) Moles of hydrochloric acid which reacted with solid
Q (1mk)
(vii) Molar mass of solid Q hence the value of x given that
the equation for the reaction between solution B and solid Q is
M2co3(s) +
2HCL (aq) → 2mcl (aq) +
H2o (l) + Co2 (g)
(M=23.0, C=1.0, H=1.0, O=16)
(viii) Volume of CO2 (g) evolved at room temperature and
pressure in the reaction in (vii) above.
(Molar gas volume=24.0dm3)
2. Using the 50ml measuring cylinder
provided, measure accurately 300cm3 of the 2M NaoH labeled solution
P. transfer this solution into a clean 100ml plastic breaker.
Fill the burette with solution R
which is dilute hydrochloric acid.
Use the thermometer provided to
determine the steady temperature of solution P in the plastic breaker (do not
remove the thermometer from the solution)
Add exactly 5 cm3 of
solution R from the burette into the beaker and stir gently using the
thermometer. Read the highest temperature reached. Repeat adding 5cm3 of
solution R after every 30 seconds up to 180 seconds and note the highest
temperature reached after the addition.
Record your results in the table (II)
below Time
(seconds) 0 30 60 90 120 150 |
Volume of solution P 30 30 30 30 30 30
|
Volume of solution R
|
Total volume (cm3)
|
Temperature (ºC)
|
(a) Plot a graph of temperature °c against volume of dilute
hydrochloric acid (solution R)
(Let temperature be on y-axis)
b) From the graph, determine
(i) The highest temperature reached
(1mk)
(ii) The volume of solution R which completely neutralized
30cm3 of 2MNaOH (solution P)
(1mk)
c) How many moles of dilute hydrochloric acid completely
neutralized 30cm3 of 2MNaOH
(2mks)
(d) Calculate the heat change (∆H) in this reaction hence
the molar heat of neutralization of hydrochloric acid
(Assume the specific heat capacity of water to be 4.2
kj/kg/k and the density of the solution to be 1 g/cm3)
(3mks)
3. You have been provided with solid K to carry out the test
given below
(a) Place a spatula end full of solid K in a clean dry test
tube. Heat the solid gently and then strongly. Test any gas using blue and red
litmus papers (keep the residue for the next step)
Observations Inference
(b) To the residue obtained in (a) above, add about 1cm3 of 2M HCL and shake well. Divide the solution into two equal portions
Observations
Inference
(1/2 Mk) (1/2mk)
c) To the first
portion add 2M NaOH drop wise until in excess
Observations
Inference 
(1mk)
(1mk)
(d) To the second portion, add 2M Ammonium hydroxide
solution drop wise till in excess
Observation Inference
(1mk)
(1mk)
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