SPM Che2 Q&A (Kedah)
Transcript of SPM Che2 Q&A (Kedah)
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PEPERIKSAAN PERCUBAAN SPM 2008
NEGERI KEDAH DARUL AMAN
MARKING SCHEME
CHEMISTRY PAPER 2
Section A
(a) An acid that dissociates/ ionises completely in water
to form a high concentration of hydrogen ions
1
1
(b) pipette 1
(c) From pink to colourless 1
(d) (i) HCl + NaOH NaCl + H2O 1
(ii) 0.1 x 20 = 1
Mb x 25 1
25 Mb = 2Mb = 0.08 mol dm
-3
1
1
(e) (i) 10 cm3
// half the volume of hydrochloric acid 1
(ii) Sulphuric acid is a diprotic acid whereas hydrochloric acid is a
monoprotic acid.So, the sulphuric acid used has twice the number of hydrogen ions
compared to hydrochloric acid .
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1
1.
Total 10
(a) (i) Zinc
hydrochloric acid / suphuric acid
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1
(ii) Zn + 2HCl ZnCl2 + H2 1
(b) (i)
Empirical formula is MO2
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1
1
(ii) MO2 + 2H2 M + 2H2O 1
( c) The air in the combustion tube must be displaced before lighting the
hydrogen gas// The heating, cooling and weighing is repeated until aconstant mass is obtained
1
(d) No.Magnesium is more reactive than hydrogen.
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2.
Total 10
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(a) Propene
Vinyl chloride // Chloroethene
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1
Advantage: Light // Cheap // convenient 1(b)
Disadvantage: Non-biodegradable // produces toxic gas when burnt 1
(c) i Increase hardness // reduce corrosion / rusting // improve theappearance//to make it more attractive 1
ii To make Medals // swords // statues // bells 1
iii 1
iv Atoms/particles in copper are arranged in an orderly manner in layers.
The presence of tin atoms disturbs the orderly arrangement of copperatoms.
This will make it difficult for the layers of tin atoms to slide on eachother.
1
1
1
3
Total 10
Tin
Copper
(a)
1
(b) i Isotopes are atoms (of the same element) with the same number ofprotons/proton number but different number of neutrons/nucleon
number. 1
ii Any example of isotope
Sample answer; carbon-14,cobalt-60, sodium-24 etc
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(c) i 12 1
iiY
1
4
(d) i Liquid 1
X
23
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(ii)
1
iii Becomes faster/ more active 1
iv correct curve
boiling point
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1
Total 10
(a)
The stopper is drawn in the correct position(half in, half out)refer the diagram
1
(b) 2HCl + CaCO3 CaCl2 + H2O + CO2 1
5
(c) 32 cm3
50 s= 0.64 cm3s-1
1
(d) (i) Both axes are labelled with the correct units
scales are suitable(cover graph paper)
All points are transferred correctlySmooth curve
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1
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(ii) A tangent is drawn on the graph
Calculation0.246 cm3s-1 + 0.024 // range [0.222 - 0.270]
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Total 10
Time / min
Temperature /oC
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6 (a) Hydrogenation// addition (of hydrogen) 1
(b) (i) Phosphoric acid // H3PO4 1
(ii) C2H4 + H2O C2H5OH 1
(iii) Fermentation 1
(c) (i) Ethanoic acid 1
(ii) Acidified potassium dichromate(VI) solution // Acidified potassiummanganate(VII) solution
1
(d) C2H5OH C2H4 + H2O 1
(e) (i) Esterification 1
(ii) - has a sweet smell// fruity smell
- a neutral compound
- colourless liquid- slightly soluble in water
- readily soluble in organic compounds[ Choose any one ]
1
(iii)H O H H
H C C O C C H
H H H
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Total 10
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Section B
Hydrogen(gas) 1(a)
2H+(aq) + 2e H2(g) 1 2
(b) Properties Cell A Cell B
1. Type of cell Voltaic cell Electrolytic cell
2. Energy change Chemical
electrical Electrical
chemical3. Electrodes Positive terminal:Copper
Negative terminal:
Magnesium
Anode: CopperCathode: Copper
4. Ions in electrolyte Cu2+
, SO42-
, H+
and OH-
ionsCu
2+, SO4
2-, H
+and OH
-
ions
Positive terminal:Cu2+ + 2e Cu
Anode:Cu Cu2+ + 2e
5. Half equation
Negative terminal
MgMg2+
+ 2e
Cathode:
Cu2+
+ 2e Cu
Positive terminal:
Copper plate becomes
thicker
Anode:
Copper
dissolves//becomethinner
6. Observation
Magnesium becomesthinner/dissolve
Cathode:Copper becomes thicker
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1
1
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1
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(c) (i) Improve the appearance//to make it more attractive
To prevent/ reduce corrosion/ rusting
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1 2
(ii) Procedure:1. Iron ring is then connected to the negative plate on the battery
while the silver plate is connected to the positive terminal of the
battery//Iron ring is made as cathode while silver plate is madeas anode
2. Both plates are immersed into the silver nitrate solution.
3. The circuit is completed
Functio
nal apparatus set-up
Label correctly:silver plateSilver nitrate solution
Iron ring
Cathode: Ag+
+ e Ag
Observation: Grey /silvery solid is depositedAnode : Ag Ag+ + eObservation: Anode/silver become thinner//dissolve
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1
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max
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(i) Atom R is located in Group 17, Period 3 1
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8 (a)
(ii) Electron arrangement of atom R is 2.8.7.It is located in Group 17 because it has seven valence
electron.It is in Period 3 because it has three shells filled with
electron
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(b) (i) Atoms P and R form covalent bond.
To achieve the stable electron arrangement,atom P needs 4 electrons while atom R needs one electron.
Thus, atom P shares 4 pairs of electrons with 4 atoms of
R,forming a molecule with the formula PR4 // diagram
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1
(ii) Atom Q and atom R form ionic bond.
Atom Q has the electron arrangement 2.8.1. and atom Rhas the electron arrangement 2.8.7.
To achieve a stable (octet )electron arrangement,atom Q donates 1 electron to form a positive ion//equation
Q Q+ + e
Atom R receives an electron to form ion R-//equation and
achieve a stable octet electron arrangement.
R + e R-
Ion Q+
and ion R-
are pulled together by the strongelectrostatic forces to form a compound with the formula
QR// diagram
1
1
1
1
1
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RR
R
R
+
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(c) The ionic compound/ (b)(ii) dissolves in water
while the covalent compound / (b)(i)does not dissolve in water.Water is a polar solvent that can cause the ionic compound todissociate into ions.
Covalent compounds are non-polar and can only dissolve in
organic solvents.
OR
The melting point of the ionic compound/ (b)(ii) is higher than
that of the covalent compound/ (b)(i) .
This is because in ionic compounds ions are held by strongelectrostatic forces.
High energy is needed to overcome these forces.In covalent compounds, molecules are held by weak
intermolecular forces.
Only a little energy is required to overcome the attractive forces.
OR
The ionic compound/(b)(ii) conducts electricity in the molten or
aqueous statewhereas the covalent compound/(b)(i) does not conduct
electricity.
This is because in the molten or aqueous state, ionic compoundsconsist of freely moving ions.
Covalent compounds are made up of molecules only
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Total 20
9 (a) (i) Based on the equation, iron(II) ion is oxidised toiron(III) ion
So, iron(II) ion acts as a reducing agent
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1
(ii) Based on the equation, iron(II) ion is reduced to
ironSo, iron(II) ion acts as an oxidising agent
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(b) eMgMg 22
Oxidation number of magnesium increases from 0 to +2, So
magnesium undergoes oxidation
CueCu 22
oxidation number of copper decreases from +2 to 0, so copper(II)ion undergoes reduction
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1 4
(c) (i) Reduction is a reaction that involves gain of electron.
Oxidation is a reaction that involves loss of electron.
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(ii) At the negative terminal:
Iron(II) ion releases one / loses one electron andis oxidised to iron(III) ion.Fe2+ Fe3+ + e
The green coloured solution of iron(II) sulphate turns brown.
The electron flows from the negative terminal// carbon
immersed in iron(II) sulphate solution to the positiveterminal// carbon immersed in bromine water.
At the positive terminal:
Bromine accepts electron andis reduced to bromide ions, Br-
Br2 + 2e 2Br-
The brown coloured bromine water turns colourless.
The deflection of the galvanometer needle shows that there is
a flow of current
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1 10
Total 20
10 (a) Exothermic reaction is a reaction that releases heat to thesurrounding
The energy content of the products is lower than the energy
content of the reactantsEndothermic reaction is a reaction that absorbs heat from the
surroundingThe energy content of the products is higher than the energy
content of the reactants
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(b) A reacts with B to form C and D
A and B are the reactants while C and D are the productsHeat energy is released //The reaction is exothermic
Total energy content of A and B/reactants is higher than totalenergy content of C and D/products
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(c)
Copper container
thermometer
water
Spirit lamp+
ethanol
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250 cm3
of water is measured using a measuring cylinder and is
then poured into a copper container.The copper container is placed on a tripod stand.The initial temperature of the water is measured and recorded.
A spirit lamp containing ethanol is weighed and recorded.
The spirit lamp is placed directly below the copper container(as
in the diagram.)The wick of the spirit lamp is lighted.
The water is stirred using a thermometer.When the increase in water temperature is 30 oC, the flame is put
off and the highest temperature reached is recorded.
The spirit lamp is weighed again.Results:
Initial temperature of water = t1oC
Highest temperature of water = t2oC
Rise in temperature = (t2 - t1)oC = T oC
Mass of lamp + ethanol before combustion = m1 g
Mass of lamp + ethanol after combustion = m2 g
Mass of ethanol burnt = (m2 m1) g
Number of mol of ethanol = (m2 m1) = n
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Heat change = 250 x 4.2 x T= q J
Heat of combustion = - q kJ mol-1
n x 1000
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Max
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Total 20
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