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5039/01Edexcel GCSEChemistryC3 – Topics 3 and 4Wednesday 18 June 2008 – AfternoonTime: 60 minutes
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Instructions to CandidatesIn the boxes above, write your centre number, candidate number, your surname, initial(s) and signature. Check that you have the correct question paper.Answer ALL the questions. Write your answers in the spaces provided in this question paper.Do not use pencil. Use blue or black ink.Some questions must be answered with a cross in a box ( ). If you change your mind about an answer, put a line through the box ( ) and then mark your new answer with a cross ( ).Show all stages in any calculations and state the units. Calculators may be used. Include diagrams in your answers where these are helpful.
Information for CandidatesThe marks for individual questions and the parts of questions are shown in round brackets: e.g. (2).There are 8 questions in this question paper. The total mark for this paper is 60. There are 16 pages in this question paper. Any blank pages are indicated.
Advice to CandidatesYou are reminded of the importance of clear English and careful presentation in your answers.
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Centre No.
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*N33025A0216*
Th
e P
eri
od
ic T
ab
le o
f th
e E
lem
en
ts
* T
he lan
than
oid
s (
ato
mic
nu
mb
ers
58-7
1)
an
d t
he a
cti
no
ids (
ato
mic
nu
mb
ers
90-1
03)
have b
een
om
itte
d.
Th
e r
ela
tive a
tom
ic m
asses o
f co
pp
er
an
d c
hlo
rin
e h
ave n
ot
been
ro
un
ded
to
th
e n
eare
st
wh
ole
nu
mb
er.
1
2
3
4
5
6
7
0
Key
1
H
hydro
gen
1
4
He
heliu
m
2
7
Li
lithiu
m
3
9
Be
bery
llium
4
rela
tive a
tom
ic m
ass
ato
mic
sym
bo
l nam
e
ato
mic
(pro
ton)
num
ber
11
B
boro
n
5
12
C
carb
on
6
14
N
nitr
ogen
7
16
O
oxygen
8
19
F
fluorine
9
20
Ne
neon
10
23
Na
sodiu
m
11
24
Mg
m
agnesiu
m
12
27
Al
alu
min
ium
13
28
Si
sili
con
14
31
P
phosphoru
s
15
32
S
sulfur
16
35.5
C
l chlo
rine
17
40
Ar
arg
on
18
39
K
pota
ssiu
m
19
40
Ca
calc
ium
20
45
Sc
scandiu
m
21
48
Ti
titaniu
m
22
51
V
vanadiu
m
23
52
Cr
chro
miu
m
24
55
Mn
m
anganese
25
56
Fe
iron
26
59
Co
cobalt
27
59
Ni
nic
kel
28
63.5
C
u
copper
29
65
Zn
zin
c
30
70
Ga
galli
um
31
73
Ge
germ
aniu
m
32
75
As
ars
enic
33
79
Se
sele
niu
m
34
80
Br
bro
min
e
35
84
Kr
kry
pto
n
36
85
Rb
ru
bid
ium
37
88
Sr
str
ontium
38
89
Y
yttrium
39
91
Zr
zirconiu
m
40
93
Nb
nio
biu
m
41
96
Mo
m
oly
bdenum
42
[98]
Tc
technetiu
m
43
101
Ru
ru
theniu
m
44
103
Rh
rh
odiu
m
45
106
Pd
palla
diu
m
46
108
Ag
silv
er
47
112
Cd
cadm
ium
48
115
In
indiu
m
49
119
Sn
tin
50
122
Sb
antim
ony
51
128
Te
tellu
rium
52
127
I io
din
e
53
131
Xe
xenon
54
133
Cs
caesiu
m
55
137
Ba
barium
56
139
La*
lanth
anum
57
178
Hf
hafn
ium
72
181
Ta
tanta
lum
73
184
W
tungste
n
74
186
Re
rheniu
m
75
190
Os
osm
ium
76
192
Ir
irid
ium
77
195
Pt
pla
tinum
78
197
Au
gold
79
201
Hg
m
erc
ury
80
204
Tl
thalli
um
81
207
Pb
le
ad
82
209
Bi
bis
muth
83
[209]
Po
polo
niu
m
84
[210]
At
asta
tine
85
[222]
Rn
ra
don
86
[223]
Fr
franciu
m
87
[226]
Ra
radiu
m
88
[227]
Ac*
actin
ium
89
[261]
Rf
ruth
erf
ord
ium
104
[262]
Db
dubniu
m
105
[266]
Sg
seaborg
ium
106
[264]
Bh
bohrium
107
[277]
Hs
hassiu
m
108
[268]
Mt
meitn
erium
109
[271]
Ds
darm
sta
dtium
110
[272]
Rg
ro
entg
eniu
m
111
E
lem
ents
with a
tom
ic n
um
bers
112-1
16 h
ave b
een r
eport
ed b
ut not fu
lly
auth
enticate
d
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1. Lithium, sodium and potassium are members of group 1 in the periodic table.
(a) What is the symbol for a lithium atom?
..................................................(1)
(b) What name is given to the elements in group 1 of the periodic table?
.......................................................................................................................................(1)
(c) When sodium is added to water, it forms sodium hydroxide and a gas.
(i) Complete the word equation for this reaction.
+ → sodium hydroxide +
(2)
(ii) Name a group 1 metal that reacts more vigorously than sodium with water.
................................................................................................................................(1)
(iii) Sodium hydroxide is used to make several products.
Put a cross in a box to show a product manufactured using sodium hydroxide.
poly(ethene)
soap
fertiliser(1) Q1
(Total 6 marks)
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*N33025A0416*
2. Read the following extract from a website.
On 6 July 1988, twenty tonnes of aluminium sulphate were accidentally emptied into the water supply at the treatment works in Lowermoor, Cornwall. As a result, the maximum aluminium concentration in the water supply exceeded that allowed by the European Community. The highly acidic water entered the system which distributed water to 12 000 local residents.
Scientists monitored the health records of residents who were supplied with this water and those who were not. They found no statistically significant difference in the number of deaths between the people who drank this water and the people who did not.
(Source: www.studentbmj.com)
(a) Explain why it is necessary to have purified water supplied to our homes.
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................(2)
(b) Give two reasons why it is important not to waste water supplied to our homes.
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................(2)
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(c) A student living in the area, tested the tap water from her home. She took a sample to her school laboratory where she was able to use the following
barium chloride solution dilute hydrochloric acid limewater sodium hydroxide solution blue litmus paper red litmus paper
Use only the above to answer the questions.
(i) What test could she do to show that the water was acidic?
................................................................................................................................(1)
(ii) What test would she do to show that the sample contained sulphate ions?
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................(3)
(iii) What test would she do to show that the sample contained aluminium ions?
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................(3)
(d) When scientists tested the polluted water in Cornwall they conducted a quantitative test.
Why did they use a quantitative test, rather than a qualitative test?
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................(1) Q2
(Total 12 marks)
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*N33025A0616*
3. Copper is a red-brown metal. It has a melting point of 1085°C. It is used to make electrical wires. Compounds of copper are often blue.
(a) Copper is in the middle section of the periodic table. What name is given to the elements in this part of the table?
.......................................................................................................................................(1)
(b) Using only the information above, state two properties of copper typical of elements found in this part of the periodic table.
.......................................................................................................................................
.......................................................................................................................................(2)
(c) The diagram shows the apparatus used to purify copper
(i) Name the electrolyte used.
................................................................................................................................(1)
(ii) What would you see happening at the cathode?
................................................................................................................................(1)
(iii) In terms of electrons, what happens to the copper ions at the cathode?
................................................................................................................................
................................................................................................................................(1) Q3
(Total 6 marks)
cathode
electrolyte
anode
6 V d.c.supply
– +
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Turn over*N33025A0716*
Q4
(Total 6 marks)
4. Sulphuric acid is manufactured by the Contact process.
(a) During the process sulphur is burned in air.
Write the balanced equation for this reaction.
.......................................................................................................................................(2)
(b) Detergents are made using sulphuric acid.
The diagram shows the interaction between detergent and grease.
(i) Explain how detergents work to remove grease.
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................(2)
(ii) Why is it better to use a detergent rather than soap in hard water areas?
................................................................................................................................
................................................................................................................................(1)
(iii) Suggest how biological detergents are more effective than non-biological detergents.
................................................................................................................................
................................................................................................................................(1)
grease
detergent anion
–
–
–
––
–
–
–
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*N33025A0816*
5. When hydrogen peroxide solution is added to a solution of iron(II) chloride, iron(III) chloride is formed.
The hydrogen peroxide causes the following change to take place:
Fe2+(aq) → Fe3+(aq) + e
(a) Explain why this is described as an oxidation reaction.
.......................................................................................................................................(1)
(b) When sodium hydroxide solution is added to iron(III) chloride solution, iron(III) hydroxide is formed.
(i) Describe what would be seen in this reaction.
................................................................................................................................
................................................................................................................................(2)
(ii) Write the ionic equation for this reaction.
................................................................................................................................(3) Q5
(Total 6 marks)
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6. In the manufacture of methanol, the final stage involves the following reaction
CO(g) + 2H2(g) CH3OH(g)
(a) What is the maximum volume of methanol vapour that can be obtained from 1000 dm3 of hydrogen gas under the conditions of the reaction?
(All gases are measured at the same temperature and pressure.)
.......................................................................................................................................
.......................................................................................................................................
volume = ...................................................(1)
(b) The structural formula of methanol is
Put a ring around the part of the molecule that is responsible for it reacting as an alcohol does.
(1)
(c) Ethanoic acid can be manufactured from methanol.
Which gas is produced when ethanoic acid solution reacts with magnesium?
.......................................................................................................................................(1)
(d) Esters are formed when alcohols react with organic acids.
(i) Name the ester formed when methanol reacts with ethanoic acid.
................................................................................................................................(1)
(ii) Draw the structural formula of this ester, showing all covalent bonds.
(2) Q6
(Total 6 marks)
H
C
H
H O H
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*N33025A01016*
7. The industrial production of sodium carbonate is a complicated process involving many stages.
(a) The equation for the overall reaction is
CaCO3(s) + 2NaCl(aq) → Na2CO3(aq) + CaCl2(s)
Calculate the minimum mass of calcium carbonate required to produce 1 million tonnes of sodium carbonate.
(Relative atomic masses: C = 12.0, O = 16.0, Na = 23.0, Ca = 40.0)
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
answer = ................................... tonnes(4)
(b) When the sodium carbonate solution crystallises, washing soda crystals are formed. These can be used to neutralise acids.
Write the balanced chemical equation for the reaction that takes place when sodium carbonate is used to neutralise sulphuric acid.
.......................................................................................................................................(3) Q7
(Total 7 marks)
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8. In an experiment to determine the solubility of calcium hydroxide in water, Jacqui shook excess calcium hydroxide with water in a large, stoppered flask. She allowed the mixture to stand for 24 hours. She then filtered the mixture to remove excess solid.
Jacqui took 100 cm3 of the solution for analysis. She titrated 10.0 cm3 portions of the solution with 0.0500 mol dm–3 hydrochloric acid, HCl, to determine how much calcium hydroxide had been dissolved. She used methyl orange as the indicator.
Here are her results.
volume of calcium hydroxide solution used for each titration = 10.0 cm3
volume of hydrochloric acid added trial titration = 9.30 cm3
1st titration = 8.90 cm3
2nd titration = 8.80 cm3
average = 8.85 cm3
(a) Jacqui used methyl orange as the indicator in the titration. Why is universal indicator not suitable for this titration?
.......................................................................................................................................
.......................................................................................................................................(1)
(b) Describe how Jacqui should carry out this titration.
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................(4)
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*N33025A01216*
(c) The equation for the reaction is
Ca(OH)2(aq) + 2HCl(aq) → CaCl2(aq) + 2H2O(l)
Calculate the number of moles of calcium hydroxide, Ca(OH)2, present in the original 100 cm3 of solution.
You may do the calculation either by following steps (i), (ii) and (iii) or by using another method in (iii) only.
(i) Calculate the number of moles of hydrochloric acid, HCl, used in the titration.
................................................................................................................................
................................................................................................................................
(ii) Use the equation for the reaction to calculate the number of moles of calcium hydroxide, Ca(OH)2, (in 10.0 cm3 of solution) that reacted with this amount of hydrochloric acid.
................................................................................................................................
................................................................................................................................
(iii) Calculate the number of moles of calcium hydroxide, Ca(OH)2, present in the original 100 cm3 solution.
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................
................................................................................................................................
answer = ...........................................(3)
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13
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(d) The relative formula mass of calcium hydroxide is 74.0. Use your answer to (c)(iii) to calculate the mass of calcium hydroxide dissolved in the
original 100 cm3 solution.
.......................................................................................................................................
answer = ........................................ g(1)
(e) The solubility of barium chloride in water cannot be determined by titrating with an acid.
Describe an alternative method for finding the mass of barium chloride present in 100 cm3 of saturated solution.
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................
.......................................................................................................................................(2)
TOTAL FOR PAPER: 60 MARKS
END
Q8
(Total 11 marks)
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