2016 Senior External Examination Chemistry Paper One ...€¦ · 2016 Senior External Examination...
Transcript of 2016 Senior External Examination Chemistry Paper One ...€¦ · 2016 Senior External Examination...
For all Queensland schools
2016 Senior External Examination
Chemistry Friday 28 October 2016
Paper One — Question and response book 9 am to 11:40 am
Time allowed
• Perusal time: 10 minutes
• Working time: 2 hours 30 minutes
Examination materials provided
• Paper One — Question and response book
• Paper One — Resource book
• Paper One Part A — Multiple-choice response sheet
Equipment allowed
• QCAA-approved equipment
• non-programmable calculator
Directions
Do not write in this book during perusal time.
Paper One has two parts:
• Part A — Knowledge of subject matter
– Section 1 — Multiple choice (attempt all questions)– Section 2 — Short response (attempt all questions)
• Part B — Scientific processes (attempt four questions only)
Suggested time allocation
• Part A: 1 hour 50 minutes
• Part B: 40 minutes
Assessment
Paper One assesses the following assessment criteria:
• Knowledge of subject matter
• Scientific processes
Assessment standards are at the end of this book.
After the examination session
The supervisor will collect this book when you leave.
––
Candidate use
Print your candidate number here
Attach barcode here
Number of books used
1 6
Supervisor use only
QCAA use only
Supervisor’s initials
Marker number
Part A — Knowledge of subject matter
Part A assesses knowledge of subject matter and its simple application based on the eight topics in the Chemistry Senior External Syllabus 1998 (amended 2006).
Part A is worth 80 marks.
Suggested time allocation: 1 hour 50 minutes.
Section 1 — Multiple choice
Section 1 has 10 questions worth 1 mark each. Attempt all questions.
Each question contains four options. Select the option that you think is correct or is the best option. Respond on the multiple-choice response sheet.
Question 1
A dilute solution of a strong acid
Question 2
Which expression below represents Keq for the following reaction?
A has a bitter taste.
B will not conduct electricity.
C turns litmus from blue to red.
D reacts with active metals to produce carbon dioxide gas.
A C
B D
Fe3O4 s 4H2+ g 3Fe s 4H2O g +
H2O g 4
H2 g 4---------------------------
Fe s 3H2O g 4
Fe3O4 s H2 g 4---------------------------------------------------
H2 g 4
H2O g 4---------------------------
Fe3O4 s H2 g 4
Fe s 3 H2O g 4---------------------------------------------------
1
Question 3
Which of the following samples of gas (under the same conditions of temperature and pressure) would have the greatest volume?
Question 4
An element whose particles are held together by dispersion forces would be located in which group of the periodic table?
Question 5
Aluminium reacts with iron(III) oxide according to the following equation:
How many grams of aluminium react to produce 84 J of heat?
Question 6
Two substances with different chemical and physical properties are found to have the same molecular formula, C2H6O.
This is best explained by which of the following?
A 1 g of carbon dioxide (CO2)
B 1 g of methane (CH4)
C 1 g of hydrogen (H2)
D 1 g of helium (He)
A 2
B 10
C 14
D 18
A 2.7
B 5.4
C 27
D 54
A Chemical tests are not very reliable.
B C2H6O is also an empirical formula.
C One of the substances must contain an impurity.
D The atoms must be arranged and bonded differently in the two substances.
2Al s Fe2O3 s + 2Fe s Al2O3 s 840 J+ +
2
Question 7
The following gaseous equilibrium is established at high temperatures in the presence of a finely divided nickel (Ni) catalyst:
A particular reaction is carried out using equal numbers of moles of CH4(g) and H2O(g).
Which of the following sets of changes in conditions would lead to the greatest increase in the proportion of the reactants converted to products?
Question 8
Carbon atoms exist in nature with mass numbers 12, 13 and 14.
All of the isotopes of carbon have
Question 9
In which of the following compounds does chromium have an oxidation number of 3?
Volume of reaction vessel Temperature
A increased decreased
B increased increased
C decreased decreased
D decreased increased
A a different number of electrons.
B very different chemical properties.
C the same number of protons in the nucleus.
D the same number of neutrons in the nucleus.
A KCr(SO4)2
B K2CrO4
C CrCl2
D CrO3
CH4 g H2+ O g CO g 3H2+ g H 206 kJ mol 1–=;
3
Question 10
Hydrogen reacts with bromine according to the following equation:
Which of the following statements is correct?
End of Section 1
A The reaction is endothermic.
B The reaction involves a phase change.
C The heat content of the products is less than the heat content of the reactants.
D The system moves towards a state of higher potential energy as the reaction occurs.
H2 g Br2 g + 2HBr g energy+
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Section 2 — Short response
Section 2 has eight questions worth 70 marks in total. Attempt all questions.
Write your responses in the spaces provided. Show all working.
If you need more space for a response, continue at the back of this book. Label any continued response with the question number.
Question 11 — Materials: Properties, bonding and structure
a. Complete the table below.
(2 marks)
b. A blue crystalline solid is heated strongly in a closed container to produce a brown gas and a black solid. The same products remain when cooled.
Has a chemical change occurred? Identify one piece of evidence that supports your response.
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(1½ marks)
c. Complete the table below by writing the name or formula of each substance listed.
(2 marks)
Definition/description Chemical term
i. A tightly bound group of atoms that behaves as a unit and carries a charge
ii. A substance that cannot be changed into simpler substances under normal laboratory conditions
Name Formula
copper(I) nitrate
S2–
carbonic acid
OF2
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d. A particular atom consists of 18 neutrons, 17 protons and 17 electrons.
i. What element is it and to which periodic table group does it belong?
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ii. What type of bonding will be present when this element reacts to form a compound with magnesium, atomic number 12?
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(1½ marks)
e. Explain why water (H2O) is a liquid whereas hydrogen sulfide (H2S) is a gas at room temperature and pressure.
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(2 marks)
f. Water (H2O) and tetrachloromethane (CCl4) both contain polar covalent bonds, but only water is composed of polar molecules. Explain why this is so. Include diagrams in your response.
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(2 marks)
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Question 12 — Reacting quantities and chemical analysis
a. Write a balanced equation to represent the reaction between lithium nitride (Li3N) and water to form ammonia (NH3) and lithium hydroxide.
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(2 marks)
b. Calculate the mass of copper(II) sulfate that must be dissolved in order to make 500 mL of a 0.25 M solution.
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(2 marks)
c. How many carbon atoms are present in 0.05 g of carbon?
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(2 marks)
d. The exhaust gases from an idling car engine contain 8% CO(g) by volume. What is the mass of carbon monoxide in one litre of exhaust gas at STP?
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(2 marks)
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e. What mass of CS2(l) is formed when 60.0 g of carbon reacts with 150.0 g of SO2(g) according to the following balanced equation?
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(3 marks)
5C s 2SO2 g + CS2 l 4CO g +
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Question 13 — Oxidation and reduction
a. Complete the sentence below.
In a voltaic cell, electrons flow from the to the
along the .
move through the salt bridge.
(2 marks)
b. State two ways an electrolytic cell differs from a galvanic (voltaic) cell.
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(1 mark)
c. Explain why the following equation represents an oxidation–reduction reaction.
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(1 mark)
d. Use appropriate chemical equations to explain the electrochemical reactions that occur when a mixture of FeSO4(aq) and Fe2(SO4)3(aq) is placed in a container made of tin.
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(3 marks)
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•
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Cu(s) 2NO3–(aq) 4H(aq) Cu2(aq) 2NO2(g) 2H2O(l)
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Question 14 — Organic chemistry
a. Complete the table below.
(2 marks)
b. Name the organic substance with the following structure:
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(2 marks)
c. To which organic chemistry family does the following molecule belong?
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(1 mark)
Definition/description Chemical term
i. A specific arrangement of atoms in an organic compound that determines the chemistry of that compound
ii. An organic compound having both –NH2 and –COOH groups in the same molecule
CH3
H
CH3
CH
H
OH
C
H
CH3
C
H
H
H
C
H
H
C
H
H
CC
CH
H
H
H
C
CH
H N
H
C
HH
H
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d. Write balanced chemical equations to represent the following reactions:
i. ethene Br2(l)
ii. ethanol ethanoic acid
iii. combustion of butane in pure oxygen
(3 marks)
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Question 15 — Chemical periodicity
a. Identify the s, p, d and f block groups of elements on the periodic table diagram below.
(2 marks)
b. What are valence electrons?
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(1 mark)
c. A student stated that 1s2 2s2 2p3 3s1 was the electron configuration for neutral oxygen atoms in their lowest energy state.
Discuss the validity of the statement.
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(1 mark)
d. Both sodium metal and fluorine gas react violently with water, but sodium fluoride just dissolves.
Explain the differences in reactivity between the elements and the compound.
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(2 marks)
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Question 16 — Gases and the atmosphere
a. State any two physical properties common to all gases.
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(1 mark)
b. Explain why the concentration of ozone in the upper atmosphere is important to humans.
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(1 mark)
c. State Dalton’s law of partial pressures.
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(1 mark)
d. A sample of methane (CH4) is held at the same temperature as a sample of ammonia (NH3).
Compare the average kinetic energies of the molecules of the two gases.
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(1 mark)
e. A meteorological balloon is filled with helium at 0 °C and 100 kPa.
By what factor will its volume change when it passes through a region of the atmosphere where the temperature is –91 °C and the pressure is 10 kPa?
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(2 marks)
•
•
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Question 17 — Energy and rates of chemical reactions
a. Define the term bond energy.
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(1 mark)
b. Sketch a potential energy–reaction coordinate diagram to represent a single-step reaction with H 200 kJ and forward reaction activation energy of 100 kJ.
Label both axes and the parts of the curve representing reactants, products and activated complex.
(3 marks)
c. Why does the equation MnO2 4HCl MnCl2 Cl2 2H2O not represent the reaction mechanism by which Cl2 is prepared from HCl and MnO2?
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(2 marks)
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d. Find the H for the reaction N2H4(l) H2(g) 2NH3(g), given the following reactions and H values:
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(3 marks)
N2H4(l) CH4O(l) CH2O(g) N2(g) 3H2(g) H 37 kJ
N2(g) 3H2(g) 2NH3(g) H 46 kJ
CH4O(l) CH2O(g) H2(g) H 65 kJ
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Question 18 — Chemical equilibrium
a. Complete the table below.
(2 marks)
b. State Le Chatelier’s Principle.
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(1 mark)
(2 marks)
d. A reaction that occurred at a temperature of 500 K had an equilibrium constant of 240.The same reaction when at a temperature of 750 K had an equilibrium constant of 3.
Is the reaction exothermic or endothermic? Explain your response.
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(2 marks)
Definition/description Chemical term
i. A substance that is almost completely ionised in aqueous solution
ii. A compound which in chemical reactions acts as a hydronium ion acceptor or an electron pair donor
c. i. Complete the following acid–base equation:
ii. On the equation above, label the Lowry–Bronsted acid–base pairs.
+.......................... ..........................NH3(aq) CH3COOH(aq)
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e. An equilibrium mixture is established according to the following equation:
Explain what change/s would occur to the composition of the mixture when:
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(2 marks)
f. A saturated solution of Ca(OH)2 has a pH of 12.4. Calculate the solubility product (Ksp) of Ca(OH)2 .
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(3 marks)
End of Section 2
End of Part A
i. the pressure was increased.
ii. additional HCl(g) was added to the system.
Cl2(g) H2(g) 2HCl(g)
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Part B — Scientific processes
Part B assesses scientific processes based on the eight topics in the Chemistry Senior External Syllabus 1998 (amended 2006) and practical work undertaken during your study of the subject.
Part B has five questions of equal value. Attempt four questions only. If you respond to all five questions, only your first four responses will be assessed.
Write your responses in the spaces provided.
Suggested time allocation: 40 minutes.
Question 1 — Oxidation and reduction
A series of experiments are carried out to investigate the redox reactions between the halogens (L2, M2, Q2 and R2) and their ions (L–, M–, Q– and R–).
To see evidence of any reaction, some CCl4 had to be added to the reaction containers.
The colours of the halogens in CCl4 are shown in Table 1. The halide ions are all colourless in CCl4 .
The colours that resulted after various halogens were mixed with halide ions (in CCl4) are shown in Table 2.
a. Use the information in Table 1 to complete the last column of Table 2, showing all products where reactions occur. Write NR if there is no reaction.
b. Arrange the halogens in order of reactivity with the most reactive halogen first.
Show how you arrived at your response.
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Table 1 Table 2
Halogen Colour in CCl4 Reactants Colour in CCl4 Products of reaction
L2 red R2 L– red
M2 green L2 M– green
Q2 pink Q2 R– pink
R2 yellow Q2 M– pink
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c. A method of arranging metals in a reactivity order is to measure the energy output (voltage) of voltaic cells.
A student sets up a cell similar to the one in Figure 1 below, using different pairs of metals. He measures the voltage of each cell.
The more reactive electrode is the negative terminal.
The greater the voltage, the greater the difference in reactivity.
The results are shown in Table 3.
Arrange the metals in order of reactivity with the most reactive metal first.
Show how you arrived at your response.
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Table 3
ElectrodesVoltage of cell
positive negative copper magnesium 2.7
lead iron 0.3
copper iron 0.8
lead magnesium 2.2
iron zinc 0.5
zinc magnesium 1.5
lead zinc 0.6
copper zinc 1.1
copper lead 0.4
iron magnesium 1.9
V
Voltmeter
metal electrodes
salt bridge
electrolyte
Figure 1
19
Question 2 — Chemical equilibrium
The concentration of acetic acid in a sample of vinegar can be determined by a reaction with a solution of sodium hydroxide using a suitable indicator. The reaction occurring will be:
In such an experiment, 10 mL of a commercial vinegar was poured into a clean volumetric flask and filled to the 100 mL mark with distilled water. 10 mL samples of the diluted vinegar were placed in clean conical flasks. Two drops of a suitable indicator were added to each flask and the diluted vinegar was titrated with 0.25 M NaOH. The procedure was repeated three more times to obtain the following data.
a. Use the table below to select a suitable indicator for the above titration. Justify your selection.
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b. What is the purpose of the trial titration? What colour would the trial solution be at the end of the titration?
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Titration Titre (mL)
Trial 33.0
1 31.4
2 31.6
3 31.7
Acid Neutral Base
[H+] (mol L–1) 100 10–1 10–2 10–3 10–4 10–5 10–6 10–7 10–8 10–9 10–10 10–11 10–12 10–13 10–14
pH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH range
phenolphthalein indicator
clear clear clear clear clear clear clear clear clear pink pink pink pink pink pink 8.3–10.0
bromothymol blue indicator
yellow yellow yellow yellow yellow yellow yellow blue blue blue blue blue blue blue blue 6.2–7.6
methyl red indicator
pink pink pink pink pink pink yellow yellow yellow yellow yellow yellow yellow yellow yellow 4.4–6.0
methyl orange indicator
red red red red yellow yellow yellow yellow yellow yellow yellow yellow yellow yellow yellow 3.1–4.4
cresol red indicator
red red red yellow yellow yellow yellow yellow yellow yellow yellow yellow yellow yellow yellow 0.2–1.8
pH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 pH range
HC2H3O2(aq) NaOH(aq) NaC2H3O2(aq) H2O(l)
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c. Calculate the concentration of acetic acid in the diluted vinegar sample.
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Question 3 — Gases and the atmosphere;Materials: Properties, bonding and structure
a. Cotton soaked in ammonia water and cotton soaked in hydrochloric acid are placed at either end of a 100 cm glass tube. Gases diffuse along the tube. When the gases meet, a reaction occurs and a white band of NH4Cl forms.
A relationship exits between the rates of diffusion of two gases and molar masses, as shown:
Use the expression above to work out which of the positions (W, X, Y or Z) in the diagram below shows where the white band will form. Show all working and reasons for your response.
(molar mass NH3 17 g, molar mass HCl 36.5 g)
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Molar mass (gas B)Rate (gas A)
Rate (gas B) Molar mass (gas A)�
cotton soaked inammonia water
cotton soaked inconcentrated HCl
unreactivecork
W X Y Z unreactivecork
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b. Electrons are found in different levels around the nucleus.
Electrons may form pairs (shown as ) or be unpaired (shown as or ).The magnetic moment () of an element is related to the number of unpaired electrons (x) by the formula:
Write the electron configuration for oxygen (atomic number 8) and then calculate for this element.
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c. The labels have fallen from three bottles containing strontium chloride (SrCl2), naphthalene (C10H8) and phenol (C6H5OH). Melting point and solubility tests were carried out, with the following results.
Identify the contents of bottles 1, 2 and 3 from the above information.Justify your selections.
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Bottle Melting point Water Ethanol Benzene
1 41 °C soluble very soluble very soluble
2 80 °C insoluble slightly soluble very soluble
3 873 °C soluble insoluble insoluble
x x 2+ =
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Question 4 — Energy and rates of chemical reactions
A piece of calcium carbonate in the form of a marble chip was added to dilute hydrochloric acid, and the carbon dioxide gas produced was collected in a graduated tube. The volume of gas collected was read at one-minute intervals. A diagram of the apparatus is shown below.
The results from the experiment were recorded as follows:
a. Plot a graph of the progress of the reaction.
Time (min) 0 1 2 3 4 5 6 7
Volume (mL) 0 3 10 29 48 51 52 52
dilute acid
marble chip
carbon dioxide gas10
20
30
40
50
(Spare graph paper is at the end of this book if required.)
24
b. On your graph, label as AB the region that represents the period of fastest reaction.
c. Explain why the reaction is fastest at this time.
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d. In this experiment the rate of the reaction was monitored by measuring the time taken to produce a certain volume of gas. Outline one other way the rate of this reaction could be monitored.
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Question 5 — Reacting quantities
Groups of chemistry students reacted an unidentified metal, X, with sulfuric acid. A gas was produced that was identified as hydrogen. The students’ results are tabulated below.
a. Plot a graph of moles of X versus moles of H2 produced.
Student group Mass of X (g) Moles of X Volume of H2 (mL) Moles of H2
3 0.0297 0.00124 22.0 0.00090
1 0.0498 0.00208 49.0 0.00201
5 0.0612 0.00255 62.0 0.00254
2 0.0708 0.00295 63.0 0.00258
4 0.0907 0.00378 63.0 0.00258
6 0.1003 0.00418 63.0 0.00258
(Spare graph paper is at the end of this book if required.)
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b. Interpret the change in shape of the graph.
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c. From the information you have derived about the metal X, suggest which column in the periodic table this metal would be placed.
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End of Part B
End of Paper One
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29
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tep
inve
stig
atio
ns.
A hi
gh a
bilit
y to
suc
ceed
in
sim
ple
scie
ntifi
c pr
oces
s ta
sks
— c
olle
ctin
g an
d or
gani
sing
da
ta, p
roce
ssin
g in
form
atio
n,
mak
ing
sim
ple
judg
men
ts,
com
mun
icat
ing
info
rmat
ion
in
vario
us c
onte
xts,
dev
isin
g an
d de
sign
ing
sim
ple
and/
or
sing
le-s
tep
inve
stig
atio
ns.
A sa
tisfa
ctor
y ab
ility
to s
ucce
ed
in s
impl
e sc
ient
ific
proc
ess
task
s —
col
lect
ing
and
orga
nisi
ng
data
, pro
cess
ing
info
rmat
ion,
m
akin
g si
mpl
e ju
dgm
ents
, co
mm
unic
atin
g in
form
atio
n in
va
rious
con
text
s, d
evis
ing
and
desi
gnin
g si
mpl
e an
d/or
si
ngle
-ste
p in
vest
igat
ions
.
Lim
ited
abilit
y to
suc
ceed
in
sim
ple
scie
ntifi
c pr
oces
s ta
sks.
Very
lim
ited
abilit
y to
suc
ceed
in
sim
ple
scie
ntifi
c pr
oces
s ta
sks.
31
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ight enquiries should be made to:
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