Australian International School - slider-chemistry-11

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1










Australian
International
School

Singapore




2010


PRELIMINARY COURSE
EXAMINATION




Chemistry







General Instructions




Reading time


㔠浩湵瑥s



Working time


㈠桯畲s



Write using black or blue pen



Draw diagrams using pencil



Approved
calculators may be
used




Write your student number in


the space provided


Student Name




























Total marks


75








This paper has two parts, Part A and Part B


Part A




浡m歳



Attempt Questions 1
-
20



Allow about 35

minutes for this part


Part B




浡m歳



Attempt Questions
21
-
34



Allow about 1 hour and 25

minutes for this part




2


Part A


20

marks

Attempt Questions 1
-
20

Allow about 35

minutes for this part



Use the multiple
-
choice answer sheet.


Select the
alternative A,B,C or D that best answers the question. Fill in the response oval
completely.


Sample:

2 + 4 =


(A) 2


(B) 6


(C) 8


(D) 9









A



B



C



D



If you think you have made a mistake, put a cross through the incorrect answer and fil
l in the
new answer.








A



B



C



D



If you change your mind and have crossed out what you consider to be the correct answer,
then indicate the correct answer by writing the word
correct

and drawing an arrow as
follows.








A



B



C



D










correct




















3



1.

Which of the following correctly shows the
most abundant

element, by mass, in each
region of Earth.




Lithosphere

Hydrosphere

Atmosphere

(A)

Oxygen

Hydrogen

Oxygen

(B)

Iron

Oxygen

Hydrogen

(C)

Aluminium

Water

Oxygen

(D)

Oxygen

Oxygen

Nitrogen



2.

The table below shows three examples of common mixtures.




MIXTURE

MAIN COMPONENTS

SEPARATION
TECHNIQUE

Blood

Blood cells and plasma

X

Purple food dye

Blue and

red dyes

Y

Wine

Ethanol and water

Z


Which of the alternatives below correctly identifies each separation technique
(X,Y and Z)?



X

Y

Z

(A)

centrifuging

chromatography

distillation

(B)

sedimentation

chromatography

crystallisation

(C)

centrifuging

distillation

evaporation

(D)

sedimentation

chromatography

filtration




3.

The characteristics of an eleme
nt (
“X”) are outlined below.


Element “X”:

-

is a gas at room temperature

-

is composed of diatomic molecules

-

forms a compound with

hydrogen with a formula XH
3


When this element reacts with calcium, the formula of the compound formed would be:



(A)

CaX

(B)

Ca
2
X
3

(C)

CaX
2

(D)

Ca
3
X
2

4


4.

Which of the following is consistent with an atom of copper?




Number of
neutrons

Mass number

(A)

29

64

(B)

34

63

(C)

29

63

(D)

34

64




5.

Deuterium is an isotope of hydrogen, often represented by the symbol D. The deuterium
nucleus consists of 1 proton and 1 neutron, and is present in all naturally
occurring hydrogen
(0.03 % by mass).



What is the closest approximation to the
molecular mass

of a methane molecule, which
includes 1 deuterium atom?


(A)

2

(B)

6

(C)

17

(D)

20



6.

What is the molar mass of iron(III) oxide?



(A)

71.85 g

(B)

87.85 g

(C)

159.70 g

(D)

199.55 g


7.

When ammonium nitrate is dissolved in water the
temperature

decreases.




Which of the following is

the best explanation for this?

(A)

The dissolution is exothermic and heat is lost to the surroundings.

(B)

The
dissolution is endothermic and heat is absorbed from the water.

(C)

The ammonium nitrate was colder than the water.

(D)

More energy was released by forming bonds than was absorbed in breaking
bonds.



5


8.

Which of the following correctly associ
ates crude oil fractions and their uses?




Fractions

Uses

(A)

C
3

C
8

C
10

bbq gas

petrol for aeroplanes

tar for road surfaces

(B)

C
20

C
4

C
8

tar for road surfaces

petrol for cars

petrol for aeroplanes

(C)

C
1

C
8

C
10

domestic cooking

petrol for cars

petrol for aeroplanes

(D)

C
3

C
10

C
12

bbq gas

petrol for cars

tar for road surfaces





9.

The formation of ammonia gas is represented by the following equation.








N
2
(
g
) + 3H
2
(
g
)
←→

㉎H
3
(
g
)



Bonds broken

Bonds formed

(A)

2

2

(B)

2

5

(C)

4

3

(D)

6

6




10.









Which of the following will NOT result in more frequent collisions in a reaction system?


(A)

increasing the pressure

(B)

increasing the concentration of reactants

(C)

adding a catalyst

(D)

increasing the
temperature


11.

Which of the following generalisations is correct?


(A)

The more active a metal, the greater the chance that it will occur in its elemental
form.

(B)

The higher the ionisation energy, the more reactive an element is
likely to be.

(C)

The less active a metal, the lower the energy requirements are to extract it from its
ore.

(D)

The less abundant a metal ore is, the lower the cost of producing the metal.


6


12.

The reaction profile below shows the chan
ge in enthalpy over the time for a particular
reaction.










Which of the following alternatives best represents the change to the profile when the
reaction is performed in the presence of a
catalyst
?





























13.

A student notes that car battery acid is 18M H
2
SO
4
(aq). What mass of H
2
SO
4

will be
present in 100 mL of battery acid?




(A)


88 g.

(B)


176 g.

(C)


880 g.

(D)


1764 g.


(A)

(D)

(B)

(C)

7


14.

A chemist added some PbCl
2

(s) to some water, stired the mixture for a few minutes,
and noted that some of the lead(II) chloride was still undissolved, on the bottom of the
beaker. He then added some radioactive PbCl
2

(s) to the beaker, and measured the
radioactivity of the soluti
on over time.


Which of the following graphs represents the chemist’s results?


























15.








A student finds a coloured solution in a bottle with its label missin
g. What test could
the student d
o in order to determine whether

the solution contains an ionic or a
covalent compound?




(A)


Test the boiling point of the solution.

(B)


Test the melting point of the solution.

(C)


Test the electrical conductivity of the solution.

(D)


Test the freezing
point of the solutio
n.







T
ime
(min)

R
adioactivity
in solution

R
adioactivity
in solution

T
ime
(min)

T
ime
(min)

R
adioactivity
in solution

T
ime
(min)

R
adioactivity
in solution

(A)

(B)

(D)

(C)

8


16.

The melting point, and effect of strong heat (ie a Bunsen flame) were tested on three
solids. The results are shown in the table below.


Solid

Melting point (
o
C)

Effect of heating the solid

X

110

A gas and a solid were produced.

Y

80
-
135

A gas,

smoke, and a solid were
produced.

Z

31.5

A liquid was produced.


Which of the following classifications of substances X, Y and Z is correct?



X

Y

Z

(A)

Compound

Element

Mixture

(B)

Element

Mixture

Compound

(C)

Mixture

Compound

Element

(D)

Compound

Mixture

Element




17.

When very reactive metals react with water, the metal hydroxide and hydrogen gas are
produced. Which of the following equations represents this for lithium?




(A)


Li(s) + H
2
O(l)


Li佈⡡焩q+⁈
2
(g)

(B)


Li(s) + 2H
2
O(l)


Li⡏䠩
2
(aq) + H
2
(g)

(C)


2Li(s) + 2H
2
O(l)


2L楏i⡡焩q+⁈
2
(g)

(D)


4Li(s) + 2H
2
O(l)


2

2
OH
(aq) + H
2
(g)


18

A swimming pool contains 20 000 L of water at 14

C.


What is the quantity of heat, in kJ, required to raise the pool temperature to 21

C?


(A)

20 000


(21


14)

(B)

4.2


20 000


(21


14)

(C)

20 000


4.2


21

(D)

4.2


(21


14)


20 000


19

Which of the following is a
renewable

source of methane?


(A)

A natural gas well

(B)

Coal seams

(C)

Sewage plants

(D)

Fractional distillation of petroleum

9


20

What is the correct IUPAC name
for the compound with the following structure?



CH
3
CH
2
CH
2
CHCHCH
3


(A)

2
-
hexene

(B)

2
-
pentene

(C)

4
-
hexene

(D)

3
-
pentene

10


Part B


Attempt questions 21
-

34

Allow about 1 hour and 25 minutes for this p
art.


Answer the questions in the spaces provided.


Show all relevant
working in questions involving calculations.




Question 21

(5 marks)


(a) Write a half equation to show the formation of calcium ions from


calcium atoms.



.....................................................................................................................



(b) Write a half equation to show the formation of chloride ions from


chlorine gas.




.....................................................................................................................



(c)
Draw an electron dot diagram of the compound formed from calcium and


chlorine.










(d)

The formulae

of all ionic compounds must be empirical”


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Marks



1






1






1













2


11



Question 22

(3 marks)


A student performed an experiment to measure the heat of solution of calcium
hydroxide, Ca(OH)
2
.


The table below shows their results
.


mass of polystyrene
cup (g)

54.55

mass of cup with water (g)

155.1

initial temperature of water (
o
C)

20.5

mass of Ca(OH)
2

used (g)

1.15

final temperature of water (
o
C)

52.5


Calculate the molar heat of solution of Ca(OH)
2

using this data.

Show all working.



.....................................................................................................................



.....................................................................................................
................



.....................................................................................................................



...................................................................................
..................................



.....................................................................................................................



Question 23

(4 marks)


Photosynthesis is one of the most important chemical
reactions on the planet.


(a) Write a balanced chemical equation for photosynthesis.



.....................................................................................................................



(b) Foss
il fuels are known as ‘non
-
renewable’ resources. Outline how fossil

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Marks














3

















1





3




12



Question 24

(7 marks)


A student added varying masses of a metal ‘X’ to excess hydrochloric acid and
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a焩q


塃l
2

(aq) + H
2

(g)


The results of the experiment are
shown in the table below.


Mass of metal added (g)

Mass of H
2

(g) collected

5

0.24

10

0.49

15

0.83

20

1.05

25

1.30


(a) Given that X is not a transition metal, to which Group (1 to 8) of the


Periodic Table must it belong
? Justify your answer.



.....................................................................................................................



.....................................................................................................................


(b) Plot the data on the grid below, and draw a line of best fit.

Marks


















1







3



































































































































































































































































































































































































































































































































































































































































































































































































































































13


Marks

Question 24 (continued)


(c)


Use the graph to estimate the mass of metal which would be required to


produce 0.5 mol of hydrogen gas.



.....................................................................................................................



(d) Use your answer to (c) to determine the molar mass of the metal used,


and hence ident
ify the metal.



.....................................................................................................................




....................................................................................
.................................



.....................................................................................................................



..................................................................
...................................................




Question 25

(4 marks)


Two interesting properties of water are the way its density changes with
temperature, and its relatively high specific heat capacity.


Explain

how each of these properties is

imp
ortant in aquatic environments.



.....................................................................................................................




.....................................................................................................................



.....................................................................................................
................



.....................................................................................................................



...................................................................................
..................................




.....................................................................................................................



................................................................
.....................................................



.....................................................................................................................





1






2


















4





14



Question 26

(6 marks)


(a)

Draw a structural diagram (formula) of 2
-
butene.






(b) 2
-
butene undergoes complete combustion in air.



Write a balanced equation for this reaction.



.....................................................................................................................



(c)

Draw a labelled energy profile diagram for the reaction in part (b) above.






(You do not need to include numerical values, nor scales on the axes.)
















(d) Outline how compounds such as 2
-
butene would be safely stored.



.....................................................................................................................




....................................................................................................
.................



.....................................................................................................................



..................................................................................
...................................



Marks



1








1





2


















2






reaction progress

energy

15



Question 27

(4 marks)


The following diagram summarises the general steps in the extraction of a metal
from its ore.









Using these steps as a guide, describe the process by which copper metal is
produced from an identified ore in Australia.



.....................................................................................................................




....................................................................................................
.................



.....................................................................................................................



..................................................................................
...................................



.....................................................................................................................




.....................................................................................................................



.....................................................................................................
................



.....................................................................................................................



...................................................................................
..................................




.....................................................................................................................



................................................................
.....................................................



.....................................................................................................................







Marks












4






Mining

Concentration

Smelting to
reduce metal ions
to metal atoms

Refining

16




Question 28

(3

marks)


Refer to
the following solubility rules to answer this question.


Marks



General Rule

Exceptions

all nitrates are soluble

none

all acetates are soluble

none

all ammonium compounds are soluble

none

all group I compounds are soluble

none

most chlorides are
soluble

silver and lead (insoluble)

most sulfates are soluble

barium and lead (insoluble)

calcium and silver (sparingly soluble)

most hydroxides are insoluble

group I and ammonium compounds (soluble)

calcium (slightly soluble)

most carbonates are
insoluble

group I and ammonium compounds (soluble)

most phosphates are insoluble

group I and ammonium compounds (soluble)



(a) A student finds a bottle containing an unknown, pale blue liquid. She


knows that it is not pure w
ater and she decides it must contain an ionic


compound. She assumes that because the solution is blue, it must contain


Cu
2+

ions.



Given this assumption, identify ALL of the ANIONS which could be


present in the solution.



.....................................................................................................................



(b) Choose ONE of the anions from your answer to (a) above, and e
xplain


how the student could determine whether it was present in the solution.



Inclu
d
e

an equation to support your answer.



...............................................................................
......................................




.....................................................................................................................



............................................................
.........................................................



.....................................................................................................................








1






2






17




Question 29

(3 marks)


Your Chemistry

teacher asks you to investigate the effect of acid concentration on
the rate of an ‘acid + metal’ reaction.


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⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮.


†††††††††
⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮
⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮⸮.







Question 30

(
2 marks)


Mercury forms two compounds with oxygen: mercury (I) oxide, and mercury (II)
oxide.


A chemist thermally decomposed 6.60g of one of these compounds and obtained
6.36g of met
allic mercury.


Determine which of the two oxides the chemist decomposed.



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Marks






3



























2
















18




Question 3
1

(
3 marks)


Explain why diamond and graphite exhibit such different electrical conductivities
and hardnesses.



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Marks



3




Question 3
2

(4 marks)


Water is an important solvent in many industrial, domestic and biological situations.


(a) A student dissolves 3.6
g of ethanol (CH
3
CH
2
OH,
or
C
2
H
6
O) in 150 mL


of water. 25 mL of this solution was then added to 125 mL of water.



Calculate the final concentration of the solution.



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(b) Exp
lain why ethanol is more soluble in water than ethane is.



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2













2

19




Question 33
(2 marks)


Explain why first ionisation energy increases from
left to right across a period in the
Periodic Table.



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Question 3
4

(5 marks)


Matter can be classified in a number of ways, depending on the context being

considered.


Describe TWO systems used to classify matter in Chemistry. Include diagrams to
illustrate your answer.



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Marks



2


















5





Continue your answer over the page if necessary.

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End of Paper