cape chemistry 2013 u1 p1

8/9/2019 CAPE Chemistry 2013 U1 P1

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TEST CODE

02 112010

MAY/JUNE2013

C R I B B E N E X M I N T IO N S C O U N C I L

CARIBBEAN ADVANCED

PROFICIENCY

EXAMINATION '

CHEMISTRY - UNIT

Paper

01

hour

3

minutes

(

21

~ Y 2013

a.m.) )

READ

THE

FOLLOWING INSTRUCTIONS

CAREFULLY.

1. This test consists of 45 items. You will have I hour and 30 minutes

to

answer them.

2.

In

addition to this test booklet, you should have an answer sheet'and a Data Booklet.

3.

Each item in this test has four suggested answers lettered (A), (B),

(C),

(D). Read each item

you are about to answer and decide which

choi


2/11

l .

2.

3.

- 2 -

Which of

he

following statements is

NOT

a part of Dalton s atomic theory?

A)

Atoms are indivisible.

B)

Atoms are characterised by their

atomic number.

C) The atoms

of

an element have

identical properties.

D) The atoms ofan element differ from

those of other elements.

Item 2 refers to the following diagram which

shows the energy levels for the hydrogen

atom and the electronic transitions which

produce lines in the visible region.

==========::::;==::i===n=S

_ =i=_ == ~ : = _ : : = ~

< : = ~ = ~

n=l

Which of the

series below

involves

transitions from higher energy levels to the

n

=

2 level?

A) Balmer

B)

Dalton

(C)

Lyman

D) Paschen

Which

of

the

following

ions has the

GREATEST polarizing power?

A)

Be +

B) Ca

2

C)

Li+

D) Sr

4.

5.

6.

Which

of

the following factors

is

important

in determining the stability of an isotope?

A) Size of atomic radius

B) Number of protons

C) Ratio ofprotons to electrons

D)

Ratio

of

protons to neutrons

Which of the following statements is

TRUE about 5 dm

3

of

hydrogen and 5 dm

of oxygen

at 0

C and I

OJ kPa?

A)

B)

C)

(D)

They react to produce 5

dm of

water.

They possess the same amount of

kinetic energy.

They contain the same number

of

molecules.

They react completely with each

other.

Which

of the following solids has a giant

molecular lattice?

A) Carbon dioxide

B) Copper oxide

C) Magnesium oxide

(D)

Silicon dioxide

GO

ON TO iE

NEXT

P GE


3/11

7.

8.

9.

10.

- 3 -

Item

7

refers to the following equation

which shows the production ofammonia.

N

2

(g)

+

3H

2

(g)

.=

2NH,(g)

f I 0

cm

of

nitrogen reacts with 30

cm

of

hydrogen at STP, what volume of NH, is

produced?

(A)

B)

C)

D)

JO

cm

15 cm

20cm

40cm

F9r complete reaction, 0.25 g

ofa

monobasic

acid requires IO

cm of0.2

mol dm' sodium

hydroxide. What is the relative molecular

mass of the acid?

(A) 12.5

B) 62.5

(C) 125

D) 250

The simplest formula for a compound that

contains 50% S and 50% 0 by mass is

(A) SO

B)

(C)

D)

so,

s,o

s,o.

Which of he following processes represents

an

oxidation?

(A)

Mn0

2

--+

2

B),

Mno.---+

Mno

2

-

(C)

Mno.---+

MnO,

(D)

Mn0

2

--+

Mno.-

~ ' .

11.

12.

13.

Item

11

refers to the following information.

A

piece

of

copper metal is placed in silver

nitrate solution, as shown in the diagram

below.

-

Cu

metal

-

I

Which

of

the following observations is

correct?

(A) Copper metal dissolves and the

solution remains colourless.

B) Copper metal is deposited and the

solution turns blue.

(C)

Silver metal forms and the solution

turns blue.

D)

Silver metal forms and the solution

remains colourless.

Which of the following gases is MOST

likely to have the characteristics

of

an ideal

gas?

(A)

B)

(C)

D)

Ammonia

Helium

Methane

Oxygen

A gas

in

a syringe occupies a volume of

50 cm and has a pressure of 0.49346

atmospheres. What is the pressure of the

gas

if

he plunger

of

he syringe is pushed in,

reducing the volume of the gas

to

20 cm'?

(I atmosphere=

IOI

325 Pa)

(A)

(B)

(C)

(D)

20kPa

125

kPa

20

OOOkPa

125 000 kPa

ONro

nm

N XT

P GE


4/11

14 The second ionisation energy

of

calcium is 1150 kJ

mo1-

1

Which

of

the following equations represents this statement?

mot

1

A)

ca g) -+ Ca

2

g) + e-

L\H = +1150

B)

Ca g) -+ Ca2+ g) + 2e-

L\

=+1150

C)

ca g)

-+

Ca

2

g) +

e- L\H =-1150

D)

Ca

g) -+ Ca,. g)

+

2e- L\H

=-1150

Item

15

refers

to

the following standard enthalpies

of

combustion for carbon, hydrogen and octane.

Carbon

Hydrogen

Octane

mot

1

-394

-286

-5476

15 The standard enthalpy

of

formation

of

octane, M

,

s calculated using

A) M J octane)= -8 -394}-9 -286)-5476 k

rnoJ-

1

B) M J octane)=

-8

-394}-9 -286)-{-5476) kJ

mo1-

1

C)

M J octane)= 8 -394)

+

9 -286)-{-5476) k mo1-

1

D)

L\ octane)= 8

-394)-9 -286)-{-5476)

kJ mo1-

1

O

TO T1IE NEXTPAOE


5/11

-5 -

Item 16 refers to the following reaction which occurs in the presence

of

dilute acid.

CH,COCH, (aq)

1

2

(aq)--+

CH)

COCH, (aq) H (aq) 1 (aq)

16. The rate equation for the reaction

is

17.

Rate = k[CH,COCH, (aq)] [H {aq)). Which

of

the following equations BEST illustrates the SLOW

step?

0

OH

II I

(A) C H , - C - C H ,

H

- CH , - C- CH ,

Ea

0 l

II I

Il)

C H , -

C - C H , 1

2

--+ CH , -C-CH , + 1

Ea

0 l

II I

(C) CH , - C - CH, 1 --+CH,- C - CH,

D)

0

II

Ea

OH

I

C H - C - C H I

+H - C H - C - C H

, , , , I ,

l

The rate Jaw for a given reaction is

Rate=

k[A)

2

[B] . What are the units

fork?

(A)

moJ-

2

dm-

2

s-

1

(B) mo)

dm-

3

s-

1

(C) moJ-

1

dm

s-

1

(D)

mo1-

2

dm s-

1

GO ON TO

liE

N XTP GE


6/11

18

19

Which of the following phrases BEST

describes the relationship between the

half-life of a second order reaction and the

reactants?

A)

B)

C)

D)

ependent on

the

ini t ia l

concentration

of

the reactants

Independent

o f the

init ial

concentration

of

the reactants

Dependent

on the state

of the

reactants

Dependent on the final concentration

of

the reactants

Item 19 refers to the following equilibrium.

N, g) + 0

2

g) 2NO g), Ll =+I 80

kJ

moJ

1

Which of the curves

in

the diagram below

shows how increasing temperature affects

the yield of he product?

(D)

- - - - - , A )

Temperature UC)

20. Which

of

the following statements

21.

22.

does

NOT

refer to a system in dynamic

equilibrium?

(A)

B)

C)

D)

The reaction is reversible.

The amounts ofall the species

in

the

system remain constant.

The concentrations of all reactants

and products are equal.

The rate

of

the forward reaction is

equal to the rate

of

the backward

reaction.

Which of he following statements about a

catalyst would be true?

I.

II.

It increases the equilibrium constant

for the forward reaction only.

It increases the equilibrium cons

tant for both the forward and

backward reactions.

Ill.

It

has no effect on the position

of

(A)

B)

(C)

.CD

equilibrium.

I only

III

only

I and

III

only

II and III only

The value of K for the equilibrium reaction

p

H

2

(g) + 1

2

(g) 2HJ (g) at 444

C

at I atm

pressure

is

50.

What is the value of KP if the pressure

is changed to 2 atm and the temperature

remains the same?

(A) 25

B) 50

(C) 100

(D) 200

ON

TO

THE NEXT

P GE


7/11

23.

7

In

pure ethanol, (C,H,OH), the following

equilibrium can exist with ammonium ions.

NH; + C

2

H

5

0H

N H , C,H,OH,+

Which of the following combinations

describes the functions

of

NH;

and C,H,OH

according to the Bronsted-Lowry theory?

NH

C

2

H

5

0H

(A) Acid Base

B)

Base Acid

(C) Conjugate acid Base

(D)

Acid Conjugate base

M 1 . , ~ , , . , , . . A ~ ' ' . . ,

24

The results for four experiments which

. investigated the reaction between

propanaone and iodine (

a ~ l y s e d

by acid)

are given

in

the table below.

Ex

pt

H]

[Propanone]

[Iodine]

Rate

I I

0.5

I

10.8

2 0.5

0.5

I

5.3

3

0 0.25

I

5.4

4

0

0.5

0.5 10.6

Which of he following graphs represents the

orderof reaction with respect to propanone?

(A)

Rate

[Propanone)

(B)

Rate

[Propanone)

(C)

Rate

[Propanone)

(D)

Rate

l s

I

ONTO1llE

N XT

P GE


8/11

25.

- 8 -

Which

of

the following expressions

represents the solubility product

of

iron(lll) hydroxide?

(A) [Fe>+] [JOH-]

(B)

[Fe

3

+] [OH-]

3

[Fe(OH)

3

]

(C) [Fe

1

]

[30H-]

3

(D)

[Fe

1

]

[OH-]

3

26. Silver chromate(VI), Ag,Cr0

4

, is

sparingly

soluble in water. The

units.

for the solubility

product (K,,,) for silver chromate(VI) are

(A) mol dm-

B)

mol

dm-6

(C) moP dm_.

0) mol

4

dm-

12

27. Whichofthe following indicators is MOST suitable for use when titrating a weak acid against a

strong base?

Indicator

pH of Change

Colour Change

Acid ~ l k a l i

(A) Methyl orange 3.5

red -+ yellow

(B)

Litmus

6.0

red-+ blue

(C)

Bromothymol blue

7.0

yenow -+ blue

(0)

Phenolphthalein 9.5

colourless -+ pink

28. A

weak

acid, HX, dissociates as follows:

HX(aq) .=

x-(aq) + H'(aq)

-The -dissocfation coiitint,

K-;

for the above reactionIs 1.0 x l lf

1

,-mol am 3 .-w tafwill

oo

t he

approximate pH

of

1.0 x 10-

2

mol dm-

1

HX?

(A) S

(B) 6

(C) 7

(D) 8

29. Using standard electrode potentials, which

of

the following reactions would be MOST feasible?

(A) Zn(s) +

Cu''(aq)-+

Zn + (aq) + Cu(s)

(B)

Zn(s) + Pb

2

(aq)

-+

Zn

2

+ (aq) + Pb(s)

(C) Pb(s) + Zn

2

(aq) -+ Pb

2

(aq) + Zn(s)

D) Ca a) Zn2+ aq)-

Cu,.

aq) +

Zn )

00ONTO11fE

NEXT

PAOE


9/11

- 9 -

Item 30 refers to the electrochemical cell

below.

Zn(s) IZn

2

(aq)

II

Ag+ (aq) IAg(s)

30.

In the cell shown above, electrons originate

from

31.

(A)

Ag (aq)

IAg(s)

(B) Zn( s)

I

Zn (aq)

(C)

D)

Ag(aq) IAg(s)

II

Zn(s) IZn

2

(aq)

Zn(s) IZn (aq) II Ag (aq) IAg(s)

Which of the following sets of oxides is

classified rorrectly?

(A)

B)

(C)

D)

Acidic Amphoteric Basic

co,

MgO

so,

so,

Al,0

3

so,

co

P,0

10

CuO

Cao

Na,O

so,

32. Which of he following elements reacts very

slowly with cold water and burns with a

bright white flame?

(A)

B)

(C)

D)

Barium

Beryllium

Magnesium

Strontium

Items 33-34 refer to the information

in

the

following table.

Feature

(A)

(B)

(C)

(D)

State at 25 C Solid

Solid

Liquid

Gas

Bonding and Ionic

Giant

Covalent

Covalen

Structure in Oxide lattice covalent molecular

molecul

pH

of

Aqueous 10 7 0 I

Solution

33.

Match EACH oxide below with one

of

the

options (A, B, C,

or D)

above. Each option

may be used once, more than once or not at

all.

Oxide

of

silicon

34. Oxide

of

sulphur

35.

36.

Group II elements

of

the periodic table have

(A)

high melting points and

low

dens4ties

(B)

high electrical

conductivities

and

low densities

)

high melting points and high

electrical conductivities

D)

low melting points

and poor

electrical conductivities

he

high meli:ing point

of

graphite n be

attributed to the

(A) delocalised electrons

(B) hexagonal arrangement of the

carbon atoms

(C) van der Waals forces between the

layers

(D) strong covalent bonds within the

layers

.. ..

_...,

____ ____

_


10/11

- I 0 -

37.

Which of the following elements in the

third period

has

the

same

oxidation num-

ber in ALL of its known compounds?

(A)

Aluminium

(B)

Chlorine

(C)

Sulphur

(D)

Phosphorus

38. When AgNO,(aq)

is

added

to

fluoride ions

followed by NH

3

(aq) the result

is

(A)

no precipitate

(B)

white silver fluoride

C),

yellow silver fluoride

D)

cream-coloured ammonium fluoride

41.

39. In which of the following options are the

halide ions placed

in

orderof INCREASING

reducing power?

A)

Br-, Cl -, 1-

(B)

Cl-,

1-,

Br

(C)

c1-, Br,1-

D)

I-, Br-,

Cl -

40.

On heating CaSO strongly, it decomposes

into CaO and SO,(g). CaCO, decomposes

ani mucfi lower temperature than CaSO .

Which of the

following

factors

BEST

explains the greater thermal stability of

42.

CaSO,?

A)

CaC0

3

has a higher lattice energy

than

Caso,.

(B)

CO, is a smaller molecule than SO,.

C)

The o

2

- ion

is more easily

polarised than the SO, -ion.

D)

The co >- ion has a higher charge

density than the so,>- ion.

0

s

g

11 1

-

Item

41

refers

to

the graph below showing

the first ionisation energy (IE)

of

some

elements.

1000

900

800

700

600

500

400

300

200

100

0

Ca Sc

Ti

V

Cr

MnFe Co Ni Cu

Zn

Elements

The sharp increase

from

copper (Cu)

to

zinc

(Zn) is caused by filled

(A) 4s-orbitals

(B) d-orbitals

(C)

4s and

d-orbitals

(D) 4s-orbitals and half-filled d-orbitals

Item

42

refers to the information in the table

below.

Element Melting Density

Point

C)

g cm-l)

I

1538

7.86

II

660

2.70

III 328

11.34

Which of the elements in the table can be

classified as transition?

(A) I only

(B)

II only

(C)

I

and II

only

(D)

II and Ill only

ONTO11fE

NEXT

P OE


11/11

43

-

11

-

Which of the following metals gives a green

flame when heated?

A) Calcium

B) Copper

C) Magnesium

D) Sodium

Items

44 45

refer to the following options.

A) A central ion in a complex

B) A

ligand

C) An octahedral complex

D)

A tetrahedral complex

Match EACH formula below with one of he

options A, B, C or D above. Each option

may be used once, more than once,

or

not at

all.

44 [Co H,O)J>+

45. CH,NH

2

END

OF

TEST

IF

YOU FINISH BEFORE TIME IS CALLED CHECK YOUR WORK ON THIS TEST.

cape chemistry 2013 u1 p1

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