741 lines
18 KiB
Plaintext
741 lines
18 KiB
Plaintext
ÜÜÜÜÜÜÜÜÜÜÜÜÜ ÜÜÜ ÜÜÜÜ
|
|
ÜÛÛÛÛÛÛÛÛßÛßßßßßÛÛÜ ÜÜßßßßÜÜÜÜ ÜÛÜ ÜÛÛÛÛÛÛÛÛÜÜÜÜÜÛßß ßÛÛ
|
|
ßÛÛÛÛÛÛÛÛÛÛÛÛÛÛÜ ßÛÛ ÜÛÛÛÜÛÛÜÜÜ ßÛÛÛÛÜ ßÛÛÛÛÛÛÛÜÛÛÜÜÜÛÛÝ Ûß
|
|
ßßßÛÛÛÛÛÛÛÛÛÛÜ ÞÝ ÛÛÛÛÛÛÛÛÛÛÛßßÛÜÞÛÛÛ ÛÛÛÛÛÜ ßßÛÛÛÞß
|
|
Mo.iMP ÜÛÛÜ ßÛÛÛÛÛÛÛÝÛ ÞÛÛÛÛÛÛÛÛÛ ÞÛÛÛÛ ÞÛÛÛÛÛÝ ßÛß
|
|
ÜÛÛÛÛÛÛÛ ÛÛÛÛÛÛÛÛÝ ÞÛÛÛÛÛÛÛÛÝ ÛÛÛ ÛÛÛÛÛÛ
|
|
ÜÛÛÛÛÛÛÛÝ ÞÛÛÛÛÛÛÛÛ ÞÛÛÛÛÛÛÛÛ ß ÞÛÛÛÛÛÛÜ ÜÛ
|
|
ÜÛÛÛÛÛÛÛÝ ÛÛÛÛÛÛÛÛ ÛÛÛÛÛÛÛÛÝ ÞÞÛÛÛÛÛÛÛÛÛß
|
|
ÜÛßÛÛÛÛÛÛ ÜÜ ÛÛÛÛÛÛÛÛÝ ÛÛÞÛÛÛÛÛÝ ÞÛÛÛÛÛÛßß
|
|
ÜÛßÛÛÛÛÛÛÜÛÛÛÛÜÞÛÛÛÛÛÛÛÛ ÞÛ ßÛÛÛÛÛ Ü ÛÝÛÛÛÛÛ Ü
|
|
ÜÛ ÞÛÛÛÛÛÛÛÛÛÛß ÛÛÛÛÛÛÛÛÛ ßÛÜ ßÛÛÛÜÜ ÜÜÛÛÛß ÞÛ ÞÛÛÛÝ ÜÜÛÛ
|
|
ÛÛ ÛÛÛÛÛÛÛÛß ÛÛÛÛÛÛÛÛÛÛÜ ßÛÜ ßßÛÛÛÛÛÛÛÛÛß ÜÜÜß ÛÛÛÛÜÜÜÜÜÜÜÛÛÛÛÛß
|
|
ßÛÜ ÜÛÛÛß ßÛÛÛÛÛÛÛÛÛÛÜ ßßÜÜ ßßÜÛÛßß ßÛÛÜ ßßßÛßÛÛÛÛÛÛÛßß
|
|
ßßßßß ßßÛÛß ßßßßß ßßßßßßßßßßßßß
|
|
ARRoGANT CoURiERS WiTH ESSaYS
|
|
|
|
Grade Level: Type of Work Subject/Topic is on:
|
|
[ ]6-8 [ ]Class Notes [Jarvis Collegiate Chem ]
|
|
[ ]9-10 [ ]Cliff Notes [Exam ]
|
|
[x]11-12 [ ]Essay/Report [ ]
|
|
[ ]College [x]Misc [ ]
|
|
|
|
Dizzed: 10/94 # of Words:2429 School: ? State: ?
|
|
ÄÄÄÄÄÄÄÄÄ>ÄÄÄÄÄÄÄÄÄ>ÄÄÄÄÄÄÄÄÄ>Chop Here>ÄÄÄÄÄÄÄÄÄ>ÄÄÄÄÄÄÄÄÄ>ÄÄÄÄÄÄÄÄÄ>ÄÄÄÄÄÄÄÄÄ
|
|
JARVIS COLLEGIATE INSTITUTE
|
|
|
|
CHEMISTRY
|
|
|
|
|
|
Grade 12.
|
|
Time: 1 1/2 hours.
|
|
11.30 a.m. to 1:00 p.m.
|
|
Tues June 20 1989
|
|
|
|
NAME HOME FORM
|
|
|
|
Circle your teacher's name and indicate the period you take Chemistry.
|
|
|
|
|
|
|
|
Marks. Part A = ___ Part B = ___ Total Marks = ___
|
|
30 55 85
|
|
|
|
|
|
INSTRUCTIONS TO STUDENTS.
|
|
|
|
1. Answer Part A on the answer sheet at the bottom of page 5.
|
|
DO NOT detach the answer sheet.
|
|
|
|
2. There is a periodic table at the back of the exam. You may
|
|
detach this.
|
|
|
|
3. The questions in Part 1 are worth 1 mark each.
|
|
|
|
4. Answer all the questions from Part B in the given space.
|
|
|
|
|
|
|
|
Part A. Answer all questions in Part A on the answer grid at the
|
|
bottom of page 5.
|
|
|
|
|
|
1. Which of the following properties is not characteristic of metals?
|
|
|
|
a) They are dull in appearance
|
|
b) They are malleable
|
|
c) They are ductile
|
|
d) They are good conductors of heat.
|
|
|
|
|
|
2. The following is a list of the usual charge found on the ions
|
|
of a series of elements:
|
|
|
|
V3+ W2+ X+ Z2-
|
|
|
|
Which elements are likely to be metals?
|
|
|
|
a) V and W b) V, W and X.
|
|
c) X and Y d) Y and Z
|
|
|
|
|
|
3. Which of the following is not a postulate of the kinetic
|
|
molecular theory?
|
|
|
|
a) There are no attractive forces between the molecules
|
|
b) Gases consist of extremely small particles called molecules
|
|
c) Molecules of different gases have the same average velocity
|
|
at the same temperature
|
|
d) All collisions of gas molecules are perfectly elastic
|
|
|
|
|
|
4. 2.00 L of dry hydrogen gas is collected at 27.0oC and 100 kPa
|
|
pressure. The volume of this hydrogen measured at 227oC and
|
|
220 kPa pressure would be
|
|
|
|
a) 2.00 x 220 x 27 L b) 2.00 x 100 x 300 L
|
|
100 227 220 500
|
|
|
|
c) 2.00 x 220 x 300 L d) 2.00 x 100 x 500 L
|
|
100 500 220 300
|
|
|
|
5. If the temperature of a fixed mass of gas is kept constant
|
|
while the volume is decreased
|
|
|
|
a) the average kinetic energy of the particles decreases
|
|
b) the average kinetic energy of the particles increases
|
|
c) the number of collisions per second increases
|
|
d) the number of collisions per second decreases
|
|
|
|
6. The compound in the following list which is the best example
|
|
of an ionic solid at room temperature is,
|
|
|
|
a) calcium bromide (CaBr2)
|
|
b) boron trifluoride (BF3)
|
|
c) tetrachloromethane (CCl4)
|
|
d) phosphorus(V) oxide (P2O5)
|
|
|
|
|
|
7. Which one of the following items correctly indicates both the
|
|
correct electron dot (Lewis) diagram and the correct structural
|
|
(line) diagrams for the molecules illustrated.
|
|
|
|
H H
|
|
|
|
a) CH4 H C H H C H
|
|
|
|
H H
|
|
|
|
|
|
b) NH3 H N N H N H
|
|
|
|
H H
|
|
|
|
c) CO2 :O::C::O: O C O
|
|
|
|
d) H2O H O: H O
|
|
|
|
H H
|
|
|
|
|
|
8. A metal which does NOT readily liberate hydrogen gas from cold
|
|
water is
|
|
|
|
a) magnesium b) sodium
|
|
c) potassium d) calcium
|
|
|
|
|
|
|
|
9. 1.00 L of a particular gas, at STP, has a mass of 4.80 g.
|
|
Its molar mass is
|
|
|
|
a) 0.210 g b) 4.80 g
|
|
c) 108 g d) 22.4 g
|
|
|
|
|
|
10 When the skeleton equation
|
|
|
|
Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4
|
|
|
|
is balanced with the smallest whole numbers, the coefficient of
|
|
Ca(OH)2 is
|
|
|
|
a) 1 b) 2 c) 3 d) 4
|
|
|
|
11 Which of the following statements describing the
|
|
characteristics of the elements in the Periodic Table is TRUE?
|
|
|
|
a) The sequence of the elements Si, P, Cl shows increasing metallic
|
|
character.
|
|
b) The sequence of the elements Li, Na, K shows decreasing metal
|
|
character.
|
|
c) The sequence of the elements C, N, O shows decreasing atomic
|
|
radius.
|
|
d) The sequence of the elements Ti, V, Cr shows increasing
|
|
electropositivity.
|
|
|
|
12 In general the valence electrons of metals are
|
|
|
|
a) few in number and weakly held
|
|
b) few in number and strongly held
|
|
b) many in number and weakly held
|
|
d) many in number and strongly held
|
|
|
|
13 Successive ionization energies, in kJ/mol, for an unknown element
|
|
are given below.
|
|
|
|
E1 = 711 E2 = 1421 E3 = 7733 E4 = 9196
|
|
|
|
To which family of the Periodic Table does the element belong?
|
|
|
|
a) IV b) III c) II d) I
|
|
|
|
|
|
14 Benzoic acid, C6H5COOH, is a component of candle wax. It burns
|
|
according to the unbalanced equation:
|
|
|
|
C6H5COOH + O2 CO2 + H2O
|
|
|
|
When the equation is balanced for 1 mole of C6H5COOH the coefficient
|
|
for oxygen is
|
|
|
|
a) 6 1\2 b) 7 1/2 c) 8 1/2 d) 15
|
|
|
|
15 The reaction between gaseous hydrogen chloride and water is best
|
|
represented by
|
|
|
|
a) HCl(g) + H2O(l) H22+(aq) + Cl-(aq)
|
|
|
|
b) HCl(g) + H2O(l) H2(g) + HClO(aq)
|
|
|
|
c) HCl(g) + H2O(l) H+(aq) + ClO-(aq)
|
|
|
|
d) HCl(g) + H2O(l) H3O+(aq) + Cl-(aq)
|
|
|
|
|
|
16 Which of the following will form an acidic solution when
|
|
dissolved in water?
|
|
|
|
a) CO2 b) Na2O c) O2 d) H2
|
|
|
|
|
|
17 The best example of a molecular solid in which the
|
|
intermolecular bonding is only London dispersion forces is
|
|
|
|
a) potassium iodide (KI) b) carbon dioxide (CO2)
|
|
c) water (H20) d) ammonia (NH3)
|
|
|
|
|
|
18 The products formed when potassium hydroxide reacts with
|
|
sulphuric acid are
|
|
|
|
a) a salt and hydrogen b) sulphur dioxide and water
|
|
c) a metallic oxide and water d) a salt and water
|
|
|
|
|
|
19 Which one of the following groups of elements will all produce
|
|
acidic solutions when their oxides are dissolved in water?
|
|
|
|
a) Cl S Br N b) S P Ca Na
|
|
c) N Mg K Ni d) Li Mg Na Cu
|
|
|
|
|
|
20 Real gases behave most like ideal gases when
|
|
|
|
a) the pressure is high and the temperature is low
|
|
b) the pressure is low and the temperature is high
|
|
c) the pressure is low and the temperature is low
|
|
d) the pressure is high and the temperature is high
|
|
|
|
21 Equal masses of hydrogen and oxygen are placed in a sealed
|
|
container.
|
|
Which of the following statements about the system is TRUE?
|
|
|
|
a) since there are more hydrogen molecules, the mass of the hydrogen is
|
|
greater
|
|
b) since both the hydrogen and the oxygen are at the same temperature
|
|
both have the same average molecular velocity
|
|
c) since the oxygen molecule is 16 times heavier than the hydrogen
|
|
molecule, the hydrogen molecules are, on the average, moving
|
|
4 times faster than the oxygen molecules.
|
|
d) since they are both at the same temperature , both exert the same
|
|
pressure
|
|
|
|
22 2KClO3 2KCl + 3O2
|
|
|
|
How many moles of oxygen are produced during the decomposition of 8.0
|
|
mol of KClO3?
|
|
|
|
a) 5.3 b) 24 c) 48 d) 12
|
|
|
|
|
|
23 Both copper metal and sodium chloride have high melting points.
|
|
Solid copper conducts electricity well but sodium chloride will
|
|
conduct electricity only when melted or dissolved in a polar
|
|
solvent.The difference in electrical conductivity of the two
|
|
solids is best explained by the
|
|
|
|
a) stronger bonding forces between particles of NaCl than in Cu
|
|
b) greater mobility of electrons in solid Cu than in solid NaCl
|
|
c) greater number of atoms in a mole of NaCl than in a mole of Cu
|
|
d) solubility of sodium chloride in water
|
|
|
|
|
|
Questions 24, 25 and 26 refer to the following table which lists some
|
|
properties of substances
|
|
|
|
Substance . Melting . Electrical conductivity . Water
|
|
Point (oC) in solid in liquid solubility
|
|
|
|
A 776 low high high
|
|
B -198 low low low
|
|
C 961 high high low
|
|
D 1640 low low low
|
|
|
|
24 Which substance is most likely to be an ionic solid?
|
|
|
|
a) A b) B c) C d) D
|
|
|
|
25 Which substance is most likely to be a network solid
|
|
|
|
a) A b) B c) C d) D
|
|
|
|
26 Which substance is most likely to be a metal
|
|
|
|
a) A b) B c) C d) D
|
|
|
|
27 The number of moles of nitrogen gas present in 21 g of the gas is
|
|
|
|
a) 0.67 b) 0.75 c) 1.3 d) 1.5
|
|
|
|
28 The density of carbon dioxide gas (relative molecular mass 44)
|
|
at STP is
|
|
|
|
a) 0.509 g/L b) 0.986 g/L c) 1.79 g/L d) 1.96 g/L
|
|
|
|
|
|
29 The concentration of NaOH in an aqueous solution containing
|
|
4.0 g of NaOH dissolved in 100 mL of solution is
|
|
|
|
|
|
30 Scientists prefer to measure quantities per mole rather than per
|
|
gram because
|
|
|
|
a) one mole of any substance has the same mass as a mole of any other
|
|
substance
|
|
b) the gram is too small a unit to be used in the laboratory
|
|
c) a mole of any substance contains the same number of particles as a
|
|
mole of any other substance
|
|
d) a mole of any substance has the same volume as any other substance
|
|
measured at STP.
|
|
|
|
|
|
|
|
|
|
Part B. Answer all questions in this section in the blank spaces
|
|
provided.
|
|
|
|
|
|
1. Name ANY FIVE of the following compounds. (l mark each).
|
|
|
|
|
|
a) H2SO3(aq) __________________ b) (NH4)2SO4 ______________________
|
|
|
|
|
|
c) Fe(OH)3 __________________ d) Zn(CH3CO2)2 ________________
|
|
|
|
5
|
|
|
|
e) SF6 ________________________ f) Ca(ClO)2 ____________________
|
|
|
|
|
|
g) Cu(NO3)2.6H2O ___________________________________________
|
|
|
|
|
|
|
|
2. Write the formula for ANY FIVE of the following compounds.
|
|
|
|
a) lead(II) phosphate ______________
|
|
|
|
b) potassium chlorate ______________
|
|
|
|
c) tetraphosphorus heptasulphide ______________
|
|
|
|
5
|
|
d) nitrous acid ______________
|
|
|
|
e) magnesium hydrogen carbonate ______________
|
|
|
|
f) sodium periodate ______________
|
|
|
|
g) barium hydroxide octahydrate ______________
|
|
|
|
|
|
Part B is continued on page 6.
|
|
|
|
|
|
ANSWERS TO PART "A".
|
|
|
|
Answer each of the questions in Part A by writing the letter that
|
|
corresponds to the most correct answer in each case in the brackets
|
|
provided. USE CAPITAL (UPPER CASE) LETTERS ONLY.
|
|
|
|
PART A.
|
|
|
|
1 ( ) 2 ( ) 3 ( ) 4 ( ) 5 ( ) 6 ( ) 7 ( )
|
|
|
|
8 ( ) 9 ( ) 10 ( ) 11 ( ) 12 ( ) 13 ( ) 14 ( )
|
|
|
|
15 ( ) 16 ( ) 17 ( ) 18 ( ) 19 ( ) 20 ( ) 21 ( )
|
|
|
|
22 ( ) 23 ( ) 24 ( ) 25 ( ) 26 ( ) 27 ( ) 28 ( )
|
|
|
|
29 ( ) 30 ( )
|
|
|
|
|
|
.
|
|
3. Write a balanced equation to represent each of the following
|
|
reactions.
|
|
|
|
a) The formation of a precipitate when aqueous solutions of
|
|
calcium nitrate and aluminum sulphate are mixed.
|
|
|
|
3
|
|
_______________________________________________________________
|
|
|
|
|
|
b) The formation of carbon dioxide by the reaction of hydrochloric
|
|
acid on marble (calcium carbonate).
|
|
|
|
3
|
|
_______________________________________________________________
|
|
|
|
|
|
|
|
4. Draw an electron dot (Lewis) diagram for the following molecules:-
|
|
|
|
|
|
a) NF3 b) O2
|
|
|
|
|
|
|
|
4
|
|
|
|
|
|
5. Draw Lewis structures (line representation) for molecules of:-
|
|
|
|
|
|
a) Ethylene CH2CH2 b) HCN
|
|
|
|
|
|
4
|
|
|
|
|
|
|
|
|
|
PLEASE NOTE. IN QUESTIONS 6, 7 AND 8 THERE IS CHOICE.
|
|
DO ONLY THE NUMBER OF QUESTIONS ASKED FOR.
|
|
EXTRA ANSWERS WILL NOT BE MARKED SO BE SURE TO
|
|
CROSS OUT ALL BUT THE SELECTIONS YOU WISH MARKED.
|
|
|
|
|
|
6. Answer any FOUR of the following questions. (2 marks each).
|
|
|
|
|
|
a) In volumetric analysis the "Stoichiometric Point" and the "End
|
|
Point" of a titration are rarely the same. Explain why this is so.
|
|
|
|
|
|
b) How does the pH scale enable us to assess the acidity or the
|
|
basicity of an aqueous solution?
|
|
|
|
|
|
8
|
|
|
|
|
|
|
|
|
|
|
|
|
|
.
|
|
c) Equal volumes of acid A and acid B, both at the same
|
|
concentration,
|
|
were tested with a conductivity apparatus. The light bulb glowed
|
|
brightly with acid B and only dimly for acid A. Comment on the
|
|
relative strength of these two acids. Explain the observations.
|
|
|
|
|
|
|
|
|
|
|
|
d) If a bottle of ammonia was spilled in a room its odour would
|
|
eventually be detected throughout the room. Explain this
|
|
observation in terms of kinetic molecular theory.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
e) How is water, a molecular substance, able to interact with, and
|
|
dissolve, ionic solids?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
f) Explain the difference between temperature and heat.
|
|
Illustrate your answer with an everyday example.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
g) What one feature of an element is the most important in deciding
|
|
on
|
|
its placement in a "Chemical Family"? Explain how this feature
|
|
is illustrated in the "Alkali Metal" family.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
.
|
|
h) If a half filled flask of water is sealed does the process of
|
|
evaporation stop? Explain your answer.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
7. Clearly explain ANY THREE of the following statements on the
|
|
basis of
|
|
chemical and physical concepts introduced in this years' course.
|
|
(3 marks each).
|
|
|
|
a) H2O and CO2 are both triatomic molecules, however, the H2O
|
|
molecule
|
|
is highly polar whereas the CO2 molecule is not.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
b) HOCl is acidic in aqueous solution but NaOH is basic when dissolved
|
|
in water.
|
|
|
|
|
|
|
|
|
|
9
|
|
|
|
|
|
|
|
|
|
|
|
|
|
c) Adding crushed limestone (CaCO3) to lakes that have become acidified
|
|
by acid rain can raise the pH of the water.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
d) Gasoline contains a very small amount of compounds of nitrogen but
|
|
the emissions from automobile exhausts cause significant amounts of
|
|
polluting oxides of nitrogen.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
.
|
|
e) Why does the air that escapes from a car tire have a lower
|
|
temperature than the air that is still in the tire but under pressure?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
f) Substances which are not ionic are often soft and pliable.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
8. Calculate ANY FOUR of the following, showing all the steps
|
|
involved in the calculation. (2 marks each).
|
|
|
|
a) If a mixture containing 100 mL of propane (C3H8) and 1000 mL of
|
|
oxygen is ignited and returned to room temperature and pressure
|
|
what gases will remain and what volume will each gas occupy?
|
|
|
|
Equation. C3H8 + 5O2 3CO2 + 4H2O.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
b) What volume of oxygen, measured at STP, is produced by the
|
|
electrolytic decomposition of l kmol of Al2O3?
|
|
|
|
Equation. 2Al2O3 4Al + 3O2
|
|
|
|
|
|
|
|
|
|
8
|
|
|
|
|
|
|
|
|
|
c) What is the mass of 5.0 L of freon-11 (CFCl3) measured at STP?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
d) What is the concentration of KOH in mol/L if 22.44 g of KOH is
|
|
dissolved in enough water to make exactly 2 L of solution?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
e) The density of a gas is 2.41 g/L at STP what is the molecular
|
|
mass of the gas?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
f) A scuba diver's tank has a volume of about 13 L. When fully
|
|
charged with compressed air the pressure of the air in the tank
|
|
is about 150 times greater than atmospheric pressure. When the
|
|
air in the tank is released at atmospheric pressure and constant
|
|
temperature what will be the volume of the air?
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
9. A welder's tank of compressed acetylene (C2H2) contains 3000 g of
|
|
fuel.
|
|
|
|
a) Calculate the mass of oxygen required for the complete combustion of
|
|
all the acetylene in the tank given the following equation for the
|
|
reaction.
|
|
|
|
2C2H2(g) + 5O2(g) 4CO2(g) + 2H2O(g)
|
|
|
|
Clearly set out all steps in your calculation.
|
|
|
|
|
|
|
|
|
|
|
|
|
|
3
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
b) What volume of carbon dioxide will be produced at 900oC and
|
|
101.3kPa? Clearly show all steps in your calculation.
|
|
|
|
|
|
|
|
|
|
3
|
|
|