Science 10H Review
1.
Lab Safety.
a)
What is the WHMIS symbol for a flammable substance?
b)
What is the household symbol which means "the contents of the container are flammable"?
c)
What is the symbol for a radioactive substance?
d)
What are the three WHMIS symbols which warn of poisons, and what is the difference between
them?
Class D, Division 1 - Poisonous and infectious material. Acute toxin; immediate and serious
toxic effects.
Class D, Division 2 - Poisonous and infectious material. Chronic toxin; other toxic effects;
may cause cancer or other diseases because of long term exposure.
Class D, Division 3 - Poisonous and infectious material. Biohazard; may cause infections and
other effects
2.
Metric System
a)
List all prefixes, base units and derived units, along with their values.
See tables in your notes.
b)
How many g are there in 0.62 kg ?
0.62 kg x
c)
How many L are there in 145 mL ?
145 mL x
d)
1000 g = 620 g
1 kg
1L
= 0.145 L
1000 mL
How many nm are there in 2.11 x 10-6 km ?
2.11 x 10-6 km x
e)
= 2.11 x 106 nm
How many m3 in 14 km3 ?
14 km3 x
f)
1012 nm
1 km
(1000 m)3 = 1.4 x 1010 m3
(1 km)3
The speed of light is 3.00 x 108 m/s. How far will light travel in 12 days ?
3.00 x 108 m x 60 s x 60 min x 24 h x 12 d = 3.11 x 1014 m
s
min
h
d
g)
An oil tanker ran aground and spilled its cargo of 240 000 barrels of oil. If a barrel of oil
contains 42 gallons and a gallon contains 4.0 L, how many litres will the spill contain ? If the oil
spreads into a slick 1 mm thick, what will be the area of the oil slick in square kilometres ?
2.4 x 105 barrels x 42 gal x 4.0 L = 4.0 x 107 L of oil
barrel
gal
4.00 x 107 L x 1000 mL = 4.00 x 1010 mL = 4.00 x 1010 cm3
1L
4.00 x 1010 cm3 x (10 mm)3 = 4.00 x 1013 mm3
(1 cm)3
Area = volume = 4.00 x 1013 mm3 = 4 x 1013 mm2
thickness
1 mm
4 x 1013 mm2 x
(1 km)2
(106 mm)2
= 40 km2
h)
The annual production of sodium hydroxide in the United States in 1999 was 23.2 billion
pounds.
i)
How many grams of sodium hydroxide were produced in that year?
23.2 billion pounds = 2.32 x 1010 lb. x
1.05 x 1010 kg NaOH x
ii)
103 g
1 kg
= 1.05 x 1010 kg NaOH
= 1.05 x 1013 g NaOH
The density of sodium hydroxide is 2.130 g/cm 3. How may cubic kilometers were
produced?
1.05 x 1013 g NaOH x
i)
1 kg
2.2046 lb
1 cm3
2.130 g
x
(1 km)3
(105 cm)3
= 4.94 x 10-3 km3
A quarter has a mass of 5.67 g and is approximately 1.55 mm thick.
i)
How many quarters would have to be stacked to reach the height of the Peace Tower
in Ottawa, 92.0 m?
1 quarter
1.55 mm
ii)
x
103 mm
1 m
How much would the stack weigh?
5.94 x 104 quarters x
iii)
5.67 g
1 quarter
= 3.37 x 105 g
How much money would the stack contain?
5.94 x 104 quarters x
iv)
x 92.0 m = 5.94 x 104 quarters
$1.00
4 quarters
= $1.48 x 104 ($14 800)
The Canadian total debt is about 4 trillion dollars. How many of these stacks of
quarters would be required to pay this debt?
$4 trillion = $4 x 1012 x
1 stack
$1.48 x 104
= 3 x 108 stacks of quarters
(300 million)
3.
Significant Digits
a)
b)
4.
Perform the following additions and subtractions:
i)
22.26 g + 19.1 g
41.4 g
iv)
2500 L - 155 L
2300 L
ii)
100.1 L + 0.025 L
100.1 L
v)
1.236 mol - 0.33 mol
0.91 mol
iii)
8.21 mL + 2.79 mL
11.00 mL
vi)
19 mol - 18.75 mol
0 mol
Perform the following multiplications and divisions
i)
233 g / 15.36 g/mol
15.2 mol
iv)
13.1 mol x 44.01 g/mol
577 g
ii)
1.59 mol / 0.12 L
13 mol/L
v)
22 L x 2.145 mol/L
47 mol
iii)
16 g x (1 kg / 1000 g)
0.016 kg
vi)
100 g / 18.02 g/mol
5 mol
Graphing
a)
Make a graph of the following data. Use graph paper and include all the components of a good
graph. Put volume on the x-axis. Draw a best-fit line. Calculate the slope. What does the
slope of this line represent? Identify the element of which these blocks were made.
volume of a block (cm3) mass of the block (g)
2.0
5.5
4.0
10.7
6.0
16.2
8.0
21.5
10.0
26.8
15.0
40.5
25.0
68.0
b)
Make a graph of the following data. Use graph paper and include all the components of a good
graph. Put distance on the x-axis. Draw a best-fit line.
distance from planet (km) Gravity (N)
0
9.8
100
9.5
150
9.4
200
9.2
300
8.9
500
8.4
1000
7.3
5000
3.1
10000
1.5
c)
Measurements were taken of small cylinders of an unknown metal:
Radius of Circular End (mm)
Length (cm)
4.0
4.0
4.0
4.6
4.6
4.6
i)
1.55
2.65
4.00
3.15
4.50
5.80
Mass (g)
15.06
25.75
38.87
40.47
57.82
74.52
Calculate the volume of each cylinder.
Volume is equal to the area of the end of the cylinder multiplied by the length:
V = lπr2
Radius (mm)
Length (cm)
4.0
4.0
4.0
4.6
4.6
4.6
ii)
Volume (cm3)
1.55
2.65
4.00
3.15
4.50
5.80
0.80
1.3
2.0
2.1
3.0
3.9
Mass (g)
15.06
25.75
38.87
40.47
57.82
74.52
Make a graph with volume on the x-axis.
See end of file
iii)
Calculate the slope of the line.
Slope = rise =
run
iv)
y2 - y1 = 74.52 g - 15.06 g
x2 - x1
3.9 cm3 - 0.8 cm3
= 19.2 g/cm3 (20 g/cm3)
What is the significance of the slope of the graph ? Can you identify the metal ?
The units of grams per cubic centimeter are the units of density, a characteristic
physical property. This density corresponds to that of gold.
5.
Nomenclature
a)
Give the formulas for the following substances:
i)
ii)
iii)
iv)
v)
magnesium hydroxide
sodium hydrogen carbonate
aluminum oxide
calcium oxide hexahydrate
phosphorus pentaoxide
Mg(OH)2
NaHCO3
Al2O3
CaO · 6 H2O
PO5
vi)
vii)
viii)
ix)
x)
iron (III) phosphate
lime
ethanol
nitric acid
lead (II) sulfate
FePO4
CaO
C2H5OH
HNO3
Pb(SO4)2
b)
c)
Give the name for the following compounds:
i) NaCl
sodium chloride
ii) NH3
ammonia
iii) CaSO4
calcium sulfate
iv) N2O4
dinitrogen tetraoxide
v) NaH
sodium hydride
vi) Ca(OH)2 ·5 H2O
calcium hydroxide pentahydrate
vii) MnO2
manganese (IV) oxide
viii) CO2
carbon dioxide
ix) NH4NO3
ammonium nitrate
x) CH3COOH
acetic acid
Draw the structures for the following:
i)
propane
v)
2-methyl-3-heptene
ii)
phenol
vii)
1,1-dichloro-2-methyl-3-pentanol
iii)
2-butyne
viii)
1,2-difluoro-3,3-diiodocyclohexane
7
iv)
ethyl propanoate
ix)
butanamide
v)
diethyl ether
x)
pentanoic acid
H
d)
H
H
C
C
H
H
H H
O
C
C H
H H
propene
1-fluoro-3-chloropentane
1-hexadecyne
butylamine
1,1,2-trifluoro-1,2,2-trichloroethane
1-hexyn-6-ol
4-heptanol
3,4-dimethyl-2-pentene
propanone
ethanal
2-chloro-4-fluorocyclohexene
toluene
8
6.
Atomic Theory
a)
Describe the nature and role of the proton, neutron, and electron in the atom.
Proton
Neutron
Electron
Location
in the nucleus.
Cannot leave
in the nucleus.
Cannot leave
in orbit about
nucleus. Can be
added to or taken
away from atom
Charge
positive (1+)
neutral (0)
negative (1-)
Mass
large
equal to proton
insignificant
Role in the Atom
- number of protons
determines atomic
number.
- gives the identity of
the atom
- with protons
determines the mass
number of the atom;
determines the
isotope
- mediates strong
nuclear force; holds
nucleus together
- with protons
determines atomic
charge
- responsible for
chemical and physical
properties of an
element.
b)
List the diatomic elements, as well as the two other polyatomic elements.
H2 N2 O2 F2 Cl2 Br2 I2 At2 S8 P4
c)
Determine the number of protons and electrons in the following:
(i) Ca2+
20 protons, 18 electrons
(ii) Ar
18 protons, 18 electrons
(iii) P3-
15 protons, 18 electrons
(iv) Mn6+
25 protons, 19 electrons
d)
9
Make a table that gives the name, the complete symbol (including atomic number, mass
number and charge), number of protons, neutrons and electrons, mass number, atomic number
and charge for each of the following:
(i)
(ii)
(iii)
(iv)
(v)
(vi)
(vii)
(viii)
Name
Calcium
20 protons, 20 neutrons, 18 electrons
33 protons, 40 neutrons, 36 electrons
atomic number 52, mass number 128, charge 2atomic number 23, mass number 51, charge 5+
mass number 137, 54 electrons, charge 2+
mass number 227, 86 electrons, charge 3+
atomic number 79, mass number 196, charge 0
atomic number 25, mass number 55, 18 electrons
Symbol
40
Ca2+
# Protons
# Electrons
# Neutrons
Atomic
Number
20
Charge
20
Mass
Number
40
20
18
33
36
40
73
33
3-
52
54
76
128
52
2-
23
18
28
51
23
5+
56
54
81
137
56
2+
89
86
138
227
89
3+
79
79
117
196
79
0
25
18
30
55
25
7+
2+
20
Arsenic
73
As3-
33
Tellurium
Vanadium
128
Te2-
52
51 5+
V
23
Barium
137
Ba2+
56
Actinium
227
Ac3+
89
196
Gold
Au
79
Manganese
55
Mn7+
25
e)
Write the symbols for the following atoms or ions; indicate the type of ion:
i) 13 protons, 10 electrons
ii) 80 protons, 78 electrons
f)
Al3+
Hg2+
iii) 54 protons, 54 electrons
iv) 34 protons, 36 electrons
Determine the number of protons and neutrons in the following:
i)
238
U
92
(ii)
14
C
(iii)
6
i)
92 protons, 146 neutrons
ii)
6 protons, 8 neutrons
iii)
10 protons, 11 neutrons
iv)
25 protons, 22 neutrons
21
Ne
10
(iv)
47
Ti
25
Xe
Se2-
10
g)
Given the following data calculate the average atomic mass of silver:
Isotope
Mass(amu)
Abundance (%)
Ag-107
Ag-109
106.90509
108.90476
51.840
48.160
Ave. Mass = (51.840%/100)(106.90509 amu) + (48.160%/100)(108.90476 amu)
= 107.87 amu
h)
Given the following data calculate the abundance of each isotope of boron:
Isotope
Mass (amu)
Abundance (%)
B-10
B-11
10.0129
11.0093
20.00
80.00
Average mass of boron is 10.81 amu
10.81 amu = (x)(10.0129 amu) + (1 - x)(11.0093 amu)
7.
x
Heat
= 0.2000
Following is a list of the specific heats of several materials
Aluminum
Copper
Ethylene glycol
Gold
Ice
Iron
a)
0.13
0.98
2.50
0.92
2.10
0.80
Silver
Water
Water vapour
Zinc
0.24
4.18
1.87
0.39
to
to
to
to
heat 150 g of water from 14°C to 36°C
cool 16 kg of sand from 45°C to 4.0°C
increase the temperature of 351 g of gold 101°C
decrease the temperature of 89 g paraffin oil 55°C
1.4 x 104 J
- 5.2 x 105 J
4600 J
1.0 x 104 J
Calculate the temperature change:
i)
ii)
iii)
c)
Lead
Magnesium
Methanol
Oxygen
Paraffin oil
Sand
Calculate the amount of energy, in Joules, required for the following:
i)
ii)
iii)
iv)
b)
0.90
0.39
2.20
0.13
2.06
0.45
(in J/g·°C):
if 4.5 kg of aluminum receives 780 J of energy
if 335 g of iron receives 16 kJ of energy
if 78.5 kg of silver loses 14.1 kJ of energy
0.19 °C
110 °C
- 0.75 °C
Calculate the mass:
i)
ii)
if 560 J of energy causes the temperature of copper to rise 67°C
21 g
if a loss of 7 kJ of energy causes the temperature of lead to go from 246°C to 182°C
800 g
11
Following is a list of heats of fusion and vapourization of several substances:
Heat of fusion (J/g)
water
methanol
ethanol
hexane
toluene
d)
2260
1076
855
335
363
Calculate the heat required:
i)
ii)
iii)
iv)
e)
333
100
109
152
72
Heat of vapourization (J/g)
to
to
to
to
melt 678 g of hexane
freeze 8.1 kg of methanol
boil 780 g of ethanol
condense 224 kg of toluene
1.03 x 105 J
- 8.10 x 105 J
6.7 x 105 J
- 8.13 x 107 J
Calculate the heat required:
i)
to change 569 g of ice at -35.0°C to steam at 172°C
Heat ice:
Melt ice:
Heat water:
Boil water:
Heat steam:
(2.06 J/g °C)(569 g)(0 °C - (-35.0 °C))
(333 J/g)(569 g)
(4.18 J/g °C)(569 g)(100 °C - 0 °C)
(2260 J/g)(569 g)
(1.87 J/g °C)(569 g)(172 °C - 100 °C)
4.10 x 104 J
1.89 x 105 J
2.38 x 105 J
1.29 x 106 J
7.7 x 104 J
= 1.84 x 106 J
Total:
ii)
=
=
=
=
=
to change 3.55 kg of water at 45°C to ice at -15°C
3.55 kg x 1000 g = 3550 g
1 kg
Cool water:
Freeze water:
Cool ice:
Total:
(4.18 J/g °C)(3550 g)(0 °C - 45 °C)
(-333 J/g)(3550 g)
(2.06 J/g °C)(3550 g)((-15 °C) - 0 °C)
= - 6.7 x 105 J
= - 1.18 x 106 J
= - 1.1 x 105 J
= 1.96 x 106 J
12
8.
Light
Speed of light = wavelength x frequency
c = λν
Energy of light = Planck’s constant x frequency E = hν
i.
4.50 x 10-7 m
6.1 x 10-7 m
2.11 x 10-12 m
1.6 x 10-5 m
(6.67 x 1014 Hz, blue)
(4.9 x 1014 s-1, orange)
(1.42 x 1020 1/s , gamma rays)
(1.9 x 1013 Hz, infrared)
(4.42 x 10-19 J)
(3.3 x 10-19 J)
(9.42 x 10-14 J)
(1.2 x 10-20 J)
Calculate the wavelength of each of the following frequencies, and indicate the ‘colour’
of the light:
a)
b)
c)
d)
iii.
h = 6.626 x 10-34 J·s
Calculate the frequency of each of the following wavelengths of light, and indicate the
‘colour’ of the light:
a)
b)
c)
d)
ii.
c = 3.00 x 108 m/s
4.44 x 1014 Hz
7.4 x 1014 s-1
9.3 x 1016 1/s
3.66 x 1015 Hz
(6.76 x 10-7 m, red)
(4.1 x 10-7 m, violet)
(3.2 x 10-9 m, x-rays)
(8.19 x 10-8 m, ultraviolet)
Calculate the energies of each of the waves of light from questions 1 & 2
(2.94 x 10-19 J)
(4.9 x 10-19 J)
(6.2 x 10-17 J)
(2.42 x 10-18 J)
13
Mass of an Unknown Metal as a Function of Volume
80
3.9, 74.52
70
60
3, 57.82
Mass (g)
50
2.1, 40.47
2, 38.87
40
30
1.3, 25.75
20
0.8, 15.06
10
0
0
0.5
1
1.5
2
2.5
Volume (cm3)
3
3.5
4
4.5
14
6.
Sustainability
a)
Can humans occupy more than 1 trophic level ? Explain.
Yes. As omnivores we are first consumers when we eat plant matter. We are second order
consumers when we eat cows, pigs or chickens. We eat carnivores when we eat fish.
b)
From the list below identify the producers, herbivores, carnivores, omnivores and detritovores.
frog
cow
garter snake
aphid
mouse
house fly
earth worm
c)
algae
pig
gopher
honey bee
beaver
spider
bacteria
hawk
grass
grasshopper
rabbit
wheatgrass
dung beetle
fox
grass
wheatgrass
wild oats
honey bee
beaver
grasshopper
Producer:
algae
Herbivore:
cow
aphid
squirrel
Carnivore:
frog
Omnivore:
house fly
earth worm
pig
Detritovore:
bacteria
dung beetle
bread mold
garter snake
spider hawk
fox
gopher
Make a food web using at least 16 species from the list above.
deer
squirrel
lady bug
coyote
wild oats
bread mold
owl
rabbit
deer
lady bug coyote
owl
15
d)
Why are there more herbivores than top carnivores ?
Energy is lost at each trophic level. Roughly 90% of the energy from one trophic level does not
make it up to the next level because animals use most of their energy to fuel daily metabolic
processes. Therefore there has to be at least 10x as many organisms at one level to support
the animals above.
e)
What are factors that affect the carrying capacity of any environment ?
Materials and energy
Food chains (see d))
Competition
Density
16
f)
If all humans became herbivores, discuss the impact on the environment. Include energy
transfer in your discussion.
More energy would be available for human populations or for organisms we share the planet
with. We would not raise animals for food, so land could be left wild. The oceans would not be
harvested so marine and aquatic ecosystems would be left intact. Other ideas are also valid.
g)
Discuss succession.
Any new environment will quickly be populated by pioneer species that can get by with little in
the way of soil or nutrients. This is called primary succession. They act to collect some of
these factors so that other species can be supported and so new species appear over the
course of time. Finally a climax community is established. These species will remain intact
until some event occurs to disturb it (fire, flood). Secondary succession will begin to reestablish
the climax community.
h)
What factors can you (or your family) control which would reduce the size of your ecological
footprint ? What factors are out of your control ?
In your control:
size of house
number, size, and age of cars
amount of driving
number and age of clothes
amount of “stuff”
water use
etc
Not in your control:
actions of city, province and federal governments
actions of industry
actions of agriculture
actions of friends and neighbors
(all can be affected by getting involved in community and political
action)
17
7.
Weather
Following is a list of the specific heats of several materials
Aluminum
Copper
Ethylene glycol
Gold
Ice
Iron
a)
0.13
0.98
2.50
0.92
2.10
0.80
Silver
Water
Water vapour
Zinc
0.24
4.18
1.87
0.39
to
to
to
to
heat 150 g of water from 14°C to 36°C
cool 16 kg of sand from 45°C to 4.0°C
increase the temperature of 351 g of gold 101°C
decrease the temperature of 89 g paraffin oil 55°C
1.4 x 104 J
- 5.2 x 105 J
4600 J
1.0 x 104 J
Calculate the temperature change:
i)
ii)
iii)
c)
Lead
Magnesium
Methanol
Oxygen
Paraffin oil
Sand
Calculate the amount of energy, in Joules, required for the following:
i)
ii)
iii)
iv)
b)
0.90
0.39
2.20
0.13
2.06
0.45
(in J/g·°C):
if 4.5 kg of aluminum receives 780 J of energy
if 335 g of iron receives 16 kJ of energy
if 78.5 kg of silver loses 14.1 kJ of energy
0.19 °C
110 °C
- 0.75 °C
Calculate the mass:
i)
ii)
if 560 J of energy causes the temperature of copper to rise 67°C
21 g
if a loss of 7 kJ of energy causes the temperature of lead to go from 246°C to 182°C
800 g
Following is a list of heats of fusion and vapourization of several substances:
Heat of fusion (J/g)
water
methanol
ethanol
hexane
toluene
d)
333
100
109
152
72
Heat of vapourization (J/g)
2260
1076
855
335
363
Calculate the heat required:
i)
ii)
iii)
iv)
to
to
to
to
melt 678 g of hexane
freeze 8.1 kg of methanol
boil 780 g of ethanol
condense 224 kg of toluene
1.03 x 105 J
- 8.10 x 105 J
6.7 x 105 J
- 8.13 x 107 J
18
e)
Calculate the heat required:
i)
to change 569 g of ice at -35.0°C to steam at 172°C
Heat ice:
Melt ice:
Heat water:
Boil water:
Heat steam:
(2.06 J/g °C)(569 g)(0 °C - (-35.0 °C))
(333 J/g)(569 g)
(4.18 J/g °C)(569 g)(100 °C - 0 °C)
(2260 J/g)(569 g)
(1.87 J/g °C)(569 g)(172 °C - 100 °C)
Total:
ii)
=
=
=
=
=
4.10 x 104 J
1.89 x 105 J
2.38 x 105 J
1.29 x 106 J
7.7 x 104 J
= 1.84 x 106 J
to change 3.55 kg of water at 45°C to ice at -15°C
3.55 kg x 1000 g = 3550 g
1 kg
Cool water:
Freeze water:
Cool ice:
Total:
f)
(4.18 J/g °C)(3550 g)(0 °C - 45 °C)
(-333 J/g)(3550 g)
(2.06 J/g °C)(3550 g)((-15 °C) - 0 °C)
= - 6.7 x 105 J
= - 1.18 x 106 J
= - 1.1 x 105 J
= 1.96 x 106 J
Contrast conduction, convection and radiation. How do they affect the energy budget of the
Earth ?
Conduction:
Convection:
Radiation:
the transfer of energy directly from atoms with more energy to atoms with less.
energy is transferred by the motion of atoms from one place to another.
energy is transferred via electromagnetic waves.
The Earth receives energy from the sun primarily via radiation. This energy is distributed to the
air, earth and water. In the atmosphere the energy is transferred via convection, but
conduction and radiation are important because atoms come into contact and heat is radiated
from one atom to another. This heat drives convection and causes weather. The oceans also
convect heat through currents, carrying heat from the equator to the poles. Land receives
energy via radiation and conduction, but solids do not convect heat.
The energy of the sun drives all weather, air currents and ocean currents. We receive radiation
in a variety of forms and transform energy into a variety of forms, but generally the Earth
radiates this energy back out into space. We radiate out as much energy as we receive each
day.
g)
Make a graph of the data found in table 13.4 on page 431 of your text. Put temperature on the
x-axis.
See end of file.
19
h)
i)
Why is it cooler at the poles than at the equator ?
The poles are at a greater angle to the sun’s rays than the equator; the sunlight is more
diffuse.
Because of the tilt of Earth’s axis the poles receive fewer hours of sunlight over much of the
year.
Snow cover increases albedo; more energy is reradiated back out into space than occurs at the
equator.
20
j)
Describe the wind patterns on the globe. Why do they occur as they do ?
See text, page 466. These patterns occur because the Earth is a large rotating sphere which
causes the north-south circulation of the atmosphere to form a fairly complicated pattern.
k)
Discuss the coriolis effect. Use it to be able to predict the prevailing wind direction at any given
latitude.
See text, pages 462 to 466.
l)
What is a characteristic physical property ? What such properties have we dealt with in class
this term ?
This is a property that can be used to identify a substance.
Melting temperature
Density
m)
Boiling temperature
Specific heat
Light
Speed of light = wavelength x frequency
c = λν
Energy of light = Planck’s constant x frequency E = hν
c = 3.00 x 108 m/s
h = 6.626 x 10-34 J·s
i.
Calculate the frequency of each of the following wavelengths of light, and indicate the
‘colour’ of the light:
a)
b)
c)
d)
4.50 x 10-7 m
6.1 x 10-7 m
2.11 x 10-12 m
1.6 x 10-5 m
ii.
Calculate the wavelength of each of the following frequencies, and indicate the ‘colour’
of the light:
a)
b)
c)
d)
4.44 x 1014 Hz
7.4 x 1014 s-1
9.3 x 1016 1/s
3.66 x 1015 Hz
iii.
Calculate the energies of each of the waves of light from questions 1 & 2
(6.67 x 1014 Hz, blue)
(4.9 x 1014 s-1, orange)
(1.42 x 1020 1/s , gamma rays)
(1.9 x 1013 Hz, infrared)
(6.76 x 10-7 m, red)
(4.1 x 10-7 m, violet)
(3.2 x 10-9 m, x-rays)
(8.19 x 10-8 m, ultraviolet)
(4.42 x 10-19 J)
(3.3 x 10-19 J)
(9.42 x 10-14 J)
(1.2 x 10-20 J)
(2.94 x 10-19 J)
(4.9 x 10-19 J)
(6.2 x 10-17 J)
(2.42 x 10-18 J)
21
Relationship Between Temperaure and Humidity
60
Mass of Water Vapour (g) in 1.0 kg of Air
50
40
30
20
10
0
-30
-20
-10
0
10
Temperature (degrees C)
20
30
40
50
22
Mass of an Unknown Metal as a Function of Volume
80
3.9, 74.52
70
60
3, 57.82
Mass (g)
50
2.1, 40.47
2, 38.87
40
30
1.3, 25.75
20
0.8, 15.06
10
0
0
0.5
1
1.5
2
2.5
Volume (cm3)
3
3.5
4
4.5