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chemistry > year 10 eoy exam > Flashcards

year 10 eoy exam Flashcards

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1
Q

describe solids in terms of the arrangement, movement, and energy of the particles

A

they are arranged in regular rows and columns, and they are very tightly packed together, they have very little energy and do not move very much (vibrate)

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2
Q

describe liquids in terms of the arrangement, movement, and energy of the particles

A

they are arranged randomly, and are still touching with some spaces between them. they have more energy than solids and the particles can move around and over each other

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3
Q

describe gasses in terms of the arrangement, movement, and energy of the particles

A

they have a lot of energy, and are randomly and widely spaced out. they can move freely

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4
Q

what is the name of the change from solid to liquid?

A

melting

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5
Q

what is the name for the change from a liquid to a gas?

A

evaporation

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6
Q

what is the name of the change from gas to solid?

A

deposition

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7
Q

what is the name of the change from a solid to a gas?

A

sublimation

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8
Q

what is the name of the change from a liquid to a solid?

A

freezing

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9
Q

what is the name for the change from a gas to a liquid?

A

condensation

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10
Q

what is a solvent?

A

the liquid in which a substance is going to be dissolved

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11
Q

what is a solute?

A

the substance that is going to be dissolved

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12
Q

what is a solution?

A

it is the mixture of a solvent and dissolved solute

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13
Q

what is a saturated solution?

A

a solution where no more solute can be dissolved

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14
Q

what is the definition of an element?

A

a substance containing only one type of atom

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15
Q

what is the definition of a compound?

A

a substance containing more than one type of atom chemically bonded together

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16
Q

what is the definition of a mixture?

A

two or more substances that are not chemically bonded

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17
Q

what is simple distillation?

A

it is a method to separate a a solvent from a solution
the solution is heated, and the solvent evaporates, and moves away and is then cooled
simple distillation works because the solvent will have a lower boiling point than the solute

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18
Q

how can you figure out if a substance is pure or not?

A

if it has a fixed boiling point, it is pure
mixtures may melt/boil over a range of temperatures

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19
Q

what is fractional distillation?

A

it is used to separation of a mixture of liquids by their boiling points
it works when the liquids have different boiling points
the liquids are vaporised and are put in the fractionating column, where they then condense at different heights/temperatures, so they can be easily separated into fractions

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20
Q

what is filtration?

A

it separates an insoluble salt (precipitation) from the salt solution
you would filter out the precipitate from the solution using filter paper

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21
Q

what is crystallisation?

A

it is used to separate a soluble salt from the solution
you heat the solution in an open container to let the solvent evaporate out, then leave it to cool. then the solid would begin to come out of the solution and crystallise.

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22
Q

what is an atom?

A

the smallest/simplest part of an element

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23
Q

what is a molecule?

A

two or more atoms that are chemically bonded

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24
Q

what is the nucleus of an atom made up of?

A

protons and neutrons

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25
Q

where are the electrons in an atom?

A

they are in the electron shells

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26
Q

what is the relative charge of sub-atomic particles?

A

proton: +1
neutron: 0
electron: -1

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27
Q

what is the relative mass of the sub-atomic particles

A

neutron: 1
proton: 1
electron: 1/2000

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28
Q

what is the atomic number?

A

the number of protons (the bottom one)

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29
Q

what is the mass number?

A

the number of protons and neutrons added together (the top one)

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30
Q

what is the number of electrons equal to?

A

the number of protons/the atomic number

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31
Q

what is an isotope?

A

atoms with the same number of protons (therefore the same element) but a different number of neutrons

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32
Q

how do you calculate the relative atomic mass from abundances?
eg. atom 1 has y neutrons 60% abundance
atom 2 has n neutrons, 40% abundance

A

(y x 60) + (n x 40)
/
100

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33
Q

how are atoms ordered in the periodic table?

A

by atomic number

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34
Q

what does the group an element is in mean?

A

the number of outer electrons

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35
Q

what does the period an element is in mean?

A

the number of electron shells

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36
Q

an atom, y has 8 electrons, what group and period is it in, and what electric configuration would it have?

A

group 6, period 2
2, 6

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37
Q

are metals able to conduct electricity?

A

yes

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38
Q

can non-metals conduct electricity?

A

no

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39
Q

what kind of oxides do metals have?

A

basic oxides

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40
Q

what kind of oxides do non-metals have?

A

acidic or neutral oxides

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41
Q

why do elements in the same group have similar chemical properties?

A

they have the same number of outer electrons so they will react and bond similarly

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42
Q

why do noble gases not react easily?

A

because they have a full outer shell so they are stable and don’t need to gain or loose any electrons

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43
Q

how do you calculate the relative formula mass (Mr) from the relative atomic mass (Ar)?

A

add the Ar of each of the elements and multiply each Ar by how many atoms of it are needed
eg. H2O= (Hx2) + (Ox1)
= (1x2) + (16x1)
= 2 + 16
= 18
so the Mr of water is 18

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44
Q

what is the unit for the amount of a substance?

A

mol

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45
Q

what is the relationship between mass, relative formula mass, number of moles?

A

mass = Mr x moles

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46
Q

how do you calculate percentage yield?

A

amount that you got divided by the total amount you could have gotten multiplied by 100

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47
Q

what is meant by the term empirical formula?

A

the simplest whole-number ratio between atoms/ions in a compound

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48
Q

what is meant by the term molecular formula?

A

the actual number of each type of element in a molecule

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49
Q

describe the method to find out the formula of a metal oxide by combustion

A
  1. measure the mass of the empty crucible and lid
  2. add a sample of magnesium into the crucible and measure the mass of it (with the lid)
  3. work out the mass of the magnesium by subtracting the mass of the empty crucible from the mass of the crucible and the magnesium
  4. put the crucible and magnesium on a tripod and gauze over a Bunsen burner and heat on a blue flame for several minutes
  5. make sure to lift the lid of the crucible while you heat it every 30 seconds/frequently to make sure the magnesium is fully oxidised
  6. after several minutes, weigh the crucible, and then heat for another minute and weigh again. if the mass has stayed the same, the magnesium has been fully oxidised, if not, continue weighing and heating until the mass stays constant
  7. measure the mass of the crucible and it’s contents. subtract the mass of the empty crucible from it to find the mass of the metal oxide formed
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50
Q

why must the lid be on when heating magnesium, to form magnesium oxide to find the formula?

A

to prevent the magnesium escaping, but the lid must be lifted frequently to let oxygen in to react with magnesium

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51
Q

how do you find the formula of magnesium oxide from the practical of combusting metal oxides to find the formula

A

find the number of moles of magnesium and oxygen:
say the mass of Mg is x and the Mr is 24, x/24=a
say the mass of O is y and the Mr is 16, y/16=b
so the ratio is a:b, Mg(a)O(b)

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52
Q

how are ions formed?

A

by electron loss or gain

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53
Q

what is the charge of metals in group 1?

A

+1 (because they loose one electron so it gets less negative/more positive)

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54
Q

what is the charge of metals in group 2?

A

+2 (because they loose 2 electrons so it gets less negative/more positive)

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55
Q

what is the charge of metals in group 3?

A

+3 (because they loose 3` electrons so it gets less negative/more positive)

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56
Q

what is the charge of non-metals in group 5?

A

-3 (because they gain 3 electrons so they get more negative/less positive)

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57
Q

what is the charge of non-metals in group 6?

A

-2 (because they gain 2 electrons so they get more negative/less positive)

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58
Q

what is the charge of non-metals in group 7?

A

-1 (because they gain 1 electrons so they get more negative/less positive)

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59
Q

what is the charge of Ag (silver)?

A

+1

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60
Q

what is the charge of Cu (copper)?

A

+2

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61
Q

what is the charge of Fe (iron)?

A

+2 or +3

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62
Q

what is the charge of Pb (lead)?

A

+2

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63
Q

what is the charge of Zn (zinc)?

A

+2

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64
Q

what is the charge of hydrogen?

A

+1

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65
Q

what is the charge of hydroxide?

A

-1

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66
Q

what is the charge of ammonium?

A

+1

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67
Q

what is the charge of carbonate?

A

-2

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68
Q

what is the charge of nitrate?

A

-1

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69
Q

what is the charge of sulphate?

A

-2

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70
Q

what is the formula of hydroxide?

A

OH-1

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71
Q

what is the formula of ammonium?

A

NH4+1

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72
Q

what is the formula of carbonate?

A

CO₃-2

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73
Q

what is the formula for nitrate?

A

NO₃-1

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74
Q

what is the formula for sulphate?

A

SO4-2

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75
Q

what is the charge of ammonia?

A

nothing, it is not an ion and therefore has no charge

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76
Q

what is the formula for ammonia?

A

NH3

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77
Q

what is an ionic bond in terms of electrostatic bond?

A

strong electrostatic attraction between positive and negative ions

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78
Q

why do compounds with giant ionic lattices have high melting points?

A

the strong electrostatic attraction requires a lot of energy to overcome

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79
Q

can ionic compounds conduct electricity as a solid, and why?

A

no, because the ions are not free to move

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80
Q

can ionic compounds conduct electricity when aqueous or molten, and why?

A

yes, because the ions are free to move

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81
Q

what is a covalent bond?

A

strong electrostatic attraction between a pair of shared electrons and the positive nuclei

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82
Q

why do simple covalent structures have low melting/boiling points?

A

because the weak intermolecular forces require little energy to overcome

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83
Q

why does the melting/boiling point of simple molecular forces increase with increasing relative molecular mass (generally)?

A

because the bigger the molecule, the stronger the intermolecular forces

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84
Q

describe how you would represent metallic lattices with a 2d diagram

A

when metal atoms join together, the outer electrons become delocalised
metals have a giant regular arrangement of layers of positive ions surrounded by a sea of delocalised electrons

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85
Q

what is metallic bonding?

A

the strong electrostatic attraction between positive metal ions and delocalised electrons

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86
Q

what are the typical physical properties of metals?

A

they are good conductors of heat and electricity
they are malleable
they have a high melting point

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87
Q

what is the trend in physical properties in group 1 metals?

A

they get lighter and softer, get dull more quickly (going down the group)

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88
Q

what happens when lithium reacts with water?

A

fizzing, moves about, gas produced

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89
Q

what happens when sodium reacts with water?

A

it turns into a sphere, exothermic reaction, moves quicker than lithium, fizzes more than lithium

90
Q

what happens when potassium reacts with water?

A

burns with a lilac flame, reacts quicker than sodium, bangs at the end

91
Q

what happens when rubidium reacts with water?

A

explodes as soon as it touches the water

92
Q

what happens when caesium reacts with water?

A

breaks tub of water due to explosion

93
Q

what happens to the reactivity going down the group 1 metals?

A

the reactivity increases

94
Q

why does the reactivity increase going down group 1 metals?

A
  • they all need to lose one electron
  • number of electron shells increases going down the group
  • outer electron gets further away from nucleus
  • attraction between nucleus and electron decrease
  • therefore it is easier to remove
95
Q

what is the colour and state of fluorine at room temperature?

A

pale yellow gas

96
Q

what colour and state is chlorine at room temperature?

A

pale green gas

97
Q

what is the colour and state of bromine at room temperature?

A

red/brown liquid

98
Q

what is the colour and state of iodine at room temperature?

A

grey solid

99
Q

what colour and state is astatine at room temperature?

A

black solid

100
Q

what happens when fluorine is reacted with iron wool?

A

too reactive to find out

101
Q

what happens when chlorine is reacted with iron wool?

A

slight heating causes a violent reaction

102
Q

what happens when bromine is reacted with iron wool?

A

strong heating causes a visible reaction

103
Q

what happens when iodine is reacted with iron wool?

A

very strong heating for a few minutes causes a slight reaction

104
Q

what happens when astatine is reacted with iron wool?

A

even less reaction than iodine

105
Q

what is the trend in reactivity going down group seven?

A

the reactivity decreases

106
Q

why does the reactivity decrease going down group seven?

A
  • they all need to gain one electron
  • number of shells increases going down the group
  • incoming electron is further away from the nucleus
  • weaker attraction between electron and nucleus
  • harder to gain electrons
107
Q

what percentage of nitrogen is in dry air?

A

78%

108
Q

what percentage of oxygen is in dry air?

A

21%

109
Q

what percentage of argon is in dry air?

A

0.8%

110
Q

what percentage of carbon dioxide is in dry air?

A

0.04%

111
Q

what happens when magnesium reacts with oxygen?

A

bright white light + white powder formed

112
Q

what happens when hydrogen reacts with oxygen?

A

causes explosive reaction (squeaky pop test)

113
Q

what happens when sulphur reacts with oxygen?

A

produces a blue flame

114
Q

what happens when copper carbonate is heated (thermal decomposition)

A

copper carbonate –> carbon dioxide + copper oxide
(CuCO3 –> CuO + CO2)

115
Q

what is the order of reactivity for metals (most reactive -> least reactive)?

A

potassium
sodium
lithium
calcium
magnesium
aluminium
carbon
zinc
iron
lead
hydrogen
copper
mercury
silver
gold
platinum

116
Q

under which conditions does iron rust?

A

when both water and oxygen are present

117
Q

what is the barrier method?

A

preventing oxygen and water from reaching the iron by covering the iron in something else (eg. plastic, oil)

118
Q

what is galvanising?

A

it is when iron is covered in zinc to prevent rusting. the zinc acts as a barrier and prevents oxygen and water reaching the iron but even if it is broken, zinc is more reactive than iron so it still wont rust

119
Q

what is sacrificial protection?

A

it is when the iron is coated in something more reactive as the oxygen will react with that first and not the iron

120
Q

what is oxidation?

A

the loss of electrons or the gain of oxygen

121
Q

what is reduction?

A

the gain of electrons or the loss of oxygen

122
Q

what is an oxidising agent?

A

something that gives oxygen, or takes electrons (something that has been reduced)

123
Q

what is a reducing agent?

A

something that takes oxygen or gives electrons (something that has been oxidised)

124
Q

how are metals more reactive than carbon extracted?

A

electrolysis (breaking down compound using electricity)

125
Q

how are metals less reactive than carbon extracted?

A

reacted with carbon - displacement reaction

126
Q

what metals do not need extraction?

A

mercury and silver (might need purifying though)
gold and platinum

127
Q

what is the use of aluminium?

A
  • it is used for cables, some cars (because it’s light), planes, pots, and pans
  • it is useful because of it’s lack of corrosion, it’s low density, it’s strength when alloyed, and it is a good conductor of heat and electricity
  • it doesn’t corrode because it forms aluminium oxide on the surface
128
Q

what is mild steel made of?

A

iron and up to 0.25% carbon

129
Q

what are the uses of mild steel?

A
  • nails, car bodies, ships, and bridges
  • mild carbon is strong, hard, malleable, and ductile
  • it rusts when exposed to oxygen and water
130
Q

what is high-carbon steel made up of?

A

iron, 0.6-1.2% carbon, and small amounts of manganese

131
Q

what are the uses of high-carbon steel?

A
  • it is used for cutting tools and masonry nails
  • it is harder and more than resistant than mild steel, but also more brittle
132
Q

what is stainless steel made of?

A

iron, chromium, and usually nickel

133
Q

what are the uses of stainless steel?

A
  • it is used in kitchen sinks, sauce pans, knives and forks, and gardening tools
  • it is also used in brewing, dairy, and chemical industries
  • it is resistant to corrosion
134
Q

what are the uses of copper?

A

it is used in electrical wires, pots and pans, surfaces in hospitals, and water pipes
- it is a good conductor of heat and electricity, it is unreactive, malleable, and has anti-microbial properties

135
Q

what is an alloy?

A

a mixture of a metal and one or more elements

136
Q

why are alloys harder than pure metals?

A

in an alloy, the elements have slightly differently sized elements, which breaks up the normal lattice arrangement and prevents the layers sliding over eachother

137
Q

what is the test for hydrogen/

A

the squeaky pop test; put a lit splint in the gas, and if it makes a squeaky pop, hydrogen is present

138
Q

what is the test for oxygen?

A

put a glowing splint in the gas, if it relights, oxygen is present

139
Q

what is the tests for carbon dioxide?

A

bubble the gas into lime water, if it goes cloudy, carbon dioxide is present

140
Q

what is the test for chlorine?

A

use damp blue litmus paper, if chlorine is present it will go white

141
Q

what is the test for chloride ions?

A

add nitric acid to remove impurities, then add silver nitrate solution. if chloride ions are present, it will form a white precipitate of silver chloride

142
Q

what is the test for bromide ions?

A

add nitric acid to remove impurities, then add silver nitrate solution. if bromide is present, it will form a cream precipitate of silver bromide

143
Q

what is the test for iodide ions?

A

add nitric acid to remove impurities, then add silver nitrate solution. if iodide ions are present, it will form a yellow precipitate of silver iodide

144
Q

how do you test for sulphate ions?

A

add hydrochloric acid to remove impurities, then add barium chloride solution. if sulphate ions are present, a white precipitate of barium sulphate will form

145
Q

how do you test for carbonate ions?

A

use hydrochloric acid, if it fizzes, carbonate ions are present

146
Q

what is a chemical test for water?

A

use anhydrous copper sulphate. if it turns from white to blue, water is present

147
Q

what is a physical test for pure water?

A

it will boil at 100 degrees celcius

148
Q

what can be used to distinguish acidic and alkaline solutions?

A

universal indicator, red and blue litmus paper, methyl orange, phenolphthalein

149
Q

what colour is methyl orange in acids?

A

red

150
Q

what colour is methyl orange in neutrals?

A

yellow

151
Q

what colour is methyl orange in alkalis?

A

yellow

152
Q

what colour is phenolphthalein in acids?

A

colourless

153
Q

what colour is phenolphthalein in neutrals?

A

colourless

154
Q

what colour is phenolphthalein in alkalis?

A

pink

155
Q

what colour is universal indicator in acids?

A

red

156
Q

what colour is universal indicator in neutrals?

A

green

157
Q

what colour is universal indicator in alkalis?

A

blue/purple

158
Q

what colour is blue litmus in acids?

A

red

159
Q

what colour is blue litmus in neutrals?

A

blue

160
Q

what colour is blue litmus in alkalis?

A

blue

161
Q

what colour is red litmus in acids?

A

red

162
Q

what colour is red litmus in neutrals?

A

red

163
Q

what colour is red litmus in acids?

A

red

164
Q

what is the pH of a strongly acidic substance?

A

0-3

165
Q

what is the pH of a weakly acidic substance?

A

4-6

166
Q

what is the pH of a neutral substance?

A

7

167
Q

what is the pH of a weakly alkaline solution?

A

8-10

168
Q

what is the pH of a strongly alkaline solution?

A

11-14

169
Q

what are acids in an aqueous solution a source of?

A

hydrogen ions

170
Q

what are alkalis in an aqueous solution a source of?

A

hydroxide ions

171
Q

can alkalis neutralise acids?

A

yes

172
Q

are common sodium, potassium, and ammonium compounds soluble?

A

yes

173
Q

are nitrates soluble?

A

yes

174
Q

are common chlorides soluble (except from silver and lead II)?

A

yes

175
Q

are silver chlorides soluble?

A

no

176
Q

are lead (II) chlorides soluble?

A

no

177
Q

are common carbonates soluble (except for those of sodium, potassium and aluminium)?

A

no

178
Q

is sodium carbonate soluble?

A

yes

179
Q

is potassium carbonate soluble?

A

yes

180
Q

is aluminium carbonate soluble?

A

yes

181
Q

are common sulphates soluble (except for those of barium, calcium, and lead (II))?

A

yes

182
Q

is barium sulphate soluble?

A

no

183
Q

is calcium sulphate soluble?

A

no

184
Q

is lead (II) sulphate soluble?

A

no

185
Q

are common hydroxides soluble (other than those of sodium, potassium, and calcium)?

A

no

186
Q

is sodium hydroxide soluble?

A

yes

187
Q

is potassium hydroxide soluble?

A

yes

188
Q

is calcium hydroxide soluble?

A

slightly

189
Q

what is an acid in terms of proton transfer?

A

acids are proton (H+) donors

190
Q

what are bases in terms of proton transfer?

A

bases are proton (H+) acceptors

191
Q

what happens when an alkali is reacted with an acid?

A

alkali + acid –> water + salt

192
Q

what happens when a base is reacted with an acid?

A

base + acid –> water + salt

193
Q

what happens when a carbonate is reacted with an acid?

A

carbonate + acid –> water + salt + carbon dioxide

194
Q

what happens when a metal is reacted with an acid (excluding nitric acid)?

A

metal + acid –> salt + hydrogen

195
Q

what are alkalis in terms of bases?

A

soluble bases

196
Q

what can act as bases?

A

metal oxides, metal hydroxides, ammonia

197
Q

describe an experiment to prepare a pure dry sample of a soluble salt from an insoluble reactant

A
  • add excess insoluble base to the acid
  • filter to react the unreacted base
  • heat the solution so water evaporates and crystals remain
198
Q

describe an experiment to prepare a pure dry sample of a soluble salt from an acid and an alkali

A
  • use titration to find the exact volume of alkali that reacts with the acid
  • mix the exact volumes of the acid and base
  • warm solution so water evaporates and crystals remain
199
Q

describe an experiment to prepare a pure, dry sample of an insoluble salt from two soluble reactants

A
  • mix solutions of two soluble reactants
  • filter mixture (insoluble salt will remain on the paper)
  • wash salt with distilled water
  • leave salt to dry
200
Q

how do you prepare pure dry copper sulphate crystals from copper (II) oxide?

A
  1. heat the sulphuric acid
  2. add copper oxide until no more disappears (while stirring continuously)
  3. filter out the excess base
  4. transfer solution into evaporating dish
  5. heat until crystals start to form
  6. leave to crystallise for a few days
  7. filter or pick out crystals
  8. pat dry with filter paper
201
Q

how do you prepare pure, dry lead (II) sulphate crystals?

A
  1. mix the aqueous lead (II) nitrate solution and the aqueous potassium sulphate solution together
  2. filter out sat precipitate
  3. rinse with distilled water
  4. dry salt by patting with filter paper
202
Q

how does temperature effect the rate of reaction?

A

rate of reaction increases with increasing temperature. the particles have more kinetic energy so the collide at the required activation energy more often, so there are more successful collisions per unit time

203
Q

how does surface area effect rate of reaction?

A

increasing surface area increases the rate of reaction. more of the reactant is exposed, so there are more frequent collisions, so there are more successful collisions per unit time

204
Q

how does concentration effect the rate of reaction?

A

increasing concentration increases the rate of reaction. there are more particles in the same volume, so there are more frequent collisions, so there are more successful collisions per unit time

205
Q

how does pressure effect rate of reaction?

A

increasing pressure increases rate of reaction because there are the same number of particles in a smaller volume, so there are more frequent collisions, so there are more successful collisions per unit time

206
Q

how do catalysts effect the rate of reaction?

A

catalysts increase the rate of reaction by providing an alternative route with a lower activation energy, so there are more successful collisions per unit time

207
Q

what are catalysts?

A

they are substances that increases the rate of reaction, but remain chemically unchanged at the end of the reaction

208
Q

what is the method to investigate how surface area of a solid effects the rate of reaction?

A
  1. measure out 3g of marble chips into a conical flask
  2. set up a delivery tube and inverted 50cm3 measuring cylinder full of water in a trough
  3. measure out 20m3 of hydrochloric acid with a measuring cylinder
  4. add the hydrochloric acid to the conical flask, fit the bung, and start the timer
  5. measure and record the volume of carbon dioxide in the measuring cylinder every 5 seconds
  6. stop either when the measuring cylinder is full or after 60 seconds (whichever is sooner)
  7. repeat with two different sizes of marble chips
209
Q

what is the method to investigate the effects of different catalysts on the decomposition of hydrogen peroxide?

A
  1. using a measuring cylinder, measure out 50cm3 of hydrogen peroxide into a conical flask
  2. connect the gas syringe to the bung using a delivery tube. make sure the syringe is close (its on zero)
  3. measure out 0.5g of the first catalyst being tested eg. manganese (IV) oxide
  4. add the manganese (IV) oxide to the conical flask and immediately attach the bung to it. start the timer
  5. measure the amount of gas in the syringe every 10 seconds. stop timing after 60 seconds
  6. repeat 1-5 for platinum, iron (V) oxide, and vanadium (V) oxide
210
Q

what is a hydrocarbon?

A

a compound containing hydrogen and carbon only

211
Q

what is crude oil?

A

a mixture of hydrocarbons

212
Q

how is crude oil separated into fractions?

A

it is vaporised then it enters the fractioning column, where it rises and the temperature falls. different fractions condense at different times, so they are separated

213
Q

what are the names of the fractions of crude oil in order of increasing boiling point?

A

refinery gasses, gasoline, kerosene, diesel, fuel oil, bitumen

214
Q

what is the trend in colour of the fractions of crude oil?

A

gets darker going down

215
Q

what is the trend in viscosity in the fractions of crude oil?

A

increases going down

216
Q

what is a fuel?

A

a substance that, when burned, releases heat energy

217
Q

what are the uses of refinery gasses?

A

fuel for heating and cooking

218
Q

what are the uses of gasoline?

A

fuel for cars (NOT VANS)

219
Q

what are the uses of kerosene?

A

fuel for planes

220
Q

what are the uses of diesel?

A

fuel for lorries/trains (NOT VANS)

221
Q

what are the uses of fuel oil?

A

fuel for boats (NOT SHIPS)

222
Q

what is the use for bitumen?

A

making roads

chemistry (5 decks)

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