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Exam Qs Flashcards

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1
Q

State why sewage and phosphates in river water is harmful (2)

A

sewage: contains microbes which cause disease (1)
phosphates: deoxygenation of water (1)

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2
Q

Describe how the general physical properties of a liquid differ from those of a solid.
Give two differences.

A

solid has a definite shape / solid has a fixed shape / liquid has no definite shape / liquid takes the shape of its container (1)
solid does not flow (over a surface easily) / liquid flows (easily over a surface) / solid does not spread out (over a
surface) / liquid spreads out (over a surface) (1)

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3
Q

State one source of the pollutant sulfur dioxide in the air other than from burning sulfur

A

combustion of fossil fuels (containing sulfur)

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4
Q

the chemical name of SiO2

A

Silicon (IV) oxide

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5
Q

State what is meant by the term covalent bond

A

pair of electrons shared between two atoms

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6
Q

Name a halide compound which can be used to detect the presence of water

A

Anhydrous cobalt (II) chloride

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7
Q

In the equation, methanoic acid is represented by the formula HCOOH.
Name this type of formula.

A

Structural

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8
Q

When but-1-ene reacts with steam, two possible products form. Identify the type of catalyst which is used in this reaction

A

Acid

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8
Q

State what is meant by the term closed system

A

nothing can enter or leave

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9
Q

Two possible products when but-1-ene reacts with steam

A

But-1-ol, but-2-ol

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10
Q

Name and describe the bonding in potassium (4)

A

metallic (1)
lattice of potassium ions (1)
sea of electrons (1)
attraction between potassium ions and electrons (1)

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11
Q

Temperature and pressure used in Haber process

A

450 degrees celsius
200 atm

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12
Q

Which element in period 2 has the highest rate of diffusion?

A

Neon

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13
Q

Which element in period 2 has the oxide responsible for acid rain?

A

Nitrogen

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14
Q

Explain, in terms of particles, what happens to the rate of reaction when the temperature is
reduced

A

M1 rate decreases and particles have less energy (1)
M2 less collisions (between particles) occur per second / per unit time (1)
M3 less of the particles/collisions have energy equal to or above the activation energy (1)

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15
Q

Two observations in the reaction of calcium chloride and nitric acid

A
  • effervescence
  • solid dissolves/disappears
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16
Q

Suggest what is meant by the term saturated solution

A

a solution that can contain no more solute at a given temperature

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17
Q

Write the chemical equation for the reaction when solid sodium nitrate is heated (decomposition)

A

2NaNO3 -> 2NaNO2 + O2

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18
Q

Bromine colour at room temp and bromine water colour

A

bromine by itself at room temp is red-brown but bromine water is orange

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19
Q

Describe the arrangement of atoms in graphite (2)

A

M1 layers
M2 hexagon(al) (rings of carbon)

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20
Q

Describe the process which converts metal ores to sulfur dioxide

A

strong heating in air / roasting in air

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21
Q

Suggest the name for a solution in which no more solute can dissolve

A

saturated

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22
Q

Suggest why more crystals of magnesium sulfate appear on cooling

A

solubility (of MgSO4 / solid) decreases (as temperature decreases)

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23
Q

Write the chemical equation for the reaction when solid magnesium nitrate is heated (2)

A

2Mg(NO3)2 → 2MgO + 4NO2 + O2

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24
Q

Give two reasons why the electrolysis is carried out on aluminium oxide dissolved in
molten cryolite instead of electrolysing molten aluminium oxide only

A

M1 improves conductivity of the electrolyte / makes the electrolyte a better conductor (1)
M2 lower operating temperature (1)

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25
Q

State what is meant by the term amphoteric

A

neutralises both acids AND alkalis

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26
Q

Name the black solid that is produced when concentrated sulfuric acid is added to sugar,
C12H22O11.

A

Carbon

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27
Q

Observations when solid copper(II) carbonate is added to aqueous potassium hydrogensulfate

A
  • solid disappears
  • blue solution
  • bubbles / effervescence / fizzing
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28
Q

Name the type of reaction in which proteins are broken down into amino acids

A

Hydrolysis

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29
Q

State the percentage of nitrogen in clean, dry air

A

78%

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30
Q

Name the substance used to remove sulfur dioxide in flue gas desulfurisation

A

calcium oxide

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31
Q

Nitrogen dioxide, NO2, is formed in car engines.
Name the equipment in a car exhaust used to remove the NO2 formed in car engines

A

catalytic converter

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32
Q

State one adverse effect of carbon monoxide on human health

A

toxic

33
Q

State what is meant by the symbol ∆H

A

enthalpy change

33
Q

State one use of ammonium sulfate

A

fertiliser

33
Q

Atm to kPa

A

1atm=100kPa

34
Q

Some physical and chemical properties of transition elements are shown.
physical properties:
● high density
● high strength
chemical properties:
● form coloured compounds
● have ions with variable oxidation numbers
(i) State one other physical property of transition elements.
(ii) State one other chemical property of transition elements.

A

i) high melting point
ii) act as catalyst

35
Q

State the meaning of the Roman numeral (II) in the name copper(II) oxide

A

the oxidation number of copper is +2

36
Q

Propanoic acid forms an ester when it reacts with ethanol in the presence of a catalyst.
(i) Suggest a suitable catalyst

A

Acid or any named inorganic acid (phosphoric acid)

37
Q

Which oxide is a reducing agent in the blast furnace?

A

Carbon monoxide

38
Q

Why does group VII have the same chemical properties?

A

Because they have the same number of valence electrons

39
Q

Describe two methods where sulfur dioxide is obtained

A
  1. Sulfur burned in air
  2. Roasting sulfide ores in air
40
Q

Silicon tetrachloride has a low melting point because it has weak forces of attraction
between particles.
Name the type of particles that are held together by these weak forces of attraction

A

Molecules

41
Q

Explain, in terms of structure and bonding, why silicon(IV) oxide has a high melting point

A

M1 covalent bonds
M2 strong bonds
and
giant (covalent) structure

42
Q

Explain, in terms of collision theory, why the rate of reaction increases if powdered zinc is used rather than lumps

A

M1 greater surface area (of zinc)
M2 frequency of collisions between (zinc and acid) particles increases

43
Q

State what is meant by the term electrolyte

A

M1 ionic compound
M2 molten and / or aqueous

44
Q

The electrolysis of aqueous copper(II) sulfate is repeated using copper electrodes.
State what happens to the anode

A

Anode dissolves

45
Q

State one disadvantage, other than cost, of using hydrogen–oxygen fuel cells to power
cars compared to using petro

A

needs high pressure to store hydrogen

46
Q

The first stage is the conversion of ammonia into nitrogen monoxide, NO.
The equation is shown.
4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)
The reaction is carried out at a temperature of 900°C and a pressure of 7 atm.
The forward reaction is exothermic.
Using explanations that do not involve cost:
● explain why a temperature less than 900°C is not used
● explain why a pressure greater than 7 atm is not used

A

temperature change:
M1 low(er) rate (of reaction)
pressure change:
M2 (position of) equilibrium shifts to the left hand side/ towards reactants

47
Q

A student makes aqueous copper(II) nitrate by adding an excess of solid copper(II) carbonate
to dilute nitric acid.
(ii) State two observations that indicate the copper(II) carbonate is in excess.

A

M1 undissolved solid
M2 effervescence stops on addition of more copper(II) carbonate

48
Q

Name one compound, other than copper(II) carbonate, that can be added to dilute
nitric acid to produce aqueous copper(II) nitrate

A

Copper oxide
Copper hydroxide

49
Q

addition polymer formed from but-2-ene

A
  • Single bond between 2 carbon atoms
  • 1 CH3 group and 1H on first carbon and same on second carbon
50
Q

two reasons why coke is added to the blast furnace

A
  • coke produces heat
  • reducing agent to reduce iron (III) oxide
51
Q

Explain how limestone removes impurities in the hematite

A

limestone thermally decomposes to form calcium oxide. Calcium oxide reacts with silicon (IV) oxide to produce slag

52
Q

Write a symbol equation for the conversion of iron (III) oxide to iron in the blast furnace

A

Fe2O3 + 3CO -> 2Fe + 3CO2

53
Q

Suggest why iron produced in the blast furnace is molten

A

Temperature in the furnace is higher than the melting point of iron

54
Q

Explain why the structure of alloys causes them to be stronger and harder than pure metals

A

M1 atoms have different sizes (1)
M2 layers cannot slide over or past each other (1)

55
Q

Substances that react with iron to form rust

A

oxygen and water

56
Q

Explain how the coating of zinc prevents rusting if the zinc is not scratched

A

Zinc acts as a barrier which prevents oxygen and water reaching the iron

57
Q

When zinc is scratched it is still protecting the iron, explain how

A

M1 zinc is more reactive than iron (1)
M2 zinc is oxidised / zinc loses electrons / zinc forms positive ions / forms zinc ions (1)

58
Q

Hydrated cobalt chloride formula

A

CoCl2.6H2O

59
Q

Name starting materials added to the blast furnace

A

limestone, coke, hot air, iron ore

60
Q

Reaction of calcium oxide and silicon oxide in blast furnace

A

Neutralisation reaction
CaO + SiO2 -> CaSiO3

61
Q

What is mixed with iron other than carbon to make stainless steel

A

Nicket/chromium

62
Q

Chemical name of rust

A

hydrated iron (III) oxide

63
Q

Methods of preventing rust that aren’t galvanising

A

Painting, greasing, coating with plastic

64
Q

Steps that student should take in preparing a pure sample of lead (II) chloride from the mixture in the beaker

A
  • Filter the precipitate
  • Wash the residue with distilled water
  • Dry the residue in between filter papers
65
Q

Explain the apparent unreactivity of aluminium

A

M1 aluminium oxide layer (1)
M2 (oxide layer) is unreactive (1)

66
Q

Explain in terms of thermal energy how greenhouse gases cause global warming (3)

A

M1 greenhouse gases absorb thermal energy (from the Earth) (1)
M2 and M3 one mark each for any two of:
* energy (from the sun) absorbed by Earth’s surface
* Earth emits or reflects thermal energy
* (greenhouse gases) reduces or stops thermal energy loss (into space)
* increasing in amount of greenhouse gas results in a higher atmospheric temperature

67
Q

Two conditions needed for fermentation of aqueous glucose

A
  1. absence of oxygen
  2. presence of yeast
68
Q

Typical temperature and pressure used for addition of steam to ethene

A

Temperature: 300
Pressure: 60 atm (6000 kPa)

69
Q

State the meaning of weak in weak acid

A

partially disassociate

70
Q

Name the oxidising agent for ethanol to ethanoic acid

A

acidified potassium manganate (VII)

71
Q

Name the process for ethene to ethanol

A

catalytic addition

72
Q

Explain in terms of structure and bonding why graphite has a much higher melting point
than carbon monoxide

A

M1 graphite has a giant covalent structure
M2 attraction between molecules in carbon monoxide
M3 weaker attraction (between particles) in carbon monoxide ORA

73
Q

State what is meant by the term electrolysis

A

M1 breakdown by (the passage of) electricity
M2 of an ionic compound in molten or aqueous (state)

74
Q

Write an ionic half-equation for the production of oxygen at the anode

A

4OH– → 2H2O + O2 + 4e–

75
Q

To make soluble salt react dilute acid and insoluble base (carbonate, oxide, hydroxide)

A
76
Q

State why the student keeps heating until mass is constant

A

To ensure all water is given off

77
Q

Explain, in terms of electrons, why magnesium is used for sacrificial protection for steel

A

M1 magnesium loses electrons more readily than / in preference to / instead of iron
M2 magnesium is more reactive than iron ORA

78
Q

Alkenes are produced by cracking alkanes.
When C12H26 is cracked, the products are ethene and an alkane which form in a 2:1 mole ratio.
Write a symbol equation for this reaction

A

C12H26 -> 2C2H4 + C8H18

79
Q
A

Chemistry IG (14 decks)

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