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Plume Academy Chemistry Paper 2 H June 2022

Total questions: 131

Worksheet time: 1hrs 20mins

Name
Class
Date
1.
What method can NOT be used to collect gas?
a)
Using a gas syringe
b)
Collecting it in a measuring cylinder under water
c)
Measuring the change in mass
d)
Seeing how quickly the solution goes cloudy
2.
What does NOT happen when the temperature is increased?
a)
Particles collide more often
b)
Particles collide with more energy
c)
Particles move faster
d)
More particles collide in the correct orientation
3.
How can you increase the rate of a reaction
a)
Decrease the pressure
b)
Increase the rate of collisions
c)
Decrease the concentration
d)
Increase the concentration
4.
What is the disadvantage of using some metal catalysts
a)
expensive
b)
difficult to extract
c)
heavy
d)
toxic
5.

List four factors that affects the rate of a reaction

a)

temperature

b)

concentration

c)

surface area

d)

volume

e)

catalysts

6.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

7.
The following graph shows two different reaction pathways for the same overall reaction at the same temperature. Which pathway is slower and why?
a)
Red, because the activation energy is larger
b)
Blue, because the activation energy is lower
c)
both reaction progress at the same rate
8.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

9.

The ______________is required to break the bonds of the reactants.

a)

Carbonic energy

b)

Activation energy

c)

Plutonic energy

d)

Energi Gaib

10.
Located on the left side of the reaction
a)
reactants
b)
products
11.

The minimum amount of energy needed for colliding particles to react is called

a)

Chemical Energy

b)

Kinetic Energy

c)

Activation Energy

d)

Potential Energy

12.
Grinding a seltzer tablet into powder increases the rate of reaction due to increased
a)
concentration
b)
surface area
c)
temperature
d)
reactants
13.
B represents
a)
energy absorbed
b)
energy released
c)
activation energy
14.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
15.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
16.
Identify where the reaction has finished
a)
A
b)
B
c)
C
d)
D
17.
Identify the part of the graph with the fastest rate of reaction.
a)
A
b)
B
c)
C
d)
D
18.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
19.
You observe bubbles after adding metal to a solution. Do you assume a chemical reaction took place?
a)
Yes
b)
No
20.
Two clear and colorless solutions are combined within a test tube. The result is very cloudy. Do you assume a chemical reaction took place?
a)
Yes
b)
No
21.
Two clear and colorless solutions are combined within a test tube. The resulting solution is purple. Do you assume a chemical reaction took place?
a)
Yes
b)
No
22.
Metal is added to a solution in a test tube. The test tube now feels cooler. Do you assume a chemical reaction took place?
a)
Yes
b)
No
23.

How can rate of reaction be measured in reactions?

a)

Measure mass lost when gas produced.

b)

Measure volume of gas produced.

c)

Measure colour change or formation of a solid.

d)

Measure time taken for liquid to disappear.

24.

Look at the graph. At what time does the reaction finish?

a)

4 minutes

b)

5 minutes

c)

6 minutes

d)

7 minutes

25.

Look at the graph. Use the tangent to the curve to work out the rate of reaction.

a)

0.5

b)

1

c)

1.5

d)

2

26.

The same mass of smaller marble chips would...

a)

React faster as they have a smaller surface area to volume ratio.

b)

React more slowly as they have a smaller surface area to volume ratio.

c)

React faster as they have a larger surface area to volume ratio.

d)

React more slowly as they have a larger surface area to volume ratio.

27.

A student investigates the rate of reaction between zinc and excess dilute hydrochloric acid.

The table shows his results. What is the rate of the reaction?

a)

8.2

b)

8.4

c)

21

d)

84

28.

The decomposition of hydrogen peroxide is catalysed by adding a small amount of manganese (IV) oxide. Which of the graphs below shows the mass of the catalyst as the reaction takes place?

a)

A

b)

B

c)

C

d)

D

29.

Zinc reacts with dilute hydrochloric acid to produce zinc chloride and hydrogen.

When zinc powder is used, instead of larger pieces of zinc, the reaction is faster. Why is this?

a)

The activation energy is lower so a greater proportion of reactions are successful.

b)

The particles have more energy so move around faster and collide more frequently.

c)

Greater surface area means particles collide more frequently.

d)

More particles are in a given volume so the activation energy decreases.

30.

A student carries out an experiment to measure accurately the temperature changes when different metals are added to iron(II) sulfate solution. State a suitable container to measure the iron(II) sulfate solution in this experiment.

a)

Beaker

b)

Measuring cylinder

c)

Spatula

d)

Mass balance

31.

As the temperature of a reaction is increased, the rate of the reaction increases because the...

a)

...reactant molecules collide less frequently.

b)

...reactant molecules collide more frequently and with greater energy per collision.

c)

...activation energy is lowered.

d)

...reactant molecules collide less frequently and with greater energy per collision.

32.

Of the following, which will lower the activation energy for a reaction?

a)

Increasing the concentrations of reactants.

b)

Raising the temperature of the reaction.

c)

Adding a catalyst for the reaction.

d)

Removing products as the reaction proceeds.

33.

Which of the following would NOT increase the rate of reaction?

a)

Raising the temperature.

b)

Adding a catalyst.

c)

Increasing the concentration of the reactants.

d)

Increasing the volume of the container.

34.

What would the rate be if 10g of product are produced in 20 seconds?

a)

5 g/s

b)

0.5 g/s

c)

1.5 g/s

d)

2 g/s

35.

What is represented by label X?

a)

Activation energy with a catalyst

b)

Activation energy without a catalyst

c)

Overall energy change with a catalyst

d)

Overall energy change without a catalyst

36.

The student used the 50 cm3 line on the conical flask to measure the volume of hydrochloric acid. Suggest a piece of equipment the student could use to make the measurement of volume more accurate.

a)

Measuring cylinder

b)

Beaker

c)

Test-tube

37.

The balance used to weigh 10.0 g of calcium carbonate lumps caused an error.

The balance always read 0.2 g before being used.

What type of error was caused by the balance?

a)

Human error

b)

Random error

c)

Systematic error

38.

The large cube of calcium carbonate was divided into eight smaller cubes.

The eight smaller cubes have a greater total surface area than the one large cube. The rate of reaction of the eight smaller cubes is ____________

a)

Faster

b)

Slower

c)

The same

39.

A nickel catalyst is used in this reaction.

Why is a catalyst used in this reaction?

Choose TWO answers.

a)

To increase the temperature

b)

To produce less carbon monoxide

c)

To reduce costs

d)

To use less energy

e)

To use less methane

40.

Student A investigated the effect of the particle size of a manganese dioxide catalyst on the rate of the reaction.

This is the method used.

1. Measure 25 cm3 hydrogen peroxide solution into a conical flask.

2. Add some fine manganese dioxide powder to the conical flask.

3. Measure the volume of oxygen produced every 30 seconds for 10 minutes.

4. Repeat steps 1 to 3 two more times.

5. Repeat steps 1 to 4 with coarse manganese dioxide lumps.

The method student A used did not give repeatable results.

How could student A make the results repeatable?

a)

Student A should make measurements every 2 minutes.

b)

Student A should measure the mass of manganese dioxide.

c)

Student A should use 50 cm3 hydrogen peroxide.

d)

Student A should use a beaker instead of a conical flask.

41.

Student B used a method which gave repeatable results. How could student B improve the accuracy of these results?

a)

Calculate a mean but do not include any anomalous results.

b)

Calculate a mean but do not include the first set of results.

c)

Record the results in a table and plot the results on a bar chart.

d)

Record the results in a table and plot the results on a line graph.

42.

Hydrogen peroxide molecules collide with manganese dioxide particles during the reaction.

Why does fine manganese dioxide powder produce a higher rate of reaction than coarse manganese dioxide lumps?

a)

Fine manganese dioxide powder has a larger surface area.

b)

Fine manganese dioxide powder has larger particles.

c)

Fine manganese dioxide powder produces less frequent collisions.

43.

The student concludes that the rate of reaction is greater when the concentration of hydrochloric acid is higher.

Why is the rate of reaction greater when the concentration of hydrochloric acid is higher?

Choose two answers.

a)

The particles are moving faster

b)

The particles have more energy

c)

The surface area of magnesium is smaller

d)

There are more particle collisions each second

e)

There are more particles in the same volume

44.

Plates are made from ceramics, paper or poly(propene).

Paper plates are biodegradable and recyclable.

Which stage of a life cycle assessment (LCA) would contain this information?

a)

Disposal at the end of useful life

b)

Extracting and processing raw materials

c)

Manufacturing and packaging

d)

Use and operation during lifetime

45.

Which two processes are used to make ceramic plates?

a)

Forming a composite

b)

Galvanising with zinc

c)

Heating in a furnace

d)

Melting sand and boron trioxide

e)

Shaping wet clay

46.

Poly(propene) is produced from an alkene.

The name for very large molecules such as poly(propene) is...

(a)  

47.

Poly(propene) is produced from an alkene.

The name of the alkene used to produce poly(propene) is

(a)  

48.

The alkene needed to make poly(propene) is produced from crude oil.

Which two processes are used to produce this alkene from crude oil?

a)

Chromatograpy

b)

Cracking

c)

Fermentation

d)

Fractional distillation

e)

Quarrying

49.

What type of bond joins the atoms in a molecule of poly(propene)?

a)

Covalent

b)

Ionic

c)

Metallic

50.

The table below shows information about two polymers used to make plates.  What type of polymer is polymer A?

a)

Thermosetting

b)

Thermosoftening

51.

The table below shows information about two polymers used to make plates.  What type of polymer is polymer B?

a)

Thermosetting

b)

Thermosoftening

52.

 Why does polymer A behave differently to polymer B when heated?

a)

A contains cross links

b)

B contains cross links

53.

Which two gases are present in smaller percentages on the Earth than on Titan?

a)

Nitrogen

b)

Oxygen

c)

Methane

d)

Argon

e)

Carbon dioxide

54.

Why are algae less likely to photosynthesise on Titan than Earth?

a)

Titan’s atmosphere contains too little argon.

b)

Titan’s atmosphere contains too little carbon dioxide.

c)

Titan’s atmosphere contains too little methane.

d)

Titan’s atmosphere contains too little nitrogen.

55.

As well as methane, the atmosphere of Titan contains small amounts of propene gas. Methane is an alkane and propene is an alkene. Bromine water is an orange solution used to identify alkenes.

What effect does methane have on bromine water?

a)

Forms a blue solution

b)

Forms a colourless solution

c)

Forms a green solution

d)

Forms a white precipitate

e)

No effect

56.

As well as methane, the atmosphere of Titan contains small amounts of propene gas. Methane is an alkane and propene is an alkene. Bromine water is an orange solution used to identify alkenes.

What effect does propene have on bromine water?

a)

Forms a blue solution

b)

Forms a colourless solution

c)

Forms a green solution

d)

Forms a white precipitate

e)

No effect

57.

Octane (C8H18) is a hydrocarbon in petrol. Cracking breaks down large hydrocarbon molecules into smaller hydrocarbon molecules.

Which hydrocarbon molecule can be cracked to produce octane, C8H18?

a)

C4H8

b)

C4H10

c)

C8H16

d)

C12H26

58.

What type of carbon compound is octane, C8H18?

a)

Alcohol

b)

Alkane

c)

Carboxylic acid

d)

Ester

59.

Particulates and sulfur dioxide are pollutants produced when some fuels burn. Give the polluting effect of the pollutant.

Pollutant: Particulates

a)

Acid rain

b)

Global dimming

c)

Global warming

d)

Landfill

e)

Sewage sludge

60.

Particulates and sulfur dioxide are pollutants produced when some fuels burn. Give the polluting effect of the pollutant.

Pollutant: Sulfur dioxide

a)

Acid rain

b)

Global dimming

c)

Global warming

d)

Landfill

e)

Sewage sludge

61.

Which two gases are produced when fuels burn in car engines?

a)

Ammonia

b)

Carbon dioxide

c)

Carbon monoxide

d)

Nitrogen

e)

Oxygen

62.

Vehicles produce most of the atmospheric pollution in cities.

How could the atmospheric pollution in cities be reduced? Choose two.

a)

Build more roads in cities

b)

Build new car factories

c)

Develop fuel efficient engines

d)

Make car tax cheaper

e)

Use electric cars

63.

Addition polymers are made from small alkene molecules.

Which type of bonding is present in small alkene molecules?

a)

Covalent

b)

Ionic

c)

Metallic

64.

What is the functional group in these small alkene molecules?

a)
b)
c)
65.

What is the functional group in a carboxylic acid?

a)
b)
c)
66.

What is the functional group in an alcohol?

a)
b)
c)
67.

The figure shows the structure of part of an addition polymer surfboard.

The outer surface of the surfboard is coated.

The coating is made from soda-lime glass fibres surrounded by a plastic.

 What type of material is the coating of the surfboard?

a)

Alloy

b)

Ceramic

c)

Composite

d)

Nanotube

68.

The materials used to make the soda-lime glass fibres are sodium carbonate, _____________________ and _____________________. Choose two.

a)

Air

b)

Ammonia

c)

Copper

d)

Limestone

e)

Sand

69.

Which alcohol in the table is liquid over the greatest temperature range?

a)

Methanol

b)

Ethanol

c)

Propanol

d)

Butanol

70.

Which statement is correct?

a)

A molecule of ethanol has 5 hydrogen atoms

b)

Butanol has the highest boiling point

c)

Methanol has the largest molecules

d)

Propanol has the highest melting point

71.

Complete the word equation for the reaction to produce ethanol.

______________________   +   ______________________  →  ethanol

a)

1. Ethene

b)

1. ethanoic acid

c)

2. Water

d)

2. Ethanoic acid

72.

What is the name of the reaction to produce ethanol from sugar?

a)

Fermentation

b)

Polymerisation

c)

Reduction

73.

Complete the word equation for the combustion of hydrogen.

hydrogen          +          oxygen          →           (a)  

74.

Which arrow, A, B or C, shows the activation energy?

 

a)

A

b)

B

c)

C

75.

What type of reaction is shown by the energy level diagram?

 

a)

Exothermic

b)

Endothermic

76.

For a reaction, the value of A is 1370 kJ and C is 3230 kJ. Calculate the value of B.

(do not add units and do not add a + or - sign)

(a)  

77.

A group of students investigated the amount of energy released when different alcohols are burned.

Give a use of alcohols.

a)

Fuels

b)

Fertilisers

c)

Cleaning products

78.

Choose the start temperature and the final temperature of the water.

a)

Start:

23.5

b)

Start:

22.5

c)

Final:

39.3

d)

Final:

38.7

79.

Work out the increase in temperature.

(a)  

80.

Which value of heat energy released is anomalous?

a)

20.1

b)

11.4

c)

13.5

d)

16.8

e)

17.2

81.

What is the functional group of the alcohol?

a)

–– C –– C

b)

–– C –– H

c)

–– O –– H

82.

Name this alcohol.

a)

Butanol

b)

Ethanol

c)

Propanol

83.

Ethanol burns in air. Complete the word equation for the reaction.

ethanol     +     _______________     -->     carbon dioxide     +     water

a)

carbon

b)

hydrogen

c)

oxygen

84.

Ethanoic acid is in ______________________________ .

a)

milk

b)

hard water

c)

vinegar

85.

Ethanoic acid is a carboxylic acid.

Which diagram, A, B or C, has a ring around the functional group of a carboxylic acid?

a)

A

b)

B

c)

C

86.

Ethyl propanoate is produced by reacting ethanol with propanoic acid.

What type of organic compound is ethyl propanoate?

a)

Alcohol

b)

Carboxylic acid

c)

Ester

87.

Organic compounds such as ethyl propanoate are used in perfumes.

Give two properties of these compounds that make them suitable for use in perfumes.

a)

Pleasant smell

b)

Volatile

c)

Liquid

d)

Burn easily

88.

Choose two correct statements about the four compounds.

a)

Methane has the lowest melting point and icosane has the highest boiling point.

b)

Ethene and methane are alkanes.

c)

Methane and decane are gases at room temperature (20°C).

d)

Decane and icosane are liquid at 100°C.

89.

Petrol contains a mixture of compounds, including octane (C8H18).

Complete the word equation for the complete combustion of octane.

octane   +   oxygen   →   ________________   +    __________________

a)

Water

b)

Carbon monoxide

c)

Carbon dioxide

d)

Sulphur dioxide

90.

Polymers are used to make the ballpoint pen.

Name the monomer used to make poly(ethene).

a)

Ethane

b)

Ethene

c)

Propene

d)

Propane

91.

Match the monomer propene to its polymer poly(propene).

a)
b)
c)
92.

 Which metal is in both of these alloys?

a)

Copper

b)

Iron

c)

Zinc

d)

Nickel

e)

Chromium

93.

What is the percentage of iron in the stainless steel?

(a)  

94.

The alloy stainless steel is used instead of pure iron for the ball of the pen.

Give two reasons why.

a)

Stainless steel is soft

b)

Stainless steel is hard

c)

Stainless steel is resistant to corrosion

d)

Stainless steel rusts

95.

 Give one advantage of recycling this type of ballpoint pen.

a)

Can be refilled and reused

b)

Conserves resources of crude oil and ores

c)

High cost of separating materials

d)

Polymers and alloys are not expensive

96.

 Give one disadvantage of recycling this type of ballpoint pen.

a)

Can be refilled and reused

b)

Conserves resources of crude oil and ores

c)

High cost of separating materials

d)

Polymers and alloys are not expensive

97.

The name of the polymer formed when many of these alkene molecules join

together is:

a)

poly(ethene)

b)

poly(ethenol)

c)

poly(propene)

98.

Ethene (C2H4) is produced when hydrocarbons are cracked.

Choose two conditions needed to crack a hydrocarbon.

a)

The presence of an emulsifier.

b)

Heating the hydrocarbon to a high temperature.

c)

Adding oxygen to the hydrocarbon.

d)

The presence of a catalyst.

99.

Name the substance added to ethene (C2H4) to produce ethanol (C2H5OH).

a)

Carbon dioxide

b)

Oxygen

c)

Water

100.

 Name the gas produced during this reaction.

a)

Carbon dioxide

b)

Oxygen

c)

Carbon monoxide

d)

Water vapour

101.

Ethene is a hydrocarbon because it contains only ________ and _________

a)

Hydrogen

b)

Oxygen

c)

Carbon

102.

 Ethene is unsaturated because it has a _____________________ bond.

a)

Double

b)

Single

103.

Disposable cups are made from coated paper or poly(styrene).

The diagram below represents the structure of poly(styrene).

 Which small molecule is used to produce poly(styrene)?

a)
b)
c)
d)
104.

Which process is used to make poly(styrene) from small molecules?

a)

Cracking

b)

Distillation

c)

Fermentation

d)

Polymerisation

105.

There are two main steps in producing drinking water from fresh water.

What is the reason for FILTRATION?

a)

Desalination

b)

Improve taste

c)

Increase pH

d)

Kill bacteria

e)

Remove solids

106.

There are two main steps in producing drinking water from fresh water.

What is the reason for STERILISATION?

a)

Desalination

b)

Improve taste

c)

Increase pH

d)

Kill bacteria

e)

Remove solids

107.

Which two substances are used to sterilise fresh water?

a)

Ammonia

b)

Chlorine

c)

Hydrogen

d)

Nitrogen

e)

Ozone

108.

A large amount of aluminium sulfate was accidentally added to the drinking water supply at a water treatment works.

Scientists tested a sample of the drinking water to show that it contained dissolved solids.

Which two methods show the presence of dissolved solids in the sample of drinking water?

a)

Add damp litmus paper to the sample.

b)

Evaporate all water from the sample.

c)

Measure the sample’s boiling point.

d)

Test the sample with a glowing splint.

109.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample for aluminium ions and the other sample for sulfate ions.

Which compound is needed to identify the ALUMINIUM IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

110.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample for aluminium ions and the other sample for sulfate ions.

Which compound is needed to identify the SULPHATE IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

111.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the CHLORIDE IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

112.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the IRON (III) IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

113.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the IRON (II) IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

114.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the COPPER IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

115.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the CALCIUM IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

116.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the IODIDE IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

117.

Scientists tested two water samples from the drinking water supply.

The scientists tested one sample a range of ions.

Which compound is needed to identify the BROMIDE IONS.

a)

Barium chloride

b)

Copper sulphate

c)

Silver nitrate

d)

Sodium hydroxide

e)

Sulphuric acid

118.

How could pure water be produced from drinking water that contained dissolved solids?

a)

Chromatography

b)

Cracking

c)

Distillation

d)

Sedimentation

119.

Which two substances are mixtures?

a)

Air

b)

Carbon dioxide

c)

Graphite

d)

Sodium Chloride

e)

Steel

120.

What is 'Pure substance in chemistry'?

a)

A substance that has had nothing added to it

b)

A single element or a single compound

c)

A substance containing only atoms which have different numbers of protons

d)

A substance that can be separated by filtration

e)

A useful product made by mixing substances

121.

What is 'Pure substance in everyday life'?

a)

A substance that has had nothing added to it

b)

A single element or a single compound

c)

A substance containing only atoms which have different numbers of protons

d)

A substance that can be separated by filtration

e)

A useful product made by mixing substances

122.

What is the test for chlorine gas?

a)

A glowing splint relights

b)

A lighted splint gives a pop

c)

Damp litmus paper turns white

d)

Limewater turns milky

123.

A student tested a metal chloride solution with sodium hydroxide solution.

A brown precipitate formed.

What was the metal ion in the metal chloride solution?

a)

Calcium

b)

Copper(II)

c)

Iron(II)

d)

Iron(III)

124.

A student tested a metal chloride solution with sodium hydroxide solution.

A white precipitate formed.

What was the metal ion in the metal chloride solution?

a)

Calcium

b)

Copper(II)

c)

Iron(II)

d)

Iron(III)

125.

The colours of fireworks are produced by chemicals.

Three of these chemicals are lithium sulfate, potassium chloride and sodium nitrate. A student wants to carry out flame tests on these three chemicals.

What colour would lithium sulphate go?

a)

green

b)

crimson

c)

yellow

d)

lilac

126.

The colours of fireworks are produced by chemicals.

Three of these chemicals are lithium sulfate, potassium chloride and sodium nitrate. A student wants to carry out flame tests on these three chemicals.

What colour would potassium chloride go?

a)

green

b)

crimson

c)

yellow

d)

lilac

127.

The colours of fireworks are produced by chemicals.

Three of these chemicals are lithium sulfate, potassium chloride and sodium nitrate. A student wants to carry out flame tests on these three chemicals.

What colour would sodium nitrate go?

a)

green

b)

crimson

c)

yellow

d)

lilac

128.

Some theories suggest that the Earth’s early atmosphere was made by

a)

burning fossil fuels.

b)

the formation of oceans.

c)

the eruption of volcanoes.

129.

Which catalyst is used when ammonia is produced from nitrogen and hydrogen?

a)

Chlorine

b)

Iron

c)

Oxygen

130.

Plants lacking essential elements do not grow well because:

•  too little phosphorus can cause slow plant growth

•  too little potassium can cause leaves to have brown edges.

Which fertiliser helps prevent slow plant growth and brown leaf edges?

a)

A

b)

B

c)

C

d)

D

131.

Plants lacking essential elements do not grow well because:

•  too little phosphorus can cause slow plant growth

•  too little potassium can cause leaves to have brown edges.

 Which fertiliser has the greatest total percentage of essential elements?

a)

A

b)

B

c)

C

d)

D

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