OCR GCSE Chemistry A (Gateway) Paper 4 Higher June 2023 question paper J248/04

1h 45m 90 marks

23 questions

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Crude oil is a resource that is being made extremely slowly.

Which word describes a resource that is being made extremely slowly?

A Finite

B Hydrocarbon

C Non‑renewable

D Petrochemical

$Question 1, shown as an image$

[1]

Answer

The Group 7 element fluorine is a gas at room temperature and pressure.

The Group 7 elements show a trend in boiling points going down the group.

Which row shows the boiling points of the Group 7 elements?

		Boiling Point (	C)
	Fluorine	Chlorine	Bromine	Iodine
A	–188	59	184	–15
B	–188	–34	59	184
C	188	184	59	–15
D	–15	184	188	59

$Question 2, shown as an image$

[1]

Answer

Copper can be extracted from copper ore by heating the copper ore with carbon.

Copper can also be extracted by bioleaching.

What is an advantage of bioleaching?

A It can produce sulfuric acid.

B It extracts copper, which is then purified by electrolysis.

C It is done at low temperatures.

D It is slow.

$Question 3, shown as an image$

[1]

Answer

Which gas was the most abundant in the Earth’s early atmosphere?

A Argon

B Carbon dioxide

C Nitrogen

D Oxygen

$Question 4, shown as an image$

[1]

Answer

This is the balanced symbol equation for the reaction of copper oxide with carbon.

$Question 5, shown as an image$

What happens to the copper oxide in this reaction?

A It is neutralised.

B It is oxidised.

C It is reduced.

D It is thermally decomposed.

$Question 5, shown as an image$

[1]

Answer

Which row in the table shows three greenhouse gases?

$Question 6, shown as an image$

[1]

Answer

The graph shows the volume of hydrogen gas made in an experiment.

What is the rate of reaction when the time is 20 s?

0.44 cm³ / s A

2.25 cm³ / s B

25 cm³ / s C

900 cm³ / s D

$Question 7, shown as an image$

[1]

Answer

Why are alloys stronger than the pure metals which they are made from?

A Alloys combine the properties of the metals they are made from.

B Alloys contain atoms of different sizes.

C Alloys contain different atoms bonded together.

D Alloys have strong bonds between their molecules.

$Question 8, shown as an image$

[1]

Answer

Which statement about chemical cells is correct?

A They produce a voltage indefinitely.

B They produce a voltage once all of the reactants are used up.

C They produce a voltage until one of the reactants is completely used up.

D They produce a voltage until the reactants are partly used up.

$Question 9, shown as an image$

[1]

Answer

Which of these homologous series can form addition polymers?

A Alcohols and carboxylic acids

B Alkenes and alkanes

C Alkenes only

D Carboxylic acids only

$Question 10, shown as an image$

[1]

Answer

Which statement about the greenhouse effect is correct?

A Greenhouse gases absorb all the infrared radiation that is emitted by the Earth’s surface.

B Greenhouse gases make up a large percentage of the Earth’s current atmosphere.

C The greenhouse effect is caused by the absorption and reflection of infrared radiation by greenhouse gases.

D The higher the concentration of greenhouse gases in the Earth’s atmosphere, the colder the Earth is likely to become.

$Question 11, shown as an image$

[1]

Answer

[1]

Answer

[1]

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Ethene, C₂H₄, reacts with bromine in an addition reaction.

What is the structural formula of the product?

$Question 14, shown as an image$

[1]

Answer

What is the half equation for the reaction at the anode in a hydrogen/oxygen fuel cell?

$Question 15, shown as an image$

[1]

Answer

A student investigates two solutions, A and B.

They know that

• one solution contains a halide ion

• the other solution contains a different anion.

They test 2 cm³ of each solution for the halide ion using this method:

• Add a few drops of dilute hydrochloric acid and shake.

• Add a few drops of silver nitrate solution.

• Record the colour of the precipitate.

(a)

The teacher says that the student should have used a different acid instead of dilute hydrochloric acid.

(a)(i)

State the name of the acid the student should have used.

[1]

Answer

(a)(ii)

Explain why using dilute hydrochloric acid would affect the results of this test.

[2]

Answer

(b)

[2]

Answer

(c)

[3]

Answer

(d)

Barium chloride solid is toxic if swallowed and harmful if inhaled.

Barium chloride solutions with concentrations of 21 g / dm³ are suitable for experiments in school.

Calculate the mass of barium chloride that should be dissolved in 25 cm³ of water to make a solution with a concentration of 21 g / dm³.

Use the equation:

$Question 16, shown as an image$

Give your answer to 2 significant figures.

[3]

Answer

The table shows information about three different polymers, A, B and C.

Tensile strength is the amount of load a material can take before it breaks.

	Melting point (C)	Softening temperature (C)	Stiffness (MPa)	Tensile strength (MPa)
A	130	72	980	15
B	240	95	3200	65
C	250	75	2400	50

(a)

A company wants to use a polymer to make a disposable cup for hot drinks.

Suggest and explain which polymer, A, B or C, the company should use.

Polymer........

Reason........

[3]

Answer

(b)

This is the repeating unit in polymer B.

Draw the structure of the monomer from which polymer B is made.

[2]

Answer

(c)

Some substances are naturally occurring polymers.

Draw lines to connect each monomer with its naturally occurring polymer.

[2]

Answer

(a)

Write the balanced symbol equation for the reaction between hydrochloric acid, HC l, and magnesium.

[2]

Answer

(b)

The teacher says, ‘The reaction is faster the more concentrated the hydrochloric acid’.

Use the results to explain why the teacher is correct.

[1]

Answer

(c)

The graph shows the teacher’s results.

(c)(i)

Use the graph to deduce the time for magnesium powder to react if 1.3 mol / dm³ (i) hydrochloric acid is used.

[1]

Answer

(c)(ii)

The teacher repeats the experiment with 0.1 g of magnesium ribbon.

Draw a line on the graph to show the results you would expect the teacher to get.

[2]

Answer

(d)

The teacher used 0.1 g of magnesium.

0.1 g of magnesium reacts with hydrochloric acid to make 0.008 g of hydrogen gas.

Calculate the volume occupied by 0.008 g of hydrogen gas in cm³.

Relative atomic mass (A_r): H = 1.0

[4]

Answer

[6]

Answer

Butane, C₄H₁₀, is an alkane.

Butane undergoes complete combustion in oxygen.

(a)

Write the balanced symbol equation for the complete combustion of butane.

[2]

Answer

(b)

Table 20.1 lists the energy given out when 1 g of different alkanes burn.

Table 20.1

Alkane	Energy given out (kJ)
butane	49.2
ethane	52.6
methane	55.6
propane	50.4

State the relationship between the number of carbon atoms in the alkane and the energy given out.

[1]

Answer

(c)

Butane is found in the LPG fraction when crude oil is separated into different fractions by fractional distillation.

Table 20.2 shows some information about four other molecules that are found in four different fractions.

Table 20.2

Molecule	Formula	Boiling point (C)
heptadecane	C₁₇H₃₆	302
eicosane	C₂₀H₄₂	342
tetracosane	C₂₄H₅₀
octacosane	C₂₈H₅₈	436

(c)(i)

Predict the boiling point of tetracosane.

Boiling point of tetracosane =........ maths symbol C

[1]

Answer

(c)(ii)

Octacosane is separated lower down the fractionating column than the other three molecules in Table 20.2.

Explain why using ideas about intermolecular forces.

[3]

Answer

(d)

Cracking breaks down large molecules produced in fractional distillation into more useful molecules.

The equation shows the cracking of octacosane to make dodecane and one other product.

Complete and balance the equation.

$Question 20, shown as an image$

[2]

Answer

(e)

Table 20.3 shows the percentage supply and demand for some of the different fractions obtained from crude oil.

Table 20.3

Fraction	Percentage supply (%)	Percentage demand (%)
LPG	2	4
petrol	5	23
naphtha	8	5
kerosene	12	7
diesel oil	17	23
fuel oil	56	38

More petrol can be obtained by cracking another fraction.

Suggest and explain which fraction is cracked to obtain petrol.

Fraction........

Reason........

[2]

Answer

Methanol, CH₃OH, is made in industry by reacting carbon monoxide with hydrogen.

This is the equation for the reaction.

$Question 21, shown as an image$

The forward reaction is exothermic.

(a)

A temperature of 250 maths symbol C and a pressure of 100 atmospheres is used for the reaction.

(a)(i)

Describe and explain the effect on the yield of methanol from using a pressure of 15 atmospheres.

[3]

Answer

(a)(ii)

The yield of methanol is greater when a temperature of 150 maths symbol C is used instead of 250 C.

Suggest why a temperature of 150 maths symbol C is not used in industry.

[1]

Answer

(b)

A catalyst is used to speed up the reaction.

Describe the effect on the position of equilibrium from using a catalyst.

[1]

Answer

(c)

A factory makes some methanol.

They predict they will make 60 tonnes of methanol. The reaction has a percentage yield of 78%.

Calculate the mass of methanol they actually make.

Mass of methanol =........ tonnes

[3]

Answer

(d)(i)

Draw the structural formula of methanol, CH₃OH.

[2]

Answer

(d)(ii)

State the functional group in methanol.

[1]

Answer

(e)

Methanol can be oxidised to methanoic acid.

State the oxidising agent used in this reaction.

[1]

Answer

(f)

Methanoic acid is a carboxylic acid.

Carboxylic acids react with alcohols to form an ester and one other product.

(f)(i)

What type of reaction is this?

Tick (✓) one box.

$Question 21, shown as an image$

[1]

Answer

(f)(ii)

State the name of the other product in this type of reaction.

[1]

Answer

Group 7 elements (halogens) react with halides in solution.

Chlorine reacts with potassium bromide to form potassium chloride and bromine.

$Question 22, shown as an image$

(a)

Describe what you would observe in the reaction.

[1]

Answer

(b)

This is the half equation that shows what happens to chlorine.

$Question 22, shown as an image$

(b)(i)

Explain why this half equation shows reduction.

[1]

Answer

(b)(ii)

Write the balanced half equation for the reaction of the bromide ions.

[2]

Answer

(c)

Chlorine displaces bromine from potassium bromide because chlorine is more reactive than bromine.

Explain why chlorine is more reactive than bromine.

[2]

Answer

(d)

The diagram shows the mass spectrum for a compound containing chlorine.

State the relative molecular mass of this compound.

[1]

Answer

(e)

Instrumental methods of analysis, such as mass spectrometry, have advantages over simple chemical methods of analysis.

State two advantages of instrumental methods of analysis.

[2]

Answer

A student plans a titration experiment.

The diagram shows some of the apparatus they use.

(a)

At the end of the titration, the student reads the final volume reading from the top of the meniscus instead of from the bottom of the meniscus.

How does the measured volume of potassium hydroxide compare to the actual volume?

Tick (✓) one box.

$Question 23, shown as an image$

[1]

Answer

(b)

(b)(i)

Calculate the average titre using the student’s concordant results.

[1]

Answer

(b)(ii)

This is the equation for the reaction in this experiment.

$Question 23, shown as an image$

Calculate the concentration of sulfuric acid in g / dm³.

Relative atomic mass (A_r): H = 1.0 O = 16.0 S = 32.0

Concentration of sulfuric acid =........ g / dm³

[5]

Answer

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OCR J248 · Paper 4

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10

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Question 12

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Question 19

Question 20

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Question 23