OCR GCSE Chemistry A (Gateway) Paper 4 Higher June 2024 question paper J248/04

1h 45m 90 marks

22 questions

Report a problem

Question

What is wrong?

Text or a picture is cut off or split Something on the paper is not here The text does not read properly The marks are wrong Something else

Goes to whoever maintains the question split. No account needed and nothing is published on this page.

Which substance is an unsaturated hydrocarbon?

A CH₄

B C₂H₆

C C₃H₆

D C₃H₈

$Question 1, shown as an image$

[1]

Answer

What happens when liquid bromine, Br₂, boils?

A Covalent bonds break

B Electrostatic forces break

C Intermolecular forces break

D Ionic bonds break

$Question 2, shown as an image$

[1]

Answer

What is a life-cycle assessment?

A Analysis of the cost of making, using, and disposing of a product.

B Analysis of the energy needed to use a product throughout its lifetime.

C Analysis of the potential environmental impact of manufacturing a product.

D Analysis of the potential environmental impact that a product may have throughout its lifetime.

$Question 3, shown as an image$

[1]

Answer

Which of these is one of the four nucleotides in the polymer DNA?

A Cytosine

B Deoxyribose

C Fructose

D Phosphate

$Question 4, shown as an image$

[1]

Answer

Polyesters are condensation polymers.

Which monomers are polyesters made from?

A A carboxylic acid and an ester

B An alcohol and a carboxylic acid

C An alcohol and an amine

D An amine and a carboxylic acid

$Question 5, shown as an image$

[1]

Answer

[1]

Answer

What is an advantage of extracting metals by phytoextraction?

A It can extract metals from contaminated soils.

B It is dependent on weather conditions.

C It is slow.

D It produces carbon dioxide gas when the plants are burnt.

$Question 7, shown as an image$

[1]

Answer

[1]

Answer

How is the mass of a solute, in g, related to the concentration of the solution, in g / dm³, and the volume of the solution, in dm³?

A mass = concentration maths symbol volume

$Question 9, shown as an image$

[1]

Answer

Which equation shows the reaction at the anode in a hydrogen/oxygen fuel cell?

$Question 10, shown as an image$

[1]

Answer

The polymer nylon can be made from hexanedioyl dichloride, Cl OC(CH₂)₄COCl, and hexane-1,6-diamine, NH₂(CH₂)₆NH₂.

Which small molecule is made as well as nylon?

A HC l

B H₂

C H₂O

D NH₃

$Question 11, shown as an image$

[1]

Answer

The reaction between hydrogen, H₂, and iodine, I₂, is reversible.

$Question 12, shown as an image$

The reaction is exothermic.

What will increase the yield of hydrogen iodide, H I ?

A Adding a catalyst

B Adding less hydrogen

C Decreasing the temperature

D Increasing the pressure

$Question 12, shown as an image$

[1]

Answer

Which statement about activation energy is correct?

A Activation energy is increased by the addition of a catalyst.

B Activation energy is lowered when the temperature is increased.

C Activation energy is the minimum amount of energy for a reaction to occur.

D The greater the activation energy, the greater the rate of reaction.

$Question 13, shown as an image$

[1]

Answer

What is the volume of 0.6 moles of nitrogen gas, N₂, at room temperature and pressure?

14.4 dm³ A

16.8 dm³ B

40.0 dm³ C

46.7 dm³ D

$Question 14, shown as an image$

[1]

Answer

Which carbon compound produces this mass spectrum?

Relative atomic mass (A_r): C = 12.0 H = 1.0

A C₂H₄

B C₃H₈

C C₄H₈

D C₅H₁₂

$Question 15, shown as an image$

[1]

Answer

(a)

The table shows some properties of four Group 1 elements.

Element	Density (g / cm³)	Melting Point (°C)	Boiling Point (°C)
Lithium	0.53	180	1342
Sodium	0.97	98	883
Potassium	0.86	63	759
Rubidium	1.53	39	688

(a)(i)

State one trend in the properties of the Group 1 elements shown in the table.

[1]

Answer

(a)(ii)

Caesium is below rubidium in Group 1.

Predict the melting point of caesium using the information in the table.

[1]

Answer

(b)

The Group 1 elements all react with Group 7 elements to form ionic compounds.

(b)(i)

Explain why the Group 1 elements all react in the same way.

[1]

Answer

(b)(ii)

The Group 1 elements become more reactive down the group.

Explain why.

[3]

Answer

(b)(iii)

Sodium reacts with bromine, Br₂, to make sodium bromide, NaBr.

Write the balanced symbol equation for this reaction.

[2]

Answer

(c)

[2]

Answer

Ammonia is made in the Haber process. This is the balanced symbol equation for this process.

$Question 17, shown as an image$

(a)

The reversible reaction is carried out in a closed system.

(a)(i)

State how you can tell that this reaction is reversible.

[1]

Answer

(a)(ii)

What is a closed system ?

[1]

Answer

(a)(iii)

[2]

Answer

(b)

The reaction in the Haber process can be reversed by altering the reaction conditions.

The reaction can be reversed by altering the pressure.

Suggest one other change that could be made to the reaction conditions.

[1]

Answer

(c)

A factory predicts they will make 800 tonnes of ammonia.

They actually make 620 tonnes of ammonia.

Calculate the percentage yield.

[2]

Answer

(d)

State why the reaction in the Haber process has an atom economy of 100%.

Use the balanced symbol equation.

[1]

Answer

(a)

The table shows the results.

Test tube	Mass of nail at start (g)	Mass of nail after a week (g)
1	4.42	.........................................
2	4.46	.........................................
3	4.51	4.51

Complete the table to estimate the mass of the nails in test tubes 1 and 2 after a week.

[2]

Answer

(b)

The student sets up another two test tubes as shown in Fig. 18.2.

Fig. 18.2

Test tube 4
Test tube 5

The iron nail in test tube 4 rusted. The iron nail in test tube 5 did not rust.

Explain why.

[3]

Answer

(c)

Copper is extracted by heating copper oxide with carbon.

(c)(i)

Explain why this is an example of a redox reaction.

[2]

Answer

(c)(ii)

Calculate the mass of copper that can be made from 15 tonnes of copper oxide.

Give your answer to 2 significant figures.

Relative atomic mass (A_r): Cu = 63.5 Relative molecular mass (M_r): CuO = 79.5

Mass of copper =........ tonnes

[3]

Answer

(c)(iii)

Copper is used in electrical wires.

The graph shows how impurities in copper affect the relative electrical conductivity of copper.

Copper extracted from copper oxide is about 99% pure.

Explain why copper extracted from copper oxide is purified to almost 100% pure using electrolysis.

Use data from the graph in your answer.

[2]

Answer

The first member of the alkane homologous series is methane, CH₄.

(a)

State the formula of the alkane with 10 carbon atoms.

[1]

Answer

(b)

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

[2]

Answer

(c)

Methane can also undergo incomplete combustion.

Carbon monoxide and water are made in incomplete combustion.

State one other possible product of the incomplete combustion of methane.

[1]

Answer

(d)

Alkanes are obtained from the fractional distillation of crude oil.

The LPG fraction contains propane and butane.

Explain why the LPG fraction leaves at the top of the fractionating column. Use ideas about intermolecular forces.

[4]

Answer

(e)

Which industry is crude oil a feedstock for?

[1]

Answer

(f)

[4]

Answer

The Earth’s early atmosphere is thought to have been mainly carbon dioxide, with smaller amounts of water vapour.

(a)

Describe how the amounts of these gases changed over time to develop an oxygen-rich atmosphere.

[3]

Answer

(b)

The graph shows how the percentages of different gases in the atmosphere have changed over

(b)(i)

Describe the relationship between the percentage of carbon dioxide and the percentage of nitrogen in the atmosphere.

[1]

Answer

(b)(ii)

Estimate when the percentage of carbon dioxide and the percentage of oxygen were equal.

Answer =........ millions of years ago

[1]

Answer

(c)

(c)(i)

Describe the link between the amount of sulfur dioxide in the atmosphere and the concentration of the hydrogen ion, H +, in the rainwater between the years 2000 and 2005.

Use the graph.

[3]

Answer

(c)(ii)

Since 2014 the amount of acid rain in the atmosphere has decreased.

Suggest why.

[1]

Answer

A student investigates the neutralisation reaction between sodium hydroxide solution and dilute hydrochloric acid.

They do a titration experiment.

The diagram shows the apparatus they use.

(a)

Describe how the student uses the apparatus to do the titration.

Include the name of a suitable indicator and state the colour change that would be seen.

[5]

Answer

(b)

The student repeats the titration four times.

They work out the average volume of sodium hydroxide from their concordant results.

(b)(i)

What is meant by concordant results?

[1]

Answer

(b)(ii)

In the titration the student:

• uses 25 cm³ of 0.12 mol / dm³ dilute hydrochloric acid in the conical flask

• adds 0.4 mol / dm³ sodium hydroxide solution from the burette.

The equation for the reaction is shown.

$Question 21, shown as an image$

Calculate the average volume of sodium hydroxide used in cm³.

[4]

Answer

A student investigates the reaction between marble chips and dilute hydrochloric acid.

The diagram shows their experiment.

The student measures the volume of carbon dioxide gas collected in the measuring cylinder every 30 seconds.

(a)

(a)(i)

Suggest another piece of equipment that could be used to measure the volume of carbon dioxide gas.

[1]

Answer

(a)(ii)

Explain how the student could tell that the dilute hydrochloric acid is the limiting reactant in this reaction.

[1]

Answer

(b)

The student plots their results on a graph.

Use the graph and a tangent line to calculate the rate of the reaction at 60 seconds.

Rate of reaction at 60 seconds =........ cm³ / s

[3]

Answer

(c)

The rate of the reaction can be changed by adding a catalyst.

(c)(i)

What happens to the final volume of carbon dioxide when a catalyst is added?

[1]

Answer

(c)(ii)

How does the mass of the catalyst change during the experiment?

[1]

Answer

(d)

* Another student reacts dilute hydrochloric acid with magnesium.

The student does two experiments.

In each experiment they use the same

• concentration of dilute hydrochloric acid

• mass of magnesium.

The table shows their results.

	Experiment 1	Experiment 2
Magnesium	large pieces	small pieces
Temperature of dilute hydrochloric acid (°C)	20	42
Rate of reaction (/s)	0.0044	0.04

Evaluate the student’s results, explaining the difference in the rate of reaction.

Use the reacting particle model.

State how the student’s experiment could be improved.

[6]

Answer

The paper as printed

Spotted a mistake on this page?Report a problem

OCR J248 · Paper 4

Question 1

Question 2

Question 3

Question 4

Question 5

Question 6

Question 7

Question 8

Question 9

Question 10

Question 11

Question 12

Question 13

Question 14

Question 15

Question 16

Question 17

Question 18

Question 19

Question 20

Question 21

Question 22