International ASChemistryEdexcelExam Questions1. Structure, Bonding & Introduction to Organic ChemistryAmount of Substance

Amount of Substance (Edexcel International AS Chemistry): Multiple Choice Questions

Exam code: XCH11

59 mins31 questions

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Amount of Substance

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1
1 mark

What volume is occupied by 0.25 mol of an ideal gas at room temperature and pressure (r.t.p.)?

[Molar volume at r.t.p. = 24.0 dm^3^ mol^-1^]

  • 6.0 dm3

  • 12.0 dm3

  • 24.0 dm3

  • 96.0 dm3

Choose your answer

2
1 mark

How many moles are there in 15.1 cm3 of liquid propan-1-ol?

[Density of propan-1-ol = 0.80 g cm−3      Mr of propan-1-ol = 60]

  • (0.80 × 15.1) ÷ 60

  • 0.80 ÷ (60 × 15.1)

  • 60 ÷ (0.80 × 15.1)

  • (60 × 15.1) ÷ 0.80

Choose your answer

3
1 mark

Chloromethane is produced by the reaction of methane with chlorine in the presence of ultraviolet radiation.

CH4 + Cl2 → CH3Cl + HCl

What is the percentage atom economy by mass for the production of chloromethane?

[Ar values: H = 1.0; C = 12.0; Cl = 35.5]

  • 42.0%

  • 58.0%

  • 71.1%

  • 100%

Choose your answer

4
1 mark

5.85 g of sodium chloride, NaCl, is dissolved in water and the solution is made up to 250 cm3.

What is the concentration of the solution, in mol dm-3? [Mr (NaCl) = 58.5]

  • 0.040

  • 0.100

  • 0.250

  • 0.400

Choose your answer

5
1 mark

Nitrogen reacts with hydrogen to form ammonia.

N2 (g) + 3H2 (g) → 2NH3 (g)

What amount of ammonia forms when 6.0 mol of hydrogen reacts with excess nitrogen?

  • 2.0 mol

  • 4.0 mol

  • 6.0 mol

  • 9.0 mol

Choose your answer

6
1 mark

The relative molecular mass, Mr, of a gas can be found using the ideal gas equation, pV = nRT.

Which expression gives Mr for a sample of the gas of mass m g?

  • Mr=mRTpV

  • Mr=pVRTm

  • Mr=mpVRT

  • Mr=pVmRT

Choose your answer

7
1 mark

A bubble of gas is released at the sea bed, where the pressure is 2020 kPa. The bubble rises to just below the surface, where the pressure is 101 kPa and its volume is 200 cm3.

The temperature at the sea bed and at the surface is the same. Assume the gas behaves ideally.

What was the volume of the bubble at the sea bed?

  • 0.05 cm3

  • 10 cm3

  • 200 cm3

  • 4000 cm3

Choose your answer

1
1 mark

A mass of 4.179 g of hydrated iron(III) sulfate, Fe2(SO4)3·H2O, was dissolved in deionised water and the solution made up to 200 cm3 .

What is the concentration of sulfate ions, SO42-, in the solution, in mol dm−3?

[Molar mass of Fe2(SO4)3·H2O = 417.9 g mol−1]

  • 0.01

  • 0.05

  • 0.10

  • 0.15

Choose your answer

2a
1 mark

A mass of 0.23 g of sodium was added to 350 cm3 water to form hydrogen and a solution of sodium hydroxide.

Na (s) + H2O (l) → NaOH (aq) + 1⁄2H2 (g)

What is the concentration, in mol dm−3, of sodium hydroxide in the solution formed?

  • 0.010

  • 0.029

  • 0.29

  • 0.66

Choose your answer

2b
1 mark

What is the maximum volume, in cm3, of hydrogen which could be formed, measured at r.t.p.?

[Molar volume of a gas at r.t.p. = 24 dm3 mol−1]

  • 120

  • 240

  • 480

  • 2800

Choose your answer

2c
1 mark

The sodium hydroxide solution was neutralised with sulfuric acid.

Which is the ionic equation for this reaction?

  • H+ (aq) + OH− (aq) → H2O (l)

  • SO42− (aq) + 2Na+ (aq) → Na2SO4 (aq)

  • H2SO4 (aq) + 2Na+ (aq) + 2OH− (aq) → Na2SO4 aq) + 2H2O (l)

  • 2H+ (aq) + SO42− (aq) + 2Na+ (aq) + 2OH− (aq) → 2Na+ (aq) + SO42− (aq) + 2H2O (l)

Choose your answer

2d
1 mark

Sodium hydroxide solution was added to magnesium sulfate solution. The equation for the reaction is shown.

2NaOH(aq) + MgSO4(aq) → Mg(OH)2(s) + Na2SO4(aq)

What is the atom economy (by mass) for the production of magnesium hydroxide?

[Ar values: H = 1.0 O = 16.0 Na = 23.0 Mg = 24.3 S = 32.1]

  • 29.1%

  • 41.0%

  • 48.4%

  • 50.0%

Choose your answer

3
1 mark

Which conversion has the lowest percentage atom economy (by mass) for the formation of CaCl2?

  • Ca + Cl2 → CaCl2

  • Ca + 2HCl → CaCl2 + H2

  • CaCO3 + 2HCl → CaCl2 + H2O + CO2

  • CaCO3 + 2NaCl → CaCl2 + Na2CO3

Choose your answer

4
1 mark

The equation for the complete combustion of propan-1-ol is shown.

C3H7OH(l) + 4 1⁄2O2(g) → 3CO2(g) + 4H2O(l)

2.00 × 10−3 mol of propan-1-ol undergoes complete combustion.

What mass of carbon dioxide is formed?

  • 0.0293g

  • 0.0880g

  • 0.132g

  • 0.264g

Choose your answer

5
1 mark

A student is provided with 25.0 cm3 of 1.00 mol dm–3 hydrochloric acid.

What volume of distilled water should the student add to this solution to make a 0.0500 mol dm–3 solution?

  • 25.0 cm3

  • 50.0 cm3

  • 475 cm3

  • 500 cm3

Choose your answer

6
1 mark

Cyclohexene may be prepared by the dehydration of cyclohexanol.

q15-paper-1-june-2021-edexcel-ial-chemistry

What mass of cyclohexene can be made from 12.5 g of cyclohexanol if the yield is 51.2%?

  • 5.25 g

  • 6.40 g

  • 7.80 g

  • 10.25 g

Choose your answer

7
1 mark

Which of these gases occupies 6.0 dm3 at room temperature and pressure (r.t.p.)?

[molar volume of gas at r.t.p. = 24.0 dm3 mol−1

Ar values: He = 4.0 C = 12.0 N = 14.0 O = 16.0]

  • 2.0 g of helium

  • 4.0 g of oxygen

  • 11.0 g of carbon dioxide

  • 14.0 g of nitrogen

Choose your answer

8
1 mark

Which of these solutions contains the greatest number of ions?

  • 20.0 cm3 of 0.5 mol dm−3 KCl

  • 0.40 dm3 of 0.03 mol dm−3 KCl

  • 10.0 cm3 of 0.6 mol dm−3 CaCl2

  • 0.15 dm3 of 0.04 mol dm−3 CaCl2

Choose your answer

9
1 mark

What volume, in dm3, of hydrogen gas will be produced when 3.00 g of lithium is reacted with water at room temperature and pressure (r.t.p.)?

2Li + 2H2O → 2LiOH + H2

[Molar volume of gas at r.t.p. = 24.0 dm3 mol–1]

  • 0.217

  • 0.435

  • 5.22

  • 10.4

Choose your answer

10
1 mark

Potassium chlorate(V) decomposes on heating to form oxygen.

2KClO3 → 2KCl + 3O2

What is the atom economy (by mass) for the formation of oxygen?

[Ar values: O = 16.0 Cl = 35.5 K = 39.1]

  • 13.1%

  • 26.1%

  • 39.2%

  • 64.3%

Choose your answer

11
1 mark

10.00 g of hydrated magnesium sulfate, MgSO4•7H2O, is heated to remove the water of crystallisation.

What mass of anhydrous magnesium sulfate, MgSO4, is formed?

[Molar mass of MgSO4•7H2O = 246.4 g mol−1 ]

  • 2.84 g

  • 4.89 g

  • 5.11 g

  • 7.16 g

Choose your answer

12
1 mark

Which aqueous solution contains the greatest number of ions?

  • 200 cm3 of 1.5 mol dm−3 MgCl2

  • 400 cm3 of 0.8 mol dm−3 MgSO4

  • 500 cm3 of 1.0 mol dm−3 NaCl

  • 1000 cm3 of 0.25 mol dm−3 Na2SO4

Choose your answer

13
1 mark

Which aqueous solution has the highest concentration, in mol dm-3, of chloride ions?

  • 0.1 g dm-3 HCl

  • 0.1 g dm-3 NaCl

  • 0.1 g dm-3 KCl

  • 0.1 g dm-3 BaCl2

Choose your answer

14
1 mark

A 4.00 mol dm−3 solution of an acid is used to prepare dilute solutions of the acid.

What volume of water is required to make up 150 cm3 of 0.35 mol dm−3 solution of the acid?

  • 13.1 cm3

  • 52.5 cm3

  • 97.5 cm3

  • 136.9 cm3

Choose your answer

1
1 mark

Barium chloride solution, BaCl2 (aq), reacts with gallium sulfate solution, Ga2(SO4)3 (aq) to form a precipitate of barium sulfate, BaSO4 (s).

What is the minimum volume of 0.100 mol dm−3 barium chloride needed to precipitate all the sulfate ions in 200 cm3 of 0.05 mol dm−3 gallium sulfate?

  • 100 cm3

  • 200 cm3

  • 300 cm3

  • 400 cm3

Choose your answer

2
1 mark

Propane burns completely in oxygen as shown.

C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4H2O (l)

100 cm3 of propane was mixed with 600 cm3 of oxygen and the mixture was ignited.

What is the total volume, in cm3, of the gas mixture at the end of the reaction?

All gas volumes were measured at room temperature and pressure.

  • 300

  • 400

  • 700

  • 800

Choose your answer

3
1 mark

Iron(III) oxide is reduced by hydrogen in a two-step process.

Step 1:

3Fe2O3 + H2 → 2Fe3O4 + H2O

Step 2:

Fe3O4 + 4H2 → 3Fe + 4H2O

What is the maximum mass of iron that could be produced from 39.9 tonnes of Fe2O3 ?

[Ar values: H = 1.0 O = 16.0 Fe = 55.8]   

  • 6.98 tonnes

  • 13.95 tonnes

  • 27.90 tonnes

  • 41.85 tonnes

Choose your answer

4
1 mark

Flask Q contains 4.0 dm3 of neon at a pressure of 10 kPa. Flask R contains 10 dm3 of helium at a pressure of 5.0 kPa.

The flasks are connected at constant temperature. Assume both gases behave ideally.

What is the final pressure in the system?

  • 2.9 kPa

  • 6.4 kPa

  • 7.5 kPa

  • 15 kPa

Choose your answer

5a
1 mark

The maximum permitted concentration of sulfur in diesel fuel is 10 mg of sulfur in 1 kg of diesel fuel.

What is this concentration of sulfur in ppm?

  • 0.00001

  • 0.01

  • 10

  • 10000

Choose your answer

5b
1 mark

3.2 kg of this diesel fuel is burned in air.

What is the maximum volume, in dm3, of sulfur dioxide which can be produced, measured at room temperature and pressure (r.t.p.)?

[Molar volume of a gas at r.t.p. = 24 dm3 mol−1]

  • 0.024

  • 0.77

  • 2.4

  • 24

Choose your answer

6
1 mark

Ammonia gas reacts with oxygen to form nitrogen monoxide and steam.

10.0 dm3 of ammonia is mixed with 12.0 dm3 of oxygen. All volumes are measured at the same temperature and pressure.

What volume of nitrogen monoxide forms?

  • 8.00 dm3

  • 9.60 dm3

  • 10.0 dm3

  • 14.4 dm3

Choose your answer

7
1 mark

A student reacted copper(II) oxide with excess sulfuric acid and crystallised 35.9 g of hydrated copper(II) sulfate, CuSO4·5H2O. Each mole of copper(II) oxide forms one mole of the crystals. The percentage yield was 80.0%.

[Ar values: H = 1.0 O = 16.0 S = 32.1 Cu = 63.5]

What mass of copper(II) oxide did the student use?

  • 9.1 g

  • 11.4 g

  • 14.3 g

  • 22.4 g

Choose your answer