Question 1

Sodium hydroxide neutralises acid.

H+ + OH- ➔ H2O

In a 11,000 dm3 sample of an aqueous solution, the concentration of acid, [H+], is 1.26 × 10-3 moldm-3.

Which mass of solid sodium hydroxide neutralises the acid?

  A  

0.0214 g

  B  

0.0504 g

  C  

236 g

  D  

554 g

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Question 2

The gas laws can be summarised in the ideal gas equation.

pV = nRT

0.960 g of oxygen gas is contained in a vessel of volume 7.00 × 10-3 m3 at a temperature of 30°C.

Assume that the gas behaves as an ideal gas.

What is the pressure in the vessel?

  A  

1.07 kPa

  B  

2.14 kPa 

  C  

10.8 kPa 

  D  

21.6 kPa

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Question 3

Which gas sample contains the fewest molecules?

  A  

1.00 dm3 of carbon dioxide at 27°C and 2.0 kPa

  B  

1.00 dm3 of hydrogen at 100°C and 2.0 kPa

  C  

1.00 dm3  of nitrogen at 300°C and 4.0 kPa

  D  

1.00 dm3 of oxygen at 250°C and 3.0 kPa

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Question 4

The relative atomic mass is defined as

  A  

the mass of an atom of an element relative to 1/12th the mass of a carbon-12 atom

  B  

the mass of an atom of an element relative to the mass of a hydrogen atom

  C  

the average mass of an element relative to 1/12th the mass of a carbon atom

  D  

the average mass of an atom of an element relative to 1/12th the mass of a carbon-12 atom

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Question 5

Which reaction produces the smallest atom economy of BaCl2?

  A  

BaCl2⸱2H2O ➔ BaCl2 + 2H2O

  B  

BaO + 2HCl ➔ BaCl2 + H2O

  C  

BaCO3 + 2HCl ➔ BaCl2 + CO2 + H2O

  D  

Ba + 2HCl ➔ BaCl2 + H2

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Question 6

A student mixes 100 cm3 of 0.200 mol dm-3 NaCl(aq) with 100 cm3 of 0.200 mol dm-3 Na2CO3(aq).

What is the total concentration of Na+ ions in the mixture formed?

  A  

0.100 mol dm-3

  B  

0.200 mol dm-3

  C  

0.300 mol dm-3

  D  

0.400 mol dm-3

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Question 7

Sodium reacts with water as shown below.

2Na(s) + 2H2O(l) ➔ 2NaOH(aq) + H2(g)

Which mass of sodium reacts with water to produce 960 cm3 of hydrogen gas at RTP?

  A  

0.46 g

  B  

0.92 g

  C  

1.84 g

  D  

3.68 g

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Question 8

What is the number of oxygen atoms in 88.0 g of CO2?


  A  

3.01 × 1023

  B  

1.20 × 1024

  C  

2.41 × 1024

  D  

4.82 × 1024

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Question 9

What is the empirical formula of an oxide of nitrogen that contains 26% nitrogen by mass?

  A  

NO2

  B  

N2O3

  C  

N2O5

  D  

N4O5

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Question 10

30 cm3 of xenon are mixed with 20 cm3 of fluorine. The gases react according to the following equation. Assume that the temperature and pressure remain constant.

Xe(g) + F2(g) ➔ XeF2(g)

What is the final volume of gas after the reaction is complete?

  A  

50 cm3

  B  

40 cm3

  C  

30 cm3

  D  

20 cm3

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Question 11

In a car airbag, sodium azide (NaN3) decomposes to form sodium metal and nitrogen gas.

2NaN3(s) ➔ 2Na(s) + 3N2(g)

The sodium metal then reacts with potassium nitrate to produce more nitrogen gas.

10Na(s) + 2KNO3(s) ➔ N2(g) + 5Na2O(s) + K2O(s)

If 2.00 mol of sodium azide react in this way, how many molecules of N2 will be formed?

The Avogadro constant, L = 6.022 x 1023 mol−1.

  A  

2.41 x 1024

  B  

1.93 x 1024

  C  

1.81 x 1024

  D  

9.63 x 1023

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Question 12

A 20.0 cm3 sample of a 0.400 mol dm-3 aqueous solution of a metal bromide (MBrn) reacts exactly with 160 cm3 of  0.100 mol dm-3 aqueous silver nitrate.

What is the formula of the metal bromide?

  A  

MBr

  B  

MBr2

  C  

MBr3

  D  

MBr4

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Question 13

What is the mass, in mg, of carbon formed when 3.0 × 10-3 mol of propene undergoes incomplete combustion?

2C3H6 + 3O2 ➔ 6C + 6H2O

  A  

9.0 × 10-3

  B  

3.6 × 10-2

  C  

1.08 × 102

  D  

2.16 × 102

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Question 14

The equation for the reaction between zinc and hydrochloric acid is

Zn + 2HCl ➔ ZnCl2 + H2

What is the minimum mass, in mg, of zinc (Ar = 65.4) needed to react with 50.0 cm3 of 1.68 mol dm-3 hydrochloric acid?

  A  

2.75 

  B  

5.49

  C  

2.75 × 103

  D  

5.49 × 103

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Question 15

A student is provided with 5.00 cm3 of 1.00 mol dm-3 ammonia solution. The student was asked to prepare an ammonia solution with a concentration of 0.050 mol dm-3

What volume of water should the student add?

  A  

45.0 cm3

  B  

95.0 cm3

  C  

100 cm3

  D  

995 cm3

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Question 16

Nitration of 1.70 g of methyl benzoate (Mr = 136.0) produces methyl 3-nitrobenzoate (Mr = 181.0). The percentage yield is 65.0%

What mass, in g, of methyl 3-nitrobenzoate is produced?

  A  

0.830

  B  

1.10

  C  

1.47

  D  

2.26

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Question 17

In an experiment to identify a group 2 metal (X), 0.102 g of X reacts with an excess of aqueous hydrochloric acid according to the following equation.

X + 2HCl ➔ XCl2 + H2

The volume of hydrogen gas given off is 65 cm3 at 99 kPa pressure and 303 K.

The gas constant is R = 8.31 J K–1 mol–1.

Which is X?

  A  

barium

  B  

calcium

  C  

magnesium

  D  

strontium

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Question 18

When heated, a sample of potassium chlorate(V) (KClO3) produced 67.2 cm3 of oxygen, measured at 298 K and 110 kPa

2KClO3(s) ➔ 2KCl(s) + 3O2(g)

What is the amount, in moles, of potassium chlorate(V) that has decomposed?

The gas constant, R = 8.31 J K–1 mol–1.

  A  

9.95 × 10-4

  B  

1.99 × 10-3

  C  

2.99 × 10-3

  D  

4.48 × 10-3

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Question 19

Which sample, measured at room temperature and pressure, contains the greatest number of the stated particles?

  A  

1 g of hydrogen molecules

  B  

1 g of helium atoms

  C  

1 dm3 of hydrogen molecules

  D  

1 dm3 of helium atoms

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Question 20

5.0 g of an oxide of molybdenum contain 4.0 g of molybdenum.

What is the empirical formula of this oxide?

  A  

MoO2

  B  

Mo4O5

  C  

Mo2O3

  D  

Mo3O2

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Question 21

What is the percentage yield when 20 g of aluminium are produced from 50 g of aluminium oxide?

2Al2O3 ➔ 4Al + 3O2

  A  

76%

  B  

40%

  C  

33%

  D  

19%

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Question 22

What is the effect on the volume when the pressure of an ideal gas is doubled at the same time as the temperature (in K) is doubled?

  A  

halved

  B  

remains the same

  C  

doubled

  D  

quadrupled

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Question 23

The general gas equation can be used to calculate the Mr value of a gas.

For a sample of a gas of mass mg, which expression will give the value of Mr?

Mr =RTmpV
Mr =mpVRT
Mr =pVmRT
Mr =mRTpV

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