Question 1

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 2

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 3

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 4

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 5

Metals are good conductors of electricity because

  A  

metal atoms are arranged in a regular lattice

  B  

metal ions are very close to each other

  C  

metal ions are free to move through the lattice

  D  

electrons are free to move through the lattice

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Question 6

The melting temperature of sodium is lower than the melting temperature of magnesium. The best explanation for this is

  A  

sodium atoms are smaller than magnesium atoms

  B  

sodium ions have a larger charge density than magnesium ions

  C  

the repulsion between the ions in sodium is less than in magnesium

  D  

the number of delocalised electrons per atom is fewer in sodium than in magnesium

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Question 7

Which statement about ideal gases is correct?

  A  

ideal gases have finite particle volume and no intermolecular forces of attraction

  B  

ideal gases have finite particle volume and weak intermolecular forces of attraction

  C  

ideal gases have zero particle volume and no intermolecular forces of attraction

  D  

ideal gases have zero particle volume and weak intermolecular forces of attraction

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Question 8

Which would behave the least like an ideal gas at room temperature?

  A  

carbon dioxide

  B  

helium

  C  

hydrogen

  D  

nitrogen

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Question 9

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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Question 10

Which gas closely approaches ideal behaviour at room temperature and pressure?

  A  

ammonia

  B  

carbon dioxide


  C  

helium

  D  

oxygen

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Question 11

What is a basic assumption of the kinetic theory, as applied to an ideal gas?

  A  

collisions between gas molecules are elastic

  B  

each gas molecule occupies a finite volume

  C  

gases consist of particles that experience the force of gravity

  D  

gas molecules attract each other with weak intermolecular forces

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Question 12

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 13

Which set of elements in the solid state contain a simple molecular lattice, a giant covalent lattice and a giant metallic lattice?

  A  

S, Si, Al

  B  

P, Si, C

  C  

S, P, Si

  D  

Mg, P, S

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Question 14

Which statement about the molecules in a sample of a gas is correct?

  A  

at a given temperature they all move at the same speed

  B  

at a given temperature their average kinetic energy is constant

  C  

as temperature increases, there are more molecules with the most probable energy

  D  

as temperature decreases, there are fewer molecules with the mean energy

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