Gas Laws Flashcards

1
Q

What is meant by a volatile liquid?

A

A liquid with a low boiling point.

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2
Q

In an experiment to determine the relative molecular mass of a volatile liquid, describe how would you carry out the experiment describe how you measured the mass, volume and temperature.

A

Mass: Get the mass of flask and foil, add liquid and arrange as in diagram. Heat until liquid is vaporised. Cool and reweigh and get mass of the sample by subtraction.
Volume: Fill the flask and empty into graduated cylinder
Temperature: Use thermometer to read the temperature of the water.

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3
Q

In an experiment to determine the relative molecular mass of a volatile liquid, how many the pressure be measured?

A

With a barometer

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4
Q

State Avogadro’s law.

A

This states that equal volumes of gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.

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5
Q

What is an ideal gas?

A

A gas that obeys all gas laws at all temperatures and pressures.

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6
Q

State one reason why ammonia deviates from ideal gas behaviour.

A

As it is polar.

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7
Q

What is an ideal gas?

A

A gas that obeys all gas laws at all temperatures and pressures.

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8
Q

Give one reason why a real gas like carbon dioxide deviates from ideal behaviour.

A

As collisions are not perfectly elastic.

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9
Q

State Avogadro’s law.

A

This states that equal volumes of gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.

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10
Q

Give one reason why carbon dioxide is more easily liquefied than helium.

A

Due to the stronger intermolecular forces.

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11
Q

State Avogadro’s law.

A

This states that equal volumes of gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.

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12
Q

Give two assumptions of the kinetic theory of gases.

A
  • The average kinetic energy of the particles is proportional to the absolute temperature i.e kelvin.
  • The collisions are elastic. There is no overall lose of energy as a result of collisions.
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13
Q

Give two reasons why real gases deviate from ideal gas behaviour.

A
  • There are forces of attraction between molecules.

- Collisions are not perfectly elastic as some energy can be lost to surroundings.

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14
Q

State Gay-Lussac’s Law of combining volumes.

A

This states that gases always react with each other in simple whole number ratios when the volumes are measured at the same temperature and pressure.

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15
Q

What is an ideal gas?

A

A gas that obeys all gas laws at all temperatures and pressures.

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16
Q

In the experiment to find the relative molecular mass of a volatile liquid, give an example of a liquid suitable for this experiment.

A

Methane / methanol

17
Q

In the experiment to find the relative molecular mass of a volatile liquid, describe how to determine the mass and the volume.

A

Mass: Weigh the flask, heat until all the liquid is vaporised, cool, dry and reweigh. The mass is the difference.
Volume: Fill the flask with water and empty into measuring cylinder.

18
Q

In the experiment to find the relative molecular mass of a volatile liquid, explain why the pressure of the vapour is the same as atmospheric pressure.

A

As the pinhole means that vapour is exposed to the air.

19
Q

In the experiment to find the relative molecular mass of a volatile liquid, explain why this method is unsuitable for non-volatile liquids.

A

As they do not vaporise easily.

20
Q

What modern instrumental technique could be used as a more accurate method to measure the relative molecular masses of volatile and non-volatile liquids as well as of solid and gaseous substances.

A

Mass spectrometer.