Chapter 10 - Properties Of Gases Flashcards

1
Q

Gas

A

A substance that has no well-defines boundaries but diffusés rapidly to fill any container in which it is placed

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2
Q

Which diffusés quicker between ammonia and hydrogen chloride

A

Lighter ammonia molecules diffuse quicker than heavier hydrogen chloride molecules

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3
Q

Properties of Gases

A

No fixed volume - take volume of container

Volume depends on temperature and pressure

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4
Q

Temperature

A

Measure of the degree of hotness of an object

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5
Q

0°C is equal to

A

273K

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6
Q

Pressure of a gas

A

The force the gas exerts on a unit area

Newtons per metre squared or pascals

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7
Q

1kPa is equal to

A

1000 Pa

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8
Q

Normal atmospheric pressure

A

100kPa

100,000 Pa

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9
Q

1 litre is equal to

A

1000cm^3

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10
Q

Standard Temperature

A

273K

0°C ~ freezing point

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11
Q

Standard pressure

A

100,000 Pa

100 kPa

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12
Q

Boyle’s Law

A

At constant temperature, the volume of a fixed mass of gas is inversely proportional to its pressure

pV=k

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13
Q

Charles’ Law

A

At constant pressure, the volume of a fixed mass of gas is directly proportional to its temperature measured on the Kelvin Scale

k = V/T

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14
Q

Combined Gas Law

A

p1V1 = p2V2
–––– –––––
T1 T2

  • Convert to Kelvin
  • Consistent units
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15
Q

Gay-Lussac’s Law of Combining Volumes

A

In a reaction between gases,
The ratio between the volumes of the reactant gases
and the gaseous products
can be expressed in simple whole numbers
Provided the volumes are measured at the same temperature and pressure

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16
Q

Avogadro’s Law

A

Equal volumes of gases contain equal numbers of molecules under the conditions of temperature and pressure

17
Q

One mole of a gas occupies

A

22.4L

18
Q

Assumptions of the Kinetic Theory of Gases

A
  • Gases are made up of particles in continuous rapid, random motion
  • No attractive or repulsive forces between the molecules of a gas
  • Gas molecules are so small and widely separated that the volume of all the molecules is tiny compared to the spec they occupy
  • The collisions are perfectly elastic
  • Average kinetic energy of molecules is proportional to temperature on Kelvin scale
19
Q

Limitations of the Kinetic Theory of Gases

A
  • All real gases DO have tiny attractive forces between the molecules .e.g. ammonia
  • Under high pressure when molecules are crowded together, the volume is not tiny compared to the distance between them
20
Q

Ideal gas

A

One that perfectly obeys all the assumptions of the kinetic theory of gases under all conditions of temperature and pressure

21
Q

Real gases

A

Forces of attraction and repulsion do exist between the molecules

The volume of the molecules is not negligible

22
Q

Rapid movement of tiny particles in a liquid or gas

A

Brownian motion

23
Q

When do gases depart from ideal behavior

A

High pressure and low temperatures, molecules are close together and moving slowly