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Ratio of the Specific Heat Capacities at Constant Pressure and Volume for Real Gases

The ratioof the specific heat capacity at constant pressure,to that at constant volume, is found experimentally by some method and the results shown below.

Gas

Temp./°C

γ

Monatomic gases

 

 

Helium

0

1.63

Argon

0

1.67

Neon

19

1.64

Krypton

19

1.69

Xenon

19

1.67

Mercury vapour

310

1.67

 

 

 

Diatomic gases

 

 

Air (dry)

−79.3

1.41

Air (dry)

0–17

1.401/2

Air (dry)

500

1.36

Air (dry)

900

1.32

Hydrogen

4–17

1.407/8

Nitrogen

20

1.4

Oxygen

5–14

1.4

Carbon monoxide

1 800

1.3

Nitric oxide

1.39

 

 

 

Triatomic gases

 

 

Ozone

1.29†

Water vapour

100

1.33

Carbon dioxide

4–11

1.3

Carbon dioxide

300

1.22

Carbon dioxide

500

1.2

Ammonia, NH-3

50

1.31

Nitrous oxide, N-2 O

1.32

Nitrogen peroxide N-2 O-4

20

1.17

Sulphur dioxide S0-2

16–34

1.26

 

 

 

Polyatomic gases

 

 

Methane, CH4

20

1.31

Ethane, C2H6

20

1.2

Propane, C3H8

20

1.14

Acetylene, C2H2

20

1.24

Ethylene, C2H4

20

1.25

Benzene C6H6

20

1.4

Benzene C6H6

99.7

1.11

Chloroform CHCl3

24–42

1.11

CCl4

1.13

Methyl alcohol

99.7

1.26

Methyl bromide

1.27

Methyl chloride

19–30

1.28

Methyl iodide

1.29

Ethyl alcohol

53

1.13

Ethyl alcohol

99.8

1.13

Ethyl bromide

1.19

Ethyl chloride

22.7

1.19

Ethyl ether

12–20

1.02

Ethyl ether

99.7

1.11

Acetic acid

136.5

1.15

The value ofis a result of many factors. Theory says that the energy is distributed over all the energy states equally – vibrational, translational, rotational, and for large molecules there may be many vibrational energy states. Since(this equation only applies to ideal gases) we expect the ratioto decrease for large molecules.

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