Properties of Carbon Dioxide Vapour
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Published: Mon, 11 Sep 2017
- Greenhouse gases in global warming
The greenhouse effect is necessary for Earth to regulate its temperature. Water vapour (H2O), carbon dioxide (CO2) methane (CH4), nitrous dioxide (N2O) and ozone (O3) are some of the gases that contribute to it. These gases are molecules that are made up of more than 2 component atoms. They vibrate upon absorbing thermal infrared radiation and then re-radiate excess energy in all directions. As the Earth’s surface is now heated by both the emitted radiation and sunlight, temperature increases and thus causing the greenhouse effect.
Common Greenhouse Gases
Greenhouse Gas Atmospheric
Absorption Region on Electromagnetic (Âµm)
Water vapour (H2O)
Carbon dioxide (CO2)
2.6, 4, >13
3.5 – 8
Nitrous oxide (N2O)
As shown in the table above, water vapour (H2O) contributes the most to the greenhouse effectWhen temperature increases, air humidity increases as well which is positive water vapour feedback. This allows a higher concentration of CO2 in the atmosphere thus further enhancing the warming effect of other greenhouse gases.
Carbon dioxide (CO2) contributes quite a fair amount to the greenhouse effect. Thanks to human activities like deforestation, land use changes and burning of fossil fuel, the atmospheric CO2 concentration has increased by about 120ppm since the Industrial Revolution began, which is more than a third.
With an absorption region of 3.5-8 microns on the electromagnetic spectrum, methane (CH4) is way more active than carbon dioxide as a greenhouse gas. Its greenhouse effect contribution is small due to its low atmospheric concentration. Being in a similar absorption spectrum as H2Oalso masks methane’s contribution as work might have been done by H2O already.
Nitrous oxide(N2O) is typically formed through production of nitric acid, combustion of fossil fuel, agriculture sector and burning of . Even though N2O has a low atmospheric concentration, it still contributes a decent amount to the greenhouse effect. This is because it is up to about 300 times stronger as a greenhouse gas than CO2.
As ozone (O3) has various concentration at different parts of the atmosphere and has a short lifespan, it is hard to gauge the contribution of the troposphere ozone layer. Ozone generally does not affect much of the greenhouse effect anyway.
- Lewis Structures of CO and CO2
- Carbon Monoxide
a) Rotational Constant, B
Taking largest B = 2.04 and smallest B = 1.51 ,
b) Bond Length, b
Reduced mass of carbon monoxide:
Since literature value for bond length, b = 113pm lies within the range of , and the uncertainty of calculated bond length value is insignificant compared to the calculated value itself, the calculated value can be said to be quite accurate.
c) Vibrational Wavenumber,
Distance of first through in P branch from 2050 cm-1= (5.45 Â± 0.05) cm
Distance of first through in R branch from 2050 cm-1= (5.72 Â± 0.05) cm
Taking smallest = 2135 and largest = 2143,
d) Force Constant, k
e) Molar Zero-Point Vibrational Energy,
- Rotational Constant,
Taking smallest = 0.302 cm-1 and largest = 0.46 cm-1,
Since literature value for = 0.390 lies within the range of , and the uncertainty of calculated bond length value is insignificant compared to the calculated value itself, the calculated value can be said to be quite accurate.
- Vibrational Modes
CO2 is a linear molecule with 3 atoms. Therefore, it has 3 translational modes, 2 rotational modes, and 3N-5 = 4 vibration modes: 1 symmetric stretch, 1 asymmetric stretch and 2 bending modes. The mode at 667 cm-1 is said to be twofold degenerate because the 2 bending motions are essentially the same, just deforming in different coordinate directions.
Exclusion Rule: no modes can be both infrared and Raman active for a molecule with a centre of symmetry. CO2 has a centre of symmetry therefore relevant to the rule.
For infrared spectroscopy, the 2 bending and the asymmetric stretching modes can be observed. This is because these modes induce a dipole change in their motions. For Raman spectroscopy, symmetric bending can be seen. This is because when the O atoms move away from the centre C atom in an equal distance, the electron density cloud changes with the change in size of molecule, thus causing a change in polarizability.
- Bond Length, b & Force Constant, k
Since literature value for lies within the range of (119.6Â±12.5)pm, and the uncertainty of calculated bond length value is insignificant compared to the calculated value itself, the calculated value can be said to be quite accurate.
For symmetric stretch,
k CO2 < k CO because the carbon-oxygen triple bond in CO is stiffer than the carbon-oxygen double bond in CO2.
- Molar constant-volume heat capacity
For CO2: Translational modes, : , Vibrational modes, : ,
Rotational mode, :
Total internal energy,
At very high temperatures, the theoretical maximum internal energy = as all modes are activated at that point.
Max. constant-volume heat capacity,
However, at low temperatures not all rotational and vibrational modes are active.
Contributions of different modes at low temperatures:
Symmetric stretch () :
Bending modes () :
Asymmetric stretch () :
- Graph of against T
Convert molar constant-volume heat capacity to molar constant-pressure heat capacity with Ideal Gas Law: , (R = ideal gas constant)
The graph for experimental and calculated data is the same until around T=1600K where the 2 lines diverge with the experimental data to be higher than calculated data. This shows that the Ideal Gas Law only applies to relatively low temperatures.
Kinetic Theory of Gases and Liquids
- Mean free path of CO2
Mean free path: average distance travelled by molecules between collisions
Rate of collision , : Collision cross-section (area covered by a molecule and within which the presence if the centre of another molecule counts as a collision)
Collisions happen at 90o angles on average, mean speed = ïƒ .
- Viscosity of CO2 vapour
Newton’s Law of Viscosity:
Newton’s 2nd Law: Force = rate of change of momentum
- From plane at 0 from plane :
mean flow velocity = ïƒ mean momentum of
- Roughly1/6th of the molecules move in the +z direction.
- Number of molecules entering 0 from per unit time = ïƒ rate of momentum =
- Rate of momentum entering 0 from = . By calculating the difference between the two rates, net rate of the momentum transported across the plane at 0, and by using , the viscosity, can be estimated. 
(mean velocity), (path length)
Viscosity is predicted to be proportional to the square root of temperature and independent of density.
Liquefaction in a condenser
Modify the Ideal Gas Law to obtain Van der Waals Equation of State.
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