LITMIR.BIZ

Figure 4‐5 A typical absorption spectrum.

      The total energy of a molecule in a specific energy state can be summarized by the approximation

      (4‐4)

The fact that transitions can occur between many of these states implies that energy will be absorbed at many different wavelengths. This gives rise to an absorption spectrum that typifies a molecule. As an example, Figure 4‐7 illustrates the vibrational–rotational absorption spectrum of SO₂ in the near‐infrared region. Such spectra are very important in the development of analytical techniques for gas monitoring.

Also, Figure 4‐2 shows that different molecules can absorb light in the same region of the spectrum. This can cause problems in developing an analyzer because it can be difficult to distinguish the relative amounts of absorption from each compound in the overlap region. Water vapor can be particularly troublesome because it absorbs in many regions of the infrared spectrum and is usually present at percent levels in the gas stream, whereas pollutant gases are present at ppm levels. Interfering gases can be removed before entering an analyzer, but this can be difficult and makes the monitoring system more complicated. An alternative to removing interfering gases is to select a region of the spectrum where there is no overlap. The wavelength‐specific light emitted by lasers has enabled a wide variety of instruments to be developed using this technique. High‐resolution instruments, once found only in the laboratory, provide another alternative. Advances in computerization along with advances in the science and technology of gas measurement have since made relatively sophisticated measurement techniques available to field instruments at reasonable cost. Different approaches to such problems are discussed further in the following chapters.

Figure 4‐6 Energy‐level diagram for a molecule.

      To this point we have discussed the fact that molecules can absorb light energy. However, the question arises as to how this phenomenon can be expressed quantitatively. The answer lies in a mathematical expression known as the Beer–Lambert law.

      The Beer–Lambert Law

When studying the absorption of light by gases, the Beer–Lambert law can be used to relate the amount of light absorbed to the concentration of the pollutant gas. First, consider the system shown in Figure 4‐8, which is composed of a light source, flue gas, and a sensor that measures light intensity.

The intensity of light passing through a stack (or sample cell) will decrease if gas molecules in the cell become “excited,” that is, if the light embodies wavelengths causing energy transitions in the molecule. Light transmittance, Tr, is the fraction of incident light passing through the cell. This can be expressed as the ratio of the light intensity transmitted through the cell, I, to the initial incident light intensity, I_o, (or the intensity with no absorbing material in the stack or cell), or:

Figure 4‐7 Infrared vibrational–rotational transmittance spectrum for SO₂.

Figure 4‐8 Example system for measuring pollutant gas concentrations.

      (4‐5)

      The Beer–Lambert law states that the transmittance of light through the medium decreases exponentially by the product α(λ) cL, or

      (4‐6)

      where

       Tr = the transmittance of the light through the flue gas

       Io = the intensity of the light entering the gas/s

       I = the intensity of the light leaving the flue gas/s

       α(λ) = molecular absorption coefficient (dependent on wavelength)

       c = concentration of the pollutant

       l = distance the light beam travels through the flue gas

      The Beer–Lambert law relates light absorbance in a medium, A = α(λ)cl, to the distance the light travels in the medium and the concentration of the light‐absorbing (and or light scattering) species.

      [Note: In the conventions of International Union of Pure and Applied Chemistry (IUPAC), the fraction of light not transmitted is

Скачать книгу