Naturally, human beings were not meant to fly like the birds. However, it is not easy for man to accept this fact. While air transport brought about much advancement to mankind, its security has been faced by numerous challenges. The changes in pressure as a result of changing altitudes in the course of flight have several effects on the human body. The effects of changing altitude on the human body can be explained using various gas laws. These gas laws include Boyles law, Charless law, Daltons law and Henrys law. These gas laws are more significant in aero medical transport where the health of the passenger is in critical conditions making the passenger more susceptible to changes in the cabin pressure especially if they have respiratory complications. The equipments used by the medical personnel are also affected by the changing environment. Understanding the effect of the changing environment by the cabin crew and the aero medical personnel is essential in order to reduce the effects of changing environment on the patient and the medical equipments (Hurd and Jernigan, 2003).
Henrys law of gases states that, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid at constant temperature and volume of liquid. In other words the amount of gas that can dissolve in a certain volume of a liquid is determined by the pressure of the gas above the liquid provided the temperature remains constant. Therefore, if the partial pressure of the gas above a liquid increases, the amount of gas dissolved also increases proportionally. Consequently, if the partial pressure of the gas above a liquid decreases, the amount of gas dissolved also reduce proportionally. A very good demonstration of the concepts of Henrys law of gases is opening a carbonated drink bottle. When the bottle is closed, the pressure above the liquid is slightly higher that the atmospheric pressure and therefore, more carbon dioxide gas is dissolved in the liquid. When the bottle is opened, some of the gases escape causing the pressure above the liquid decrease to atmospheric pressure. As the pressure reduces some of the dissolved gases in the liquid are also released in form of bubbles. The bubbling continues until equilibrium of the partial pressure of the gas above the liquid and the dissolved gas is attained (Hurd and Jernigan, 2003).
Henrys law of gases is very significant in air transport especially among the divers. The law leads to the development of a condition known as the bends. The law can be used to explain why hypoxia increases with increase in altitude (Hurd and Jernigan, 2003, pg 204). The increase in altitude leads to a reduction in the atmospheric pressure which has a negative effect on the amount of oxygen dissolved in the blood. Divers on the other hand are affected by changes in the atmospheric pressure where the rapid changes in pressure result in decompression sickness. The adverse effect of changes in the atmospheric pressure on security of air transport can however be reduced by restricting the altitudes for diver and commercial aircrafts.
Pressurized cabins also reduce problems related to gas pressures although it has some limitations such as increased weight of the aircraft, very advanced controls of gases is required and possible decompression hazards. It is also important to access the health of the passengers before flights to determine the possible effect of changes in the gas pressures (Hurd and Jernigan, 2003).
Henrys law of gases states that, the amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid at constant temperature and volume of liquid. In other words the amount of gas that can dissolve in a certain volume of a liquid is determined by the pressure of the gas above the liquid provided the temperature remains constant. Therefore, if the partial pressure of the gas above a liquid increases, the amount of gas dissolved also increases proportionally. Consequently, if the partial pressure of the gas above a liquid decreases, the amount of gas dissolved also reduce proportionally. A very good demonstration of the concepts of Henrys law of gases is opening a carbonated drink bottle. When the bottle is closed, the pressure above the liquid is slightly higher that the atmospheric pressure and therefore, more carbon dioxide gas is dissolved in the liquid. When the bottle is opened, some of the gases escape causing the pressure above the liquid decrease to atmospheric pressure. As the pressure reduces some of the dissolved gases in the liquid are also released in form of bubbles. The bubbling continues until equilibrium of the partial pressure of the gas above the liquid and the dissolved gas is attained (Hurd and Jernigan, 2003).
Henrys law of gases is very significant in air transport especially among the divers. The law leads to the development of a condition known as the bends. The law can be used to explain why hypoxia increases with increase in altitude (Hurd and Jernigan, 2003, pg 204). The increase in altitude leads to a reduction in the atmospheric pressure which has a negative effect on the amount of oxygen dissolved in the blood. Divers on the other hand are affected by changes in the atmospheric pressure where the rapid changes in pressure result in decompression sickness. The adverse effect of changes in the atmospheric pressure on security of air transport can however be reduced by restricting the altitudes for diver and commercial aircrafts.
Pressurized cabins also reduce problems related to gas pressures although it has some limitations such as increased weight of the aircraft, very advanced controls of gases is required and possible decompression hazards. It is also important to access the health of the passengers before flights to determine the possible effect of changes in the gas pressures (Hurd and Jernigan, 2003).
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