Boyle's Dalton's and Henry's Laws Term Paper

Excerpt from Term Paper :

relationship among Boyle's, Dalton's, and Henry's Laws and the physiology of the lung. Robert Boyle investigated the relationship between the volume of a dry ideal gas and its pressure. Since there are four variables that can be altered in a gas sample, in order to investigate how one variable will affect another, all other variables must be held constant or fixed. Boyle fixed the amount of gas and its temperature during his investigation. He found that when he manipulated the pressure that the volume responded in the opposite direction. For example, when Boyle increased the pressure on a gas sample, the volume would decrease.

A physiological example of Boyle's Law is the action of the diaphragm. This muscle is located just below the lungs. When one inhales, the diaphragm moves downward allowing the lungs an increased volume. Consequently, this decreases the pressure inside the lungs so that the pressure is less than the outer pressure. As a result, air is forced into the lungs. When one exhales, the diaphragm moves upward and decreases the volume of the lungs. This increases the pressure inside the lungs above the pressure on the outside of the lungs so that gases are forced out of the lungs. Pathologic conditions such as acute diaphragmatic injury may result in respiration difficulties due to incomplete ventilatory volumes.

John Dalton studied the effect of gases in a mixture. He observed that the total pressure of a gas mixture was the sum of the partial pressure of each gas as illustrated below:

Pressure (P) total = P1 + P2 + P3 + Pn

The partial pressure is defined as the pressure of a single gas in a mixture. Dalton maintained that since there was an enormous amount of space between gas molecules within a mixture, the gas molecules had…

Sources Used in Document:

REFERENCES

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West, J.B. (1999). The original presentation of Boyle's law. J Appl Physiol, 87(4), 1543-1545.

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