Have you ever thought about how a hot-air balloon goes from being on the ground to floating high in the sky with just the pull of a cord? Gases respond in predictable ways to changes in pressure, temperature and volume. In a hot-air balloon, the burners raise the temperature of the air inside the balloon to keep it aloft. A respiratory care practitioner must have an understanding of physical theories and laws and be able to relate them to clinical practice. Whether it’s operating medical equipment or delivering medications you must understand how physical principles apply to respiratory care and how they are related to clinical practice as well as the physiologic implication they have on the body.
Robert Boyle, an Irish chemist, was able to illustrate through experiments he designed, the relationship between the pressure and the volume of a gas. Boyle’s law states that the volume of a fixed amount of gas held at a constant temperature varies inversely with the pressure. He was able to show that if the temperature and the amount of gas are constant, that increasing the pressure decreases the volume. Boyle’s law can be expressed mathematically as follows:
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Get Help Now!P1V1=P2V2
P represents pressure.
V represents volume
Jacques Charles, a French physicist, studied the relationship between volume and temperature. He observed that as temperature increases, so does the volume of a gas sample when the amount of gas and the pressure remain constant. As temperature increases, gas particles move faster, striking the walls of their container more frequently and with greater force. Because pressure depends on the frequency and force with which gas particles strike the walls of their container, this would increase the pressure. In order for pressure to remain constant, volume must increase so that the particles have farther to travel before striking the walls. Having to travel farther decreases the frequency with which the particles strike the walls of the container maintaining a constant pressure.
Charles’s law states that the volume of a given amount of a gas is directly proportional to its Kelvin temperature at constant pressure. Charles’s law can be expressed as follows:
V1 = V2
T1 T2
Pressure is a direct result of collisions between gas particles and the walls of their container. An increase in temperature increases collision frequency and energy, so raising the temperature should also raise the pressure if the volume is not changed. Joseph Gay-Lussac (1778-1850) found that a direct proportion exists between Kelvin temperature and pressure. Gay-Lussac’s law states that the pressure of a fixed amount of gas varies directly with the Kelvin temperature when the volume remains constant. Therefore, as temperature increases, pressure also increases as long as the amount of gas and the volume remains constant. Gay-Lussac’s law can be expressed mathematically as follows:
P1 = P2
T1 T2
What’s the main idea? The main idea is that for a fixed amount of gas, a change in one variable – pressure, temperature, or volume – affects the other two.
Let’s look at the clinical application of these laws to the practice of respiratory therapy. Let’s take a look at Boyle’s law first. You take a breath about 20 times per minute, exchanging carbon dioxide gas for life-sustaining oxygen. How do pressure and volume change in your lungs as you breathe?
The spongy, elastic tissue that makes up your lungs allows them to expand and contract in response to movement of the diaphragm, a strong muscle beneath the lungs. As your diaphragm moves downward, the pressure within your thoracic cavity decreases resulting in lung volumes increasing, this is called inhalation. As your diaphragm moves upward, the pressure becomes greater or increases resulting in your lung volumes decreasing, this is called exhalation.
Let’s take a look at Charles’s law. A helium balloon in a closed car occupies a volume of 3.2 L at 42 degrees C. If the car is parked on a hot day and the temperature inside rises to 87degrees C, how will the volume of the balloon be affected, assuming the pressure remains constant?
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The post Have you ever thought about how a hot-air balloon goes from being on the ground to floating high in the sky with just the pull of a cord? Gases respond in predictable ways to changes in pressure, temperature and volume. In a hot-air balloon, the burners raise the temperature of the air inside the balloon to keep it aloft. A respiratory care practitioner must have an understanding of physical theories and laws and be able to relate them to clinical practice. Whether it’s operating medical equipment or delivering medications you must understand how physical principles apply to respiratory care and how they are related to clinical practice as well as the physiologic implication they have on the body. appeared first on My Nursing Papers.
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