Question 13 options: From the list of terms provided, copy and paste terms appro

Question

Question 13 options:

From the list of terms provided, copy and paste terms appropriated from the list into the blanks of the text passages that follow such that, upon completion, the text passages correctly identify and distinguish the gas laws that govern pulmonary physiology from one another.

Terms: 0.21, 21, 78, 760, altitude, blood, Boyle's, Dalton's, decimal, decreased, diaphragm, directly, external intercostal, Henry's, into, inverse, lowers, out of, oxygen, parasternal, partial, percent concentration, pressure, solubility, temperature, total, volume,

_________ law states that there is a/an ________ relationship between [listed alphabetically] the _________ of a gas and the ___________ of the gas. That is, an increase in one of the factors is associated with a decrease in the other factor and vice versa. Thoracic cavity size determines the volume of the air in the lungs. Thus, this law is fundamental to explaining why an increase in the thoracic cavity size due to expansion of the rib cage in the horizontal [front-to-back and side-to-side] directions via contraction of the ___________ and _________ muscles, (listed alphabetically) and vertical [up-and-down] direction via contraction of the ___________ causes a resultant decrease in intrapulmonary pressure, creating a pressure gradient that drives air _____________ the lungs. Conversely, it explains why when the size of the thoracic cavity is _________ by relaxing the muscles used during inspiration, the pressure of the gas in the lungs increases, exceeding atmospheric pressure, creating a pressure gradient that then forces air _________ the lungs.

________ law states that the _______ pressure of a mixed gas is equal to the sum of the ___________ pressures exerted by each of the individual gasses in the mix, which are exerted independent of one another. This law is important to pulmonary physiology because the atmospheric air we breath is a mixed gas that contains roughly __________% nitrogen and _______% oxygen. Moreover, according to Henry's law, it is the partial pressure of the oxygen in the air we breath that is the main determinant of how much of the air's oxygen we can drive into our blood and make available to the body. A gas's partial pressure can be calculated by multiplying the total pressure of the mixed gas by the gas's ____________ in the mixed gas. Thus, the partial pressure of oxygen, at sea level is determined by multiplying total atmospheric pressure at sea level - which equals ___________ millimeters of mercury (denoted mm Hg) by ________ - oxygen's percent concentration in atmospheric air, expressed as a ____________.

________ law actually states that the amount of gas we can drive into solution is _________ dependent upon 3 factors. These 3 factors are 1) the solubility of the particular liquid for the particular gas you are considering, 2) the temperature (more gas can be driven into liquids at lower temperatures than at higher temperatures) and 3) the partial pressure of the gas under consideration. In the body, the particular gas we are interested in driving into a fluid is __________ and the particular fluid we are interested in driving the gas into is our ___________. Because blood has a particular solubility for oxygen - and this is constant, and because the homeostatic mechanisms in the body keep body temperature relatively constant, this means the single most important factor that determines how much oxygen can be driven in to our blood is the partial pressure of the oxygen in the air we breath. At sea level - the partial pressure of oxygen in atmospheric air = 760 x 0.21 = 159 mm Hg. However, if one climbs to the peak of Mt. Everest, where the air is still a mixed gas that contains only ~21% oxygen, but the air there is 'thinner' i.e. there is just less of it up there, the total pressure of the gas drops to about 250 mm Hg, which significantly __________ the the partial pressure of oxygen and the amount of air that can be forced into the blood at that altitude. Thus this gas law explains why many individuals initially experience ____________ sickness when they vacation in the Rockies or the Swiss Alps but normally live at much lower elevations.

Explanation / Answer

__Boyle's_______ law states that there is a/an __inverse______ relationship between [listed alphabetically] the ____pressure_____ of a gas and the __volume_________ of the gas. That is, an increase in one of the factors is associated with a decrease in the other factor and vice versa. Thoracic cavity size determines the volume of the air in the lungs. Thus, this law is fundamental to explaining why an increase in the thoracic cavity size due to expansion of the rib cage in the horizontal [front-to-back and side-to-side] directions via contraction of the __external intercostal_________ and ___parasternal______ muscles, (listed alphabetically) and vertical [up-and-down] direction via contraction of the ____diaphragm_______ causes a resultant decrease in intrapulmonary pressure, creating a pressure gradient that drives air ___into__________ the lungs. Conversely, it explains why when the size of the thoracic cavity is __decreased_______ by relaxing the muscles used during inspiration, the pressure of the gas in the lungs increases, exceeding atmospheric pressure, creating a pressure gradient that then forces air _out of________ the lungs.

_Dalton's_______ law states that the _total______ pressure of a mixed gas is equal to the sum of the _partial__________ pressures exerted by each of the individual gasses in the mix, which are exerted independent of one another. This law is important to pulmonary physiology because the atmospheric air we breath is a mixed gas that contains roughly ____78______% nitrogen and __21_____% oxygen. Moreover, according to Henry's law, it is the partial pressure of the oxygen in the air we breath that is the main determinant of how much of the air's oxygen we can drive into our blood and make available to the body. A gas's partial pressure can be calculated by multiplying the total pressure of the mixed gas by the gas's _percent concentration___________ in the mixed gas. Thus, the partial pressure of oxygen, at sea level is determined by multiplying total atmospheric pressure at sea level - which equals ___760________ millimeters of mercury (denoted mm Hg) by ________ - oxygen's percent concentration in atmospheric air, expressed as a ___0.21_________.

_Henry's_______ law actually states that the amount of gas we can drive into solution is __directly_______ dependent upon 3 factors. These 3 factors are 1) the solubility of the particular liquid for the particular gas you are considering, 2) the temperature (more gas can be driven into liquids at lower temperatures than at higher temperatures) and 3) the partial pressure of the gas under consideration. In the body, the particular gas we are interested in driving into a fluid is _oxygen_________ and the particular fluid we are interested in driving the gas into is our __blood_________. Because blood has a particular solubility for oxygen - and this is constant, and because the homeostatic mechanisms in the body keep body temperature relatively constant, this means the single most important factor that determines how much oxygen can be driven in to our blood is the partial pressure of the oxygen in the air we breath. At sea level - the partial pressure of oxygen in atmospheric air = 760 x 0.21 = 159 mm Hg. However, if one climbs to the peak of Mt. Everest, where the air is still a mixed gas that contains only ~21% oxygen, but the air there is 'thinner' i.e. there is just less of it up there, the total pressure of the gas drops to about 250 mm Hg, which significantly __lowers________ the partial pressure of oxygen and the amount of air that can be forced into the blood at that altitude. Thus this gas law explains why many individuals initially experience __ altitude__________ sickness when they vacation in the Rockies or the Swiss Alps but normally live at much lower elevations.

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