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The Partial Pressure of Oxygen in ambient air in Denver (610mmHg) is 128.1mmHg.
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What is the particial pressure of oxygen?
The partial pressure of oxygen is a measure of the pressure exerted by oxygen in a mixture of gases. In atmospheric air at sea level, the partial pressure of oxygen is around 160 mmHg. The partial pressure of oxygen can also be calculated using the equation: partial pressure of oxygen = total pressure of gas mixture * mole fraction of oxygen gas in the mixture.
Why is the partial pressure of oxygen in tissue lower than the partial pressure of oxygen in the blood?
The partial pressure of oxygen in tissue is lower due to oxygen being delivered from the blood to the tissues for cellular respiration. As tissues consume oxygen for metabolic processes, the partial pressure decreases. Additionally, factors like distance from capillaries and tissue oxygen consumption rate impact the partial pressure of oxygen in tissues.
In a 2 liter container what is the partial pressure of oxygen?
The partial pressure of oxygen in a 2 liter container depends on the concentration of oxygen present in the container. If you know the concentration of oxygen in the container, you can use the ideal gas law to calculate the partial pressure. The formula is: partial pressure = concentration of oxygen x gas constant x temperature.
What partial pressure of oxygen is a scuba diver breathing if the total pressure is 6.3 ATM and 20 percent of the air is oxygen?
The partial pressure of oxygen can be calculated by multiplying the percentage of oxygen in the air by the total pressure. In this case, 20 percent of 6.3 ATM is 1.26 ATM. Therefore, the scuba diver is breathing oxygen at a partial pressure of 1.26 ATM.
A mixture of gases with a pressure of 800.0 mm Hg contains 60 percent nitrogen and 40 percent oxygen by volume What is the partial pressure of oxygen in this mixture?
The partial pressure of oxygen in the mixture can be calculated using Dalton's Law of partial pressures. First, convert the percentages to decimal form (60% = 0.60, 40% = 0.40). Then, multiply the total pressure of 800.0 mm Hg by the volume percentage of oxygen (0.40) to find the partial pressure of oxygen in the mixture. This gives a partial pressure of oxygen of 320.0 mm Hg.
What is the particial pressure of oxygen?
The partial pressure of oxygen is a measure of the pressure exerted by oxygen in a mixture of gases. In atmospheric air at sea level, the partial pressure of oxygen is around 160 mmHg. The partial pressure of oxygen can also be calculated using the equation: partial pressure of oxygen = total pressure of gas mixture * mole fraction of oxygen gas in the mixture.
Why is the partial pressure of oxygen in tissue lower than the partial pressure of oxygen in the blood?
The partial pressure of oxygen in tissue is lower due to oxygen being delivered from the blood to the tissues for cellular respiration. As tissues consume oxygen for metabolic processes, the partial pressure decreases. Additionally, factors like distance from capillaries and tissue oxygen consumption rate impact the partial pressure of oxygen in tissues.
Is there as much oxygen in the air in Denver as there is in Boston?
No, Denver has less oxygen in the air than Boston. This is because Denver is located at a higher altitude, which means the air is thinner and contains less oxygen molecules compared to lower altitude cities like Boston.
In a 2 liter container what is the partial pressure of oxygen?
The partial pressure of oxygen in a 2 liter container depends on the concentration of oxygen present in the container. If you know the concentration of oxygen in the container, you can use the ideal gas law to calculate the partial pressure. The formula is: partial pressure = concentration of oxygen x gas constant x temperature.
What is PC02?
partial pressure of oxygen
A pressurized tank contains a mixture of oxygen and helium.if the partial pressure of oxygen is 10atm and the partial pressure of helium is 32.8 ATM what is the total pressure inside the tank?
The total pressure inside the tank is the sum of the partial pressures of the gases present. In this case, Total pressure = partial pressure of oxygen + partial pressure of helium = 10 atm + 32.8 atm = 42.8 atm.
What partial pressure of oxygen is a scuba diver breathing if the total pressure is 6.3 ATM and 20 percent of the air is oxygen?
The partial pressure of oxygen can be calculated by multiplying the percentage of oxygen in the air by the total pressure. In this case, 20 percent of 6.3 ATM is 1.26 ATM. Therefore, the scuba diver is breathing oxygen at a partial pressure of 1.26 ATM.
How would gas exchange be affected at the top of a tall mountain where air pressure is lower and there is less oxygen then lower elevations?
At high altitudes, atmospheric pressure is lower. Therefore, the partial pressure (partial oxygen) is lower. As partial pressure of oxygen goes down, the body's desire for oxygen goes up.
How would gas exchange be affected at the top of a tall mountain where air pressure is lower and there is less oxygen then at lower elevations?
At high altitudes, atmospheric pressure is lower. Therefore, the partial pressure (partial oxygen) is lower. As partial pressure of oxygen goes down, the body's desire for oxygen goes up.
What is the partial pressure of CO2 in the arterial and venous blood?
The normal partial pressure of oxygen in arterial blood is 75-100 millimeters of mercury. In comparison the partial pressure of oxygen at sea level is 750 millimeters of mercury.
A mixture of gases with a pressure of 800.0 mm Hg contains 60 percent nitrogen and 40 percent oxygen by volume What is the partial pressure of oxygen in this mixture?
The partial pressure of oxygen in the mixture can be calculated using Dalton's Law of partial pressures. First, convert the percentages to decimal form (60% = 0.60, 40% = 0.40). Then, multiply the total pressure of 800.0 mm Hg by the volume percentage of oxygen (0.40) to find the partial pressure of oxygen in the mixture. This gives a partial pressure of oxygen of 320.0 mm Hg.
In deoxygenated blood is the partial pressure of carbon dioxide is greater than the partial pressure of oxygen left?
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