How do you calculate the density of oxygen gas (O2) at 30 degree C. and 700 mmHg?
The volume is 0,446 L.
The partial pressure of oxygen in expired air is 109 mmHg. Partial pressure is calculated at the proportion of oxygen in the air, so at 1 atmosphere for dry air pressure is 713 mmHg (which is 760 total pressure - 47 mmHg water vapor) and oxygen is 21% of the dry gas concentration so inspired pO2 is 150 mmHg.
4.5 ATM (760 mmHg/1 ATM) = 3,420 mmHg
These three components are the three largest components of air. The total pressure of a gas mixture is just the sum of the partial pressures of each component. Air is a mixture and nitrogen, oxygen, and argon are the three biggest components. So, the atmospheric pressure (or air pressure) would be the sum of the partial pressure of each component of the air: Ptot=PPnitrogen + PPoxygen+ PPargon = 442 mmHg + 118.34 mmHg + 5.66 mmHg = 566 mmHg
4.5 ATM (760 mmHg/1 ATM) = 3,420 mmHg
How To Calculate The Density Of Oxygen Gas ,O2, At 30 Deg. C And 700 MmHg
About 20%% of the air we breath is oxygen. The PaO2 (oxygen breathed in mmhg) is approximately 100 mmhg.
The volume is 0,446 L.
270 mmHg.
The density is approx. 1,2 g/L.
The partial pressure of oxygen in expired air is 109 mmHg. Partial pressure is calculated at the proportion of oxygen in the air, so at 1 atmosphere for dry air pressure is 713 mmHg (which is 760 total pressure - 47 mmHg water vapor) and oxygen is 21% of the dry gas concentration so inspired pO2 is 150 mmHg.
blood entering the lungs has a partial pressure of oxygen (PO2) of 40 mmHg and a partial pressure of carbon dioxide (PCO2) of 46 mmHg; alveoli, on the other hand, have a PO2 of 105 mmHg and a PCO2 of 40 mmHg. As the blood moves past the alveoli, oxygen and carbon dioxide will diffuse down their respective partial pressure gradients. Oxygen will move from the alveolar space (PO2 of 105 mmHg) to the blood stream (PO2 of 40 mmHg). Carbon dioxide will move from the blood (PCO2 of 46 mmHg) to the alveolar space (PCO2 of 40 mmHg). As the blood leaves the alveolus, the PO2 and PCO2 will have essentially equilibrated with the alveolar air.
Convert all the pressures into one unit and then, using Dalton's Law of Partial Pressure, you just add all the pressures together. Using these conversions(101325Pa equals 1 ATM, 1 ATM equals 760 mmHg, 1 mmHg equals 1 torr), calculate each pressure into one unit(I used mmHg) 1013000 Pa nitrogen equals 7598 mmHg of nitrogen(make sure you round using sig figs) 700 mmHg of argon equals 700 mmHg of argon 1.20 ATM of helium equals 912 mmHg of helium 790 torr oxygen equals 790 mmHg of oxygen 0.50 ATM of carbon dioxide equals 380 mmHg of Carbon Dioxide Now add all the pressures and you get: 7598+700+912+790+380= 10380 mmHg If you need to have the answer in a particular unit: 10380 mmHg = 10380 torr = 13.66 ATM = 1384000 Pa = 1,384 kPa
40 mmHg
Personally, I would go from mmHg to Atm which the conversion factor is 760mmHg/1Atm. From there, go to kPa which is 101.325KPa/1Atm. Your answer should come out to be 60.43KPa.
The density of hydrogen is 0,08988 g/L at 20 oC and 760 mmHg.
The partial pressure of oxygen will vary according to where you look. Atmospheric oxygen partial pressure is approximately 21% of the atmospheric pressure of the location at which you measure (typically around 1 atmosphere at sea level, making the partial pressure of oxygen at seal level 0.21 ATM or 21.3KPa). The value varies geographically and with time, but also varies in different tissues of organisms, since not all oxygen available is absorbed, and complex multicellular organisms will have certain tissues (respiring muscle) that use up oxygen, resulting in a lower partial pressure there.normal oxygen partial185.4 kPa or in another unit:100 mmHg in the arterial blood. The partial pressure on the alveolar site is about 105 mmHg.