Ideal Gas Law: PV=nRT
Density: d=m/V
Molar mass: M=m/n
The molar mass of oxygen gas (O2) is 32.00.
PV=nRT
PV=mRT/M
m/V=PM/RT
d=PM/RT
d=(2atm)(32g/mol)/[(.08206atmL/Kmol)(400K)]
d=1.95g/L
Total pressure = ppO2 + ppH2 + ppN2ppN2 = Total pressure - (ppO2 + ppH2)ppN2 = 282 kPa - (110+106 kPa) = 282kPa - 216kPappN2 = 66 kPa = partial pressure of nitrogen
As the altitude increases, the density of oxygen decreases.
Yes, every substance has density.
Oxygen - Atomic Mass: 15.9994.
The vapour density of equimolar mixture of methane and oxygen is 0.0831 lbm/ft3.
why is the temperature and the pressure important when giving the density of oxygen and nitrogen
P02 is the partial pressure that oxygen exerts on a vein, artery or any other blood vessel.
This treatment involves placing the patient in a chamber breathing 100% oxygen at a pressure of more than one atmosphere (the normal pressure the atmosphere exerts at sea level). The increased pressure forces more oxygen into the blood.
there is oxygen depending on the air density of pressure divided by the quantity of air mass.
because of the density of the air and the pressure
Capillary density within tissues varies directly with tissues' rates and metabolism.
The percentage of oxygen in the air is for the most the same in the entire atmosphere.It is only in the very high altitudes that the percentage of oxygen actually diminishes. This because it is heavier than the helium and hydrogen that is up there.What matters however is the pressure of the air.At high altitude you breathe less oxygen because pressure is lower.At low altitude you breathe more oxygen due to higher pressure.The pressure of the atmosphere drops by approximately 50% every 18.000 feet (5.600 Meters, 5.6 Kilometer's)Oxygen, being a gas, exerts a partial pressure, which is determined by the prevailing environmental pressure. At sea level, the atmospheric pressure is 760mmHg, and oxygen makes up 21% (20.094% to be exact) of inspired air: so oxygen exerts a partial pressure of 760 x 0.21 = 159mmHg.The partial pressure does not actually change much at all with altitude since the percentage of oxygen remains the same.Our body however (with altitude) utilizes less oxygen because there is less of it and this effectively reduces partial pressure of oxygen in our bodies.Read more on related link down below.
Oxygen sensor
Total pressure = ppO2 + ppH2 + ppN2ppN2 = Total pressure - (ppO2 + ppH2)ppN2 = 282 kPa - (110+106 kPa) = 282kPa - 216kPappN2 = 66 kPa = partial pressure of nitrogen
Oxygen is a gas under normal conditions and so has no hardness or luster. The melting or freezing point of oxygen at standard temperature and pressure is 54.36 K ​(−218.79 °C, ​−361.82 °F) The density of oxygen gas at standard temperature and pressure is 1.429 g/L. the density of liquid oxygen at its boiling point (−182.962 °C or ​−297.332 °F) is 1.141 g/cm3. The atomic weight is about 15.999 Oxygen as a gas has no color. As a liquid it is a light blue.
Density of oxygen is 1.429 (g/cm3)
At standard temperature and pressure it is approx 1.3*10-3 grams per mL.