## Partial pressure

The pressure of a particular gas in a gaseous mixture is known as partial pressure of that gas. It is a measure of the concentration of a gas in a gaseous mixture and measured in mmHg or kPa. Like normal gas pressure, this pressure is also due to the impact of moving molecules against the wall of container. For example; in Oxygen constitutes 21 % of the atmospheric air, therefore its partial-pressure is 21 % of 760 that is 159 mmHg. Similarly the partial pressure of Nitrogen (78 %) in atmospheric air 78 % of 760 = 593 mmHg, for Carbon dioxide (0.04 %) it is 0.04 % of 760 = 0.3 mmHg. Please express your views of this topic Alpha Decay Equation by commenting on blog

Partial-pressure of gas can be written in the form of Partial Pressure Equation;

Pi = Xi P.....(a)

Where; Pi = partial pressure in pascals

xi = volume fraction or mole fraction of the gas in the mixture

P = total pressure

Let's discuss, How to Find Partial-Pressure of any gas present in a gaseous mixture by taking an example of pressure of carbon dioxide in a sample of dry air at sea-level is 101,325 Pa and volume fraction is 0.000285. Therefore the partial-pressure of CO2 would be;

Pi = 0.000285 x 101325 = 28.9 Pa

Partial pressure of any gas is the convenient way to determine the amount of gas present. All gases exert some pressure on the walls of their container due to their regular collisions with other molecules and wall of container. If there is only one gas in container, the total pressure would be the pressure of that gas only. However in the case of mixture of gases, it’s difficult to describe the pressure of gas, therefore this pressure is used. Generally Dalton’s law is used to calculate the partial amount of pressure of gaseous mixture which states that the total pressure of gaseous mixture is equals to the sum of the partial pressures of all of the gases in a mixture.

Gases dissolved in solution such as in blood can also described by using partial form of pressure. The partial-pressure of dissolved gas in blood is the partial-pressure that the gas would have. The main condition for that is the blood must allow equilibrating with a volume of gas.Is this topic What are Quarks hard for you? Watch out for my coming posts.

The total pressure (Pt) of gaseous mixture can be written as:

Pt = P1 + P2 +.....= n1RT1/V1 + n2RT2/V2+.............

At constant temperature and volume, equation can be written as;

Pt = P1 + P2 +.....= n1RT/V + n2RT/V+.............

Or Pt = P1 + P2 +.....= (n1 + n2 ) RT/V

Total moles in gaseous mixture nt is the sum of moles of all component of mixture;

nt= n1 +n2+......

Pt = nt RT/V

Therefore At constant temperature and volume, the total pressure of a gas sample can determine by the total number of moles of constituent gases present in mixture.

Partial-pressure of gas can be written in the form of Partial Pressure Equation;

Pi = Xi P.....(a)

Where; Pi = partial pressure in pascals

xi = volume fraction or mole fraction of the gas in the mixture

P = total pressure

Let's discuss, How to Find Partial-Pressure of any gas present in a gaseous mixture by taking an example of pressure of carbon dioxide in a sample of dry air at sea-level is 101,325 Pa and volume fraction is 0.000285. Therefore the partial-pressure of CO2 would be;

Pi = 0.000285 x 101325 = 28.9 Pa

Partial pressure of any gas is the convenient way to determine the amount of gas present. All gases exert some pressure on the walls of their container due to their regular collisions with other molecules and wall of container. If there is only one gas in container, the total pressure would be the pressure of that gas only. However in the case of mixture of gases, it’s difficult to describe the pressure of gas, therefore this pressure is used. Generally Dalton’s law is used to calculate the partial amount of pressure of gaseous mixture which states that the total pressure of gaseous mixture is equals to the sum of the partial pressures of all of the gases in a mixture.

Gases dissolved in solution such as in blood can also described by using partial form of pressure. The partial-pressure of dissolved gas in blood is the partial-pressure that the gas would have. The main condition for that is the blood must allow equilibrating with a volume of gas.Is this topic What are Quarks hard for you? Watch out for my coming posts.

The total pressure (Pt) of gaseous mixture can be written as:

Pt = P1 + P2 +.....= n1RT1/V1 + n2RT2/V2+.............

At constant temperature and volume, equation can be written as;

Pt = P1 + P2 +.....= n1RT/V + n2RT/V+.............

Or Pt = P1 + P2 +.....= (n1 + n2 ) RT/V

Total moles in gaseous mixture nt is the sum of moles of all component of mixture;

nt= n1 +n2+......

Pt = nt RT/V

Therefore At constant temperature and volume, the total pressure of a gas sample can determine by the total number of moles of constituent gases present in mixture.