Partial Pressure Help-Please Check

In summary, partial pressure is a measure of the individual pressure exerted by a gas in a mixture of gases and can be calculated by multiplying the total pressure by the mole fraction. It is important in determining gas behavior, such as diffusion and solubility, and has applications in fields like medicine, chemistry, and engineering. Increasing temperature leads to higher partial pressures according to the Ideal Gas Law.
  • #1
Nimmy
41
0
Partial Pressure Help---Please Check

The Partial Pressure of water vapor at T = 273 K is 6.11 mbar. Find the corresponding mass concentration of water vapor. Assume P = 1 atm.


So...

ρH20 = (PH20*MH20/(R*T)
ρH20= (6.11*10^2 Pa)*(18.01 g/mol)/(8.314*273 K)
ρH20 = 11004.11/2269.722 = 4.85 g/mol

Correct?
 
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  • #2


Essentially correct, yes -- except for the units. You can either (1) think about what the units associated with "mass concentration" should be, or (2) include the units in R=8.314___?, and work out the units in the calculation. I recommend trying both approaches, in the order given here.
 

1. What is partial pressure?

Partial pressure is a measure of the individual pressure exerted by a gas in a mixture of gases. It is proportional to the concentration of that gas and represents the contribution of that gas to the total pressure in the mixture.

2. How is partial pressure calculated?

Partial pressure can be calculated by multiplying the total pressure of the mixture by the mole fraction of the gas in question. The mole fraction is the ratio of moles of the gas to the total moles of all gases in the mixture.

3. Why is partial pressure important in gas mixtures?

Partial pressure helps to determine the behavior of gases in a mixture, such as their rate of diffusion and solubility in liquids. It is also used in various industrial processes, such as gas chromatography and gas blending for scuba diving.

4. How does temperature affect partial pressure?

In accordance with the Ideal Gas Law, increasing the temperature of a gas mixture will increase the average kinetic energy of the gas particles, leading to higher pressures and therefore higher partial pressures for each gas in the mixture.

5. What are some real-world applications of partial pressure?

Partial pressure is used in various fields such as chemistry, physics, and engineering. It is commonly used in the medical field to monitor oxygen levels in the blood and to assist with mechanical ventilation. It is also used in industrial processes for gas separation and purification.

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