Respuesta :
Explanation:
Partial pressure is defined as the pressure that is exerted by one of the gases present in a mixture if it occupies the same volume on its own.
As both nitrogen and xenon have occupied same volume. Therefore, both the gases will have same partial pressure.
It is known that average velocity is inversely proportional to molar mass of a gas. Hence, more is the molar mass of a gas lesser will be its average velocity.
Therefore, xenon having high molar mass will have less average velocity and nitrogen gas will have greatest average velocity.
Also, smaller is the molar mass of a gas more will be its rate of effusion because then its molecules will be able to spread readily into the surrounding.
Hence, nitrogen gas will have a higher rate of effusion through a small hole opened in the flask.
Average kinetic energy is represented as follows.
K.E = [tex]\frac{3}{2}kT[/tex]
As kinetic energy is directly proportional to temperature. So, with increase in temperature there will occur an increase in kinetic energy of the molecules.
Hence, average of kinetic energy will be same for both the gases.
A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. Both gases have the same partial pressure. Nitrogen is the gas for which the molecules or atoms have the greatest average velocity. Nitrogen is the gas that would have a higher rate of effusion through a small hole opened in the flask. The atoms or molecules of both gases have the same kinetic energy.
A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. Let's compare some properties.
A. Partial pressure
The partial pressure of a gas, according to Dalton's law, is a function of the number of moles, under the same conditions of volume and temperature. Thus, both gases will have the same partial pressure.
B. Average velocity
We can calculate the root-mean-square speed of the gas using the following expression.
[tex]v_{rms} = \sqrt{\frac{3RT}{M} }[/tex]
where,
- R: ideal gas constant
- T: absolute temperature
- M: molar mass
Nitrogen, with a lower molar mass, will have a higher average velocity.
C. Rate of effusion
According to Graham's law, the rate of effusion of a gas is inversely proportional to its molar mass.
Then, nitrogen, with a lower molar mass, will have a higher rate of effusion.
D. Kinetic energy
We can calculate the average kinetic energy per mole of gas using the following expression.
[tex]KE = \frac{3}{2} RT[/tex]
- R: ideal gas constant
- T: absolute temperature
At the same temperature, both gases have the same average kinetic energy.
A flask at room temperature contains exactly equal amounts (in moles) of nitrogen and xenon. Both gases have the same partial pressure. Nitrogen is the gas for which the molecules or atoms have the greatest average velocity. Nitrogen is the gas that would have a higher rate of effusion through a small hole opened in the flask. The atoms or molecules of both gases have the same kinetic energy.
Learn more: https://brainly.com/question/15217448
