Answered

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Suppose you have two identical 1.0 L sealed containers. Both containers are kept at exactly 25oC. One vessel contains only neon gas at 1.5 atm, and the other contains only xenon gas at 2.5 atm.


A) Is the average kinetic energy possessed by the neon atoms greater than, equal to, or less than that of the xenon atoms? Explain.



B) What variable must be changed in order to decrease the average kinetic energy of the xenon atoms?



C) Does the vessel with the xenon gas contain more, fewer, or the same number of gas particles as the vessel of neon gas? Explain.

Sagot :

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Answer:

See explanation

Explanation:

a)  The average kinetic energy of the molecules of a gas depends on the temperature and the molar mass of the gas. However, at the same temperature, all gases have the same average kinetic energy. Hence Xe and Ne atoms have the same average kinetic energy.

b) To decrease the kinetic energy of Xe atoms the temperature must be changed. When the temperature is changed, Xe a lower average kinetic energy due to its larger molar mass.

c) All gases occupying the same volume have equal number of particles at the same temperature and pressure according to Avogadro's law. Therefore, since Xe and Ne occupy the same volume at the same temperature but different pressures they do not contain the same number of particles. Xe gas contains more particles because there are more moles of Xe gas present than moles of Ne gas. The greater the number of moles of gas present, the more the number of gas particles present.

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